1. Chapter 11: Chemical Reactions
Reactions in Aqueous Solution

2. Learning Targets
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.
You will write a complete ionic and net ionic equation from a molecular equation and determine the spectator ions.

3. Molecular, Ionic and Net Ionic Equations
A precipitate of silver chloride forms when aqueous solutions of silver nitrate and sodium chloride are mixed.
Which ions do not participate in the reaction?
You will write a complete ionic and net ionic equation from a molecular equation and determine the spectator ions.

4. FeCl3 (aq) + 3 KOH (aq)  Fe(OH)3 (s) + 3 KCl (aq)
Molecular Equations
A molecular equation is what we have been performing this entire unit.
Balanced chemical equation that shows reactants, products and physical states.
FeCl3 (aq) + 3 KOH (aq)  Fe(OH)3 (s) + 3 KCl (aq)
You will write a complete ionic and net ionic equation from a molecular equation and determine the spectator ions.

5. FeCl3 (aq) + 3 KOH (aq)  Fe(OH)3 (s) + 3 KCl (aq)
Ionic Equations
An ionic equation shows the molecular equation as dissociated free ions with physical states.
If something is a liquid, solid or gas, it would not dissociate.
FeCl3 (aq) + 3 KOH (aq)  Fe(OH)3 (s) + 3 KCl (aq)
Fe+3(aq)+ 3 Cl1- (aq) + 3 K1+ (aq) + 3 OH-1 (aq)  Fe(OH)3 (s) + 3 K1+(aq) + 3 Cl-1 (aq)
You will write a complete ionic and net ionic equation from a molecular equation and determine the spectator ions.

6. Fe+3 (aq) + 3 OH1- (aq)  Fe(OH)3 (s)
Net Ionic Equations
A net ionic equation includes only ions directly involved in the chemical reaction.
Ions not directly involved in the chemical reaction are called spectator ions.
Fe+3 (aq)+ 3 Cl1- (aq) + 3 K1+ (aq) + 3 OH-1 (aq)  Fe(OH)3 (s) + 3 K1+ (aq) + 3 Cl-1 (aq)
Fe+3 (aq) + 3 OH1- (aq)  Fe(OH)3 (s)
You will write a complete ionic and net ionic equation from a molecular equation and determine the spectator ions.

7. Let’s try one together …
Write the molecular equation, the complete ionic equation, and the net ionic equation for the following reaction:
Aqueous sodium sulfide is mixed with aqueous copper (II) nitrate.
You will write a complete ionic and net ionic equation from a molecular equation and determine the spectator ions.

8. Answer Molecular: S2- (aq) + Cu2+ (aq)  CuS (s)
Na2S (aq) + Cu(NO3)2 (aq)  2 NaNO3 (aq) + CuS (s)
Ionic:
2 Na+ (aq) + S2- (aq) + Cu2+ (aq) + 2 NO3- (aq)  2 Na+ (aq) + 2 NO3- (aq) + CuS (s)
Net Ionic:
S2- (aq) + Cu2+ (aq)  CuS (s)
You will write a complete ionic and net ionic equation from a molecular equation and determine the spectator ions.

9. Aqueous ammonium chloride and aqueous lead (II) nitrate react.
Try on your own
Write the molecular equation, the complete ionic equation, and the net ionic equation for the following reaction:
Aqueous ammonium chloride and aqueous lead (II) nitrate react.
You will write a complete ionic and net ionic equation from a molecular equation and determine the spectator ions.

10. Answer Molecular: 2 Cl- (aq) + Pb2+ (aq)  PbCl2 (s)
2 NH4Cl (aq) + Pb(NO3)2 (aq)  PbCl2 (s) + 2 NH4NO3 (aq)
Ionic:
2 NH4+ (aq) + 2 Cl- (aq) + Pb2+ (aq) + 2 NO3- (aq)  PbCl2 (s) + 2 NH4+ (aq) + 2 NO3- (aq)
Net Ionic:
2 Cl- (aq) + Pb2+ (aq)  PbCl2 (s)
You will write a complete ionic and net ionic equation from a molecular equation and determine the spectator ions.

11. LiOH (aq) + HCl (aq)  H2O (l) + LiCl (aq)
Acid-Base Reactions
You are familiar with acid formulas; base formulas contain hydroxide ions
Double replacement reactions in which the products are liquid water and a salt.
A salt is interpreted as the ionic compound formed in addition to water.
Example:
LiOH (aq) + HCl (aq)  H2O (l) + LiCl (aq)
Notice water as a product
Notice the salt as the product
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.

12. Oxidation-Reduction Reactions
Reactions that involve a transfer of electrons
Examples:
2 Na (s) + Cl2 (g)  2 NaCl (s)
Zn (s) + CuCl2 (aq)  ZnCl2 (aq) + Cu (s)
You will recognize the type of chemical reaction taking place: oxidation-reduction – synthesis, decomposition, single replacement, combustion; double replacement – precipitation, acid base reactions, gas forming reactions.