WELCOME TO MRS CANALE’S CHEMISTRY CLASS!

FIND YOUR SEAT- YOUR NAME IS ON A NOTE CARD.

FILL OUT YOUR NOTE CARD AND TURN INTO TOP BIN ON

FRONT DESK.

Name Nick name

1. Hobbies and activities

2. Do you have a job? And/or do you play a sport?

3. Why did you take this course.

4. What do you want to be when you grow up?

5. Last science course you took Teacher Final grade Regents grade

6. Last math course you took Teacher Final grade Regents grade

7. Math you are taking this year

8. Any information that you think I should know about you.

(medical, seating, IEP, interest….)

Regents

Chemistry

Chemistry Matter

Observation Conclusion

is the study of matter and

how it interacts with the

environment

anything that has

mass and takes up

space (volume)

Use your 5 senses to describe

an event

Qualitative- a description (I.e.,

it’s red, it’s brittle, it shines)

Quantitative- measurement

(number, 5 cm long)

an assumption based on

your observation

General statement

You assess everything you’ve

gathered and make a statement

about your observations

Your Turn!

A clear colorless liquid is combined with a second clear colorless liquid and the mixture is observed. Which of these is not an observation?

a. The test tube became hot.

b. The reaction is exothermic.

c. The mixture is cloudy.

d. The mixture is white.

1-4

Thinking Like a Chemist

Copyright 2011 John Wiley & Sons,

Inc

1-5

Figure 1.1 Inside a drop of lake water

we find water molecules, dissolved

substances and algae cells.

Read the sentence in the box. Count the number of F’s you

see. Only read it once and do not go back.

FINISHED FILES ARE THE RE-

SULT OF YEARS OF SCIENTIF-

IC STUDY COMBINED WITH THE

EXPEREINCE OF MANY YEARS.

Scientific Method

Observation Hypothesis Experiments Theory

Observation

Experiments

Scientific Law

If experiments prove your hypothesis false,

then go back and propose a new hypothesis.

The theory is tested by further

experiments and modified if necessary.

5 senses Educated

guess Controlled

Collect data Conclusion

A generally

Accepted

principle

Independent variable: the variable that scientist

control and change. (x-axis)

Dependant variable: the variable that responds

to changes in the independent variable (y-axis)

The same

observations

made over and

over lead to a

hypothesis

Carefully designed

experiments test the

hypothesis. If results

consistently support

hypothesis, then a

law can be proposed

https://www.youtube.com/watch?v=k2MhMsLn9B0

The Scientific Method

1-9

Hypothesis: A tentative explanation of

the facts that can be tested further

Theory: Well-tested hypothesis.

Law: Statements of natural

phenomena to which there are

no known exceptions.

Your Turn!

Which of these is a law?

a. Atoms consist of protons, neutrons, and electrons.

b. All matter is composed of atoms.

c. Atoms can form chemical bonds by sharing electrons.

d. The volume of a gas increases with increasing temperature.

Copyright 2011 John Wiley & Sons,

Inc

1-10

Your Turn!

The statement, “An atom consists of

a dense nucleus surrounded by a

cloud of electrons”, is an example

of

a. a theory

b. a law

c. an hypothesis

d. an observation 1-11

States of Matter

Solid Liquid Gas

definite volume

definite shape

regular geometric

pattern

crystalline structure

vibrate in a fixed

location

strong forces of

attraction

Molecules farther

apart

definite volume

no definite shape

intermolecular forces

noncompressible

Molecules far apart

no definite shape

no definite volume

no force of

attractions

Compressible

Completely fills any

container

Classification of Matter

Matter

Substance Mixture of Substances Physically separated

contains only one

element or

compound

Pure

Definite composition

homogenous

contains two or more

element and/or

compounds

physically

associated

Impure

Variable composition

i.e., using a

magnet,

filtering, size

separation

Substance

Element Compound

Chemically Separated

Monatomic – made on 1 atom

Diatomic---made of two atoms (thus di)

located on PT

only one type of atom

smallest form is the

atom

can not be decomposed or

broken down

•two or more different

elements chemically

combined

• elements take on new

properties in the

compound

• smallest form is the

molecule

• can be decomposed

or broken down

into its elements

• combine in fixed ratios

Electrolysis,

decomposition

by light

Na C

I2 Br2 Cl2 F2 O2 N2 H2

I Bring Clay From Our New Home

H2O NaCl

Memorize these

Mixture of Substances

HomogeneousMixture

HeterogeneousMixture

uniform throughout

same throughout

Can’t tell the difference

Solution: (aq)

NaCl (aq)-- dissolved in water

nonuniform

not same throughout

distinct phases

contains regions with different

properties

can tell the difference

layers

Separating Mixtures

Filtration Evaporation

Chromatography

Other

separate large

particles by using a

membrane

(Solids & liquids)

does not separate out

dissolved particles

(ions)

1. Gravity: just let

mixture drip

2. Vacuum: pulls the

mixture through a

funnel by suction

separate dyes or

pigments by size

using filter paper

Centrifuge

(density)

“recover” something

dissolved by boiling

off the solvent (water)

Distillation

•Use to separate a

mixture of Liquids

• Based on their

boiling points

• Must have different

boiling points

Physically

• Separate by size

or physical

characteristic • Use a magnet to

separate magnetic

from non magnetic

• Use a sieve to

separate different

sized material

Extensive Intensive

DensityVolume

Physical Property

A quality or condition of a substance that can be observed or

measured without changing the substance’s composition

Dependent on how much

is present

Does not depend on how

much is present

V = l x w x h

Water displacement

Density = mass/volume

Table T **The density for each

element is listed on Table S

Evidence of achemical reaction

Chemical Property

The ability of a substance to undergo a chemical reaction and to form

a new substance.

Change in temperature (absorb or release heat)

Change color

Produce a gas

Produce a solid (precipitate)

Physical

Change

Chemical

Change A change that does not alter the

chemical composition of the

material.

Can get the original back

Results in a change in chemical

composition of the substances

involved.

Can not get the original back

Something new

Phase change dissolve React burn oxidize corrode

SI Units Prefixes

Measuring Matter

mass

length

Time

Temp

Electric current

Amount of a substance

Pressure

Energy

Kilogram kg (grams)

Meter m

seconds sec

Kelvin K (°C)

ampheres

mole

kiloPascales kPa

Atmospheres atm

Joules J

Calories cal

Kilo k 103

hecto h 102

deca da 101

base - 100

deci d 10-1

centi c 10-2

mili m 10-3

Table D Table C

Converting Measurements

k

h

da

o

d

c

m

Kids have dropped over dead converting metrics

Down Right Move decimal

point to the right

Up Left Move decimal

point to the left

DRUL: down right up left

Base unit

No prefix

OR

King Henry dallied while drinking chocolate milk

Accuracy

PrecisionHow close a set of numbers are to each other

repeatability

How close a number is to the accepted or true value.

Precise, not accurate Not precise,

not accurate

Not precise,

but accurate

Percent ErrorUsed to determine accuracy

% Error = measured value - accepted value X 100

accepted value

Table T

Uncertainty

Always measure one place past the graduated mark.

Last number in a measure is estimated, all others you know

for sure

The more graduated the instrument, more significant figures

you will have

Significant Figures

QuickTime™ and aTIFF (Uncompressed) decompressor

are needed to see this picture.

Draw a line until you hit your first nonzero, all digits not

crossed out are significant.

2400 A P Decimal point

is absent Decimal point

Is present

2 sig fig

0.006450 101 4 sig fig 3 sig fig

Multiplication/

Division

Addition/

Subtraction Your answer will have

the same number of decimal

places as the least in the

problem.

Answer should have 2 decimal

places

21

4

2 34.0435

7.98

+ 0.002

42.0255 20.64

3

2 3

42.03

Your answer will have

the same number of

significant figures

as the least in the

problem.

Answer should have 2 sig fig

6.45

x 3.2

Scientific Notation

___ . ___ ___ x 10exp

Number

1-9 Up to 2

digits after

the decimal

Some power of 10

If original number is

Larger than 1 pos

Less than 1 neg

However many places

you move the decimal