1. Net Ionic Equations Double Replacement Redox / Single Replacement
Synthesis/Decomposition
Complex Ions
Combustion

2. Identification of Double Replacement Reaction
Acid / Base
NH3 + HF  NH4+ + F –
Precipitation
Ba2+ + SO42-  BaSO4
Both
H+ + HSO4- + Ca OH-  CaSO H2O

3. Redox and Single Replacement
Use of key terms
MnO4- H2O2 Cr2O72- HNO3
Metals with multiple oxidation states
Sn2+ Sn4+ Cr2+ Cr3+ Cr6+
Acidic and Basic conditions
2 MnO H H2O2  2 Mn O H2O

4. Redox / Single Replacement
Like will replace like
2 Na + 2 H2O  2 Na OH- + H2
Cl I-  2 Cl- + I2

5. Combustion
Reaction of a compound with oxygen gas to produce oxides of all elements in the compound
C3H O2 → 3 CO H2O
CH3CH2OH O2 → 2 CO H2O
4 CH3NH O2 → 4 CO H2O NO2

6. Decomposition/Synthesis
Decomposition has only one reactant and it breaks up into elements and /or compounds
MgCO3  MgO + CO2
Ba(OH)2  BaO + H2O
2 Al2O3  4 Al + 3 O2

7. Decomposition / Synthesis
Composition has two reactants that combine into one product
S O2  8 SO2
nonmetal oxides plus water make acids
SO3 + H2O  H HSO4-
metal oxides plus water makes metal hydroxide
CaO + H2O  Ca OH-

8. Complex Ions
Particles that generally combine with ammonia or hydroxide to form complex ions with a charge
AgCl NH3  Ag(NH3)2+ + Cl-
Cu NH3  Cu(NH3)42+
Al OH-  Al(OH)4-
having the correct ligand number is not required but being consistent with number and charge is important

9. In Review Identify type of reaction Equations MUST be balanced
Check for appropriate charges
Remember not to include spectator ions