Workbook - Oxidation Reduction KEY
Define each
1. Oxidation 2. Reduction 3. Oxidizing agent 4. Reducing agent
- loss of electrons - gain of electrons - causes oxidation by undergoing reduction - causes reduction by undergoing oxidation
Write half reactions for each of the following atoms or ions. Label each as oxidation or reduction.
5.
Al -----------> Al3+ + 3e-
oxidation
6.
S
+ 2e- ---------> S2-
reduction
7.
2O2- ---------->
O2 + 4e-
oxidation
8.
Ba2+ + 2e- -----------> Ba
reduction
9.
2N3- ---------->
N2 + 6e-
oxidation
10.
Br2 + 2e- ---------> 2Br-
reduction
11.
P + 3e- ----------> P3-
reduction
12.
Ca -----------> Ca2+ + 2e-
oxidation
13
Ga3+ + 3e- -----------> Ga
reduction
14.
S
+ 2e- ---------> S2-
reduction
15.
H2 --------->
2H+ + 2e-
oxidation
16.
2H+ + 2e- ---------> H2
reduction
17.
2F- ----------> F2 + 2e-
oxidation
18.
P3- ---------->
P + 3e-
oxidation
Balance each spontaneous redox equation. Identify the entities reduced and oxidized. State the reducing agent and the oxidizing agent.
19. Al
&
Zn2+
2Al + oxidized reducing agent
3Zn2+
2Al3+ +
3Zn
reduced
oxidizing agent
20. F2
&
O2-
2F2 +
2O2-
4F- +
O2
reduced
oxidized
oxidizing agent reducing agent
21. O2
& Ca
2Ca + oxidized reducing agent
O2
reduced
oxidizing agent
2Ca2+ +
2O2-
22. Al3+
& Li
Al3+ + reduced oxidizing agent
3Li
Al
oxidized
reducing agent
+
3Li+
Label the species that is reduced, that is oxidized, the reducing agent and the oxidizing agent.
23.
Fe2+
+ Co
Co2+
+
Fe
Co Co2+ + 2e- oxidation 2e- Fe reduction
Fe2+ +
24.
3 Ag+
+ Ni
Ni3+
+
3 Ag
Ni Ni2+ + 2e1e- Agreduction
oxidation
Ag+ +
25.
Cu2+
+ Pb
Pb2+
+
Cu
Pb 2e- Cu
Pb2+ + 2ereduction
oxidation
Cu2+ +
26.
O2
2 Sn2+
+ 2 Sn
O2-
+
Sn Sn2+ + 2e-
oxidation
O2
+
4e- 2O2-
reduction
27.
Co2+
+
2 F-
F2
Co
+
+ 2e-
2F- F2 Coreduction
+ 2e-
oxidation
Co2+
28. List the species (formulas from above) that lose electrons: Co Ni Pb Sn F-
29. List the species (formulas from above) that gain electrons: Fe2+ Ag+ Cu2+ O2 Co2+
For each of the following reactions, identify: -The Oxidizing Agent. -The Reducing Agent. -The Substance Oxidized. -The Substance Reduced.
30. I-
+
Cl2 ---------->
Cl- +
I2
Substance oxidized I-
Oxidizing agent
Cl2
31. Co +
Fe3+
----------->
Reducing agent
I-
Substance reduced Cl2
Co2+ +
Fe2+
Substance oxidized Co
Oxidizing agent
Fe3+
Reducing agent
Co
Substance reduced Fe3+
32. Cr6+ +
Fe2+
----------->
Cr3+ +
Fe3+
Substance oxidized Fe2+
Oxidizing agent
Cr6+
Reducing agent
Fe2+
Substance reduced Cr6+
Redox Half Reactions and Reactions WS #2
1. State the Oxidation Number of each of the elements that is underlined.
a) NH3
-3
b) H2SO4
6
c) ZnSO3
4
d) Al(OH)3
3
e) Na
0
f) Cl2
0
g) AgNO3
5
h) ClO4-
7
i) SO2
4
j) K2Cr2O4
3
k) Ca(ClO3)2
5
m) HPO32-
3
l) K2Cr2O7
6
n) HClO
1
o) MnO2
4
p) KClO3
5
q) PbO2
4
s) K2SO4
6
r) PbSO4
2
t) NH4+
-3
u) Na2O2
-1
v) FeO
2
w) Fe2O3
3
x) SiO44-
-2
y) NaIO3
5
z) ClO3-
5
aa) NO3-
5
cc) CaH2
-1
ee) Fe(H2O)63+
+3
bb) Cr(OH)4
4
dd) Pt(H20)5(0H)2+ +3
ff) CH3COOH
0
2. What is the oxidation number of carbon in each of the following substances?
a) CO c) CO2
2
b) C
4
d) CO32-
0 4
e) C2H6
-3
f) CH3OH
-2
3. For each of the following reactions, identify: the oxidizing agent, the reducing agent,
the substance oxidized and the substance reduced.
a) Cu2+ (aq) +
Zn (s)
-------->
Cu (s) +
Zn2+ (aq)
Cu2+
Substance oxidized
Oxidizing agent Zn
Zn
Substance reduced
Cu2+
Reducing agent
b) Cl2 (g)
+
2 Na (s) -------->
2 Na+ (aq)
+
2 Cl- (aq)
Substance oxidized Cl2
Oxidizing agent Na
Na
Substance reduced
Cl2
Reducing agent
WS # 3
Spontaneous and Non-spontaneous Redox Reactions
Describe each reaction as spontaneous or non-spontaneous.
1. Au+3 + Fe+3 -----> Fe+2 oxidizing agents)
+ Au
nonspontaneous (two
2. Pb + Fe+3 ------> Fe+2
+ Pb+2
spontaneous
3. Cl2 + F-
------> F2
+ 2Cl-
nonspontaneous
4. S2O8-2 + Pb ------> 2SO4-2 + Pb+2
spontaneous
5.Cu+2 + 2Br- ------> Cu + Br2
nonspontaneous
6. Sn+2 + Br2 ------> Sn+4 + 2Br-
spontaneous
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