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

Identification of Double Replacement Reaction Acid / Base NH3 + HF  NH4+ + F – Precipitation Ba2+ + SO42-  BaSO4 Both H+ + HSO4- + Ca2+ + 2 OH-  CaSO4 + 2 H2O

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 MnO4- + 6 H+ + 5 H2O2  2 Mn2+ + 5 O2 + 8 H2O

Redox / Single Replacement Like will replace like 2 Na + 2 H2O  2 Na+ + 2 OH- + H2 Cl2 + 2 I-  2 Cl- + I2

Combustion Reaction of a compound with oxygen gas to produce oxides of all elements in the compound C3H8 + 5 O2 → 3 CO2 + 4 H2O CH3CH2OH + 3 O2 → 2 CO2 + 3 H2O 4 CH3NH2 + 13 O2 → 4 CO2 + 10 H2O + 4 NO2

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

Decomposition / Synthesis Composition has two reactants that combine into one product S8 + 8 O2  8 SO2 nonmetal oxides plus water make acids SO3 + H2O  H+ + HSO4- metal oxides plus water makes metal hydroxide CaO + H2O  Ca2+ + 2 OH-

Complex Ions Particles that generally combine with ammonia or hydroxide to form complex ions with a charge AgCl + 2 NH3  Ag(NH3)2+ + Cl- Cu2+ + 4 NH3  Cu(NH3)42+ Al3+ + 4 OH-  Al(OH)4- having the correct ligand number is not required but being consistent with number and charge is important

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