Post on 31-Dec-2015
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