1. Types of Reactions

2. precipitate: a solid product that forms in an
aqueous solution reaction
Na2CO Ca(NO3)2
(aq)
CaCO
(s) 2
NaNO3
(aq)
(aq)
“chunks”
“sinkies”
“floaties”
ppt
clear
Na2CO3
solution
clear
Ca(NO3)2
solution
cloudy solution
containing CaCO3(s)
and NaNO3(aq)

3. Key Terms Term Definition In an Equation soluble able to be dissolved
(aq) 
insoluble
does not dissolve in solution (or water)
 (ins)
precipitate
an insoluble solid formed when two solutions are mixed
(s) 

4. Using Solubility Rules
Most solubility rules are written based on the negative ion or anion

5. How to Determine if a Compound is Soluble or Insoluble?
Find the anion in the compound.
Find the rule in the solubility tables that matches the ion.
Double check to make sure the cation isn’t listed as an exception.

6. Predict if the following compounds are soluble or insoluble.
CaCl2
CuSO4
Al2(CrO4)3
Mg(OH)2
AgCl
SrS
Soluble
Insoluble
Insoluble
Insoluble
Soluble

7. Predicting if a Precipitate will Form
Precipitate reactions are precipitation reactions.
In order for a reaction to be a precipitation reaction, there must be
one solid product, which is the precipitate, and
both reactants should be aqueous solutions

8. Determine which reactions are precipitation reactions or reactions that will form a precipitate.
Pb(NO3) KI  PbI KNO3
(NH4)2CO3 + K2S  K2CO (NH4)2S
Ag + Cu(NO3)2  AgNO3 + Cu
Ba(OH) Fe(ClO4)3  Ba(ClO4) Fe(OH)3
(aq)
(aq)
(s)
(aq)
YES NO
(aq)
(aq)
(aq)
(aq) NO
(s)
(s)
(aq)
(aq)
YES
(aq)
(aq)
(aq)
(s)

9. Neutralization Reaction
A reaction between and acid and a base which results in the production of a salt and water.
ACID + BASE = SALT + WATER
HCl(aq) + NaOH(aq) = H2O(l) + NaCl(aq)
Mg(OH)2(s) + 2HCl(aq) = MgCl2(aq) + 2H2O(l)

10. Reduction-Oxidation Reaction REDOX
A reaction in which electrons are transferred from one species to another.
Oxidation means the loss of electrons.
Reduction means the gain of electrons.
LEO says GER
Loss Electrons = Oxidation
Gain Electrons = Reduction
Many oxidation-reduction reactions are single replacement reactions

11. Oxidation Reduction Reactions (Redox)
Each sodium atom loses one electron:
Each chlorine atom gains one electron:

12. Lose Electrons = Oxidation
LEO says GER :
Lose Electrons = Oxidation
Sodium is oxidized
Gain Electrons = Reduction
Chlorine is reduced

13. Rules for Assigning Oxidation Numbers Rules 1 & 2
The oxidation number of any uncombined element is zero
2. The oxidation number of a monatomic ion
equals its charge

14. Rules for Assigning Oxidation Numbers Rules 3 & 4
3. The oxidation number of oxygen in
compounds is -2
4. The oxidation number of hydrogen in compounds is +1

15. Rules for Assigning Oxidation Number Rule 5
5. The sum of the oxidation numbers in the formula of a compound is 0
2(+1) + (-2) = 0
H O
(+2) + 2(-2) + 2(+1) = 0
Ca O H

16. Rules for Assigning Oxidation Numbers Rule 6
6. The sum of the oxidation numbers in the
formula of a polyatomic ion is equal to
its charge
X + 4(-2) = -2
S O
X + 3(-2) = -1
N O
 X = +5
 X = +6

17. Assigning Oxidation States
Example: Assign oxidation states to all atoms in the
following.
CO2  O =
SF6  F =
NO3-  O =
MnO4-  O =
HSO3-  O =
H2O  H =
Li3N  Li =
-2 (for each oxygen); C = +4
-1 (for each fluorine); S = +6
-2 (each oxygen); N = +5
-2 (each oxygen); Mn = +7
-2 (each oxygen); H = +1, S = +4
+1 (each); O = -2
+1 (each); N = -3