1. Predicting Products of Reactions
Synthesis: Reactants combine to form a single product – make sure the product has an acceptable formula (ions are correct charges, etc.)
Decomposition: Reactant breaks down into simpler products
Binary compounds decompose into elements
Carbonates produce CO2 and oxide
Na2CO3  Na2O + CO2
Explosives produce gases

2. Predicting Products of Reactions
Single Replacement – Element replaces another element (generally, metal or hydrogen replace one another, nonmetal replaces nonmetal)
Double Replacement – Positive ions “switch” partners
Combustion – reaction with O2 produces oxides (often H2O and CO2)

3. Examples – Predict products and write balanced equations
Decomposition of calcium carbonate
Decomposition of aluminum oxide
Al + Cl2 
Zn + HCl 
Combustion of butane (C4H10)
Ca(NO3)2 + K2CO3 
Ca + H2O 

4. Energy and Chemical Reactions
Endothermic – A process that absorbs heat energy from its surroundings.
* Causes the temperature of surrounding substances to decrease.
EXAMPLES?
Exothermic – A process that gives off heat to its surroundings.
* Causes the temperature of surrounding substances to increase.

5. Acids and Bases
Acid – a compound that yields H+ ions in aqueous solution.
Formula contains H as first element.
Base – a compound that yields OH- ions in aqueous solution.
Formula contains hydroxide (OH-) ions.

6. Acid-Base Reactions Double Replacement Example HNO3 + NaOH 
Products of acid-base reactions:
Water (HOH = H2O)
Ionic Compound (salt – general term)

7. Examples Complete and balance the following acid base reactions:
HCl + KOH 
H3PO4 + Mg(OH)2 
H2SO4 + NaOH 