1. INTRODUCTION

2. CHEMISTRY
The science that deals with the materials of the universe and the changes that these materials undergo
Wood burns
Plants grow
Iron rusts
Bread bakes
Human digestion

3. The Scientific Method State the problem Make observations
Form a hypothesis
Perform an experiment
Develop a Law
A summary of observed behavior
Develop a theory
An explanation of behavior
Continue to experiment
Modify theory as needed

4. Important Terms Matter Mass Volume Qualitative observations
Anything that has mass and volume
Mass
Amount of matter in an object
Volume
Amount of space an object occupies
Qualitative observations
Observations not requiring measurements
Quantitative observations
Observations requiring measurements

5. Classification of matter
has mass and volume
PURE
SUBSTANCES
Can write chemical formula
ELEMENT
One type of atom
COMPOUND
Two or more different
atoms chemically bonded
MIXTURES
Variable ratio
HOMOGENEOUS
solutions
HETEROGENEOUS
Colloids and suspensions

6. Energy All objects possess energy
An object has two general forms of energy
Potential energy
The energy of an object due to its position
Kinetic energy
The energy possessed by an object due to its motion
Law of conservation of energy
Energy is neither created or destroyed
Energy can be converted from one form to another

7. PHASES OF MATTER Solid Liquid Gas Definite volume and shape
Definite volume but takes shape of container
Gas
No definite volume and no definite shape

8. Physical and Chemical Properties and Changes
Physical Property
Characteristics that describe a substance
Physical Change
A change that does not affect the composition of the substance
Chemical Property
Characteristics that refer to the ability to form new substances
Chemical Change
A change which produces new substances

9. Measurements

10. SIGNIFICANT FIGURES
The reliable digits in a measurement based on the measuring instrument
Atlantic-Pacific Method
A = decimal Absent, begin counting from right
P = decimal Present, begin counting from left

11. TRY THESE
1,000
1 sig fig
0.001
0.0010
2 sig fig
1000.0
5 sig fig

13. Rules for Using Sig Figs
Multiplication/Division
The number of sig figs in the result is the same as that in the measurement with the smallest number of sig figs
4.56 x = or 6.4
8.315/298 = or
Addition/Subtraction
The limiting term is the one with the smallest number of decimal places
= or 31.1

14. where 1.00 ≥ M < 10 and n is an integer
SCIENTIFIC NOTATION
The expression of numbers in terms of
M x 10n
where 1.00 ≥ M < 10 and n is an integer

15. TRY THESE
25,000
2.5 X 104 X
0.0100 X

16. ACCURACY/PRECISION Accuracy Precision
How close a measurement is to the actual value
Precision
How close a set of measurements are to each other

17. Dartboard analogy

18. DENSITY Mass Volume Density
Amount of matter in an object
Volume
Amount of space an object occupies
Density
Mass per unit volume
Percent Error = /actual-experimental/ x 100
actual

19. Formula for density
What is the density of an object with a mass of 7.65 g and a volume of 4.5 mL?

20. Factor Labeling/Dimensional Analysis
1 in = 2.54 cm ft = 1 mi
Convert 3.1 miles to kilometers

21. 1 kg = 2.2 lbs
Convert 3.3 lbs to grams

22. Convert 8.00 km to miles

23. CHEMICAL REACTIONS Chemical Reaction Reactant Product
A change in which one or more substances are changed into one or more new substances
Reactant
A starting substance in a chemical reaction
Product
A substance produced as the result of a chemical change