Equations Double Replacement Redox Single Replacement (another redox) CompositionDecomposition Complex Ions Combustion

Net Ionic Equations In Chem 1 we wrote molecular equations In Chem 1 we wrote molecular equations In AP Chem we write net ionic equations – equations that omit any spectator ions In AP Chem we write net ionic equations – equations that omit any spectator ions To write net ionic equations, we must KNOW our solubility rules and strong acids/strong bases (MAKE FLASHCARDS) To write net ionic equations, we must KNOW our solubility rules and strong acids/strong bases (MAKE FLASHCARDS)

Identification of Double Replacement Reaction Acid / Base Acid / Base OH - + H +  H 2 O OH - + H +  H 2 O NH 3 + HF  NH F - Precipitation Precipitation Ba 2+ + SO 4 2-  BaSO 4 Ba 2+ + SO 4 2-  BaSO 4 Both Both 2 H + + SO Ca(OH) 2  CaSO HOH 2 H + + SO Ca(OH) 2  CaSO HOH

Redox oxidation and reduction reaction (oxidation is loss of electrons, reduction is gain of electrons – OIL RIG) (oxidation is loss of electrons, reduction is gain of electrons – OIL RIG) Use of key terms Use of key terms MnO 4 - H 2 O 2 Cr 2 O 7 2- HNO 3 MnO 4 - H 2 O 2 Cr 2 O 7 2- HNO 3 Metals with multiple oxidation states Metals with multiple oxidation states Sn 2+ Sn 4+ Cr 2+ Cr 3+ Cr 6+ Sn 2+ Sn 4+ Cr 2+ Cr 3+ Cr 6+ Acidic and Basic conditions Acidic and Basic conditions 4 MnO H H 2 O 2  4 Mn O H 2 O 4 MnO H H 2 O 2  4 Mn O H 2 O (We will deal with this type MUCH later)

Redox / Single Replacement Single Replacement Single Replacement Like will replace like Like will replace like 2 Na + 2 H 2 O  2 Na OH - + H 2 2 Na + 2 H 2 O  2 Na OH - + H 2 Cl KI  2 K Cl - + I 2 Cl KI  2 K Cl - + I 2

Combustion Reaction of a hydrocarbon/alcohol or other organic molecule with oxygen gas to produce carbon dioxide and water Reaction of a hydrocarbon/alcohol or other organic molecule with oxygen gas to produce carbon dioxide and water C 3 H O 2 → 3 CO H 2 O C 3 H O 2 → 3 CO H 2 O CH 3 CH 2 OH + 3 O 2 → 2 CO H 2 O CH 3 CH 2 OH + 3 O 2 → 2 CO H 2 O

Decomposition/Composition Decomposition has only one reactant and it breaks up into elements and /or compounds Decomposition has only one reactant and it breaks up into elements and /or compounds MgCO 3  MgO + CO 2 MgCO 3  MgO + CO 2 Ba(OH) 2  BaO + H 2 O Ba(OH) 2  BaO + H 2 O 2 Al 2 O 3  4 Al + 3 O 2 2 Al 2 O 3  4 Al + 3 O 2

Decomposition / Composition Composition has two reactants that combine into one product Composition has two reactants that combine into one product S O 2  8 SO 2 S O 2  8 SO 2 nonmetal oxides plus water makes nonmetal oxides plus water makes acids acids SO 3 + H 2 O  2 H + + SO 4 2- SO 3 + H 2 O  2 H + + SO 4 2- metal oxides plus water makes bases metal oxides plus water makes bases CaO + H 2 O  Ca(OH) 2 CaO + H 2 O  Ca(OH) 2

Complex Ions Particles that generally combine with ammonia and hydroxides to form complex ions with a charge Particles that generally combine with ammonia and hydroxides to form complex ions with a charge AgCl + 2 NH 3  Ag(NH 3 ) Cl - AgCl + 2 NH 3  Ag(NH 3 ) Cl - Cu NH 3  Cu(NH 3 ) 4 2+ Cu NH 3  Cu(NH 3 ) 4 2+ Al OH -  Al(OH) 4 - Al OH -  Al(OH) 4 - having the correct ligand number is not required but being consistent with number and charge is important having the correct ligand number is not required but being consistent with number and charge is important

In Review Identify type of reaction from list of 5 types Identify type of reaction from list of 5 types Equations need to be balanced Equations need to be balanced Check for appropriate charges Check for appropriate charges Remember not to include spectator Remember not to include spectator ions ions Remember practice questions about each of the 3 balanced net ionic equations Remember practice questions about each of the 3 balanced net ionic equations