1. CHAPTER 1
CE CHEMISTRY

2. MATTER Anything that has mass and occupies space Weight Mass
Measure of earth’s gravity
Mass
Measure of the quantity of matter
Law of conservation of matter
Matter cannot be created or destroyed
States of matter
Solid
Liquid
Gas

3. PROPERTIES OF MATTER
THE PROPERTIES OF MATTER CANNOT BE BROKEN DOWN WITHOUT A CHEMICAL CHANGE
PHYSICAL PROPERTIES
Such properties are color, density, boiling point , melting point, and hardness
PHYSICAL CHANGE- Properties never change
Liquid turning into a gas
CHEMICAL PROPERTIES
The way a substance reacts with another substance
2Na(s) + Cl2(g)  2NaCl(s)
CHEMICAL CHANGE-Properties are altered

4. SUBSTANCES PURE SUBSTANCE - Properties the same
ELEMENT - cannot be broken down by a chemical change. Silver, gold or aluminum
COMPOUND - two or more elements that have been chemically bonded together. This can be broken down chemically into the elements. Sugar, baking soda, etc.

5. MIXTURES MIXTURE - Each substance retains their properties
HOMOGENEOUS - all particles are in the same phase, a uniformed mixture. Salt water or air
HETEROGENEOUS - all particles are not in the same phase, not uniformly mixed. Sand or wood
MIXTURES CAN BE SEPARATED BY PHYSICAL MEANS
Filtration, chromatography, or distillation (depends on volatility)

6. SOLUTIONS Solutions are usually homogenous liquids
You can have solutions that are a mixture of gas and liquid. Also you can have gas solutions like air.

7. ATOMS AND MOLECULES MOLECULES Smallest particle in a compound
Diatomic molecule has two same atoms (know these), Hydrogen gas(H2), Nitrogen gas(N2), Oxygen gas(O2), Fluorine gas(F2), Chlorine gas(Cl2), Bromine liquid(Br2), Iodine solid(I2)
Polyatomic molecules have more than two elements in it
ATOMS
Smallest particle in a element
All elements are single atoms Carbon (C), Aluminum (Al), except for the diatomic molecules

8. SI UNITS Length is measured in METERS m
Mass is measured in KILOGRAMS kg
Time is measured in SECONDS s
Temperature is measured in KELVIN K
Amount of substance is
measured in MOLES mol

9. CONVERSIONS THINGS TO REMEMBER
In the metric system, the smaller prefix unit will always have a larger number than the prefix unit it is equal to.
1000 m = 1km (overhead)
METER IS A SMALLER PREFIX UNIT
Kelvin is absolute zero or oC. You can not have a temperature lower than this so KELVIN CAN NEVER BE A NEGATIVE NUMBER
oC = K
K = oC

10. ROUNDING NUMBERS OFF
In a series of calculations carry all digits unit the final solution, THEN ROUND
If a digit needs to be rounded
If it is less than 5, the preceding digit remains the same
If the digits are equals or is greater than 5, the preceding digit is increased by one.

11. UNCERTAINTIES IN MULTIPLICATION, DIVISION, ADDITION, AND SUBTRACTION
Multiplication and division
Significant figures are the same as the least precise (number with the smallest number of significant figures) measurements
Addition and subtraction
The answer will have the same number of digits beyond the decimal point as the integer (that was added or subtracted) with the least accurate number (last significant number is in the highest place holder)

12. SCIENTIFIC NOTATION All chemistry uses scientific notation
Uses the base 10
1000 = 10 x 10x 10 =103
0.001=1/1000=1/10 x 1/10 x 1/10=10-3

13. PERCENTAGES Calculating percentages
Percent =number of specific items x 100
Total items in the group

14. DENSITY
Density
Measure of the mass of a substance that occupies one unit of volume
Density = mass = gram = g
Volume Centimeters cubed cm3