Double Replacement
Redox
Single Replacement (another redox)
Composition
Decomposition
Complex Ions
Combustion

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In Chem 1 we wrote molecular equations
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)

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

oxidation and reduction reaction

(oxidation is loss of electrons, reduction is gain of electrons – OIL RIG)
Use of key terms

MnO
4
H
2
O
2
Cr
2
O
7
2HNO
3
Metals with multiple oxidation states

Sn 2+ Sn 4+ Cr 2+ Cr 3+ Cr 6+
Acidic and Basic conditions
4 MnO
4
+ 12 H + + 20 H
2
O
2
 4 Mn 2+ + 15 O
2
+ 26 H
(We will deal with this type MUCH later)
2
O

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

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Reaction of a hydrocarbon/alcohol or other organic molecule with oxygen gas to produce carbon dioxide and water
C
3
H
8
+ 5 O
2
→ 3 CO
2
+ 4 H
2
O
CH
3
CH
2
OH + 3 O
2
→ 2 CO
2
+ 3 H
2
O

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

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

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

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