chapter 1: matter and change. 1.1 chemistry chemistry affects the things you do everyday; chemistry...

Chapter 1: Matter Chapter 1: Matter and Changeand Change

1.1 Chemistry1.1 Chemistry Chemistry affects the things you do Chemistry affects the things you do

everyday; chemistry is everywhereeveryday; chemistry is everywhere Examples of things that wouldn’t be possible Examples of things that wouldn’t be possible

without chemistry:without chemistry: PlasticsPlastics GasolineGasoline Pharmaceuticals; modern medicine wouldn’t Pharmaceuticals; modern medicine wouldn’t

existexist Water PurificationWater Purification Synthetic Fertilizers and Insecticides – farming Synthetic Fertilizers and Insecticides – farming

would be much less productivewould be much less productive Processed foods, air conditioning, soap, TV, Processed foods, air conditioning, soap, TV,

refrigeration, batteries, electricity, computers, or refrigeration, batteries, electricity, computers, or cell phonescell phones

1.1 Defining Chemistry1.1 Defining Chemistry

chemistrychemistry – the study of the – the study of the composition of substances and the composition of substances and the changes they undergochanges they undergo

Chemists do a variety of jobs:Chemists do a variety of jobs: Develop new products, work on Develop new products, work on

environmental issues, teach, analyze environmental issues, teach, analyze substances, check quality control, and substances, check quality control, and so much more.so much more.

1.1 Applied Chemistry vs. Pure 1.1 Applied Chemistry vs. Pure ChemistryChemistry

In In applied chemistryapplied chemistry (or chemical (or chemical technology) scientific knowledge can technology) scientific knowledge can be used in ways that either benefit be used in ways that either benefit or harm people or the environment.or harm people or the environment.

In In pure chemistrypure chemistry knowledge is knowledge is collected for its own sakecollected for its own sake

1.1 Five Major Divisions in 1.1 Five Major Divisions in ChemistryChemistry

Organic ChemistryOrganic Chemistry – the study of – the study of essentially all substances that contain essentially all substances that contain carboncarbon

Inorganic ChemistryInorganic Chemistry – largely – largely concerns substances without carbonconcerns substances without carbon

Analytical ChemistryAnalytical Chemistry – concerned – concerned primarily with the composition of primarily with the composition of substancessubstances

Physical ChemistryPhysical Chemistry – concerned with – concerned with theories and experiments that describe theories and experiments that describe the behavior of chemicalsthe behavior of chemicals

BiochemistryBiochemistry – the study of the – the study of the chemistry of living organismschemistry of living organisms

1.1 Concept Practice1.1 Concept Practice1. Distinguish between pure and applied 1. Distinguish between pure and applied

chemistry.chemistry.

2. In which divisions of chemistry might you 2. In which divisions of chemistry might you work on the following?work on the following?a. Determining mercury levels in fish.a. Determining mercury levels in fish.

b. Improving the fuel characteristics of b. Improving the fuel characteristics of gasoline.gasoline.

c. Developing new blood-clotting agents.c. Developing new blood-clotting agents.

1.2 The Scientific 1.2 The Scientific MethodMethod

Many questions require science to Many questions require science to make informed decisionsmake informed decisions What sources and technology should be What sources and technology should be

used to provide energy?used to provide energy? What is an appropriate response to What is an appropriate response to

global climate change?global climate change? Given limited resources, what deserves Given limited resources, what deserves

the most support: the space program or the most support: the space program or cancer research?cancer research?

An understanding of the basics of An understanding of the basics of science is helpful in arriving at science is helpful in arriving at informed opinions on these questions.informed opinions on these questions.


The The scientific methodscientific method is an approach is an approach to solving scientific problemsto solving scientific problems

You are familiar with this process in You are familiar with this process in your everyday life because it follows your everyday life because it follows ordinary common senseordinary common sense Example: You try to use a flashlight, but it Example: You try to use a flashlight, but it

doesn’t turn on. You have made an doesn’t turn on. You have made an observation and have encountered a observation and have encountered a question/problem, what would you do?question/problem, what would you do?


ObservationObservation – leads to a scientific problem or – leads to a scientific problem or question that requires further investigationquestion that requires further investigation

HypothesisHypothesis – a proposed reason/explanation – a proposed reason/explanation for what is observedfor what is observed

ExperimentExperiment – a means of testing a hypothesis – a means of testing a hypothesis Experimental results must be repeatable – peer Experimental results must be repeatable – peer

reviewreview Analyzing DataAnalyzing Data – processing experimental – processing experimental

informationinformation Drawing a ConclusionDrawing a Conclusion – interpret data to – interpret data to

determine if you accept or reject your determine if you accept or reject your hypothesishypothesis

1.2 Scientific Theory vs. 1.2 Scientific Theory vs. LawLaw

theorytheory – a well tested explanation that – a well tested explanation that unifies a broad range of observations unifies a broad range of observations Allow scientists to predict the behavior of Allow scientists to predict the behavior of

natural systems under varying circumstancesnatural systems under varying circumstances Theories are never provenTheories are never proven

lawlaw – a concise statement that summarizes – a concise statement that summarizes the results of a broad spectrum of the results of a broad spectrum of observations and experimentsobservations and experiments Describes a natural phenomenon without Describes a natural phenomenon without

attempting to explain itattempting to explain it

1.2 Concept Practice1.2 Concept Practice

3. When you solve a problem using the 3. When you solve a problem using the scientific method, why must you have a scientific method, why must you have a hypothesis before you do experiments?hypothesis before you do experiments?

4. Later in this chapter you will learn 4. Later in this chapter you will learn that matter is neither created nor that matter is neither created nor destroyed in any chemical change. Is destroyed in any chemical change. Is this statement a theory or a law? Why?this statement a theory or a law? Why?

1.3 Properties of Matter1.3 Properties of Matter

MatterMatter includes anything that has includes anything that has massmass and and takes up spacetakes up space..massmass – measurement of the amount of – measurement of the amount of

matter that an object containsmatter that an object contains A A substance substance is a particular type of is a particular type of

matter that has a matter that has a uniformuniform and and definite compositiondefinite composition.. Which is a substance: sucrose

(C12H22O11) or lemonade? Explain.

1.3 Properties of Matter1.3 Properties of Matter

Physical PropertyPhysical Property – a quality or – a quality or condition of a substance that can be condition of a substance that can be observed or measured without observed or measured without changing the substance’s changing the substance’s compositioncomposition Examples: color, solubility, mass, odor, Examples: color, solubility, mass, odor,

hardness, density, boiling pointhardness, density, boiling point Chemists use physical properties Chemists use physical properties

to identify substancesto identify substances


6. Use Table 1.2 to find three properties 6. Use Table 1.2 to find three properties of sucrose that distinguish it from of sucrose that distinguish it from sodium chloride.sodium chloride.

1.4 The States of Matter1.4 The States of Matter

HH22O → ice, water, steamO → ice, water, steam Four physical states of mater are Four physical states of mater are

solid, liquid, gas, and plasma.solid, liquid, gas, and plasma. 99% of all matter in the solar system 99% of all matter in the solar system

exists as plasma (the sun)exists as plasma (the sun) Plasma – matter at high temperatures Plasma – matter at high temperatures

(+5000°C); gas like substance of (+5000°C); gas like substance of negatively and positively charged negatively and positively charged particlesparticles

1.4 The States of Matter1.4 The States of Matter

solidsolid – matter that has a definite – matter that has a definite shape and volumeshape and volume Particles in a solid are tightly packed Particles in a solid are tightly packed

togethertogether Expand slightly when heated; nearly Expand slightly when heated; nearly

incompressibleincompressible

1.4 States of Matter1.4 States of Matter

liquidliquid – a form of matter that flows, – a form of matter that flows, has a fixed volume, and takes the has a fixed volume, and takes the shape of its containershape of its container Expand moderately when heated; Expand moderately when heated;

nearly incompressiblenearly incompressible

1.4 States of Matter1.4 States of Matter

gasgas – matter that takes both the shape – matter that takes both the shape and volume of its containerand volume of its container Large expansion when heated; compressibleLarge expansion when heated; compressible

Gas vs. VaporGas vs. Vapor Substances that are in a gaseous state at Substances that are in a gaseous state at

room temperature are considered room temperature are considered gasesgases.. Substances that are in a gaseous state, but Substances that are in a gaseous state, but

are usually solids or liquids at room are usually solids or liquids at room temperature are considered temperature are considered vaporsvapors. .

* Room Temperature = 20°C-25°C (68°F-* Room Temperature = 20°C-25°C (68°F-77°F)77°F)


7. What is the physical state of each of 7. What is the physical state of each of the following at room temperature?the following at room temperature?

a. gold a. gold

b. gasoline b. gasoline

c. helium c. helium

8. Fingernail polish remover (mostly 8. Fingernail polish remover (mostly acetone) is a liquid at room acetone) is a liquid at room temperature. Would you describe temperature. Would you describe acetone in the gaseous state as a acetone in the gaseous state as a vapor or gas?vapor or gas?

1.5 Physical Change1.5 Physical Change

A A physical changephysical change alters a alters a substance without changing its substance without changing its composition.composition. Terms that signify a physical change: Terms that signify a physical change:

boil, freeze, melt, dissolve, condense, boil, freeze, melt, dissolve, condense, break, split, crack, and crush.break, split, crack, and crush.


9. Which of these are physical changes?9. Which of these are physical changes?

a. baking a potato b. carving a wooden a. baking a potato b. carving a wooden figurinefigurine

c. freezing mercury d. dissolving sugar in c. freezing mercury d. dissolving sugar in waterwater

10. Use Table 1.2 to identify four substances 10. Use Table 1.2 to identify four substances that undergo a physical change if the that undergo a physical change if the temperature is decreased from 50°C to -50°C.temperature is decreased from 50°C to -50°C.

1.6 Mixtures1.6 Mixtures

mixturesmixtures – consist of a physical blend – consist of a physical blend of two or more substancesof two or more substances Unlike substances, mixture have a Unlike substances, mixture have a

variable composition (it can be made variable composition (it can be made with different ratios of substanceswith different ratios of substances

Example: lemonade, a saladExample: lemonade, a salad

1.6 Heterogeneous vs. 1.6 Heterogeneous vs. HomogeneousHomogeneous

heterogeneous mixtureheterogeneous mixture – not uniform in – not uniform in compositition → can differ from portion compositition → can differ from portion to portionto portion Example: chicken noodle soupExample: chicken noodle soup

homogenous mixturehomogenous mixture – has a – has a completely uniform composition → completely uniform composition → components of the mixture are evenly components of the mixture are evenly distributed throughout the sampledistributed throughout the sample Example: salt waterExample: salt water A A solutionsolution is a type of homogenous mixture is a type of homogenous mixture

1.6 Heterogeneous vs. 1.6 Heterogeneous vs. HomogeneousHomogeneous

Any part of a system with a uniform Any part of a system with a uniform composition and properties is called composition and properties is called a a phasephase Homogenous mixtures consist of a

single phase Heterogeneous mixtures consist of two

or more phases Example: Oil and Vinegar Salad Dressing

1.6 Separating Mixtures1.6 Separating Mixtures

Some mixtures can be separated into Some mixtures can be separated into their various components by simple their various components by simple physical meansphysical means Example: a taco, iron filings and sulfurExample: a taco, iron filings and sulfur

How would you separate the How would you separate the components in tap water components in tap water (homogenous mixture)?(homogenous mixture)?

1.6 Separating Mixtures1.6 Separating Mixtures

distillationdistillation – a liquid is boiled to – a liquid is boiled to produce a vapor that is then produce a vapor that is then condensed again to a liquidcondensed again to a liquid Example: Figure 1.9, page 13Example: Figure 1.9, page 13

1.6 Example1.6 ExampleHow would you separate a mixture of How would you separate a mixture of

sawdust, sand, iron, and salt?sawdust, sand, iron, and salt?


11. How many phases does every solution 11. How many phases does every solution have?have?

12. Classify each of the following as 12. Classify each of the following as homogeneous or heterogeneous homogeneous or heterogeneous mixtures.mixtures.

a. blooda. blood

b. peanut butter b. peanut butter

c. motor oilc. motor oil

1.7 Elements and 1.7 Elements and CompoundsCompounds

By separating mixtures into their By separating mixtures into their component parts you obtain pure component parts you obtain pure substancessubstances Pure substances have a Pure substances have a uniformuniform and and

definite compositiondefinite composition Substances are divided into two Substances are divided into two

groups: groups: elementselements and and compoundscompounds

1.7 Elements1.7 Elements

elementselements – the simplest forms of – the simplest forms of matter that can exist under normal matter that can exist under normal laboratory conditionslaboratory conditions Elements cannot be separated into Elements cannot be separated into

simpler substances by chemical reactionssimpler substances by chemical reactions Elements are the building blocks for all Elements are the building blocks for all

mattermatter Examples: Hydrogen, Oxygen, Carbon, Examples: Hydrogen, Oxygen, Carbon,

Gold, IronGold, Iron

1.7 Compounds1.7 Compounds

compoundscompounds – substances that can be – substances that can be separated into simpler substances separated into simpler substances only by chemical reactionsonly by chemical reactions The different elements that make up a The different elements that make up a

compound are always present in that compound are always present in that compound in the same proportionscompound in the same proportions

Example: Water – HExample: Water – H220; Table Salt - NaCl0; Table Salt - NaCl

Every element and every compound Every element and every compound has its own unique set of propertieshas its own unique set of properties

1.7 Compounds1.7 Compounds

Example: Upon strong heating sugar Example: Upon strong heating sugar decomposes completely into carbon decomposes completely into carbon and waterand water

sugar → carbon + watersugar → carbon + water

Water can be broken down into Water can be broken down into hydrogen and oxygenhydrogen and oxygen

water → hydrogen + oxygenwater → hydrogen + oxygen

compound compoundelement

compound element element


13. Classify these as elements, 13. Classify these as elements, compounds, or mixtures.compounds, or mixtures.

a. silvera. silver

b. a pine treeb. a pine tree

c. orange juicec. orange juice

d. oxygend. oxygen

e. iced teae. iced tea

f. airf. air

1.8 Chemical Symbols1.8 Chemical Symbols All matter in the universe is composed of All matter in the universe is composed of

elements (94 elements known to occur elements (94 elements known to occur naturally)naturally)

Each element is represented by a Each element is represented by a chemical symbolchemical symbol Chemical symbols consist of one or two lettersChemical symbols consist of one or two letters The first letter must be capitalized; the second The first letter must be capitalized; the second

letter (if there is one) is always lowercaseletter (if there is one) is always lowercase You are required to know the names You are required to know the names

and symbols of the common elements and symbols of the common elements listed in the inside cover (opposite listed in the inside cover (opposite page) of your textbook.page) of your textbook.

1.8 Chemical Symbols1.8 Chemical Symbols

Chemical symbols provide a shorthand Chemical symbols provide a shorthand way to write way to write chemical formulaschemical formulas of of compoundscompounds Example: Water – HExample: Water – H22OO

Table Sugar (sucrose) – CTable Sugar (sucrose) – C1212HH2222OO1111

The numbers in the subscripts of the The numbers in the subscripts of the chemical formula represent the chemical formula represent the proportions of the various elements in a proportions of the various elements in a compoundcompound A specific compound is always made up of the A specific compound is always made up of the

same elements in the same proportionsame elements in the same proportion


15. What is the chemical name for 15. What is the chemical name for each of these symbols?each of these symbols?

a. Sna. Sn

b. Cub. Cu

c. Sc. S

d. Cdd. Cd

e. Pe. P

f. Clf. Cl


16. What elements are in baking soda, 16. What elements are in baking soda, NaHCONaHCO33??

1.9 Chemical Reactions1.9 Chemical Reactions Compounds can only be separated into Compounds can only be separated into

simpler substances by simpler substances by chemical chemical reactionsreactionschemical reactionchemical reaction – one or more – one or more substances change into new substancessubstances change into new substances In a chemical reaction the starting In a chemical reaction the starting

substances are called substances are called reactantsreactants and the new and the new substances are called substances are called productsproducts

Chemical symbols and formulas are used Chemical symbols and formulas are used in in chemical equationschemical equations to explain what to explain what occurs in chemical reactionsoccurs in chemical reactions

1.9 Chemical Reactions1.9 Chemical Reactions

The ability of a substance to undergo The ability of a substance to undergo chemical reactions and to form new chemical reactions and to form new substances constitutes its substances constitutes its chemical chemical propertiesproperties

In chemical reaction heat is either In chemical reaction heat is either absorbed (endothermic) or heat is absorbed (endothermic) or heat is released (exothermic)released (exothermic) Key words indicating chemical change: rot, Key words indicating chemical change: rot,

rust, decompose, ferment, corrode, grow, rust, decompose, ferment, corrode, grow, decay, and sproutdecay, and sprout

1.9 Concept Practice1.9 Concept Practice17. List four probable indicators of 17. List four probable indicators of

chemical change.chemical change.

18. Classify the following changes as 18. Classify the following changes as physical or chemical.physical or chemical.

a. bread is bakeda. bread is baked

b. salt dissolves in waterb. salt dissolves in water

c. milk spoilsc. milk spoils

d. a snowflake meltsd. a snowflake melts

1.10 Conservation of 1.10 Conservation of MassMass

Law of Conservation of MassLaw of Conservation of Mass In any physical or chemical In any physical or chemical

reaction, mass is neither created reaction, mass is neither created or destroyed; it is conserved.or destroyed; it is conserved. In a chemical reaction the mass of the In a chemical reaction the mass of the

productsproducts equals the mass of the equals the mass of the reactants.reactants.


19. Why is the statement of the 19. Why is the statement of the conservation of mass a law and not a conservation of mass a law and not a theory?theory?

20. When powdered iron is left exposed 20. When powdered iron is left exposed to the air it rusts. Explain why the to the air it rusts. Explain why the rust weighs more than the original rust weighs more than the original powdered iron.powdered iron.


21. Hydrogen and oxygen react 21. Hydrogen and oxygen react chemically to form water. How much chemically to form water. How much water will be formed if 4.8 grams of water will be formed if 4.8 grams of hydrogen reacted with 38.4 grams of hydrogen reacted with 38.4 grams of oxygen?oxygen?

1.1 Concept Practice1.1 Concept Practice1. Distinguish between pure and applied 1. Distinguish between pure and applied

chemistry.chemistry.A: Pure chemistry accumulates knowledge for its A: Pure chemistry accumulates knowledge for its

own sake. Applied chemistry aims to attain own sake. Applied chemistry aims to attain specific goals.specific goals.

2. In which divisions of chemistry might you work 2. In which divisions of chemistry might you work on the following?on the following?a. Determining mercury levels in fish.a. Determining mercury levels in fish.A: Analytical ChemistryA: Analytical Chemistryb. Improving the fuel characteristics of gasoline.b. Improving the fuel characteristics of gasoline.A: Organic ChemistryA: Organic Chemistryc. Developing new blood-clotting agents.c. Developing new blood-clotting agents.A: BiochemistryA: Biochemistry


3. When you solve a problem using the 3. When you solve a problem using the scientific method, why must you have a scientific method, why must you have a hypothesis before you do experiments?hypothesis before you do experiments?

A: The hypothesis guides the design of the A: The hypothesis guides the design of the experiment.experiment.

4. Later in this chapter you will learn that 4. Later in this chapter you will learn that matter is neither created nor destroyed matter is neither created nor destroyed in any chemical change. Is this in any chemical change. Is this statement a theory or a law? Why?statement a theory or a law? Why?

A: A law. The statement summarizes facts; A: A law. The statement summarizes facts; it does not give an explanation.it does not give an explanation.


6. Use Table 1.2 to find three properties of 6. Use Table 1.2 to find three properties of sucrose that distinguish it from sodium sucrose that distinguish it from sodium chloride.chloride.

A: - Melting point. A: - Melting point.

Sucrose: 185°C; Sodium Chloride: 801°CSucrose: 185°C; Sodium Chloride: 801°C

- Boiling Point.- Boiling Point.

Sucrose: decomposes; Sodium Chloride: Sucrose: decomposes; Sodium Chloride: 1413°C1413°C

- Density- Density

Sucrose: 1.59 g/cmSucrose: 1.59 g/cm33; Sodium Chloride: 2.17 ; Sodium Chloride: 2.17 g/cmg/cm33


7. What is the physical state of each of the 7. What is the physical state of each of the following at room temperature?following at room temperature?

a. gold - solida. gold - solid

b. gasoline - liquidb. gasoline - liquid

c. helium – gasc. helium – gas

8. Fingernail polish remover (mostly 8. Fingernail polish remover (mostly acetone) is a liquid at room temperature. acetone) is a liquid at room temperature. Would you describe acetone in the Would you describe acetone in the gaseous state as a vapor or gas?gaseous state as a vapor or gas?

A: a vaporA: a vapor


9. Which of these are physical changes?9. Which of these are physical changes?

a. baking a potato b. carving a wooden a. baking a potato b. carving a wooden figurinefigurine

c. freezing mercury d. dissolving sugar in c. freezing mercury d. dissolving sugar in waterwater

A: b, c, and dA: b, c, and d

10. Use Table 1.2 to identify four substances 10. Use Table 1.2 to identify four substances that undergo a physical change if the that undergo a physical change if the temperature is decreased from 50°C to -50°C.temperature is decreased from 50°C to -50°C.

A: chlorine, mercury, bromine, and waterA: chlorine, mercury, bromine, and water


11. How many phases does every solution 11. How many phases does every solution have?have?

A: oneA: one

12. Classify each of the following as 12. Classify each of the following as homogeneous or heterogeneous homogeneous or heterogeneous mixtures.mixtures.

a. blooda. blood

b. peanut butter b. peanut butter

c. motor oilc. motor oil

- heterogeneous- heterogeneous

- heterogeneous- heterogeneous

- homogeneous


13. Classify these as elements, 13. Classify these as elements, compounds, or mixtures.compounds, or mixtures.

a. silvera. silver

b. a pine treeb. a pine tree

c. orange juicec. orange juice

d. oxygend. oxygen

e. iced teae. iced tea

f. airf. air

- element

- element

- mixture

- mixture

- mixture- mixture


15. What is the chemical name for 15. What is the chemical name for each of these symbols?each of these symbols?

a. Sna. Sn

b. Cub. Cu

c. Sc. S

d. Cdd. Cd

e. Pe. P

f. Clf. Cl

- tin

- copper

- sulfur- cadmium

- phosphorous- chlorine


16. What elements are in baking soda, 16. What elements are in baking soda, NaHCONaHCO33??

A: Sodium, Hydrogen, Carbon, and A: Sodium, Hydrogen, Carbon, and OxygenOxygen

1.9 Concept Practice1.9 Concept Practice17. List four probable indicators of chemical 17. List four probable indicators of chemical

change.change.

A: Color change, energy absorbed or evolved, A: Color change, energy absorbed or evolved, gas or solid produced, odor change.gas or solid produced, odor change.

18. Classify the following changes as physical 18. Classify the following changes as physical or chemical.or chemical.

a. bread is bakeda. bread is baked

b. salt dissolves in waterb. salt dissolves in water

c. milk spoilsc. milk spoils

d. a snowflake meltsd. a snowflake melts

- chemical change

- chemical change

- physical change

- physical change


19. Why is the statement of the conservation 19. Why is the statement of the conservation of mass a law and not a theory?of mass a law and not a theory?

A: It does not attempt to explain; therefore, it A: It does not attempt to explain; therefore, it is not a theory.is not a theory.

20. When powdered iron is left exposed to the 20. When powdered iron is left exposed to the air it rusts. Explain why the rust weighs air it rusts. Explain why the rust weighs more than the original powdered iron.more than the original powdered iron.

A: The iron combines with oxygen from the A: The iron combines with oxygen from the air.air.


21. Hydrogen and oxygen react 21. Hydrogen and oxygen react chemically to form water. How much chemically to form water. How much water will be formed if 4.8 grams of water will be formed if 4.8 grams of hydrogen reacted with 38.4 grams of hydrogen reacted with 38.4 grams of oxygen?oxygen?

A: 43.2 g A: 43.2 g

chapter 1: matter and change. 1.1 chemistry chemistry affects the things you do everyday; chemistry...

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chemistry chemistry

chemistry organic chemistry

applied chemistry

everyday chemistry

divisions of chemistry

pure chemistry knowledge

carbon inorganic chemistry

carbon organic chemistry