Oxidation Reduction Worksheet
1. Determine the oxidation number of each atom in the following substances
a. NF3
N
+3
F
-1
b. K2CO3
K
+1
C
4
c. NO3-
N____+5_____
d. HIO4
H
+1
O
-2
O____-2______
I
+7
O
-2
2. For the following balanced redox reaction answer the following questions
2 Fe+2(aq) + H2O2(aq)  2Fe+3(aq) + 2 OH-1(aq)
a. What is the oxidation state of oxygen in H2O2?
-1
b. What is the element that is oxidized?
Fe
c. What is the element that is reduced?
O
d. What is the oxidizing agent?
H2O2
e. What is the reducing agent?
Fe+2
f. How many electrons are transferred in the reaction as it is balanced?
2 e-
3. For the following balanced redox reaction answer the following questions
4NaOH(aq) + Ca(OH)2(aq) + C(s) + 4ClO2(g)  4NaClO2(aq) + CaCO3(s) + 3H2O(l)
a. What is the oxidation state of Cl in ClO2(g)?
b. What is the oxidation state of C in C(s)?
4
0
c. What is the element that is oxidized?
C
d. What is the element that is reduced?
Cl
e. What is the oxidizing agent?
ClO2
f. What is the reducing agent?
C(s)
g. How many electrons are transferred in the reaction as it is balanced?
4 e-
4. Balance the following equations using the half-reaction method:
a. Sn2+(aq) + NO3-(aq)  Sn4+(aq) + NO(g) (in acid)
(Sn+2

Sn+4 + 2e-) x 3
(3e- + NO3- + 4H+  NO + 2H2O) x 2
3Sn+2 + 6e- + 2NO3- + 8H+  3Sn+4 + 6e- + 2NO + 4H2O
3Sn+2 + 2NO3- + 8H+  3Sn+4 + 2NO + 4H2O
b. MnO4-(aq) + NO2-(aq)  MnO2(s) + NO3-(aq) (in base)
(MnO4- + 4H+ + 3e-  MnO2 + 2H2O) x 2
(NO2- + H2O  NO3- + 2H+ + 2e-) x 3
2MnO4- + 8H+ + 6e- + 3NO2- + 3H2O  2MnO2 + 4H2O + 3NO3- + 6H+ + 6e2H+ + 2MnO4- + 3NO2-  2MnO2 + 3NO3- + H2O
2 H2O  2 H+ + 2 OHH2O + 2 MnO4-1 + 3 NO2-1  2 OH-1 + 2 MnO2 + 3 NO3-1
c. 2 MnO4- + 10 Cl- + 16 H+ = 8 H2O + 5 Cl2 + Mn2+
d. MnO4- + 8H+ + 5e-  Mn2+ + 4H2O
e. 14 H+ + Cr2O72- + 6Fe2+  6Fe3+ + 2Cr3+ + 7H2O
g. MnO4- + 5Fe2+ + 8H+ 5Fe3+ + Mn2+ + 4H2O