WORKSHEET:
Redox reactions
1. Define the process of oxidation in terms of :
a) transfer (gain or loss) of oxygen ____________
b) transfer (gain or loss) of electrons ___________
2. Define the process of reduction in terms of:
a) transfer (gain or loss) of oxygen ____________
b) transfer (gain or loss) of electrons ___________
3. Why are redox reactions important?
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4. What is unique about redox reactions that make them useful in electrochemistry?
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5. a) Complete the half equations by balancing it and identify each half reaction as
either an oxidation (O) or reduction (R) reaction.
(i)
Na (s)

(iii)
Fe (s)

v)
K(s)

K+ (aq)
vi)
O2 (g)
vii)
F- (aq)

F2 (g)
viii)
Cu 2+ (aq)
ix)
S (s)
Na+ (aq)
Fe3+(aq)
 S2- (aq)
(ii)
Mg2+(aq)

(iv)
Cl- (aq)

x)
H2 (g)

Mg (s)
Cl2 (g)
O2- (aq)


Cu(s)
H+ (aq)
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Consider the reaction given below:
A)
Cu2+
+
Zn

Zn2+
+
Cu
i) Identify the chemical substance (species) that has undergone oxidation
ii) Identify the chemical substance (species) that has undergone reduction
iii) Identify (from the reactants) the oxidising agent (oxidant) in this reaction;
iv) Identify (from the reactants) the reducing agent (reductant) in this reaction
For the following equations balance them and fill in the table below
B)
Cl2 (aq) + Br- (aq)  Br2(aq) +
C)
Fe (s)
D)
Al (s)
#
What is
oxidized?
+
Ag +(aq)

Ag (s)
+ Fe 2+ (aq)  Al3+(aq)
What is
reduced?
Cl- (aq)
Oxidizing
agent?
+
+
Fe2+ (aq)
Fe (s)
Reducing
agent?
# of electrons
transferred?
B
C
D
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