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Skills Worksheet
Concept Review
Section: Oxidation-Reduction Reactions
Choose the statement from Column B that best matches the term in Column A, and
write the corresponding letter in the space provided.
Column A
Column B
______ 1. reduction
a. a chemical reaction in which a substance
gains electrons
______ 2. oxidation
b. any chemical process in which electrons
are transferred from one substance to
another
______ 3. redox reaction
c. a chemical reaction in which a substance
loses electrons
______ 4. oxidation number
d. substance that causes reduction to happen
and is itself oxidized
______ 5. reducing agent
e. number assigned to an atom in a polyatomic ion or molecular compound based
on the assumption of complete transfer of
electrons
______ 6. half-reaction
f. substance that causes the oxidation of
other substances and is itself reduced
______ 7. oxidizing agent
g. the part of a reaction that involves only
oxidation or reduction
Determine the oxidation number for each atom in the following chemical formulas.
8. ZnCl2
9. SO3
10. HNO3
11. Al2(SO4)3
12. PbO
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Holt Chemistry
1
Oxidation, Reduction, and Electrochemistry
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Concept Review continued
13. CO2
14. H2SO4
15. Write the half-reaction for the conversion of hydrogen peroxide to water.
16. Identify which of the following reactions is a reduction reaction and which is
an oxidation reaction. Write the balanced overall ionic equation for the redox
reaction between these two.
Mg £ Mg 2 2e
O2 4e £ 2O2
Balance the following equations using the half-reaction method.
2
2
17. MnO
(in acidic solution)
2 SO2 £ SO4 Mn
2
18. NO
(in acidic solution)
3 Cu £ NO Cu
19. H2S NO
3 £ NO2 S8 (in acidic solution)
20. In this equation identify which atoms where reduced and which were oxidized.
2K(s) Cl2(g) £ 2KCl(s)
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Holt Chemistry
2
Oxidation, Reduction, and Electrochemistry
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TEACHER RESOURCE
Answer Key
Concept Review: OxidationReduction Reactions
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
a
c
b
e
d
g
f
Zn: 2, Cl: 1
S: 6, O: 2
H: 1, N: 5, O: 2
Al: 3, S: 6, O: 2
Pb: 2, O: 2
C: 4, O: 2
H: 1, S: 6, O: 2
H2O2(aq) 2H(aq) 2e £ 2H2O(l)
oxidation, reduction, 2Mg O2
£ 2Mg2 2O2 ; Mg O2 2MgO
2
2MnO
4 5SO2 2H2O £ 2Mn
2
5SO4 4H
2
2NO
3 3Cu 8H £ 2NO 3Cu
4H2O
8H2S 16NO
3 16H £ 16NO2
S8 16H20
K is oxidized and Cl is reduced.
Concept Review:
Introduction to
Electrochemistry
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17. salt bridge or porous barrier
18. Electrons flow from the higher
voltage
electric current, ampere
electrode
electrochemical
c
b
e
d
f
a
h
g
cathode
electrolyte
oxidation
reduction
“pressure” in the negative terminal
through a metal circuit, which
includes the light blub, towards the
positive terminal.
19. Zn(s) £ Zn2(aq) 2e, anode
20. Cu2(aq) 2e £ Cu(s), reduction
Concept Review:
Galvanic Cells
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
simple
two, outside, two, thin
indirectly, inefficient
directly, simple, efficient
possible
galvanic
chemical, electrical
portable
acidic
alkaline
carbon
alkaline
steel
lead
lead(II) sulfate
galvanic, electrolytic
rechargeable
galvanic
Daniell
Ag, cathode; Zn, anode; 1.5614 V
Cu, cathode; Pb, anode;
0.4681 V
2e
2
Zn(s) Cu (aq) –£ Zn2(aq)
Cu(s), spontaneously to the right
E (0.34) (0.76)
1.10 V
2e
£ Cl2(g) 2I(aq)
I2(s) 2Cl(aq) –
spontaneously to the left
E (0.54) (1.36)
0.82 V
2e
£ Cu2(aq)
2Ag(aq) Cu(s) –
2Ag(s) spontaneously to the right
E (0.80) (0.34) 0.46 V
the deterioration of metals due to
oxidation reactions with their
environment
oxygen, water, and ions
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Holt Chemistry
101
Oxidation, Reduction, and Electrochemistry