1. Reaction Prediction
What you MUST know before you even begin trying to predict a reaction:
Element names & symbols
Know your diatomics
Oxidation states for main group elements
Nomenclature rules for acids, ionic, & covalent compounds.
Balancing equations
Interpreting word equations

2. I. Synthesis Reactions A. Two elements produce a compound Ag + O2 
S + O2 
B. Metal oxide + water produce a base (metallic hydroxide)
Na2O + H2O 
C. Nonmetal oxide + water produce an oxyacid
SO2 + H2O 
D. Metal oxide + nonmetal oxide produce a salt (ionic solid)
BaO + CO2 
CaO + SO2 

3. II. Decomposition A. Reverse of synthesis reactions
NaCl + electricity 
B. Metallic chlorates produce metallic chlorides + O2
KClO3 
C. Metallic carbonates produce metallic oxides + CO2
ZnCO3 
D. Compound electrolyzed produce foundational elements (may involve solute or water)
H2O + electricity 
E. Hydrated salts decompose into the salt and water.
Ex. Na2CO3 * H2O  Na2CO3 + H2O Na2SO4 * 10 H2O 

4. Exceptions Hydrogen peroxide decomposes into water and oxygen.
Sulfurous acid decomposes into water and sulfur dioxide.
Carbonic acid decomposes into water and carbon dioxide.
Ammonium hydroxide decomposes into ammonia and water.

5. III. Single Replacement
A. Metal replaces metal ion in compound if metal is more active (use activity series)
Al + CuSO4 
B. Metal replaces H in acids if metal is more active than H in the compound
Zn + HCl 
C. Halogen replaces a halogen in compound if halogen more active
Br2 + NaCl 
D. Very active metal replaces H in H2O; forms metallic hydroxide & H2
K + H2O 
Ca + H2O 

6. Quick View of Solubility Rules
All compounds containing alkali metal cations and the ammonium ions are soluble – no exceptions.
All compounds containing nitrate, chlorate, perchlorate, acetate, and bicarbonate anions are soluble – no exceptions.
All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+, Hg2+, & Hg22+.
All sulfates are soluble except those containing Hg2+, Pb2+, Sr, Ca, or Ba.
All hydroxides are insoluble except compounds of the alkali metals, Ca,  Sr, and Ba.
All compounds containing phosphate, sulfide (exception alkaline metals of sulfides are soluble), carbonate, and sulfite ions are insoluble except those that also contain alkali metals or NH4+.

7. IV. Double Replacement:
Two aqueous ionic compounds react if one product is a precipitate, gas, or molecule (such as water). Must know solubility rules & be able to write net ionic equations.
K2CO3 + HNO3 
KOH + HI
K2CO3 + Ba(OH)2 
Fe2(SO4)3 + Ba(OH)2 
Hg2(NO3)2 + KI 
NH4I + AgNO3 

8. V. Combustion
Oxygen (also termed as air in a problem) + compound (usually a hydrocarbon) produce oxides (usually carbon dioxide) of elements in compound and water.
Complete and balance the reactions for the combustion of the following compounds:
CH4
C2H2
CH3OH
C6H12O6
C8H18

9. Additional Practice
Use the Pre-AP Equation notes (word document) for in depth explanations and extra practice.
The answers may be checked using the Pre-AP notes power point.
Study, Study, Study!!!!!!!