I II III IV V

Ch. 11 – Chemical Reactions

IV. Predicting Products

C3H8(g)+ O2(g)

A. Combustion

Reactants:

Often hydrocarbons

O2

Products: All contain oxygen hydrocarbons form CO2 + H2O

Fe(s)+ CuSO4(aq)

D. Single Replacement Products:

metal metal (+) nonmetal nonmetal (-)

Br2(l)+ NaCl(aq)

Pb(NO3)2(aq)+ KI(aq)

E. Double Replacement

Products: switch negative ions

NaNO3(aq)+ NiCl2 (aq)

Neutralization Reaction

Neutralization Reactions always result in the formation of a salt and water

HBr + LiOH

H2SO4 + Al(OH)3

Practice

Na + CaCl2

HCl + Ba(OH)2

MgSO4 + PbCl2

C3H8 + O2

Net Ionic Equations Complete ionic equation = equation

that shows all dissolved ionic compounds as dissociated free ions

Net ionic equation = Equation for a reaction in solution that shows only those substances who do not remain as ions on both sides of the equation

Spectator Ion = an ion that appears on both sides of an equation and is not directly involved in the reaction

Net Ionic Equations

Substances that are solid, liquid, or gas should not be broken down into ions

The formulas of these substances remains unchanged

Net Ionic Equations

AgNO3(aq) + KCl(aq) AgCl(s) + KNO3(aq)

Ag+(aq) + NO3–

(aq) + K+(aq) + Cl–(aq) AgCl(s) + K+(aq) + NO3–(aq)

CIE:

Molecular (or Full) Equation:

NIE: Ag+(aq) + Cl–(aq) AgCl(s)

SI: K+(aq) and NO3–(aq)

Example

K3PO4 (aq) + Al(NO3)3 (aq) AlPO4(s) + 3KNO3(aq)

Practice

BeI2(aq) + Cu2SO4(aq) 2CuI(s) + BeSO4(aq)

Ni(NO3)3(aq) + 3KBr(aq) NiBr3(s) + 3KNO3(aq)

3Ca(OH)2(aq) + 2FeCl3(aq) 2Fe(OH)3(s) + 3CaCl2(aq)

Solubility Rules

All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+, or Hg2

2+.

All compounds containing NO3-, ClO4

-, ClO3

-, and C2H3O2- anions are soluble.

All sulfates (SO4-2) are soluble except

those containing Hg22+, Pb2+, Sr2+,

Ca2+, or Ba2+.

All compounds containing alkali metal cations (Na+, K+, H+) and the ammonium ion (NH4+) are soluble

All compounds containing OH-,  PO43-, S2-,

CO32-, O2-,CrO4

-2 and SO32-ions are 

insoluble, OH- or S2- soluble with group 1, Ba2+, NH4

+

CO32-, O2-, SO3

2- soluble with group 1 and NH4

+

CrO42- soluble with group 1, Ca2+

, Sr2+, and

NH4+

A double replacement reaction will "fail" if One or more of the reactants are

insoluble. Example: PbS + AgNO3 -->

If both products are soluble. Example: NaCl + HC2H3O2 -->

NaC2H3O2 + HCl No reaction. No ppt. Rule 2 and Rule 4

Practice

KBr PbCO3

Li2SO3

Zn(OH)2

NaC2H3O2

AgI CdS ZnCO3

Soluble

Soluble

Soluble

Insoluble

Insoluble

Insoluble

Insoluble

Insoluble