unit 1 introduction to chemistry chapter 1 read sections 1.1; 1.2 and 1.3
TRANSCRIPT
Unit 1Introduction to Chemistry
Chapter 1
Read sections 11 12 and 13
WorldviewA perspective from which we see and interpret all of life
ChristianJesus at the Center
Vs
HumanistMan at the Center
The Creation Mandate
bull And God said Let us make man in our image after our likeness and let them have dominion over the fish of the sea and over the fowl of the air and over the cattle and over all the earth and over every creeping thing that creepeth upon the earth
bull 27So God created man in his own image in the image of God created he him male and female created he them
bull 28And God blessed them and God said unto them Be fruitful and multiply and replenish the earth and subdue it and have dominion over the fish of the sea and over the fowl of the air and over every living thing that moveth
upon the earth
1st and 2nd Commandment
Love God
Love one Another
Dominion Science
Scientific Activity that Exercises Dominion for
the glory of God and the good of
others
What if microbes
were intelligentWorldview
1014 Microbes in a human body
bullQUIZ
What is Chemistry
the study of matter
and its changes
Matter is anything that occupies spaceAnd has mass
The Beginning
The Greeks believed there
were four elements
Early practical chemistry
household goods weapons
soap fermentation basic medicine
earth wind fire water
D ~~D___
D
___
Alchemy
Allegedly this substance would turn cheap metals into gold
the quest for the Philosopherrsquos Stone
(~500 ndash 1300 AD)
(the elixir the Sorcererrsquos Stone)
Alchemical symbols for substanceshellip
GOLD SILVER COPPER IRON SAND
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
WorldviewA perspective from which we see and interpret all of life
ChristianJesus at the Center
Vs
HumanistMan at the Center
The Creation Mandate
bull And God said Let us make man in our image after our likeness and let them have dominion over the fish of the sea and over the fowl of the air and over the cattle and over all the earth and over every creeping thing that creepeth upon the earth
bull 27So God created man in his own image in the image of God created he him male and female created he them
bull 28And God blessed them and God said unto them Be fruitful and multiply and replenish the earth and subdue it and have dominion over the fish of the sea and over the fowl of the air and over every living thing that moveth
upon the earth
1st and 2nd Commandment
Love God
Love one Another
Dominion Science
Scientific Activity that Exercises Dominion for
the glory of God and the good of
others
What if microbes
were intelligentWorldview
1014 Microbes in a human body
bullQUIZ
What is Chemistry
the study of matter
and its changes
Matter is anything that occupies spaceAnd has mass
The Beginning
The Greeks believed there
were four elements
Early practical chemistry
household goods weapons
soap fermentation basic medicine
earth wind fire water
D ~~D___
D
___
Alchemy
Allegedly this substance would turn cheap metals into gold
the quest for the Philosopherrsquos Stone
(~500 ndash 1300 AD)
(the elixir the Sorcererrsquos Stone)
Alchemical symbols for substanceshellip
GOLD SILVER COPPER IRON SAND
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
The Creation Mandate
bull And God said Let us make man in our image after our likeness and let them have dominion over the fish of the sea and over the fowl of the air and over the cattle and over all the earth and over every creeping thing that creepeth upon the earth
bull 27So God created man in his own image in the image of God created he him male and female created he them
bull 28And God blessed them and God said unto them Be fruitful and multiply and replenish the earth and subdue it and have dominion over the fish of the sea and over the fowl of the air and over every living thing that moveth
upon the earth
1st and 2nd Commandment
Love God
Love one Another
Dominion Science
Scientific Activity that Exercises Dominion for
the glory of God and the good of
others
What if microbes
were intelligentWorldview
1014 Microbes in a human body
bullQUIZ
What is Chemistry
the study of matter
and its changes
Matter is anything that occupies spaceAnd has mass
The Beginning
The Greeks believed there
were four elements
Early practical chemistry
household goods weapons
soap fermentation basic medicine
earth wind fire water
D ~~D___
D
___
Alchemy
Allegedly this substance would turn cheap metals into gold
the quest for the Philosopherrsquos Stone
(~500 ndash 1300 AD)
(the elixir the Sorcererrsquos Stone)
Alchemical symbols for substanceshellip
GOLD SILVER COPPER IRON SAND
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
1st and 2nd Commandment
Love God
Love one Another
Dominion Science
Scientific Activity that Exercises Dominion for
the glory of God and the good of
others
What if microbes
were intelligentWorldview
1014 Microbes in a human body
bullQUIZ
What is Chemistry
the study of matter
and its changes
Matter is anything that occupies spaceAnd has mass
The Beginning
The Greeks believed there
were four elements
Early practical chemistry
household goods weapons
soap fermentation basic medicine
earth wind fire water
D ~~D___
D
___
Alchemy
Allegedly this substance would turn cheap metals into gold
the quest for the Philosopherrsquos Stone
(~500 ndash 1300 AD)
(the elixir the Sorcererrsquos Stone)
Alchemical symbols for substanceshellip
GOLD SILVER COPPER IRON SAND
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Dominion Science
Scientific Activity that Exercises Dominion for
the glory of God and the good of
others
What if microbes
were intelligentWorldview
1014 Microbes in a human body
bullQUIZ
What is Chemistry
the study of matter
and its changes
Matter is anything that occupies spaceAnd has mass
The Beginning
The Greeks believed there
were four elements
Early practical chemistry
household goods weapons
soap fermentation basic medicine
earth wind fire water
D ~~D___
D
___
Alchemy
Allegedly this substance would turn cheap metals into gold
the quest for the Philosopherrsquos Stone
(~500 ndash 1300 AD)
(the elixir the Sorcererrsquos Stone)
Alchemical symbols for substanceshellip
GOLD SILVER COPPER IRON SAND
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
What if microbes
were intelligentWorldview
1014 Microbes in a human body
bullQUIZ
What is Chemistry
the study of matter
and its changes
Matter is anything that occupies spaceAnd has mass
The Beginning
The Greeks believed there
were four elements
Early practical chemistry
household goods weapons
soap fermentation basic medicine
earth wind fire water
D ~~D___
D
___
Alchemy
Allegedly this substance would turn cheap metals into gold
the quest for the Philosopherrsquos Stone
(~500 ndash 1300 AD)
(the elixir the Sorcererrsquos Stone)
Alchemical symbols for substanceshellip
GOLD SILVER COPPER IRON SAND
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
bullQUIZ
What is Chemistry
the study of matter
and its changes
Matter is anything that occupies spaceAnd has mass
The Beginning
The Greeks believed there
were four elements
Early practical chemistry
household goods weapons
soap fermentation basic medicine
earth wind fire water
D ~~D___
D
___
Alchemy
Allegedly this substance would turn cheap metals into gold
the quest for the Philosopherrsquos Stone
(~500 ndash 1300 AD)
(the elixir the Sorcererrsquos Stone)
Alchemical symbols for substanceshellip
GOLD SILVER COPPER IRON SAND
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
What is Chemistry
the study of matter
and its changes
Matter is anything that occupies spaceAnd has mass
The Beginning
The Greeks believed there
were four elements
Early practical chemistry
household goods weapons
soap fermentation basic medicine
earth wind fire water
D ~~D___
D
___
Alchemy
Allegedly this substance would turn cheap metals into gold
the quest for the Philosopherrsquos Stone
(~500 ndash 1300 AD)
(the elixir the Sorcererrsquos Stone)
Alchemical symbols for substanceshellip
GOLD SILVER COPPER IRON SAND
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Matter is anything that occupies spaceAnd has mass
The Beginning
The Greeks believed there
were four elements
Early practical chemistry
household goods weapons
soap fermentation basic medicine
earth wind fire water
D ~~D___
D
___
Alchemy
Allegedly this substance would turn cheap metals into gold
the quest for the Philosopherrsquos Stone
(~500 ndash 1300 AD)
(the elixir the Sorcererrsquos Stone)
Alchemical symbols for substanceshellip
GOLD SILVER COPPER IRON SAND
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
The Beginning
The Greeks believed there
were four elements
Early practical chemistry
household goods weapons
soap fermentation basic medicine
earth wind fire water
D ~~D___
D
___
Alchemy
Allegedly this substance would turn cheap metals into gold
the quest for the Philosopherrsquos Stone
(~500 ndash 1300 AD)
(the elixir the Sorcererrsquos Stone)
Alchemical symbols for substanceshellip
GOLD SILVER COPPER IRON SAND
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Alchemy
Allegedly this substance would turn cheap metals into gold
the quest for the Philosopherrsquos Stone
(~500 ndash 1300 AD)
(the elixir the Sorcererrsquos Stone)
Alchemical symbols for substanceshellip
GOLD SILVER COPPER IRON SAND
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
transmutation
we cannot
transmute elements into different elements
changing one substance
into another
COPPER GOLD
Philosopherrsquos
Stone
In ordinary chemical reactionshellip
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Alchemy was practiced in many regions of the
world including China and the Middle East
Alchemy arrived in western Europe
around the year 500 AD
Modern chemistry evolved from alchemy
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Contributions of alchemists
bull experimental techniquesbull new glasswarebull information about elementsbull developed several alloys
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Natural Science
Physical Science Earth and Space Science Life Science
Physics Chemistry Geology Astronomy Botany Zoology
Meteorology
Oceanography
Ecology
Genetics
Natural science covers a very broad range of knowledge
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 4
Modern Science
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Areas of Chemistryorganic
physicalinorganic
biochemistry
studies everything
except carbon
eg compounds
containing metals
the study of carbon
containing compounds
measuring physicalproperties ofsubstances
the chemistry ofliving things
eg the meltingpoint of gold
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Careers in Chemistry
bull research (new products)bull production (quality control)bull development (manufacturing)bull chemical salesbull software engineeringbull teaching
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
The skills you will develop by an earnest study
of chemistry will help you in any career field
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
The Scope of Chemistry
pharmaceuticals
nylon polyester rayon
bulk chemical manufacturing
petroleum products
synthetic fibers
acids bases fertilizers
fuels oils greases asphalt
1 in 10000 new products gets FDA approval
spandex
sulfuric acid (H2SO4) = 1 chemical
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Government Regulation of Chemicals
The various levels of government regulate
chemicals to protect the
OSHAworker
FDA
USDA
CPSC
consumer
EPAenvironment
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Chemistry impacts everyone
all fields of endeavor
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Letrsquos pause for a Quiz
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Safety ndash Extremely important in the Chemistry
Lab
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Safety Features of the Lab
safety showerfire blanketfire extinguisher eye wash
These are NOT toys but are important in emergencies
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
SAFETY in the Science Classroom
Obey the safety contractndash Use common sensendash No unauthorized experimentsndash Wear safety glassesndash Safety is an attitudendash Donrsquot take anything out of labndash Read and follow all instructions
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Toxicity
Which is more toxic
httplanscelanlgovtrainingFST2004images04chemicals1gif
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Material Safety Data Sheet (MSDS)
gives informationabout a chemical
-- lists ldquoDosrdquo and ldquoDonrsquotsrdquo
emergency procedures
--
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Chemical Exposure
a one-time exposure that causes damage
acute exposure vs chronic exposure
damage occurs after repeated exposure
reaction to drugs
or medicationeg eg smoking
asbestos
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
How Toxic is ldquoToxicrdquo
bull Flammablebull Explosivebull Radioactivebull Corrosivebull Irritantbull Carcinogenic (cancer causing)bull Mutagenic (mutations)bull Teratogenic (birth defects)
Chemicals may cause harm in many different ways
Science
The Functions of Science
pure science applied science
the search for knowledge facts
using knowledgein a practical way
eg properties of aluminum
strong
lightweight
good conductor
Corning Glass
NASArsquos Problem Design a materialthat is clear and can with-stand extreme differences in temperature without fail-ing (cracking)
Corning Glass Company FAILEDhellipbut SUCCEEDED at making great cookware that can withstand extremes in temperature Design a face shield
to protect and provideclear vision
The Functions of Science
pure science applied science
the search for knowledge facts
using knowledgein a practical way
eg properties of aluminum
strong
lightweight
good conductor
Corning Glass
NASArsquos Problem Design a materialthat is clear and can with-stand extreme differences in temperature without fail-ing (cracking)
Corning Glass Company FAILEDhellipbut SUCCEEDED at making great cookware that can withstand extremes in temperature Design a face shield
to protect and provideclear vision
Corning Glass
NASArsquos Problem Design a materialthat is clear and can with-stand extreme differences in temperature without fail-ing (cracking)
Corning Glass Company FAILEDhellipbut SUCCEEDED at making great cookware that can withstand extremes in temperature Design a face shield
to protect and provideclear vision
Aluminum Mining
bull 1850s aluminum sold for $500 lb
bull Charles Martin Hallbull Developed method to
extract aluminum from bauxite
bull Hallrsquos methodndash As a result $030lb
4-6 pounds bauxite
current 1 lb Al
+
=
Science attempts to establish causeeffect relationships
Science can NEVER prove a causeeffect relationship only make a
correlationhellip
risk-benefit analysis
weigh pros and cons before deciding
Because there are many considerations for each case ldquoblackwhite thinkingrdquo rarely
applies It is usually shades of grey
How doesscientific
knowledgeadvance
1 curiosity2 determination3 persistence4 good observations
The Scientific Method
The Skeptical Chemist
Robert Boyle
In ldquoThe Sceptical Chymistrdquo
Boyle stated that scientific speculation was worthless unless it was supportedby experimental evidence
This principle led to the development of the scientific method
(1661)
Key Be a good observer
observation inference
involves a judgmentor an assumption
uses the fivesenses
Types of DataObservations are also called data
qualitative data quantitative data
colorless liquid --
-- eg eg
descriptions
measurements 17 mL 83oC
(vs clear liquid)
Candle Observation Activity
A Description of a Burning Candle
A photograph of a burning candle is shown1 in the upper right corner The candle is cylindrical2 and has a diameter3 of about 3 cm The length of the candle was initially about 16 centimeters4 and it changed slowly5 during observation decreasing about 1 cm in one hour6 The candle is made of a translucent7 white8 solid9 which has a slight odor10 and no taste11 It is soft enough to be scratched with the fingernail12 There is a wick13 which extends from top to bottom14 of the candle along its central axis15 and protrudes about 5 mm above the top of the candle16 The wick is made of three strands of string braided together17 A candle is lit by holding a source of flame close to the wick for a few seconds Thereafter the source of flame can be removed and the flame sustains itself at the wick18 The burning candle makes no sound19 While burning the body of the candle remains cool to the touch20 except near the top Within about 15 cm of the top the candle is warm21 (but not hot) and sufficiently soft to mold easily22 The flame flickers in response to air currents23 and tends to become quite smoky while flickering24 In the absence of air currents the flame is of the form shown in the photograph though it retains some movement at all times25 The flame begins about 2 mm above the top of the candle26 and at itsbase the flame has a blue tint27 Immediately around the wick in a region about 2 mm wide and extending about 5 mm above the top of the wick28 the flame is dark29 This dark region is roughly conical in shape30 Around this zone and extending about 1 cm above the dark zone is a region which emits yellow light31 bright but not blinding32 The flame has rather sharply defined sides33 but a ragged top34 The wick is white where it emerges from the candle35 but from the base of the flame to the end of the wick36 it is black appearing burnt except for the last 05 cm where it glows red37 The wick curls over about 3 mm from its end38 As the candle becomes shorter the wick shortens too so as to extend roughly a constant length above the top of the candle39 Heat is emitted by the flame40 enough so that it becomes uncomfortable in 10 to 20 seconds if one holds his finger 10 cm to the side of the quiet flame41 or 10 ndash 12 cm above the flame42
Parts of the Scientific Method1 Identify an unknown
2 Make a hypothesis a testable prediction
3 Repeatedly experiment to test
hypothesis
a procedure order of events in
experiment
b variable any factor that couldinfluence the result
(ie a recipe of what was done)
4 conclusion must be supported with evidence from the data collected
A ScientificExperiment
Experiments must be controlled
Only one variable can be changed at a time The rest must be kept constant This allows the scientist to see what effect changing the IV has on the system
Independent variable
Dependent variable
the variable that is
manipulated (x-axis in a graph)
the variable that is measured It changes as you change the IV (y-axis)
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
risk-benefit analysis
weigh pros and cons before deciding
Because there are many considerations for each case ldquoblackwhite thinkingrdquo rarely
applies It is usually shades of grey
How doesscientific
knowledgeadvance
1 curiosity2 determination3 persistence4 good observations
The Scientific Method
The Skeptical Chemist
Robert Boyle
In ldquoThe Sceptical Chymistrdquo
Boyle stated that scientific speculation was worthless unless it was supportedby experimental evidence
This principle led to the development of the scientific method
(1661)
Key Be a good observer
observation inference
involves a judgmentor an assumption
uses the fivesenses
Types of DataObservations are also called data
qualitative data quantitative data
colorless liquid --
-- eg eg
descriptions
measurements 17 mL 83oC
(vs clear liquid)
Candle Observation Activity
A Description of a Burning Candle
A photograph of a burning candle is shown1 in the upper right corner The candle is cylindrical2 and has a diameter3 of about 3 cm The length of the candle was initially about 16 centimeters4 and it changed slowly5 during observation decreasing about 1 cm in one hour6 The candle is made of a translucent7 white8 solid9 which has a slight odor10 and no taste11 It is soft enough to be scratched with the fingernail12 There is a wick13 which extends from top to bottom14 of the candle along its central axis15 and protrudes about 5 mm above the top of the candle16 The wick is made of three strands of string braided together17 A candle is lit by holding a source of flame close to the wick for a few seconds Thereafter the source of flame can be removed and the flame sustains itself at the wick18 The burning candle makes no sound19 While burning the body of the candle remains cool to the touch20 except near the top Within about 15 cm of the top the candle is warm21 (but not hot) and sufficiently soft to mold easily22 The flame flickers in response to air currents23 and tends to become quite smoky while flickering24 In the absence of air currents the flame is of the form shown in the photograph though it retains some movement at all times25 The flame begins about 2 mm above the top of the candle26 and at itsbase the flame has a blue tint27 Immediately around the wick in a region about 2 mm wide and extending about 5 mm above the top of the wick28 the flame is dark29 This dark region is roughly conical in shape30 Around this zone and extending about 1 cm above the dark zone is a region which emits yellow light31 bright but not blinding32 The flame has rather sharply defined sides33 but a ragged top34 The wick is white where it emerges from the candle35 but from the base of the flame to the end of the wick36 it is black appearing burnt except for the last 05 cm where it glows red37 The wick curls over about 3 mm from its end38 As the candle becomes shorter the wick shortens too so as to extend roughly a constant length above the top of the candle39 Heat is emitted by the flame40 enough so that it becomes uncomfortable in 10 to 20 seconds if one holds his finger 10 cm to the side of the quiet flame41 or 10 ndash 12 cm above the flame42
Parts of the Scientific Method1 Identify an unknown
2 Make a hypothesis a testable prediction
3 Repeatedly experiment to test
hypothesis
a procedure order of events in
experiment
b variable any factor that couldinfluence the result
(ie a recipe of what was done)
4 conclusion must be supported with evidence from the data collected
A ScientificExperiment
Experiments must be controlled
Only one variable can be changed at a time The rest must be kept constant This allows the scientist to see what effect changing the IV has on the system
Independent variable
Dependent variable
the variable that is
manipulated (x-axis in a graph)
the variable that is measured It changes as you change the IV (y-axis)
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
How doesscientific
knowledgeadvance
1 curiosity2 determination3 persistence4 good observations
The Scientific Method
The Skeptical Chemist
Robert Boyle
In ldquoThe Sceptical Chymistrdquo
Boyle stated that scientific speculation was worthless unless it was supportedby experimental evidence
This principle led to the development of the scientific method
(1661)
Key Be a good observer
observation inference
involves a judgmentor an assumption
uses the fivesenses
Types of DataObservations are also called data
qualitative data quantitative data
colorless liquid --
-- eg eg
descriptions
measurements 17 mL 83oC
(vs clear liquid)
Candle Observation Activity
A Description of a Burning Candle
A photograph of a burning candle is shown1 in the upper right corner The candle is cylindrical2 and has a diameter3 of about 3 cm The length of the candle was initially about 16 centimeters4 and it changed slowly5 during observation decreasing about 1 cm in one hour6 The candle is made of a translucent7 white8 solid9 which has a slight odor10 and no taste11 It is soft enough to be scratched with the fingernail12 There is a wick13 which extends from top to bottom14 of the candle along its central axis15 and protrudes about 5 mm above the top of the candle16 The wick is made of three strands of string braided together17 A candle is lit by holding a source of flame close to the wick for a few seconds Thereafter the source of flame can be removed and the flame sustains itself at the wick18 The burning candle makes no sound19 While burning the body of the candle remains cool to the touch20 except near the top Within about 15 cm of the top the candle is warm21 (but not hot) and sufficiently soft to mold easily22 The flame flickers in response to air currents23 and tends to become quite smoky while flickering24 In the absence of air currents the flame is of the form shown in the photograph though it retains some movement at all times25 The flame begins about 2 mm above the top of the candle26 and at itsbase the flame has a blue tint27 Immediately around the wick in a region about 2 mm wide and extending about 5 mm above the top of the wick28 the flame is dark29 This dark region is roughly conical in shape30 Around this zone and extending about 1 cm above the dark zone is a region which emits yellow light31 bright but not blinding32 The flame has rather sharply defined sides33 but a ragged top34 The wick is white where it emerges from the candle35 but from the base of the flame to the end of the wick36 it is black appearing burnt except for the last 05 cm where it glows red37 The wick curls over about 3 mm from its end38 As the candle becomes shorter the wick shortens too so as to extend roughly a constant length above the top of the candle39 Heat is emitted by the flame40 enough so that it becomes uncomfortable in 10 to 20 seconds if one holds his finger 10 cm to the side of the quiet flame41 or 10 ndash 12 cm above the flame42
Parts of the Scientific Method1 Identify an unknown
2 Make a hypothesis a testable prediction
3 Repeatedly experiment to test
hypothesis
a procedure order of events in
experiment
b variable any factor that couldinfluence the result
(ie a recipe of what was done)
4 conclusion must be supported with evidence from the data collected
A ScientificExperiment
Experiments must be controlled
Only one variable can be changed at a time The rest must be kept constant This allows the scientist to see what effect changing the IV has on the system
Independent variable
Dependent variable
the variable that is
manipulated (x-axis in a graph)
the variable that is measured It changes as you change the IV (y-axis)
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
The Scientific Method
The Skeptical Chemist
Robert Boyle
In ldquoThe Sceptical Chymistrdquo
Boyle stated that scientific speculation was worthless unless it was supportedby experimental evidence
This principle led to the development of the scientific method
(1661)
Key Be a good observer
observation inference
involves a judgmentor an assumption
uses the fivesenses
Types of DataObservations are also called data
qualitative data quantitative data
colorless liquid --
-- eg eg
descriptions
measurements 17 mL 83oC
(vs clear liquid)
Candle Observation Activity
A Description of a Burning Candle
A photograph of a burning candle is shown1 in the upper right corner The candle is cylindrical2 and has a diameter3 of about 3 cm The length of the candle was initially about 16 centimeters4 and it changed slowly5 during observation decreasing about 1 cm in one hour6 The candle is made of a translucent7 white8 solid9 which has a slight odor10 and no taste11 It is soft enough to be scratched with the fingernail12 There is a wick13 which extends from top to bottom14 of the candle along its central axis15 and protrudes about 5 mm above the top of the candle16 The wick is made of three strands of string braided together17 A candle is lit by holding a source of flame close to the wick for a few seconds Thereafter the source of flame can be removed and the flame sustains itself at the wick18 The burning candle makes no sound19 While burning the body of the candle remains cool to the touch20 except near the top Within about 15 cm of the top the candle is warm21 (but not hot) and sufficiently soft to mold easily22 The flame flickers in response to air currents23 and tends to become quite smoky while flickering24 In the absence of air currents the flame is of the form shown in the photograph though it retains some movement at all times25 The flame begins about 2 mm above the top of the candle26 and at itsbase the flame has a blue tint27 Immediately around the wick in a region about 2 mm wide and extending about 5 mm above the top of the wick28 the flame is dark29 This dark region is roughly conical in shape30 Around this zone and extending about 1 cm above the dark zone is a region which emits yellow light31 bright but not blinding32 The flame has rather sharply defined sides33 but a ragged top34 The wick is white where it emerges from the candle35 but from the base of the flame to the end of the wick36 it is black appearing burnt except for the last 05 cm where it glows red37 The wick curls over about 3 mm from its end38 As the candle becomes shorter the wick shortens too so as to extend roughly a constant length above the top of the candle39 Heat is emitted by the flame40 enough so that it becomes uncomfortable in 10 to 20 seconds if one holds his finger 10 cm to the side of the quiet flame41 or 10 ndash 12 cm above the flame42
Parts of the Scientific Method1 Identify an unknown
2 Make a hypothesis a testable prediction
3 Repeatedly experiment to test
hypothesis
a procedure order of events in
experiment
b variable any factor that couldinfluence the result
(ie a recipe of what was done)
4 conclusion must be supported with evidence from the data collected
A ScientificExperiment
Experiments must be controlled
Only one variable can be changed at a time The rest must be kept constant This allows the scientist to see what effect changing the IV has on the system
Independent variable
Dependent variable
the variable that is
manipulated (x-axis in a graph)
the variable that is measured It changes as you change the IV (y-axis)
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
The Skeptical Chemist
Robert Boyle
In ldquoThe Sceptical Chymistrdquo
Boyle stated that scientific speculation was worthless unless it was supportedby experimental evidence
This principle led to the development of the scientific method
(1661)
Key Be a good observer
observation inference
involves a judgmentor an assumption
uses the fivesenses
Types of DataObservations are also called data
qualitative data quantitative data
colorless liquid --
-- eg eg
descriptions
measurements 17 mL 83oC
(vs clear liquid)
Candle Observation Activity
A Description of a Burning Candle
A photograph of a burning candle is shown1 in the upper right corner The candle is cylindrical2 and has a diameter3 of about 3 cm The length of the candle was initially about 16 centimeters4 and it changed slowly5 during observation decreasing about 1 cm in one hour6 The candle is made of a translucent7 white8 solid9 which has a slight odor10 and no taste11 It is soft enough to be scratched with the fingernail12 There is a wick13 which extends from top to bottom14 of the candle along its central axis15 and protrudes about 5 mm above the top of the candle16 The wick is made of three strands of string braided together17 A candle is lit by holding a source of flame close to the wick for a few seconds Thereafter the source of flame can be removed and the flame sustains itself at the wick18 The burning candle makes no sound19 While burning the body of the candle remains cool to the touch20 except near the top Within about 15 cm of the top the candle is warm21 (but not hot) and sufficiently soft to mold easily22 The flame flickers in response to air currents23 and tends to become quite smoky while flickering24 In the absence of air currents the flame is of the form shown in the photograph though it retains some movement at all times25 The flame begins about 2 mm above the top of the candle26 and at itsbase the flame has a blue tint27 Immediately around the wick in a region about 2 mm wide and extending about 5 mm above the top of the wick28 the flame is dark29 This dark region is roughly conical in shape30 Around this zone and extending about 1 cm above the dark zone is a region which emits yellow light31 bright but not blinding32 The flame has rather sharply defined sides33 but a ragged top34 The wick is white where it emerges from the candle35 but from the base of the flame to the end of the wick36 it is black appearing burnt except for the last 05 cm where it glows red37 The wick curls over about 3 mm from its end38 As the candle becomes shorter the wick shortens too so as to extend roughly a constant length above the top of the candle39 Heat is emitted by the flame40 enough so that it becomes uncomfortable in 10 to 20 seconds if one holds his finger 10 cm to the side of the quiet flame41 or 10 ndash 12 cm above the flame42
Parts of the Scientific Method1 Identify an unknown
2 Make a hypothesis a testable prediction
3 Repeatedly experiment to test
hypothesis
a procedure order of events in
experiment
b variable any factor that couldinfluence the result
(ie a recipe of what was done)
4 conclusion must be supported with evidence from the data collected
A ScientificExperiment
Experiments must be controlled
Only one variable can be changed at a time The rest must be kept constant This allows the scientist to see what effect changing the IV has on the system
Independent variable
Dependent variable
the variable that is
manipulated (x-axis in a graph)
the variable that is measured It changes as you change the IV (y-axis)
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Key Be a good observer
observation inference
involves a judgmentor an assumption
uses the fivesenses
Types of DataObservations are also called data
qualitative data quantitative data
colorless liquid --
-- eg eg
descriptions
measurements 17 mL 83oC
(vs clear liquid)
Candle Observation Activity
A Description of a Burning Candle
A photograph of a burning candle is shown1 in the upper right corner The candle is cylindrical2 and has a diameter3 of about 3 cm The length of the candle was initially about 16 centimeters4 and it changed slowly5 during observation decreasing about 1 cm in one hour6 The candle is made of a translucent7 white8 solid9 which has a slight odor10 and no taste11 It is soft enough to be scratched with the fingernail12 There is a wick13 which extends from top to bottom14 of the candle along its central axis15 and protrudes about 5 mm above the top of the candle16 The wick is made of three strands of string braided together17 A candle is lit by holding a source of flame close to the wick for a few seconds Thereafter the source of flame can be removed and the flame sustains itself at the wick18 The burning candle makes no sound19 While burning the body of the candle remains cool to the touch20 except near the top Within about 15 cm of the top the candle is warm21 (but not hot) and sufficiently soft to mold easily22 The flame flickers in response to air currents23 and tends to become quite smoky while flickering24 In the absence of air currents the flame is of the form shown in the photograph though it retains some movement at all times25 The flame begins about 2 mm above the top of the candle26 and at itsbase the flame has a blue tint27 Immediately around the wick in a region about 2 mm wide and extending about 5 mm above the top of the wick28 the flame is dark29 This dark region is roughly conical in shape30 Around this zone and extending about 1 cm above the dark zone is a region which emits yellow light31 bright but not blinding32 The flame has rather sharply defined sides33 but a ragged top34 The wick is white where it emerges from the candle35 but from the base of the flame to the end of the wick36 it is black appearing burnt except for the last 05 cm where it glows red37 The wick curls over about 3 mm from its end38 As the candle becomes shorter the wick shortens too so as to extend roughly a constant length above the top of the candle39 Heat is emitted by the flame40 enough so that it becomes uncomfortable in 10 to 20 seconds if one holds his finger 10 cm to the side of the quiet flame41 or 10 ndash 12 cm above the flame42
Parts of the Scientific Method1 Identify an unknown
2 Make a hypothesis a testable prediction
3 Repeatedly experiment to test
hypothesis
a procedure order of events in
experiment
b variable any factor that couldinfluence the result
(ie a recipe of what was done)
4 conclusion must be supported with evidence from the data collected
A ScientificExperiment
Experiments must be controlled
Only one variable can be changed at a time The rest must be kept constant This allows the scientist to see what effect changing the IV has on the system
Independent variable
Dependent variable
the variable that is
manipulated (x-axis in a graph)
the variable that is measured It changes as you change the IV (y-axis)
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Types of DataObservations are also called data
qualitative data quantitative data
colorless liquid --
-- eg eg
descriptions
measurements 17 mL 83oC
(vs clear liquid)
Candle Observation Activity
A Description of a Burning Candle
A photograph of a burning candle is shown1 in the upper right corner The candle is cylindrical2 and has a diameter3 of about 3 cm The length of the candle was initially about 16 centimeters4 and it changed slowly5 during observation decreasing about 1 cm in one hour6 The candle is made of a translucent7 white8 solid9 which has a slight odor10 and no taste11 It is soft enough to be scratched with the fingernail12 There is a wick13 which extends from top to bottom14 of the candle along its central axis15 and protrudes about 5 mm above the top of the candle16 The wick is made of three strands of string braided together17 A candle is lit by holding a source of flame close to the wick for a few seconds Thereafter the source of flame can be removed and the flame sustains itself at the wick18 The burning candle makes no sound19 While burning the body of the candle remains cool to the touch20 except near the top Within about 15 cm of the top the candle is warm21 (but not hot) and sufficiently soft to mold easily22 The flame flickers in response to air currents23 and tends to become quite smoky while flickering24 In the absence of air currents the flame is of the form shown in the photograph though it retains some movement at all times25 The flame begins about 2 mm above the top of the candle26 and at itsbase the flame has a blue tint27 Immediately around the wick in a region about 2 mm wide and extending about 5 mm above the top of the wick28 the flame is dark29 This dark region is roughly conical in shape30 Around this zone and extending about 1 cm above the dark zone is a region which emits yellow light31 bright but not blinding32 The flame has rather sharply defined sides33 but a ragged top34 The wick is white where it emerges from the candle35 but from the base of the flame to the end of the wick36 it is black appearing burnt except for the last 05 cm where it glows red37 The wick curls over about 3 mm from its end38 As the candle becomes shorter the wick shortens too so as to extend roughly a constant length above the top of the candle39 Heat is emitted by the flame40 enough so that it becomes uncomfortable in 10 to 20 seconds if one holds his finger 10 cm to the side of the quiet flame41 or 10 ndash 12 cm above the flame42
Parts of the Scientific Method1 Identify an unknown
2 Make a hypothesis a testable prediction
3 Repeatedly experiment to test
hypothesis
a procedure order of events in
experiment
b variable any factor that couldinfluence the result
(ie a recipe of what was done)
4 conclusion must be supported with evidence from the data collected
A ScientificExperiment
Experiments must be controlled
Only one variable can be changed at a time The rest must be kept constant This allows the scientist to see what effect changing the IV has on the system
Independent variable
Dependent variable
the variable that is
manipulated (x-axis in a graph)
the variable that is measured It changes as you change the IV (y-axis)
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Candle Observation Activity
A Description of a Burning Candle
A photograph of a burning candle is shown1 in the upper right corner The candle is cylindrical2 and has a diameter3 of about 3 cm The length of the candle was initially about 16 centimeters4 and it changed slowly5 during observation decreasing about 1 cm in one hour6 The candle is made of a translucent7 white8 solid9 which has a slight odor10 and no taste11 It is soft enough to be scratched with the fingernail12 There is a wick13 which extends from top to bottom14 of the candle along its central axis15 and protrudes about 5 mm above the top of the candle16 The wick is made of three strands of string braided together17 A candle is lit by holding a source of flame close to the wick for a few seconds Thereafter the source of flame can be removed and the flame sustains itself at the wick18 The burning candle makes no sound19 While burning the body of the candle remains cool to the touch20 except near the top Within about 15 cm of the top the candle is warm21 (but not hot) and sufficiently soft to mold easily22 The flame flickers in response to air currents23 and tends to become quite smoky while flickering24 In the absence of air currents the flame is of the form shown in the photograph though it retains some movement at all times25 The flame begins about 2 mm above the top of the candle26 and at itsbase the flame has a blue tint27 Immediately around the wick in a region about 2 mm wide and extending about 5 mm above the top of the wick28 the flame is dark29 This dark region is roughly conical in shape30 Around this zone and extending about 1 cm above the dark zone is a region which emits yellow light31 bright but not blinding32 The flame has rather sharply defined sides33 but a ragged top34 The wick is white where it emerges from the candle35 but from the base of the flame to the end of the wick36 it is black appearing burnt except for the last 05 cm where it glows red37 The wick curls over about 3 mm from its end38 As the candle becomes shorter the wick shortens too so as to extend roughly a constant length above the top of the candle39 Heat is emitted by the flame40 enough so that it becomes uncomfortable in 10 to 20 seconds if one holds his finger 10 cm to the side of the quiet flame41 or 10 ndash 12 cm above the flame42
Parts of the Scientific Method1 Identify an unknown
2 Make a hypothesis a testable prediction
3 Repeatedly experiment to test
hypothesis
a procedure order of events in
experiment
b variable any factor that couldinfluence the result
(ie a recipe of what was done)
4 conclusion must be supported with evidence from the data collected
A ScientificExperiment
Experiments must be controlled
Only one variable can be changed at a time The rest must be kept constant This allows the scientist to see what effect changing the IV has on the system
Independent variable
Dependent variable
the variable that is
manipulated (x-axis in a graph)
the variable that is measured It changes as you change the IV (y-axis)
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
A Description of a Burning Candle
A photograph of a burning candle is shown1 in the upper right corner The candle is cylindrical2 and has a diameter3 of about 3 cm The length of the candle was initially about 16 centimeters4 and it changed slowly5 during observation decreasing about 1 cm in one hour6 The candle is made of a translucent7 white8 solid9 which has a slight odor10 and no taste11 It is soft enough to be scratched with the fingernail12 There is a wick13 which extends from top to bottom14 of the candle along its central axis15 and protrudes about 5 mm above the top of the candle16 The wick is made of three strands of string braided together17 A candle is lit by holding a source of flame close to the wick for a few seconds Thereafter the source of flame can be removed and the flame sustains itself at the wick18 The burning candle makes no sound19 While burning the body of the candle remains cool to the touch20 except near the top Within about 15 cm of the top the candle is warm21 (but not hot) and sufficiently soft to mold easily22 The flame flickers in response to air currents23 and tends to become quite smoky while flickering24 In the absence of air currents the flame is of the form shown in the photograph though it retains some movement at all times25 The flame begins about 2 mm above the top of the candle26 and at itsbase the flame has a blue tint27 Immediately around the wick in a region about 2 mm wide and extending about 5 mm above the top of the wick28 the flame is dark29 This dark region is roughly conical in shape30 Around this zone and extending about 1 cm above the dark zone is a region which emits yellow light31 bright but not blinding32 The flame has rather sharply defined sides33 but a ragged top34 The wick is white where it emerges from the candle35 but from the base of the flame to the end of the wick36 it is black appearing burnt except for the last 05 cm where it glows red37 The wick curls over about 3 mm from its end38 As the candle becomes shorter the wick shortens too so as to extend roughly a constant length above the top of the candle39 Heat is emitted by the flame40 enough so that it becomes uncomfortable in 10 to 20 seconds if one holds his finger 10 cm to the side of the quiet flame41 or 10 ndash 12 cm above the flame42
Parts of the Scientific Method1 Identify an unknown
2 Make a hypothesis a testable prediction
3 Repeatedly experiment to test
hypothesis
a procedure order of events in
experiment
b variable any factor that couldinfluence the result
(ie a recipe of what was done)
4 conclusion must be supported with evidence from the data collected
A ScientificExperiment
Experiments must be controlled
Only one variable can be changed at a time The rest must be kept constant This allows the scientist to see what effect changing the IV has on the system
Independent variable
Dependent variable
the variable that is
manipulated (x-axis in a graph)
the variable that is measured It changes as you change the IV (y-axis)
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Parts of the Scientific Method1 Identify an unknown
2 Make a hypothesis a testable prediction
3 Repeatedly experiment to test
hypothesis
a procedure order of events in
experiment
b variable any factor that couldinfluence the result
(ie a recipe of what was done)
4 conclusion must be supported with evidence from the data collected
A ScientificExperiment
Experiments must be controlled
Only one variable can be changed at a time The rest must be kept constant This allows the scientist to see what effect changing the IV has on the system
Independent variable
Dependent variable
the variable that is
manipulated (x-axis in a graph)
the variable that is measured It changes as you change the IV (y-axis)
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
A ScientificExperiment
Experiments must be controlled
Only one variable can be changed at a time The rest must be kept constant This allows the scientist to see what effect changing the IV has on the system
Independent variable
Dependent variable
the variable that is
manipulated (x-axis in a graph)
the variable that is measured It changes as you change the IV (y-axis)
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
A Controlled Experiment
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Make observationMake observation
Ask questionAsk question
Develophypothesis
Develophypothesis
Test hypothesis with an
experiment
Test hypothesis with an
experiment
Analyze dataand draw
conclusions
Analyze dataand draw
conclusions
Hypothesis IS
supported
Hypothesis IS
supported
Hypothesis is NOT
supported
Hypothesis is NOT
supported
Developtheory
Developtheory
Test hypothesis with furtherexperiments
Test hypothesis with furtherexperiments
Revisehypothesis
Revisehypothesis
Wysession Frank Yancopoulos Physical Science Concepts in Action 2004 page 8
Scientific Method
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Letrsquos pause for a Quiz
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Scientific Law vs Scientific Theory
law states what happens ie a relationship between various quantities
-- eg Newtonrsquos law of
gravity
-- Laws are often written in
the form ofhellip an equation1 22g
G m mF
r
laws of conservation
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Theory of Gravity
Atomic Theory
tries to explain WHY or
HOW something happens
theory
-- eg
-- based on current evidence
images of nickel atomstaken by an STM
a scanning tunneling microscope (STM)
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Manipulating Numerical Data
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Graphs
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Bar Graphshows how many of something
are in each category
0
2
4
6
8
10
A B C D F
Chemistry Grades
o
f st
ud
ents
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Pie Graph shows how a whole is broken into parts
Entertainment (40)
Food (25)
Clothing (20)
Savings (15)
Percentage ofWeekly Income
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Line Graphshows continuous change
0
10
20
30
40
50
60
Jan Feb Mar Apr
Month
Sh
are
Pri
ce (
$)
Stock Price over Time
you will always use a line graph In chemistryhellip
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Elements of a ldquogoodrdquo line graph
2 axes labeled with units
Temp v Vol for a Gas at Constant Pressure
0123456789
10
120 140 160 180 200 220 240
Temp (K)
Vo
lum
e (
L)
4 use the available space
1 title
3 neat
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Graphing HW
TimeTotal Dist
cycled (km)8 am 0
9 am 12
10 am 23
11 am 33
noon 42
1 pm 50
2 pm 57
3 pm 63
4 pm 688 am 9 am 10 am 11 am noon 1 pm 2 pm 3 pm 4 pm
0
10
20
30
40
50
60
70
80
Total Distance Cycled (km)
Time (h)
Dis
tan
ce C
ycle
d (
km)
Extrapolation predicting a pattern outside of a data set using the graph
Interpolation estimating a data point within the set of data using the pattern of the graph
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Letrsquos Pause for a Test
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Essential Mathof Chemistry
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Scientific Notationhellipused to express very large or very small
numbers Also used to maintain correct Significant Figures
Form ( from 1 to 9999) x 10exponent
800 = 8 x 10 x 10
= 8 x 102
2531 = 2531 x 10 x 10 x 10
= 2531 x 103
00014 = 14 10 10 10
= 14 x 10ndash3
(-) exponent = number lt 1 (+) exponent = number gt 1
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Put in standard form
187 x 10ndash5 = 00000187
37 x 108 = 370000000
788 x 101 = 788
2164 x 10ndash2 = 002164
Change to scientific notation
12340 = 1234 x 104
0369 = 369 x 10ndash1
0008 = 8 x 10ndash3
1000000000 = 1 x 109
602 x 1023 = 602000000000000000000000
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Using the Exponent Key EXPEE
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
The EE or EXP or E key means ldquotimes 10 to thehelliprdquo
How to type out 602 x 1023
6 EE 0 32 2
6 y x 0 32 2
x 16 0 2 EE 320
y x 32x 16 0 2 0
nothellip
orhellip
and nothellip
How to type out 602 x 1023
6 EE 0 32 2
WRONG
WRONG
TOO MUCH WORK
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Also know when to hit your (ndash) sign
(before the number
after the number
or either one)
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Now letrsquos do some multiplication and division
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
43 x 10ndash15 43 E ndash15or
12 x 105 28 x 1019
But instead is writtenhellip
=
1 2 EE 5
92 8 EE 1
Type this calculation in like this
This is NOT writtenhellip 43ndash15
42857143 ndash15Calculator giveshellip
42857143 Endash15orhellip
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
ndash65 x 10ndash19
535 x 103 or 5350
29 x 1023
75 x 10ndash6 (ndash87 x 10ndash14) =
435 x 106 (123 x 10ndash3) =
576 x 10ndash16 986 x 10ndash4 =
88 x 1011 x 33 x 1011 =
584 x 10ndash13
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
All numerical data are the result
of uncertain measurements
8 m
Accuracy and Precision
precision a measure of the degree of
fineness of a measurement it
depends on the extent to which the
instrument is calibrated
eg vs 800 m vs 800000 m
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
0653 m
When repeated precise measurements yield similar answers each time
eg precisehellip
imprecisehellip
0652 m
0654 m
07 m
08 m
06 m
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
accuracy how close a measured
value is to the true value
Three types of error can affect accuracy
human error
method error
instrument error
(minimized with repeated measurements)
eg parallax in measuring with a meter stick
eg bathroom scale that always reads 5 lbs too heavy
mistake in reading instrument
or recording results
measuring device is
improperly calibrated
using measuring instrument improperly
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Percent Error
bull Indicates accuracy of a measurement
001
accepted
alexperimenterror
accepted
your value
accepted valueCourtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Percent Errorbull A student determines the density of a
substance to be 140 gmL Find the error if the accepted value of the density is 136 gmL
100gmL 136
gmL 136gmL 140error
error = 29
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Significant Figures
bull Indicates precision of a measurementbull Sig figs in a measurement include the known
digits plus a final estimated digit
235 cm
Courtesy Christy Johannesson wwwnisdnetcommunicationsartspageschem
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Practice Measuring
45 cm
454 cm
30 cm
Timberlake Chemistry 7th Edition page 7
cm0 1 2 3 4 5
cm0 1 2 3 4 5
cm0 1 2 3 4 5
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Significant Figures ExampleA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples 9287 mL NO
Because the samples were each measured with a different level of precision we must factor that into our calculations by identifying significant figures (sig figs)
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Measurement and Precisionbull The last digit of any measured number is
assumed to be an estimate (uncertain)bull The second to last digit is assumed to be
known with certainty
A (255 mL) B (1637 mL) C (51 mL)
26
25 164
163
60
50
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Rules for Identifying the Number of Significant Figures
Counting SF in a numberNon-zero numbers ALWAYS count as SFZeroes
Left NEVER count as SF (0000345)Middle ALWAYS count as SF (5001)Right sometimeshellip
w decimal point count as SF (2510)wo decimal point DO NOT count as SF (8200)
Exact Numbers IGNORE SF (assumed to have an infinite number of SF)
Counts (28 students in this class)Constants (1 mol = 6022 x 1023)Conversions (1 in = 254 cm)
Relative to the non-zero numbers
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
How many Sig Figs
Measurement Number of SF Measurement Number of SF
25 g
0030 kg
1240560 x 106 mg
6 x 104 sec
24631 g
2006 cm
1050 m
012 kg
1240560 cm
6000000 kg
600 x 106 kg
409 cm
29200 dm
002500 g
2
2
7
1
5
4
4
2
7
1
3
3
5
4
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Sig Figs with CalculationsNote For any calculations always perform the entire calculation without rounding and then round the final answer
AdditionSubtractionbull Round the answer to the LEAST number of
decimal places found (least precise)1131 + 33264 + 41 = 48674
MultiplicationDivisionbull Round the answer to the smallest number of
SF found5282 x 342 = 1806444
rarr rounded to 487
rarr rounded to 181 (342 only has 3 SF)
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Back to the original questionhellipA student is combining separate water samples all of differing volumes into one large bucket Samples A B and C are 255 mL 1637 mL and 51 mL respectively Once combined what is the total volume of all the samples
255 mL + 1637 mL + 51 mL = 9287 mL
93 mL
Could I write that as 930 NO
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Round to the correct number of significant figures
Calculator sayshellip 2 sig figs 3 sig figs 5 sig figs
756
0528396
387600
4200
84845E-4
76 756 75600
38760 x 105388000390000
0528400528053
85 x 10ndash4
42000 x 103 420 x 1034200
848 x 10ndash4 84845 x 10ndash4
= requires scientific notation
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Units must be carried into the
answer unless they cancel
064 kgms2
52 kg (29 m)
(18 s)(13 s)=
48 g (23 s)
(18 s)(37 s)= 017 g
s
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Solve for x x + y = z
x + y = z ndash y ndash y
x = z ndash y
x and y are connected by addition Separate them using subtraction In general use opposing functions to separate things
The +y and ndashy cancel on the left
leaving us withhellip
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Solve for x x ndash 24 = 13
x ndash 24 = 13 +24 +24
x = 37
x and 24 are connected by subtraction Separate them using the opposite function addition
The ndash24 and +24 cancel on the left
leaving us withhellip
Numerical Example
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Solve for x F = k x
F = k xk k
x = Fk __
x and k are connected by multiplication Separate them using the opposite function division
( )__1k
F = k x( )__1k
(or)
The two krsquos cancel on the right
leaving us withhellip
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Numerical Example
Solve for x 8 = 7 x
8 = 7 x7 7
x and 7 are connected by multiplication Separate them using the opposite function division
( )__17
8 = 7 x( )__17
(or)
The two 7rsquos cancel on the right
leaving us withhellipx =
87 __
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Solve for x ___ x
BA = TRH
___
BAH = xTR
One way to solve this is to cross-multiply BAH = xTR
Then divide both sides by TR
The answer ishellip ___BAHTR
x =
1TR( )___1
TR( )___
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Solve for T2 wherehellip
P1 = 108 atm
P2 = 086 atm
V1 = 322 L
V2 = 143 L
T1 = 373 K
P1V1T2 =P2V2T1
____ T1
P1V1 = P2V2
T2
____
1P1V1
( )____ 1P1V1
( )____
T2 = P1V1
______P2V2T1
130T2 = (108 atm)(322 L)_____________________(086 atm)(143 L)(373 K)
= K
Yes you will do math like this You will learn to love it
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Letrsquos pause for a Quiz
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
The Metric System
from
Indu
stry
Wee
k 1
981
Nov
embe
r 30
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
The SI (Metric) Systembull Recall
kilo hecto deca
Base Units
metergramliter
deci centi milli
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
How can you remember the order of the metric system prefixes
bull King Henry Died by Drinking Chocolate Milk (Use this pneumonic device)ndash King Kilondash Henry Hectondash Died Decandash By Base (m L g)ndash Drinking Decindash Chocolate Centindash Milk Milli
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Prefixes to know in the SI (Metric) System
Power of 10 for Prefix Symbol Meaning Scientific Notation_______________________________________________________________________
mega- M 1000000 106
kilo- k 1000 103
deci- d 01 10-1
centi- c 001 10-2
milli- m 0001 10-3
micro- m 0000001 10-6
nano- n 0000000001 10-9
The Commonly Used Prefixes in the SI System
Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 118
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Common SI Equivalents
Also
1 mL = 1 cm3 and 1 L = 1 dm3
You will be responsible for knowing these
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Letrsquos have another quiz
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Conversion Factors andUnit Cancellation
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
How many cm are in 132 meters
conversion factors
equality
or
132 m = 132 cm
1 m = 100 cm
______1 m100 cm
We use the idea of unit cancellation
to decide upon which one of the two
conversion factors we choose
______1 m
100 cm
1 m100 cm
(or 001 m = 1 cm)
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
How many m is 872 cm
conversion factors
equality
or
872 cm = 00872 m
1 m = 100 cm
______1 m100 cm
Again the units must cancel
______1 m
100 cm
1 m100 cm
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
How many kilometers is 15000 decimeters
15000 dm
= 15 km1000 m
1 km10 dm
1 m
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
How many seconds is 438 days
= 378432 s1 h
60 min24 h1 d 1 min
60 s____( ) ( )____( )_____438 d
378 x 105 sIf we are accounting for significant figures we would change this tohellip
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
4 Convert 412 cm2 to mm2
412 cm2
Recall thathellip 1 cm = 10 mm
= 4120 mm2
1 cm2
102 mm2
( )2 ( )2
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Simple Mathwith
Conversion Factors
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Find area of rectangle
A = L W
= (46 cm)(91 cm)
91 cm= 42 cm2 cm
46 cm
Convert to m2 42 cm2 ( )______100 cm
1 m 2 = 00042 m2
Convert to mm2 42 cm2 ( )______ 1 cm10 mm 2 = 4200 mm2
cmcm
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
For the rectangular solid
Find volume
Length = 142 cm
Width = 86 cm
Height = 215 cm
V = L W H
= (142 cm)(86 cm)(215 cm)
= 2600 cm3
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Density how tightly packed the particles are
Density =
Typical units
gcm3 for solids gmL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass liquid or solid
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
To find volume usehellip
1 a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V =
VfinalVinitial
Vobject = Vfinal ndash Vinitial
2
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Density Calculations
1 A sample of lead (Pb) has mass 2270 g and volume 2000 cm3
Find samplersquos density
Vm
D 3cm 20g 227
m
V D
2 Another sample of lead occupies 162 cm3
of space Find samplersquos mass
33 cm 162
cmg
1135 m = D V = 184
3cmg
= 1135
g
V
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Indiana Jones Density
bull Watch the famous opening scene to Indiana Jones and the Raiders of the Lost Ark
bull The ldquopure goldrdquo idol has a density of 193 gcm3 How much would it mass
bull Indy replaces the idol with a bag of sand (density = 25 gcm3) Why did he activate the booby trap How much sand should he have used
bull Did you see that toss at the end How much would the idol weigh in lbs (22 lb per kg)
19300 g
7720 cm3 or 772 L
425 lbs
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
3cmg
3 A 119 g solid cylinder has radius 180 cm and height 150 cm Find samplersquos density
15 cm
18 cm
m
V D
m
V = p r2 h
Vm
D
= p (18 cm)2(15 cm)
= 15268
3cm 15268
g 1195 = 779
cm3
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
4 A 153 g rectangular solid has edge lengths 820 cm 510 cm and 470 cm Will this object sink in water
82 cm
51 cm
47 cm
m
V D
Vm
D
(Find the objectrsquos density and compare it to waterrsquos density)
m
V = l w h
= 820 cm (510 cm)(470 cm)
3cmg
= 19655
3cm 19655
g 153 = 0778
cm3
lt 1 No it floats
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Galilean Thermometer ProblemOn a cold morning a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group Where are the bulbs At thetop of the thermometer at the bottom or elsewhere
1 Bulbs have essentially fixed masses
and volumes Therefore each bulb has a fixed density 2 The surrounding liquid has a fixed
mass but its volume is extremely
temperature-dependent
D1
D2
D3
D4
D5
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
D1
D2
D3
D4
D5
3 The density of the liquid can be written ashellip
liq
liqliq V
m D sohellip
hellipif the liquid is cold hellipbut if itrsquos hot
mliq =
On a cold morningwhere are the bulbs AT THE TOP
Vliq
mliq Dliq=
VliqDliq
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Basic Concepts in Chemistry
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
chemical any substance that takes part in
or occurs as a result of
a chemical reaction
All matter can be considered to be
chemicals or mixtures of chemicals
chemical reaction a rearrangement ofatoms such thathellip
ldquowhat you started withrdquodiffers from
ldquowhat you end up withrdquo products
reactants
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
methane + oxygen
+ H2O(g)
carbondioxide
O2(g) CO2(g)CH4(g) +
water+
22
Reactants Products
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
NaOH(aq)
water
Na(s) H2O(l) H2(g) 2
sodium
2 2
hydrogen sodiumhydroxide
+ +
+ +
Reactants Products
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Law of Conservation of Mass
total mass total mass
of products of reactants
Pmass = Rmass
=
2 Cu + H2O + CO2 + O2 CuCO3 + Cu(OH)2
Copper ldquopatinardquo is a mixture ofcopper(II) carbonate and copper(II) hydroxide
It has a characteristic green color
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-
Letrsquos read about Lavoisier
bull Letrsquos watch a video on Lavoisierrsquos hypothesis regarding the conservation of mass
- Unit 1 Introduction to Chemistry
- Worldview A perspective from which we see and interpret all of
- The Creation Mandate
- 1st and 2nd Commandment
- Dominion Science
- What if microbes were intelligent Worldview
- Slide 7
- What is Chemistry
- Slide 9
- The Beginning
- Alchemy
- Slide 12
- Slide 13
- Slide 14
- Slide 15
- Areas of Chemistry
- Careers in Chemistry
- Slide 18
- The Scope of Chemistry
- Government Regulation of Chemicals
- Slide 21
- Letrsquos pause for a Quiz
- Safety ndash Extremely important in the Chemistry Lab
- Safety Features of the Lab
- SAFETY in the Science Classroom
- Toxicity
- Material Safety Data Sheet (MSDS)
- Chemical Exposure
- How Toxic is ldquoToxicrdquo
- Science
- The Functions of Science
- Corning Glass
- Aluminum Mining
- Slide 34
- Slide 35
- How does scientific knowledge advance
- The Scientific Method
- The Skeptical Chemist
- Slide 39
- Types of Data
- Candle Observation Activity
- A Description of a Burning Candle
- Parts of the Scientific Method
- A Scientific Experiment
- A Controlled Experiment
- Slide 46
- Letrsquos pause for a Quiz (2)
- Scientific Law vs Scientific Theory
- Slide 49
- Manipulating Numerical Data
- Graphs
- Bar Graph
- Pie Graph
- Line Graph
- Elements of a ldquogoodrdquo line graph
- Graphing HW
- Letrsquos Pause for a Test
- Essential Math of Chemistry
- Scientific Notation
- Slide 60
- Using the Exponent Key
- Slide 62
- Slide 63
- Now letrsquos do some multiplication and division
- Slide 65
- Slide 66
- Slide 67
- Slide 68
- Slide 69
- Percent Error
- Percent Error (2)
- Significant Figures
- Practice Measuring
- Significant Figures Example
- Measurement and Precision
- Rules for Identifying the Number of Significant Figures
- How many Sig Figs
- Sig Figs with Calculations
- Back to the original questionhellip
- Slide 80
- Slide 81
- Slide 82
- Numerical Example
- Slide 84
- Numerical Example (2)
- Slide 86
- Slide 87
- Letrsquos pause for a Quiz (3)
- The Metric System
- The SI (Metric) System
- How can you remember the order of the metric system prefixes
- Prefixes to know in the SI (Metric) System
- Common SI Equivalents
- Letrsquos have another quiz
- Conversion Factors and Unit Cancellation
- Slide 96
- Slide 97
- Slide 98
- Slide 99
- Slide 100
- Simple Math with Conversion Factors
- Slide 102
- Slide 103
- Slide 104
- Slide 105
- Slide 106
- Indiana Jones Density
- Slide 108
- Slide 109
- Slide 110
- Slide 111
- Basic Concepts in Chemistry
- Slide 113
- Slide 114
- Slide 115
- Law of Conservation of Mass
- Letrsquos read about Lavoisier
-