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Review REDOX Quiz

Total questions: 50

Worksheet time: 37mins

Name
Class
Date
1.

Which particles are transferred during a redox reaction?

a)

atoms

b)

electrons

c)

neutrons

d)

positrons

2.

Which particles are transferred during a redox reaction?

a)

atoms

b)

electrons

c)

neutrons

d)

positrons

3.

Given the equation representing a reaction: 2Ca(s) + O2(g) → 2CaO(s), during this reaction, each element changes in

a)

atomic number

b)

oxidation number

c)

number of protons per atom

d)

number of neutrons per atom

4.

Given the equation representing a reaction:

3CuCl2(aq) + 2Al(s) → 3Cu(s) + 2AlCl3(aq)

the oxidation number of copper changes from

a)

+1 to 0

b)

+2 to 0

c)

+2 to +1

d)

+6 to +3

5.

What are the two oxidation states of nitrogen in NH4NO2?

a)

+3 and +5

b)

+3 and -5

c)

-3 and +3

d)

-3 and -3

6.

Given the balanced equation representing a reaction:

Ni(s) + 2HCl(aq) → NiCl2(aq) + H2(g)

in this reaction, each Ni atom

a)

loses 1 electron

b)

loses 2 electrons

c)

gains 1 electron

d)

gains 2 electrons

7.

Which process involves the transfer of electrons?

a)

double replacement

b)

neutralization

c)

oxidation-reduction

d)

sublimation

8.

Which balanced equation represents a redox reaction?

a)

Mg + Cl₂ → MgCl₂

b)

CaO + H₂O → Ca(OH)₂

c)

HNO₃ + NaOH → NaNO₃ + H₂O

d)

NaCl + AgNO₃ → AgCl + NaNO₃

9.

What is the oxidation number of manganese in KMnO₄?

a)

+7

b)

+2

c)

+3

d)

+4

10.

What is the oxidation number of iodine in KIO₄?

a)

+1

b)

-1

c)

+7

d)

-7

11.

Given the balanced equation representing a reaction:

2KClO₃(s) → 2KCl(s) + 3O₂(g)

the oxidation state of chlorine in this reaction changes from

a)

-1 to +1

b)

-1 to +5

c)

+1 to -1

d)

+5 to -1

12.

A substance that oxidizes another substance by accepting its electrons is called an ____.

a)

reducing agent

b)

oxidation number

c)

oxidizing agent

13.

What is the reducing agent here: N2 + 3H2 --> 2NH3

a)

N2

b)

H2

c)

NH3

d)

2NH3

14.

An increase in oxidation number is caused by ____.

a)

evaporation

b)

gaining electrons

c)

losing electrons

15.

An increase in oxidation number is caused by ____.

a)

evaporation

b)

gaining electrons

c)

losing electrons

16.

Oxidation-reduction reactions occur because of the competition between particles for...

a)

protons

b)

neutrons

c)

electrons

d)

positrons

17.

Which equation represents a reduction half-reaction?

a)

Fe → Fe3+ + 3e-

b)

Fe + 3e- → Fe3+

c)

Fe3+ → Fe + 3e-

d)

Fe3+ + 3e- → Fe

18.

Which half-reaction equation represents reduction?

a)

Cu → Cu2+ + 2e-

b)

Cu2+ + 2e- → Cu

c)

Ag + e- → Ag+

d)

Ag+ → Ag + e-

19.

Given the equation representing a reaction:

Cd + NiO2 + 2H2O → Cd(OH)2 + Ni(OH)2

Which half-reaction equation represents the oxidation in the reaction?

a)

Ni4+ + 2e- → Ni2+

b)

Ni4+ → Ni2+ + 2e-

c)

Cd → Cd2+ +2e-

d)

Cd + 2e- → Cd2+

20.

Given the balanced ionic equation:

Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)

which equation represents the oxidation half-reaction?

a)

Zn(s) + 2e⁻ → Zn²⁺(aq)

b)

Zn(s) → Zn²⁺(aq) + 2e⁻

c)

Cu²⁺(aq) → Cu(s) + 2e⁻

d)

Cu²⁺(aq) + 2e⁻ → Cu(s)

21.

Given the reaction for the corrosion of aluminum:

4 Al + 3 O₂ → 2 Al₂O₃

which half-reaction correctly represents the oxidation that occurs?

a)

Al + 3e⁻ → Al³⁺

b)

Al → Al³⁺ + 3e⁻

c)

O₂ + 4e⁻ → 2 O²⁻

d)

O₂ → 2 O²⁻ + 4e⁻

22.

Which statement correctly describes a redox reaction?

a)

The oxidation half-reaction and the reduction half-reaction occur simultaneously.

b)

The oxidation half-reaction occurs before the reduction half-reaction.

c)

The oxidation half-reaction occurs after the reduction half-reaction.

d)

The oxidation half-reaction occurs spontaneously but the reduction half-reaction does not.

23.

Which statement correctly describes a redox reaction?

a)

The oxidation half-reaction and the reduction half-reaction occur simultaneously.

b)

The oxidation half-reaction occurs before the reduction half-reaction.

c)

The oxidation half-reaction occurs after the reduction half-reaction.

d)

The oxidation half-reaction occurs spontaneously but the reduction half-reaction does not.

24.

Given the reaction:

Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g)

which equation represents the correct oxidation half-reaction?

a)

Zn(s) → Zn²⁺ + 2e⁻

b)

2H⁺ + 2e⁻ → H₂(g)

c)

Zn²⁺ + 2e⁻ → Zn(s)

d)

2Cl⁻ → Cl₂(g) + 2e⁻

25.

Given the reaction:

Fe(s) + Sn4+(aq) → Fe2+(aq) + Sn2+(aq)

the oxidizing agent is

a)

Fe(s)

b)

Sn4+(aq)

c)

Fe2+(aq)

d)

Sn2+(aq)

26.

In the reaction:

Pb + 2Ag+ → Pb2+ + 2Ag

the reducing agent is

a)

Ag+

b)

Ag

c)

Pb

d)

Pb2+

27.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
28.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
29.
What is oxidation number of O in O2 ?
a)
0
b)
-2
c)
+1
d)
+2
30.
What is oxidation number of O in O2 ?
a)
0
b)
-2
c)
+1
d)
+2
31.
What is oxidation number of O in O2 ?
a)
0
b)
-2
c)
+1
d)
+2
32.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
33.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
34.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
35.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
36.
Which of these results in the formation of a precipitate?
a)
AgNO3(aq)  +  NaOH(aq)→
b)
BaNO3(aq)  +  CaCl2(aq)→
c)
NaNO3(aq)  +  KOH(aq)→
d)
More than one of these form precipitates
37.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
38.
Is calcium oxidized or reduced in the following reaction? 
2CaO--> 2Ca + O2
a)
Oxidized
b)
Reduced
39.
The following is what type of reaction:
NH3 + HCl  → NH4Cl
a)
Synthesis
b)
Decomposition
c)
Single Replacement Replacement
d)
Double Replacement Replacement
40.
The following is what type of reaction:
NH3 + HCl  → NH4Cl
a)
Synthesis
b)
Decomposition
c)
Single Replacement Replacement
d)
Double Replacement Replacement
41.
What type of chemical reaction is this?
Al(OH)3 → Al2O3  + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
42.
What coefficients are needed to correctly balance the equation?
_Bi   +   _O2   →  _Bi2O3
a)
3,2,3
b)
2,3,2
c)
4,3,2
d)
none of these
43.
Which of the following is an example of a synthesis reaction:
a)
2 H2O → 2 H2 + O2 
b)
2 Na + Cl2 → 2 NaCl
c)
CH4 + 2 O2 → 2 H2O + CO2
d)
2 HCl + Zn → ZnCl2 + H2
44.

When Mg(OH)2 reacts with H2SO4 what are the products?

a)

MgO and H2SO4

b)

MgSO4 and H2O

c)

MgSO4 and SO2

d)

Mg(OH)2 and H2SO4

e)

No reaction

45.

Given the equation representing a reaction:

Cd + NiO2 + 2H2O → Cd(OH)2 + Ni(OH)2

Which half-reaction equation represents the oxidation in the reaction?

a)

Ni4+ + 2e- → Ni2+

b)

Ni4+ → Ni2+ + 2e-

c)

Cd → Cd2+ +2e-

d)

Cd + 2e- → Cd2+

46.

Which half-reaction shows conservation of charge?

a)

Cu + e⁻ → Cu⁺

b)

Cu²⁺ + 2e⁻ → Cu

c)

Cu⁺ → Cu + e⁻

d)

Cu²⁺ → Cu + 2e⁻

47.

Given the reaction for the corrosion of aluminum:

4 Al + 3 O₂ → 2 Al₂O₃

which half-reaction correctly represents the oxidation that occurs?

a)

Al + 3e⁻ → Al³⁺

b)

Al → Al³⁺ + 3e⁻

c)

O₂ + 4e⁻ → 2 O²⁻

d)

O₂ → 2 O²⁻ + 4e⁻

48.

Given the reaction:

Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g)

which equation represents the correct oxidation half-reaction?

a)

Zn(s) → Zn²⁺ + 2e⁻

b)

2H⁺ + 2e⁻ → H₂(g)

c)

Zn²⁺ + 2e⁻ → Zn(s)

d)

2Cl⁻ → Cl₂(g) + 2e⁻

49.

Which equation is an example of an oxidation-reduction reaction?

a)

Ca²⁺ + SO₄²⁻ → CaSO₄

b)

H⁺ + OH⁻ → H₂O

c)

Cu + 2AgNO₃ → Cu(NO₃)₂ + 2Ag

d)

Pb(NO₃)₂ + 2NaI → 2NaNO₃ + PbI₂

50.

Given the reaction:

Fe(s) + Sn4+(aq) → Fe2+(aq) + Sn2+(aq)

the oxidizing agent is

a)

Fe(s)

b)

Sn4+(aq)

c)

Fe2+(aq)

d)

Sn2+(aq)

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