1. Equations
1. Multiply each atom in a compound by a coefficient so each side is equal
2. Exothermic – energy out (releases) (-)
Endothermic energy in (absorbs) (+)

2. Equations
3. Describe the following types of reactions (EXTREMELY IMPORTANT)
Synthesis: 2 or more  1
Decomposition: 1  2 or more
Combustion: hydrocarbon (HC) + O2 CO2 + H2O
Single replacement: AY + B  BY + A
Double replacement: AY + BX  AX + BY
Neutralization: HX (acid) + YOH (base)  YX (salt) + H2O
Polymerization: Making a large molecule by repeating the same small molecule (called a monomer) over and over again [Can be natural (DNA, proteins) or synthetic (plastics, nylon)]

3. Equations
4. the number of electrons gained or lost when a chemical bond is made.
5. a. H2SO
(because 2(+1) + 1(+6) + 4(-2) = 0)
b. F2 0
c. Cl-1 -1
d. CO (+4 + 3(-2) = -2(charge))
e. TiO
f. TiO
6. Reaction that involves reduction and oxidation

4. Equations 7. Reduction – gains e- so oxidation # goes down
Oxidation – loses e- so oxidation # goes up
Mg + H2SO4  MgSO4 + H2
Mg went up (0+2)  oxidation
H went down (+10)  reduction