Chapter 11.1
Pages 330-339
 Synthesis
 A + B  AB
 Practice
• Sodium metal reacts with chlorine gas
Na(s) + Cl2(g) 
• Solid Magnesium reacts with fluorine gas
Mg(s) + F2(g) 
• Aluminum metal reacts with fluorine gas
Al(s) + F2(g) 
 Decomposition
 AB  A + B
 Practice
• Solid Lead (IV) oxide decomposes
PbO2(s) 
• Aluminum nitride decomposes
AlN(s) 
 Single Replacement
 AB + C  AC + B
 Must use activity series to determine if
a reaction will take place (page 333)
 Practice
• Sodium chloride solid reacts with fluorine gas
NaCl(s) + F2(g) 
• Aluminum metal reacts with aqueous copper
(II) nitrate
Al(s)+ Cu(NO3)2(aq)
 Double Replacement
 AB + CD  AD + CB
 Practice
 Calcium chloride reacts with sodium
phosphate
CaCl2(aq) + Na3PO4(aq) 
 Lead (II) nitrate reacts with barium chloride
Pb(NO3)2(aq) + BaCl2(aq) 
 Acid/Base (a special type of double
replacement reaction)
 HA + B(OH)  H2O + BA
 Practice
 Hydrochloric acid reacts with sodium
hydroxide
HCl(aq) + NaOH(aq) 
 Sulfuric acid reacts with copper (II) hydroxide
H2SO4(aq) + Cu(OH)2(aq) 
 Combustion
 Always produces carbon dioxide and
water
 Practice
 Pentane reacts with oxygen
C5H12 + O2 
 Decane reacts with oxygen
C10H22 + O2 
 A complete ionic equation shows dissolved ionic
compounds as dissociated free ions.
 Example:
 Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)  AgCl (s) + Na+ (aq) +
NO3- (aq)
 Spectator ions – those ions not directly involved in the
chemical reaction.
 Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)  AgCl (s) + Na+ (aq) +
NO3- (aq)
 Net ionic equation – equation for reaction in solution
that shows only those particles that are directly
involved the chemical change.
 Ag+ (aq) + Cl- (aq)  AgCl (s)
 You can predict which compounds are the spectator
ions by using the following solubility rules:
Compounds
Solubility
Salts of alkali metals and ammonia
Soluble (aq)
Nitrate salts (NO3) and chlorate salts
(ClO3)
Soluble (aq)
Sulfate (SO4) salts except compounds
with
Pb 2+, Ag +, Hg2 2+, Ba 2+, Sr 2+,
and Ca 2+
Soluble (aq)
Chloride (Cl) salts except compounds
with Ag +, Pb 2+, and Hg2 2+
Soluble (aq)
Carbonates, Phosphates, Chromates,
Sulfides, and hydroxides
Insoluble (s)
 Pb(NO3) 2 (aq) + H2SO4 (aq)  PbSO4 (s) + HNO3 (aq)
 Pb 2+ + (NO3) - + H2+ + SO4  PbSO4 + H+ + NO3-
 H+ + NO3- spectator ions because nitrate salts are soluble an
will not form precipitates.
 PbSO4 is not a spectator ion because the sulfate is combined
with lead, one of the noted exceptions.
 Net ionic reaction
Pb 2+ + SO4  PbSO4