Chapter 11.1Pages 330-339

SynthesisA + B ABPractice

•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)

DecompositionAB A + BPractice

•Solid Lead (IV) oxide decomposes PbO2(s)

•Aluminum nitride decomposes AlN(s)

Single ReplacementAB + C AC + BMust 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 ReplacementAB + CD AD + CBPractice

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 + BAPractice

Hydrochloric acid reacts with sodium hydroxide

HCl(aq) + NaOH(aq) Sulfuric acid reacts with copper (II)

hydroxide H2SO4(aq) + Cu(OH)2(aq)

CombustionAlways produces carbon dioxide and water

PracticePentane 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 and will not form precipitates.

PbSO4 is not a spectator ion because the sulfate is combined with lead, one of the noted exceptions.

Net ionic reactionPb 2+ + SO4 PbSO4