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Grade 12 Oxidation and Reduction Quiz

Total questions: 75

Worksheet time: 2hrs 18mins

Name
Class
Date
1.

What is the oxidation number of a monatomic ion?

a)

+2

b)

0

c)

-1

d)

+1

2.

What are the oxidation numbers in the compound KC1?

a)

K = 0, Cl = 0

b)

K = -1, Cl = +1

c)

K = +1, C1=-1

d)

K = +2, Cl = -2

3.

In the reaction represented by the equation 02 + 4e¯ → 2 02-, the species O₂ is

a)

C. neutralized.

b)

disproportionated.

c)

oxidized.

d)

reduced.

4.

The conversion of Mg → Mg2+ + 2e¯ is

a)

disproportionation.

b)

neutralized.

c)

reduction.

d)

oxidation.

5.

During redox reactions, reducing agents

a)

increase their oxidation number.

b)

decrease their oxidation number.

c)

keep the same oxidation number.

d)

do not participate.

6.

When Na(s) reacts with Cl₂ (g) to produce NaCl (s), Na(s) is the

a)

oxidizing agent.

b)

reducing agent.

c)

neutralizing agent.

d)

ionizing agent.

7.

Which of the following statements refers to an oxidation process?

a)

Hydrogen is added to ethene

b)

Oxygen is removed from carbon dioxide

c)

Chlorine accepts electrons

d)

Increase in the oxidation number of magnesium metal

8.

Which of these equations represents a redox reaction?

a)

Ca(HCO3)2 --> CaCO3 + H2O + CO2

b)

CH3COOH + NaOH --> CH3COONa + H2O

c)

Zn + 2FeCl3 --> ZnCl2 + 2FeCl2

d)

NaCl + AgNO3 --> AgCl + NaNO3

9.

What is the oxidation number of chlorine in ClO3- ?

a)

-1

b)

+1

c)

-1

d)

+5

10.

What are the oxidation numbers of manganese in the manganese compounds shown below?

a)

A

b)

B

c)

C

d)

D

11.

The table shows four chemical changes. Which changes involve donation of electrons?

a)

P and Q

P and R

Q and S

R and S

b)

P and R

c)

Q and S

d)

R and S

12.

In a redox reaction, the species reduced

a)

gains electrons and is the oxidizing agent

b)

loses electrons and is the oxidizing agent

c)

loses electrons and is the reducing agent

d)

gains electrons and is the reducing agent

13.
Which statement is true:
Mg → Mg2+ + 2e–
a)
Mg gains 2 electrons
b)
Mg2+ loses 2 electrons
c)
Mg loses 1 electron
d)
Mg loses 2 electrons
14.
Which of the following half reactions correctly represents a reduction half reaction?
a)
Fe →Fe2+ + 2e-
b)
Pb4+ + 2e- →Pb2+
c)
2O-2 →O2 + 4e-
d)
Fe + 3e- →Fe3+
15.

In a reaction, copper is reduced; its number of electrons has:

a)

Increased

b)

Decreased

c)

Remained Constant

d)

Varies Randomly

16.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
17.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
18.

Substance that oxidizes another substance by accepting its electrons.

a)

reducing agent

b)

oxidation number

c)

combustion

d)

oxidizing agent

19.
     In the reaction Zn + H2O --> ZnO2 + H2
 which element, if any, is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
20.
What substance is oxidized in the following reaction?
4Fe + 3O2 --> 2Fe2O3
a)
Iron
b)
Fluorine
c)
Oxygen
21.

The below reaction is an example of _________reaction.

F2 → 2 F- + 2 e-

a)

Oxidation

b)

Reduction

c)

Neutralization

d)

decomposition

e)

combustion

22.

Identify the species reduced in the following reaction.


Fe(s) + 2 Ag+(aq) → Fe2+(aq) + 2 Ag(s)

a)

Fe

b)

Ag

c)

none of these

d)

None of the above

23.

Determine the oxidation number of the selected element in each ion/ compound.

a) N in N2O4

b) Cr in CrO4 2-

c) I in IO3-

a)

+8, -6, +5

b)

+2, +8, +6

c)

+4, +6, +5

d)

-4, -6, -5

e)

-4, -8, -6

24.

Find the oxidation number of S in S2O4 2-

a)

+3

b)

+6

c)

-6

d)

-3

e)

-4

25.

What is the oxidation number of Nitrogen in HNO3

a)

-7

b)

-5

c)

+5

d)

+7

e)

+2

26.

The change of I‾ to I2 is ________________

a)

oxidation

b)

reduction

c)

neutralization

d)

Decomposition

e)

Combustion

27.

What is the oxidation number of Nitrogen in HNO3

a)

-7

b)

-5

c)

+5

d)

+7

e)

+2

28.

Identify the species reduced in the following reaction.


Fe(s) + 2 Ag+(aq) → Fe2+(aq) + 2 Ag(s)

a)

Fe

b)

Ag

c)

none of these

d)

None of the above

29.

Find the oxidation number of Ca in CaH2

a)

-2

b)

-4

c)

+2

d)

+4

e)

0

30.

What is the oxidation state of Nitrogen in N2 (g)?

a)

4

b)

6

c)

2

d)

0

31.

Identify the substance that is reduced in the reaction between copper(II) ion and magnesium.

Cu2+ + Mg → Cu + Mg2+

a)

Cu2+

b)

Mg

c)

Cu

d)

Mg2+

32.
Which of the following half reactions correctly represents a reduction half reaction?
a)
Fe →Fe2+ + 2e-
b)
Pb4+ + 2e- →Pb2+
c)
2O-2 →O2 + 4e-
d)
Fe + 3e- →Fe3+
33.
What substance is oxidized in the following reaction?
4Fe + 3O2 --> 2Fe2O3
a)
Iron
b)
Fluorine
c)
Oxygen
34.

In the reaction


4 NH3 + 5 O2 → 4 NO + 6 H2O


the oxidation number of nitrogen changes from

a)

–2 to –3

b)

–2 to +3

c)

–3 to –2

d)

–3 to +2

35.

What is the oxidation number of chromium in K2Cr2O7 ?

a)

+12

b)

+2

c)

+3

d)

+6

36.

In which substance does hydrogen have an oxidation number of zero?

a)

LiH

b)

H2O

c)

H2S

d)

H2

37.

In which substance is the oxidation number of Cl equal to +1?

a)

Cl2

b)

Cl2O

c)

AlCl3

d)

HClO2

38.

What is the oxidation state of phosphorus in the

compound Na3PO3?

a)

0

b)

-3

c)

+3

d)

+5

39.

In which compound does hydrogen have an oxidation state of –1?

a)

NaH

b)

HCl

c)

H2O

d)

NH3

40.

Oxygen has an oxidation number of –2 in

a)

O2

b)

NO2

c)

Na2O2

d)

OF2

41.

Given the reaction:


Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)


The oxidation number of Zn(s) increases because it

a)

loses electrons

b)

gains electrons

c)

loses protons

d)

gains protons

42.

Which change in oxidation number represents reduction?

a)

–1 to +1

b)

–1 to –2

c)

–1 to +2

d)

–1 to 0

43.

Given the oxidation-reduction reaction:


H2 + 2 Fe+3 → 2 H+ + 2 Fe+2


Which species undergoes reduction?

a)

H2

b)

Fe3+

c)

H+

d)

Fe2+

44.

Given the cell reaction:


Ca(s) + Mg2+(aq) → Ca2+(aq) + Mg(s)


Which substance was oxidized?

a)

Ca(s)

b)

Mg2+(aq)

c)

Ca2+(aq)

d)

Mg(s)

45.

In the reaction


2 Fe3+ + S2– → 2 Fe2+ + S0,


the species oxidized is

a)

Fe3+

b)

S2–

c)

Fe2+

d)

S0

46.

In the reaction


2 Mg + O2 → 2 MgO


the magnesium is the

a)

oxidizing agent and is reduced

b)

oxidizing agent and is oxidized

c)

reducing agent and is reduced

d)

reducing agent and is oxidized

47.

Given the redox reaction:


Fe2+(aq) + Zn(s) → Zn2+(aq) + Fe(s)


Which species acts as a reducing agent?

a)

Fe(s)

b)

Fe2+(aq)

c)

Zn(s)

d)

Zn2+(aq)

48.

Which half-reaction correctly represents oxidation?

a)

Sn2+ + 2e– → Sn0

b)

Sn4+ + 2e– → Sn2+

c)

Sn2+ → Sn0 + 2e–

d)

Sn2+ → Sn4+ + 2e–

49.

Which balanced equation represents an oxidation-reduction reaction?

a)

AgNO3 + NaCl → AgCl + NaNO3

b)

BaCl2 +K2CO3 → BaCO3 +2KCl

c)

CuO + CO → Cu + CO2

d)

HCl + KOH → KCl + H2O

50.

Which balanced equation represents an oxidation-reduction reaction?

a)

Ba(NO3)2 + Na2SO4 →BaSO4 + 2NaNO3

b)

H3PO4 + 3KOH →K3PO4 + 3H2O

c)

Fe(s) + S(s) →FeS(s)

d)

NH3(g) + HCl(g) →NH4Cl(s)

51.

What is the oxidation number of chlorine in ClO3- ?

a)

5

b)

1

c)

0

d)

2

52.

In which substance does sulfur have a negative oxidation number?

a)

Na2S

b)

SO2

c)

S

53.

What is the oxidation number assigned to manganese in KMnO4?

a)

7

b)

5

c)

4

d)

0

54.

Which of the following is the balanced half -reaction for the oxidation of Cu to Cu+2?

a)

Cu --> Cu+2

b)

Cu + 2 e- --> Cu+2

c)

Cu - 2e- --> Cu+2

d)

Cu --> Cu+2 + 2 e-

55.

Determine the oxidation number of chromium in CrO42-.

a)

5

b)

6

c)

4

d)

2

56.

What is the oxidation number of iodine in KIO3?

a)

5

b)

1

c)

0

d)

-1

57.

Find the oxidation number of S in S2O4 2-

a)

+3

b)

+6

c)

-6

d)

-3

e)

-4

58.

Determine the oxidation number of chromium in CrO42-.

a)

5

b)

6

c)

4

d)

2

59.

What is the oxidation number of: Br2?

a)

-1

b)

+1

c)

-2

d)

0

60.

What is the oxidation number of Sr+2?

a)

-2

b)

0

c)

+2

d)

+1

61.

Which of the following would be considered oxidized in the following reaction:
2 Li + ZnCl2→ 2 LiCl + Zn2\ Li\ +\ ZnCl_{2_{ }}\rightarrow\ 2\ LiCl\ +\ Zn   

a)

Li

b)

Zn

c)

Cl

d)

None of the elements were oxidized

62.

What is the oxidation number on the nitrogen in NO2-?

a)

-1

b)

+3

c)

-3

d)

+4

63.

What is the oxidation number on the nitrogen in Mg3N2?

a)

0

b)

-2

c)

-3

d)

+3

64.

What is the oxidation number on the nitrogen in NO?

a)

0

b)

-1

c)

-2

d)

+2

65.

Identify the species oxidized in the following reaction.


2 Al(s) + 3 Cu2+(aq) → 2 Al3+(aq) + 3 Cu(s)

a)

Al

b)

Al3+

c)

Cu

d)

Cu2+

66.

Identify which reactant is oxidized and which is reduced in the following reaction.

2Al(s) + 3Cu2+(aq) →2Al3+(aq) + 3Cu(s)

a)

Al is oxidized and Cu2+ is reduced.

b)

Cu2+ is oxidized and Al is reduced.

c)

Both Al and Cu2+ are oxidized.

d)

Both Al and Cu2+ are reduced.

67.

Identify which reactant is oxidized and which is reduced in the following reaction.

2Cr3+(aq) + 3Zn(s) →2Cr(s) + Zn2+(aq)

a)

Cr3+ is oxidized and Zn is reduced.

b)

Cr3+ is reduced and Zn is oxidized.

c)

Both Cr3+ and Zn are oxidized.

d)

Both Cr3+ and Zn are reduced.

68.

Identify which reactant is oxidized and which is reduced in the following reaction.

2Au3+(aq) + 3Cd(s) →2Au(s) + 3Cd2+(aq)

a)

Au3+ is oxidized and Cd is reduced.

b)

Au3+ is reduced and Cd is oxidized

c)

Both Au3+ and Cd are reduced.

d)

Both Au3+ and Cd are oxidzed.

69.

What is the oxidizing agent when iron rusts? The oxidizing agent gains electrons.

2Fe(s) + O2(g) →FeO(s)

0 0 +2 -2

a)

Fe is the oxidizing agent

b)

O is the oxidizing agent

70.

What is the reducing agent when iron rusts? The reducing agent loses electrons.

2Fe(s) + O2(g) →FeO(s)

0 0 +2 -2

a)

Fe is the reducing agent.

b)

O is the reducing agent.

71.

The redox equation 4H+ + N2 --> NH4+ + N is

a)

correctly balanced

b)

correctly balanced for number of atoms but not for charge

c)

correctly balanced for charge but not for atoms

d)

not balanced for number of atoms or charge

72.

The redox equation is MnO4-1 + 4 CO2 + 4 H+ --> 4 CO3+ + Mn2+ + 4 H2O is

a)

correctly balanced

b)

correctly balanced for atoms but not for charge

c)

correctly balanced for charge but not for atoms

d)

not balanced for atoms or for charge

73.

The redox equation Cu2+ + 2 Fe --> Cu + 2 Fe2+ is

a)

correctly balanced

b)

correctly balanced for atoms but not for charge

c)

correctly balanced for charge but not for atoms

d)

not balanced for atoms or for charge

74.

The redox equation H2 + O2 --> 2 H+ + O2- is

a)

correctly balanced

b)

correctly balanced for atoms but not for charge

c)

correctly balanced for charge but not for atoms

d)

not balanced for atoms or for charge

75.

The redox equation H2 + S + 2 O2 --> 2 H+ + SO42- is

a)

correctly balanced

b)

correctly balanced for atoms but not for charge

c)

correctly balanced for charge but not for atoms

d)

not correctly balanced for atoms or for charge

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