College Chemistry II PHS 1035 Practice Exam 4
Name___________________________________
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) Which of the following terms can be used to describe an electrochemical cell in which a
spontaneous chemical reaction generates an electric current?
I. an electrolytic cell
II. a galvanic cell
III. a voltaic cell
A) only I
B) only II
C) only III
D) II and III
1)
2) Which cell involves a nonspontaneous redox reaction?
A) concentration cell
B) electrolytic cell
C) fuel cell
D) galvanic cell
2)
3) During an electrochemical reaction, electrons move through the external circuit toward the
________ and positive ions in the cell move toward the ________.
A) anode, anode
B) anode, cathode
C) cathode, anode
D) cathode, cathode
3)
4) For a galvanic cell, the cathode has a ________ sign and is the site of ________.
A) negative, oxidation
B) negative, reduction
C) positive, oxidation
D) positive, reduction
4)
5) A salt bridge is used to
A) provide reactants in a fuel cell.
B) determine the direction of the cell reaction.
C) control whether the cell is electrolytic or galvanic.
D) allow the ion flow necessary for cell neutrality.
5)
6) In a galvanic cell, the half-reaction MnO4 -(aq) + 8 H+ (aq) + 5 eA) an oxidation half-reaction and occurs at the anode.
B) an oxidation half-reaction and occurs at the cathode.
C) a reduction half-reaction and occurs at the anode.
D) a reduction half-reaction and occurs at the cathode.
Mn2+ (aq) + 4 H2 O(l) is
6)
7) In a galvanic cell, the half-reaction H2 (g) + 2 OH-(aq) 2 H2 O(l) + 2 e- is
A) an oxidation half-reaction and occurs at the anode.
B) an oxidation half-reaction and occurs at the cathode.
C) a reduction half-reaction and occurs at the anode.
D) a reduction half-reaction and occurs at the cathode.
7)
8) What species is oxidized in the reaction: CuSO4 (aq) + Fe(s) FeSO4(aq) + Cu(s)?
A) CuSO4 (aq)
B) Fe (s)
C) FeSO4 (aq)
D) Cu (s)
8)
1
9) Given that Cl2 (g) + 2 e- 2 Cl- (aq) is the reduction half-reaction for the overall reaction
2 Ag(s) + Cl2 (g) 2 AgCl(s), what is the oxidation half reaction?
A) Ag(s) Ag+ (aq) + eB) Ag(s) + Cl- (aq) AgCl(s) + eC) Ag(s) + Cl2 (g) + e-
AgCl(s) + Cl- (aq)
D) 2 Cl- (aq)
9)
Cl2 (g) + 2 e-
10) What is the reduction half-reaction for the following overall cell reaction?
Ni2+ (aq) + 2 Ag(s) Ni(s) + 2 Ag+ (aq)
Ag+ (aq)
A) Ag(s) + eB) Ag+ (aq) + e- Ag(s)
2+
Ni(s)
C) Ni (aq) + 2 e
D) Ni2+ (aq) + e- Ni(s)
10)
11) The iron content of foods can be determined by dissolving them in acid (forming Fe3+ ), reducing
the iron(III) to iron(II), and titrating with cerium(IV):
Fe2+ (aq) + Ce4+ (aq) Fe3+ (aq) + Ce3+ (aq).
Identify the two half-reactions in the above reaction.
11)
oxidation half-reaction
A) Fe2+ (aq) + e- Fe3+ (aq)
B) Fe2+ (aq) Fe3+ (aq) + eC) Ce4+ (aq) + e- Ce3+ (aq)
D) Ce4+ (aq) Ce3+ (aq) + e-
reduction half-reaction
Ce4+ (aq) Ce3+ (aq) + eCe4+ (aq) + e- Ce3+ (aq)
Fe2+ (aq) Fe3+ (aq) + eFe2+ (aq) + e- Fe3+ (aq)
12) For a galvanic cell that uses the following two half-reactions,
Cr2 O7 2- (aq) + 14 H+ (aq) + 6 e- 2 Cr3+ (aq) + 7 H2 O(l)
Pb(s) Pb2+ (aq) + 2 ehow many moles of Pb(s) are oxidized by one mole of Cr2 O7 2-?
12)
13) A galvanic cell employs the reaction
Mg2+ (aq) + Cu(s)
13)
A) 1
B) 2
C) 3
D) 6
Mg(s) + Cu2+ (aq)
and NaNO3 is the salt used in the salt bridge. During the course of the reaction
A) Na+ leaves the salt bridge and enters the anode compartment.
B) NaNO3 leaves the salt bridge and enters the anode compartment.
C) Na+ leaves the salt bridge and enters the cathode compartment.
D) NaNO3 leaves the salt bridge and enters the cathode compartment.
14) What is the shorthand notation that represents the following galvanic cell reaction?
Fe(s) + Cu(NO3 )2 (aq) Fe(NO3 )2 (aq) + Cu(s)
A) Fe(s) Fe2+ (aq) Cu2+ (aq) Cu(s)
B) Cu(s) Cu2+ (aq) Fe2+ (aq) Fe(s)
C) Fe(s) NO3 - (aq) NO3 - (aq) Cu(s)
D) Cu(s) Cu(NO3 )2 (aq) Fe(NO3 )2 (aq) Fe(s)
2
14)
15) What is the shorthand notation that represents the following galvanic cell reaction?
2 Fe2+ (aq) + Cl2 (g) 2 Fe3+ (aq) + 2 Cl-(aq)
A) Fe2+ (aq) Fe3+ (aq) Cl2 (g) Cl-(aq)
15)
16) For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs
at the cathode?
Zn(s) Zn2+ (aq) Ni2+ (aq) Ni(s)
A) Zn(s) Zn2+ (aq) + 2 eB) Zn2+ (aq) + 2 e- Zn(s)
2+
C) Ni(s) Ni (aq) + 2 e
D) Ni2+ (aq) + 2 e- Ni(s)
16)
17) For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs
at the anode?
Mg(s) Mg2+ (aq) Cd2+ (aq) Cd(s)
A) Mg(s) Mg2+ (aq) + 2 eB) Mg2+ (aq) + 2 e- Mg(s)
17)
B) Fe(s) Fe2+ (aq) Fe3+ (aq) Cl2 (g) Cl- (aq) C(s)
C) Pt(s) Fe3+(aq), Fe2+ (aq), Cl2 (g) Cl- (aq) C(s)
D) Pt(s) Fe2+(aq), Fe3+ (aq) Cl2 (g) Cl-(aq) C(s)
C) Cd(s)
Cd2+ (aq) + 2 e-
D) Cd2+ (aq) + 2 e-
Cd(s)
18) What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand
notation below?
Al(s) Al3+ (aq) Ni2+ (aq) Ni(s)
2+
3+
A) 2 Al(s) + 3 Ni (aq) 2 Al (aq) + 3 Ni(s)
B) 3 Al(s) + 2 Ni2+ (aq) 3 Al3+ (aq) + 2 Ni(s)
C) 2 Ni(s) + 3 Al3+ (aq) 2 Ni2+ (aq) + 3 Al(s)
D) 3 Ni(s) + 2 Al3+ (aq) 3 Ni2+ (aq) + 2 Al(s)
18)
19) What is the balanced equation for the galvanic cell reaction expressed using shorthand notation
below?
Mg(s) Mg2+ (aq) Cl2 (g) Cl-(aq) C(s)
A) Mg(s) + 2 Cl- (aq) Mg2+ (aq) + Cl2 (g)
B) Mg(s) + Cl2 (g) Mg2+ (aq) + 2 Cl-(aq)
19)
C) Mg2+ (aq) + 2 Cl- (aq)
D) Mg2+ (aq) + 2 Cl- (aq)
Mg(s) + Cl2 (g)
MgCl2 (s)
20) For the galvanic cell Pt(s) Sn2+ (aq), Sn4+ (aq) Pb2+ (aq) Pb(s), what is the function of the Pt(s)?
A) Pt is the anode and is a reactant in the overall cell reaction.
B) Pt is the anode and does not appear in the overall cell reaction.
C) Pt is the cathode and is a product in the overall cell reaction.
D) Pt is the cathode and does not appear in the overall cell reaction.
20)
21) Write the overall cell reaction for the galvanic cell given below.
Pt(s) H2 (g) H+ (aq) Cl2 (g) Cl- (aq) Pt(s)
A) Pt(s) + H2 (g) + Cl- (aq) Pt(s) + 2 H+ (aq) + 2 Cl2 (g)
21)
B) 2 H+ (aq) + 2 Cl2 (g)
2 HCl(aq)
C) H2 (g) + Cl2 (g) 2 H+ (aq) + 2 Cl- (aq)
D) No reaction would occur because there is no salt bridge.
3
22) What is the relation between joules (J), volts (V), and coulombs (C)?
A) 1 J = 1 V × 1 C
B) 1 J = 1 V ÷ 1 C
C) 1 J = 1 C ÷ 1 V
D) 1 J = 1 V × 1 C2
22)
23) In the relationship G = – nFE°, what is the value of n for the reaction shown below?
3 Cu2+(aq) + 2 Al(s) 3 Cu(s) + 2 Al3+ (aq)
23)
24) The cell reaction for a dry cell battery is
Zn(s) + 2 MnO2 (s) + 2 NH4 + (aq) 2 NH3 (aq) + Mn2 O3 (s) + Zn2+ (aq) + H2 O(l).
The standard cell potential for this cell is 1.56 V. What is the standard free energy change for this
cell?
A) +151 kJ
B) -151 kJ
C) -301 kJ
D) -602 kJ
24)
25) For the reaction 2 Al(s) + 3 Co2+ (aq) 2 Al3+ (aq) + 3 Co(s), G° is -799 kJ. What is E° for a standard
cell based on this reaction?
A) +1.38 V
B) +2.76 V
C) +4.14 V
D) +8.28 V
25)
26) The nickel-cadmium battery cell has a standard potential of +1.20 V. The cell reaction is
2 NiO(OH)(s) + Cd(s) + 2 H2O(l) 2 Ni(OH)2 (s) + Cd(OH)2 (s).
What is the standard free energy change for this reaction?
A) -38.7 kJ
B) -116 kJ
C) -232 kJ
D) -463 kJ
26)
27) Doubling all the coefficients in the equation for the cell reaction
A) doubles both E° and G°.
B) doubles E°, but does not change G°.
C) doubles G°, but does not change E°.
D) does not change E° or G°.
27)
28) What is the relation between G° and E° for the cell reaction below?
Ni2+ (aq) + Cd(s) Cd2+(aq) + Ni(s)
A) G° = F E°
B) G° = 2 F E°
C) G° = -F E°
28)
A) 1
B) 2
C) 3
D) 6
D) G° = -2 F E°
29) Which is not true for standard electrode potentials?
A) Cell constituents are in their standard states.
B) E° for oxidation is the negative of E° for reduction.
C) The half-reactions are written as reductions.
D) The potential for the standard hydrogen electrode is chosen to be +1.00 V.
29)
30) What is the relationship between the standard cell potentials, E°, for the following two galvanic cell
reactions?
I. 3 Cu2+(aq) + 2 Al(s) 3 Cu(s) + 2 Al3+ (aq)
30)
II. 6 Cu2+(aq) + 4 Al(s)
A) E°(I) = E°(II)
B) E°(I) =
6 Cu(s) + 4 Al3+ (aq)
1
E°(II)
2
C) E°(I) = 2E°(II)
4
D) E°(I) = E°(II)2
31) What is the relationship between the standard cell potentials, E°, for the following two galvanic cell
reactions?
I. 2 Ag+ (aq) + Sn2+ (aq) Sn4+ (aq) + 2 Ag(s)
II. Ag(s) + 1/2 Sn4+ (aq) 1/2 Sn2+ (aq) + Ag+(aq)
A) E°(I) = E°(II)
B) E°(I) = 2E°(II)
C) E°(I) = – E°(II)
D) E°(I) = – 2E°(II)
31)
32) What is the standard cell potential for the reaction below?
Mg(s) + Br2 (l) Mg2+ (aq) + 2 Br- (aq)
The standard reduction potential is -2.37 V for the Mg2+ /Mg half-cell and +1.09 V for the Br2 /Br-
32)
half-cell.
A) -3.46 V
B) -1.28 V
C) +1.28 V
D) +3.46 V
33) The standard potential for the following galvanic cell is +0.90 V:
3 Cu2+ (aq) + 2 Ga(s) 3 Cu(s) + 2 Ga3+ (aq)
Given that the standard reduction potential for the Cu2+ /Cu half-cell is +0.34 V, what is the
standard reduction potential for the Ga3+ /Ga half-cell?
A) -1.34 V
B) -0.56 V
C) +0.56 V
D) +1.36 V
33)
34) A galvanic cell consists of a La3+ /La half-cell and a standard hydrogen electrode. If the La3+ /La
half-cell standard cell functions as the anode, and the standard cell potential is 2.52 V, what is the
standard reduction potential for the La3+ /La half-cell?
A) -2.52 V
B) -0.84 V
C) +0.84 V
D) +2.52 V
34)
35) A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that
contains Cu(s) and Cu2+ (aq). What species are produced at the electrodes under standard
35)
36) Consider the following standard reduction potentials,
Al3+ (aq) + 3 e- Al(s)
E° = -1.66 V
I2 (s) + 2 e- 2 I- (aq)
E° = +0.54 V
Under standard conditions,
A) Al3+ (aq) is a stronger oxidizing agent than I2 (s), and I- (aq) is a stronger reducing agent than
Al(s).
B) I2(s) is a stronger oxidizing agent than Al3+ (aq), and Al(s) is a stronger reducing agent than
I-(aq).
C) Al(s) is a stronger oxidizing agent than I- (aq), and Al3+ (aq) is a stronger reducing agent than
I2(s).
D) I-(aq) is a stronger oxidizing agent than Al(s), and I2(s) is a stronger reducing agent than
36)
conditions?
Ag+ (aq) + e- Ag(s)
E° = +0.80 V
Cu2+ (aq) + 2 e- Cu(s)
E° = +0.34 V
A) Ag(s) is formed at the cathode, and Cu(s) is formed at the anode.
B) Ag(s) is formed at the cathode, and Cu 2+ (aq) is formed at the anode.
C) Cu(s) is formed at the cathode, and Ag+ (aq) is formed at the anode.
D) Cu2+ (aq) is formed at the cathode, and Cu(s) is formed at the anode.
Al3+ (aq).
5
37) Based on the following information,
F2 (g) + 2 e- 2 F- (aq)
E° = +2.87 V
Mg2+ (aq) + 2 e- 2 Mg(s)
E° = -2.37 V
which of the following chemical species is the strongest reducing agent?
A) F2 (g)
B) Mg2+ (aq)
C) F- (aq)
37)
D) Mg(s)
38) Using the following standard reduction potentials
Fe3+ (aq) + e- Fe2+ (aq)
E° = +0.77 V
2+
Pb (aq) + 2 e
Pb(s)
E° = -0.13 V
calculate the standard cell potential for the galvanic cell reaction given below, and determine
whether or not this reaction is spontaneous under standard conditions.
Pb2+ (aq) + 2 Fe2+ (aq) 2 Fe3+ (aq) + Pb(s)
A) E° = -0.90 V, nonspontaneous
B) E° = -0.90 V, spontaneous
C) E° = +0.90 V, nonspontaneous
D) E° = +0.90 V, spontaneous
38)
E° = +0.799 V
39) Given: Ag+ (aq) + e- Ag(s)
AgI(s) + e- Ag(s) + I- (aq) E° = -0.152 V
Ni2+ (aq) + 2 e- Ni(s)
E° = -0.267 V
Which of the following reactions should be spontaneous under standard conditions?
I. 2 AgI(s) + Ni(s) 2 Ag(s) + 2 I- (aq) + Ni2+ (aq)
II. Ag+(aq) + I- (aq) AgI(s)
A) I and II are both nonspontaneous.
B) I is nonspontaneous and II is spontaneous.
C) I is spontaneous and II is nonspontaneous.
D) I and II are both spontaneous.
39)
6
40) According to Table 17.1, which aqueous metal ion will reduce Ag+ , but not Cu2+?
A) Fe2+
B) Fe3+
C) Mn2+
D) Sn2+
40)
41) According to Table 17.1, which will reduce water but not Mg2+?
A) Al3+ (aq)
B) Al(s)
C) Na+ (aq)
41)
D) Na(s)
42) Using Table 17.1, find E° for 2 H2 O(l) 2 H2 (g) + O2 (g).
A) -2.06 V
B) -1.23 V
C) -0.80 V
D) -0.40 V
43) Use Table 17.1 to calculate the standard potential for the reaction
O2 (g) + 4 H+ (aq) + 2 Cu(s) 2 Cu2+ (aq) + 2 H2 O(l).
A) -1.57 V
B) -0.89 V
C) +0.89 V
42)
43)
D) +1.57 V
44) Use Table 17.1 to determine which of the following is the best oxidizing agent.
A) Fe3+
B) I2
C) MnO4 D) Pb2+
7
44)
45) Consider the following table of standard half-cell potentials:
A2 + 2 e– 2 A–
E° = + 1.09 V
B4+ + 2 e–
C3+ + 3 e–
B2+
45)
E° = + 0.15 V
C
E° = – 1.66 V
D2+ + 2 e– D
E° = – 2.37 V
Which substance is the strongest oxidizing agent?
A) A2
B) B4+
C) C3+
D) D2+
46) Consider the galvanic cell, Pb(s) Pb2+ (aq) Cu2+ (aq) Cu(s). Which one of the following changes
to the cell would cause the cell potential to increase (i.e., become more positive)?
A) increase the [Pb2+ ] concentration
B) increase the [Cu2+ ] concentration
C) increase the mass of Pb(s)
D) decrease the mass of Pb(s)
46)
47) Consider the galvanic cell, Pt(s) H2(1 atm)|H+ (1 M) Cl– (1 M) Hg2 Cl2 (s)|Hg(l).
Which one of the following changes to the cell would cause the cell potential to increase (i.e.,
become more positive)?
A) decrease the mass of Pt
B) increase the mass of Pt
C) decrease the pH
D) increase the pH
47)
48) Calculate the value of the reaction quotient, Q, for the galvanic cell expressed using shorthand
notation below.Use the balanced chemical equation that has the smallest, whole number
stoichiometric coefficients.
Zn(s) Zn2+ (aq, 0.0100 M) Ag+(aq, 1.25 M) Ag(s)
A) 156
B) 125
C) 8.00 × 10-3
D) 6.40 × 10-3
48)
49) Calculate the cell potential at 25°C for the cell
Fe(s) (Fe2+ (0.100 M) Pd2+ (1.0 × 10-5 M) Pd(s)
given that the standard reduction potential for Fe2+ /Fe is -0.45 V and for Pd2+ /Pd is +0.95 V.
A) +1.16 V
B) +1.28 V
C) +1.52 V
D) +1.68 V
49)
50) Calculate the cell potential E at 25°C for the reaction
2 Al(s) + 3 Fe2+ (aq) 2 Al3+ (aq) + 3 Fe(s)
given that [Fe2+ ] = 0.020 M, [Al3+ ] = 0.10 M, and the standard reduction potential is -1.66 V for
Al3+ /Al and -0.45 V for Fe2+ /Fe.
A) +1.03 V
B) +1.17 V
C) +1.18 V
D) +1.20 V
50)
51) At 25°C, E° = +1.88 V for a cell based on the reaction
3 AgCl(s) + Al(s) 3 Ag(s) + Al3+ (aq) + 3 Cl- (aq).
Find the cell potential E if [Al3+ ] = 0.20 M and [Cl- ] = 0.010 M.
A) +2.01 V
B) +2.04 V
C) +2.28 V
D) cannot be calculated without the amounts of AgCl, Al, and Ag
51)
52) Given that E° = +0.897 V, calculate E at 25°C for
Pb(s) Pb2+ (0.0400 M) Fe3+ (0.200 M), Fe2+ (0.0100 M) Pt(s)
A) +0.779 V
B) +0.935 V
C) +1.015 V
52)
8
D) +1.134 V
53) Given that E°red = -0.26 V for Ni2+ /Ni at 25°C, find E° and E for the concentration cell expressed
using shorthand notation below.
Ni(s) Ni2+ (aq, 1.0 × 10-5 M) Ni2+ (aq, 0.100 M) Ni(s)
A) E° = 0.00 V and E = +0.24 V
B) E° = 0.00 V and E = +0.12 V
C) E° = -0.26 V and E = -0.02 V
D) E° = -0.26 V and E = -0.14 V
53)
54) Given p H2 = 0.100 atm, [Cd2+ ] = 0.200 M, and [H+ ] = 1.00 × 10-5 M, calculate E at 25°C for a cell
54)
based on the reaction:
Cd(s) + 2 H+ (aq)
A) -0.09 V
H2 (g) + Cd2+ (aq) E° = +0.40 V.
B) +0.12 V
C) +0.15 V
D) +0.30 V
55) If the cell reaction involves ions in solution, as the cell reaction in a galvanic cell continues,
A) E for the cell increases.
B) E for the cell decreases.
C) E° for the cell increases.
D) E° for the cell decreases.
55)
56) How many moles of electrons, n, are transferred in the following reduction-oxidation reaction?
2 MnO4 - (aq) + 16 H+ (aq) + 10 Cl- (aq) 2 Mn2+ (aq) + 5 Cl2 (g) + 8 H2 O(l)?
A) 2
B) 4
C) 5
D) 10
56)
57) Consider the half-reaction: MnO4 -(aq) + 8 H+ (aq) + 5 e- Mn2+ (aq) + 4 H2 O(l). The formation of
MnO4 - from Mn2+ occurs most readily when the solution is
57)
58) Which is most often used in the laboratory to measure pH?
A) a standard hydrogen electrode
B) a glass electrode
C) a Daniell cell
D) a conductivity cell
58)
59) The following cell has a potential of 0.45 V at 25°C.
Pt(s) H2 (1 atm)|H+ (? M) Cl– (1 M) Hg2 Cl2 (s)|Hg(l)
The standard half-cell potential for the half-reaction Hg2 Cl2 (s) + 2 e– 2 Hg(l) + 2 Cl– (aq) is 0.28
59)
A) acidic.
C) basic.
B) neutral.
D) The reaction is not dependent upon pH.
V. What is the pH in the anode compartment?
A) 2.9
B) 4.7
C) 7.6
D) 12.3
60) A cell based on the reaction below has a standard potential of +0.42 V at 25°C. If all of the species
are at standard conditions except [H+ ], at what pH will the cell have a potential of zero?
H2 O2 (aq) + 2 H+ (aq) + 2 Cl- (aq) Cl2 (aq) + 2 H2 O(l)
A) 3.55
B) 7.09
C) 10.6
D) 14.2
60)
61) Consider a cell based on the following reaction:
GeO(s) + H2 O(l) + 2 Ag+ (aq) GeO2 (s) + 2 H+ (aq) + 2 Ag(s)
If [Ag+ ] = 1 M, at 25°C,
A) pH = 2(E° - E)/0.0592 V.
B) pH = (E° - E)/0.0592 V.
C) pH = (E - E°)/0.0592 V.
D) pH = 2(E - E°)/0.0592 V.
61)
9
62) Consider the following cell:
Pt(s) H2 (g, p1 ) H+ (aq, pHA) H+ (aq, pHC) H2 (g, p2 ) Pt(s)
Where pHA is the pH of the aqueous solution in the anode half-cell and pHC is the pH of the
aqueous solution in the cathode half-cell. If the partial pressure of H2 (g) is the same for both
half-cells, (p1 = p2 ), then E for the cell at 25°C is
A) 0.0296 V log (pHA/pHC).
B) 0.0296 V log (pHC/pHA).
C) 0.0592 V (pHA - pHC).
D) 0.0592 V (pHC - pHA).
62)
63) When a cell reaction reaches equilibrium,
A) E° = 0.
C) both E° and E = 0.
63)
B) E = 0.
D) neither E° nor E = 0.
64) The equilibrium constant, K, can be calculated from
A) E°.
C) either E° or E.
64)
B) E.
D) neither E° nor E.
65) Calculate the equilibrium constant, K, at 25°C for the galvanic cell reaction shown below:
8 H+(aq) + 5 Fe2+ (aq) + MnO4 - (aq) Mn2+ (aq) + 5 Fe3+ (aq) + 4 H2 O(l) E° = +0.74 V
A) 3.2 × 10-63
B) 3.2 × 10-13
C) 3.2 × 1012
D) 3.2 × 1062
66)
Ag+ (aq) + e- Ag(s)
E° = +0.800 V
AgBr(s) + e- Ag(s) + Br- (aq)
E° = +0.071 V
Br2 (l) + 2 e- 2 Br- (aq)
E° = +1.066 V
Use some of the data above to calculate Ksp at 25°C for AgBr.
A) 6.3 × 10-2
B) 4.9 × 10-13
C) 1.9 × 10-15
65)
66)
D) 2.4 × 10-34
67) For a particular cell based on the reaction:
3 AgCl(s) + Al(s) 3 Ag(s) + Al3+ (aq) + 3 Cl- (aq)
E = +1.750 V and E° = +1.884 V at 25°C. What is the value of the equilibrium constant, K, at 25°C for
the reaction?
A) 3.6 × 1029
B) 6.7 × 1031
C) 4.8 × 1088
D) 3.0 × 1095
67)
68) A particular 12V battery is based on a reaction having a standard cell potential, E° = +1.92 V. What
happens when the battery "dies" ?
A) E° = 0 V and E = 0 V
B) E° = 0 V and E = 12 V
C) E° = +1.92 V and E = 0 V
D) E° = +1.92 V and E = 12 V
68)
69) For a particular battery based on one of the following reactions, E is expected to remain constant
with time until the cell reactants are almost completely consumed. Which is the appropriate
reaction?
A) Zn(s) + 2 MnO2 (s) + 2 NH4 + (aq) 2 NH3 (aq) + Mn2 O3 (s) + Zn2+ (aq) + H2 O(l)
B) 2 NiO(OH)(s) + Cd(s) + 2 H2O(l) 2 Ni(OH)2 (s) + Cd(OH)2 (s)
C) Pb(s) + PbO2 (s) + 2 H+ (aq) + 2 HSO4 -(aq) 2 PbSO4(s) + 2 H2 O(l)
69)
D) Zn(s) + Cu2+ (aq)
Zn2+ (aq) + Cu(s)
10
70) The cell reaction for a lead storage battery is:
Pb(s) + PbO2 (s) + 2 H+ (aq) + 2 HSO4 -(aq)
70)
2 PbSO4 (s) + 2 H2 O(l)
E° = +1.92 V
To provide a potential of about 12 V, one could
A) adjust the pH to 12.
B) adjust the pH to 1.
C) connect six cells in series.
D) greatly increase the surface area of the Pb(s) and PbO2 (s).
71) Which battery does not use MnO2 (s) as a cell reactant?
A) an alkaline dry cell.
B) a Leclanche' dry cell.
C) a lithium battery.
D) a "ni-cad" battery.
71)
72) Which statement below is not true?
A) The cell reactants in a fuel cell are continuously supplied from an external source.
B) A fuel cell is a galvanic cell.
C) Modern fuel cells can be easily regenerated using household current.
D) One of the reactants in a fuel cell is a traditional fuel.
72)
73) Which of the following reactions is most suitable for a fuel cell?
A) MnO2 (s) + Li(s) LiMnO2 (s)
B) Pb(s) + PbO2 (s) + 2 H+ (aq) + HSO4 - (aq) PbSO4 (s) + 2 H2 O(l)
73)
74) Which of the following statements concerning a lithium battery is false?
A) A lithium battery is rechargeable.
B) A lithium battery has a relatively high voltage, due in part to the high oxidation potential of
lithium.
C) It takes a small mass of lithium to provide one mole of electrons in the cell reaction.
D) The cell reaction produces toxic mercury, so the batteries should be recycled.
74)
75) Shown below are the reactions occurring in the direct methanol fuel cell (DMFC).
I
2 CH3 OH(aq) + 2 H2 O(l) 2 CO2 (g) +12 H+ (aq) +12 e–
75)
C) HgO(l) + Zn(s) ZnO(s) + Hg(l)
D) 2 CO(g) + O2(g) 2 CO2 (g)
II
Overall
3 O2 (g) + 12 H+ (aq) + 12 e–
2 CH3 OH(aq) + 3 O2(g)
6 H2 O(l)
2 CO2 (g) + 4 H2 O(l)
Which is the anode reaction, and what is being oxidized in the overall reaction?
A) I, CH3 OH
B) I, H2 O
C) II, O2
D) II, H+
76) Shown below are the reactions occurring in the proton-exchange membrane (PEM) fuel cell.
I
2 H2 (g) 4 H+ (aq) + 4 e–
II
Overall
O2 (g) + 4 H+ (aq) + 4 e– 2 H2 O(l)
2 H2 (g) + O2 (g) 2 H2 O(l)
Which is the cathode reaction, and what is being oxidized in the overall reaction?
A) I, H2
B) I, O2
C) II, H2
D) II, O2
11
76)
77) Which of the following statements concerning the rusting of iron is false?
A) The oxidation site can occur at a different place on the metal surface than the reduction site.
B) The metal is reduced.
C) The rusting of iron requires both oxygen and water.
D) Salt increases the rate of corrosion by providing ions to carry the current.
77)
78) Galvanized steel is steel coated with a layer of
A) Fe2 O3 .
B) Mg.
78)
C) Sn.
79) What is least easily oxidized?
A) Al
B) Fe
C) Mg
D) Zn.
D) Zn
79)
80) Aluminum requires relatively little protection from corrosion because
A) aluminum has little tendency to react with oxygen.
B) the reduction potential for Al3+ /Al is very low.
C) the oxidation of aluminum produces a hard, relatively impenetrable film of Al2 O3 .
D) aluminum is protected by cathodic protection.
80)
81) A steel pipe can be protected from corrosion by attaching the pipe to a piece of magnesium because
A) magnesium forms a tight oxide coating.
B) magnesium is more easily oxidized than iron.
C) magnesium is inert.
D) magnesium and steel form a corrosion resistant alloy.
81)
82) An electrolytic cell is
A) a battery.
B) a cell in which the cell reaction is spontaneous.
C) a cell in which an electric current drives a nonspontaneous reaction.
D) a cell in which reactants are continuously supplied to the cell.
82)
83) For an electrolytic cell
A) E is negative and
B) E is negative and
C) E is positive and
D) E is positive and
83)
G is negative for the cell reaction.
G is positive for the cell reaction.
G is negative for the cell reaction.
G is positive for the cell reaction.
84) For a dead battery
A) E is negative and G is positive for the cell reaction.
B) E is negative and G is negative for the cell reaction.
C) E is zero and G is positive for the cell reaction.
D) E is zero and G is zero for the cell reaction.
84)
85) Which statement is true?
A) The cathode is positive for a galvanic cell and negative for an electrolytic cell.
B) Electrons flow through the external circuit to the cathode in a galvanic cell and to the anode in
an electrolytic cell.
C) Oxidation occurs at the anode in a galvanic cell and at the cathode in an electrolytic cell.
D) Oxidation occurs at the cathode in a galvanic cell and at the anode in an electrolytic cell.
85)
12
86) Which statement concerning overvoltage is false?
A) Overvoltage is the additional voltage above the calculated voltage required to bring about
electrolysis.
B) Overvoltage is often due to a high activation energy for the reaction at one electrode.
C) Overvoltage is small for half-reactions involving the formation of O2 (g) or H2 (g).
D) Overvoltage must be experimentally determined.
87)
O2 (g) + 4 H+ (aq) + 4 e- 2 H2 O(l)
I2 (s) + 2 e- 2 I- (aq)
2 H2 O(l) + 2 e- H2 (g) + 2 OH- (aq)
Mg2+ (aq) + 2 e-
Mg(s)
E° = +1.23 V
86)
87)
E° = +0.54 V
E° = -0.83 V
E° = -2.37 V
Based on the data above, electrolysis of an aqueous solution of MgI2 , with inert electrodes, is
expected to produce
A) Mg at the cathode and I2 at the anode.
B) H2 at the cathode and I2 at the anode.
C) Mg at the cathode and O2 at the anode.
D) H2 at the cathode and O2 at the anode.
88)
O2 (g) + 4 H+(aq) + 4 e- 2 H2 O(l)
Pb2+ (aq) + 2 e- Pb(s)
2 H2 O(l) + 2 e- H2 (g) + 2 OH- (aq)
E° = +1.23 V
88)
E° = -0.13 V
E° = -0.83 V
Based on the half-reactions above, electrolysis of an aqueous solution of Pb(NO3)2 is expected to
produce.
A) Pb at the cathode and H2 at the anode.
B) Pb at the cathode and O2 at the anode.
C) H2 at the cathode and Pb at the anode.
D) O2 at the cathode and Pb at the anode.
89) The chlor-alkali industry is based on the electrolysis of aqueous NaCl. What are the products of
this electrolysis?
A) Na and Cl2
B) NaOH, H2 , and O2
C) NaOH, H2 , and Cl2
D) NaOH, O2 , and Cl2
89)
90) The Hall-Heroult process for the production of aluminum involves the electrolysis of
A) an aqueous solution of Al(NO3 )3 .
B) molten Al2 O3 .
C) molten cryolite, Na3 AlF6 .
D) a molten mixture of Al2 O3 and Na3AlF6 .
90)
91) Which requires the most electricity (in terms of faradays of charge transferred) per gram of useful
product formed?
A) electrolysis of aqueous NaCl (chlor-alkali industry)
B) electrolysis of molten NaCl/CaCl2 in a Downs cell
C) electrorefining copper metal
D) production of aluminum in the Hall-Heroult process
91)
92) Which of the following statements concerning the electrorefining of copper in not true?
A) The anode is constructed of chalcocite, Cu2 S.
B) The anode mud is a valuable source of silver, gold, and platinum.
C) Copper is oxidized at the anode and copper(II) ions are reduced at the cathode.
D) The process is used to purify copper.
92)
13
93) The gas OF2 can be produced from the electrolysis of an aqueous solution of KF, as shown in the
equation below.
OF2 (g) + 2 H+ (aq) + 4 e- H2 O(l) + 2 F- (aq)
E° = +2.15 V
Using the given standard reduction potential, calculate the amount of OF2 that is produced, and
93)
the electrode at which the OF2 is produced, upon the passage of 0.240 faradays through an aqueous
KF solution.
A) 3.24 g of OF2 at the anode
C) 3.24 g of OF2 at the cathode
B) 13.0 g of OF2 at the anode
D) 13.0 g of OF2 at the cathode
94) How many grams of chromium metal are plated out when a constant current of 8.00 A is passed
through an aqueous solution containing Cr3+ ions for 40.0 minutes?
A) 3.45 g
B) 6.15 g
C) 10.3 g
D) 31.0 g
94)
95) How many grams of nickel metal are plated out when a constant current of 15.0 A is passed
through aqueous NiCl2 for 80.0 minutes?
A) 14.7 g
B) 21.9 g
C) 43.8 g
D) 48.4 g
95)
96) How long must a constant current of 50.0 A be passed through an electrolytic cell containing
aqueous Cu2+ ions to produce 3.00 moles of copper metal?
96)
97) Chromium can be electroplated from an aqueous solution containing sulfuric acid and chromic
acid, H2 CrO4 . What current is required to deposit chromium at a rate of 1.25 g/min?
A) 38.1 A
B) 38.7 A
C) 116 A
D) 232 A
97)
98) A constant current is passed through a solution containing Cu2+ (aq) resulting in the deposition of
4.40 g of Cu at the cathode. Assuming a current efficiency of 100%, if this same current is passed
through a solution of TcO4 – for the same amount of time, how many grams of Tc would form at the
98)
A) 0.311 hours
cathode?
A) 0.969 g
B) 0.621 hours
C) 1.61 hours
B) 1.94 g
C) 6.78 g
99) The bright colors of anodized aluminum are due to
A) electrodeposition of organic dyes on the aluminum surface.
B) the formation of an aluminum alloy with chromium and copper.
C) iridescence involving the semitransparent outer layer of Al2 O3 .
D) trapping of organic dye molecules in a spongy Al2 O3 matrix.
100) The bright colors of anodized titanium are due to
A) electrodeposition of organic dyes on the titanium surface.
B) the formation of a titanium alloy with chromium and copper.
C) iridescence involving the semitransparent outer layer of TiO2 .
D) trapping of organic dye molecules in a spongy TiO2 matrix.
14
D) 3.22 hours
D) 13.6 g
99)
100)
101) For the galvanic cell shown above, in what direction should the anions and cations in half-cell A
move?
A) The anions tend to move to the solid electrode and the cations into the salt bridge.
B) The anions tend to move into the salt bridge and the cations toward the solid electrode.
C) The anions tend to move toward the solid electrode and the cations should not move.
D) The cations tend to move toward the solid electrode and the anions should not move.
101)
102) The cell reaction 2 Fe3+ (aq) + Zn(s) Zn2+ (aq) + 2 Fe2+ (aq) occurs in the galvanic cell shown above.
Where should the Fe3+ (aq) and Fe2+ (aq) be found?
A) Half-cell (A) contains Fe3+ (aq) and half-cell (B) contains Fe2+ (aq).
B) Half-cell (A) contains Fe2+ (aq) and half-cell (B) contains Fe3+ (aq).
C) Half-cell (A) contains Fe3+ (aq) and Fe2+ (aq).
D) Half-cell (B) contains Fe3+ (aq) and Fe2+ (aq).
102)
103) The cell reaction 2 Fe3+ (aq) + Zn(s) Zn2+ (aq) + 2 Fe2+ (aq) occurs in the galvanic cell shown above.
Which would be the most appropriate choices for the solid electrode in half-cell (A) and in half-cell
(B)?
A) Fe(s) for half-cell (A) and Zn(s) for half-cell (B)
B) Pt(s) for half-cell (A) and Zn(s) for half-cell (B)
C) Fe(s) for half-cell (A) and Fe(s) for half-cell (B)
D) Zn(s) for half-cell (A) and Pt(s) for half-cell (B)
103)
15
Consider the galvanic cell shown below.
104) Identify the anode and cathode, and indicate the direction of Na+ ion and NO3 - ion flow from the
104)
salt bridge.
A) Al is the anode and Co is the cathode; Na+ ions flow into half-cell compartment (A) and
NO3 - ions flow into half-cell compartment (B).
B) Al is the anode and Co is the cathode; NO3 - ions flow into half-cell compartment (A) and
Na+ ions flow into half-cell compartment (B).
C) Co is the anode and Al is the cathode; Na+ ions flow into half-cell compartment (A) and
NO3 - ions flow into half-cell compartment (B).
D) Co is the anode and Al is the cathode; NO3 - ions flow into half-cell compartment (A) and
Na+ ions flow into half-cell compartment (B).
105) Identify the anode and cathode, and indicate the direction of ion flow to and from each electrode.
A) Al is the anode and Co is the cathode; Al3+ ions flow to the anode and Co2+ ions flow from
105)
the cathode.
B) Al is the anode and Co is the cathode; Co2+ ions flow to the cathode and Al3+ ions flow from
the anode.
C) Co is the anode and Al is the cathode; Al3+ ions flow to the cathode and Co2+ ions flow from
the anode.
D) Co is the anode and Al is the cathode; Co2+ ions flow to the anode and Al3+ ions flow from
the cathode.
106) What is the balanced equation for the cell reaction?
A) 2 Al(s) + 3 Co(s) 2 Al3+ (aq) + 3 Co2+ (aq)
C) 2 Al(s) + 3 Co2+ (aq)
B) 2 Al3+ (aq) + 3 Co2+ (aq) 2 Al(s) + 3 Co(s)
D) 2 Al3+ (aq) + 3 Co(s) 2 Al(s) + 3 Co2+ (aq)
2 Al3+ (aq) + 3 Co(s)
107) What is the shorthand notation for the cell?
A) Al(s) | Al3+ (aq) || Co(s) | Co2+ (aq)
B) Al(s) | Al3+ (aq) || Co2+ (aq) | Co(s)
D) Co(s) | Co2+ (aq) || Al3+ (aq)| Al(s)
C) Co(s) | Co2+ (aq) || Al(s) | Al3+ (aq)
16
106)
107)
Consider the following galvanic cell.
108) Identify the anode and cathode, and indicate the direction of Na+ ion and NO3 - ion flow from the
108)
salt bridge.
A) Fe is the anode and Sn is the cathode; Na+ ions flow into half-cell compartment (A) and
NO3 - ions flow into half-cell compartment (B).
B) Fe is the anode and Sn is the cathode; NO3 - ions flow into half-cell compartment (A) and
Na+ ions flow into half-cell compartment (B).
C) Sn is the anode and Fe is the cathode; Na+ ions flow into half-cell compartment (A) and
NO3 - ions flow into half-cell compartment (B).
D) Sn is the anode and Fe is the cathode; NO3 - ions flow into half-cell compartment (A) and
Na+ ions flow into half-cell compartment (B).
109) Identify the anode and cathode, and indicate the direction of ion flow to and from each electrode.
A) Fe is the anode and Sn is the cathode; Fe2+ ions flow to the anode and Sn2+ ions flow from
109)
the cathode.
B) Fe is the anode and Sn is the cathode; Sn2+ ions flow to the cathode and Fe2+ ions flow from
the anode.
C) Sn is the anode and Al is the cathode; Fe2+ ions flow to the cathode and Sn2+ ions flow from
the anode.
D) Sn is the anode and Al is the cathode; Sn2+ ions flow to the anode and Fe2+ ions flow from
the cathode.
110) What is the balanced equation for the cell reaction?
A) Fe(s) + Sn(s) Fe2+ (aq) + Sn2+ (aq)
C) Fe(s) + Sn2+ (aq)
B) Fe2+ (aq) + Sn2+ (aq) Fe(s) + Sn(s)
D) Fe2+ (aq) + Sn(s) Fe(s) + Sn2+ (aq)
Fe2+ (aq) + Sn(s)
111) What is the shorthand notation for the cell?
A) Fe(s) | Fe2+ (aq) || Sn(s) | Sn2+ (aq)
B) Fe(s) | Fe2+ (aq) || Sn2+ (aq) | Sn(s)
D) Sn(s) | Sn2+ (aq) || Fe2+ (aq) | Fe(s)
C) Sn(s) | Sn2+ (aq) || Fe(s) | Fe2+ (aq)
17
110)
111)
Shown below is a galvanic cell with anode compartment b containing anode a and cathode compartment d containing
cathode c. Electrons flow through wire f, ions flow through salt bridge e, and the cell potential is read using voltmeter g.
This galvanic cell uses the reaction: Cu(s) + 2 Ag+ (aq)
2 Ag(s) + Cu2+ (aq).
112) Identify the electrodes and the direction of electron flow.
A) a is Ag, c is Cu and electrons flow from a to c.
B) a is Ag, c is Cu and electrons flow from c to a.
C) a is Cu, c is Ag and electrons flow from a to c.
D) a is Cu, c is Ag and electrons flow from c to a.
112)
113) Identify and give the sign of each electrode.
A) a is Ag and (+), c is Cu and (-).
C) a is Cu and (+), c is Ag and (-).
113)
B) a is Ag and (-), c is Cu and (+).
D) a is Cu and (-), c is Ag and (+).
114) NaNO3 (aq) is employed in the salt bridge. Give the direction of electron flow and the direction of
ion flow from the salt bridge.
A) Electrons flow from a to c; Na+ flows into b and NO3 - flows into d.
B) Electrons flow from a to c; NO3 - flows into b and Na+ flows into d.
114)
C) Electrons flow from c to a; Na+ flows into b and NO3 - flows into d.
D) Electrons flow from c to a; NO3 - flows into b and Na+ flows into d.
115) Identify the anode and cathode half-reactions and categorize each as either oxidation or reduction.
A) Anode reaction: Ag+ (aq) + e- Ag(s) (oxidation)
Cathode reaction: Cu(s) Cu2+ (aq) + 2e- (reduction)
B) Anode reaction: Ag+ (aq) + e- Ag(s) (reduction)
Cathode reaction: Cu(s) Cu2+ (aq) + 2e- (oxidation)
C) Anode reaction: Cu(s) Cu2+ (aq) + 2e- (oxidation)
Cathode reaction: Ag+ (aq) + e- Ag(s) (reduction)
D) Anode reaction: Cu(s) Cu2+ (aq) + 2e- (reduction)
Cathode reaction: Ag+ (aq) + e- Ag(s) (oxidation)
115)
116) What is the shorthand notation for this cell?
A) Cu2+ (aq) Cu(s) Ag+ (aq) Ag(s)
C) Cu2+ (aq) Cu(s) Ag(s) Ag+ (aq)
116)
B) Cu(s) Cu2+(aq) Ag(s) Ag+ (aq)
D) Cu(s) Cu2+(aq) Ag+ (aq) Ag(s)
18
117) Given the half-cell potentials below, calculate the cell potential.
Ag+ (aq) + e- Ag(s)
Cu2+ (aq) + 2 e- Cu(s)
A) 0.46 V
117)
0.80 V
0.34 V
B) 1.14 V
C) 1.26 V
D) 1.94 V
118) If the concentrations of Ag+ (aq) and Cu2+ (aq) are varied in this galvanic cell, which of the following
four cells has the largest cell potential?
A) [Ag+ ] = 0.10 M and [Cu2+ ] = 0.10 M
B) [Ag+ ] = 1.0 M and [Cu2+ ] = 0.10 M
C) [Ag+ ] = 0.10 M and [Cu2+ ] = 1.0 M
D) [Ag+ ] = 1.0 M and [Cu2+ ] = 1.0 M
118)
119) The initial concentrations of Ag+(aq) and Cu2+ (aq) are both 1.0 M. What will happen to the cell
voltage if 5.0 M Cu(NO3 )2 is added to the compartment containing the 1.0 M Cu2+(aq)? The cell
voltage will
A) decrease.
B) increase.
C) remain the same.
D) can't tell from the information given
119)
120) The initial concentrations of Ag+(aq) and Cu2+ (aq) are both 1.0 M. What will happen to the cell
voltage if 1.0 M Cu(NO3 )2 is added to the compartment containing the 1.0 M Cu2+(aq)? The cell
voltage will
A) decrease.
B) increase.
C) remain the same.
D) can't tell from the information given
120)
121) The initial concentrations of Ag+(aq) and Cu2+ (aq) are both 1.0 M. What will happen to the cell
voltage if 5.0 M AgNO3 is added to the compartment containing the 1.0 M Ag+ (aq)? The cell
voltage will
A) decrease.
B) increase.
C) remain the same.
D) can't tell from the information given
121)
Consider the following galvanic cell.
122) What is the quantitative change in the cell voltage on increasing the ion concentration in the anode
compartment by a factor of 10?
A) +0.06 V
B) +0.03 V
C) -0.03 V
D) -0.06 V
19
122)
123) What is the quantitative change in the cell voltage on increasing the ion concentration in the
cathode compartment by a factor of 10?
A) +0.06 V
B) +0.03 V
C) -0.03 V
D) -0.06 V
123)
Consider the galvanic cell shown below.
124) What is the quantitative change in the cell voltage on increasing the ion concentration in the anode
compartment by a factor of 10?
A) +0.03 V
B) +0.02 V
C) -0.02 V
D) -0.03 V
124)
125) What is the quantitative change in the cell voltage on increasing the ion concentration in the
cathode compartment by a factor of 10?
A) +0.03 V
B) +0.02 V
C) -0.02 V
D) -0.03 V
125)
126) Is the cell shown above a galvanic or an electrolytic cell? Which is the anode and which is the
cathode?
A) Electolytic cell; electrode x is the anode and electrode y is the cathode.
B) Electolytic cell; electrode y is the anode and electrode x is the cathode.
C) Galvanic cell; electrode x is the anode and electrode y is the cathode.
D) Galvanic cell; electrode y is the anode and electrode x is the cathode.
126)
20
127) Is the cell shown above a galvanic or an electrolytic cell? What is the direction of ion flow?
A) Electolytic cell; Cu2+ ions flow toward electrode x and SO4 2- ions flow toward electrode y.
127)
B) Electolytic cell; Cu2+ ions flow toward electrode y and SO4 2- ions flow toward electrode x.
C) Galvanic cell; Cu2+ ions flow toward electrode x and SO4 2- ions flow toward electrode y.
D) Galvanic cell; Cu2+ ions flow toward electrode y and SO4 2- ions flow toward electrode x.
Shown below is an electrochemical cell with anode a and cathode c. Both the anode and the cathode are inert electrodes. The
liquid shown in compartment b of the cell is molten potassium chloride, KCl(l).
128) Determine whether this is a galvanic or an electrolytic cell and give the reaction occurring at the
anode and the reaction occurring at the cathode.
A) Electrolytic cell
B) Electrolytic cell
Anode reaction: K(s) K+ (l) + eAnode reaction: 2 Cl- (l) Cl2(g) + 2eCathode reaction: Cl2 (g) + 2e- 2 Cl- (l)
Cathode reaction: K+ (l) + e- K(s)
128)
129) Determine the direction of electron flow and the direction of ion flow.
A) Electrons flow from a to c; K+ ions flow toward a and Cl- ions flow toward c.
B) Electrons flow from a to c; Cl- ions flow toward a and K+ ions flow toward c.
C) Electrons flow from c to a; K+ ions flow toward a and Cl- ions flow toward c.
D) Electrons flow from c to a; Cl- ions flow toward a and K+ ions flow toward c.
129)
130) For a galvanic cell that uses the following two half-reactions,
Cr2 O7 2- (aq) + 14 H+ (aq) + 6 e- 2 Cr3+ (aq) + 7 H2 O(l)
Pb(s) Pb2+(aq) + 2 e-
130)
C) Galvanic cell
Anode reaction: K(s) K+ (l) + eCathode reaction: Cl2 (g) + 2e- 2 Cl- (l)
D) Galvanic cell
Anode reaction: K(s) K+ (l) + eCathode reaction: Cl2 (g) + 2e- 2 Cl- (l)
how many moles of Pb(s) are oxidized by three moles of Cr2 O7 2- ?
A) 3
B) 6
C) 9
131) What is the reduction half-reaction for the following overall cell reaction?
Co2+ (aq) + 2 Ag(s) Co(s) + 2 Ag+ (aq)
Ag+ (aq)
A) Ag(s) + eB) Ag+ (aq) + e- Ag(s)
C) Co2+ (aq) + 2 e- Co(s)
D) Co2+ (aq) + e- Co(s)
21
D) 18
131)
132) What is the shorthand notation that represents the following galvanic cell reaction?
Pb(s) + Cu(NO3 )2 (aq) Pb(NO3 )2 (aq) + Cu(s)
A) Pb(s) Pb2+ (aq) Cu2+ (aq) Cu(s)
B) Cu(s) Cu2+ (aq) Pb2+ (aq) Pb(s)
C) Pb(s) NO3 - (aq) NO3 - (aq) Cu(s)
132)
133) What is the shorthand notation that represents the following galvanic cell reaction?
2 Fe2+ (aq) + F2 (g) 2 Fe3+ (aq) + 2 F- (aq)
A) Fe2+ (aq) Fe3+ (aq) F2 (g) F- (aq)
133)
134) For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs
at the cathode?
Zn(s) Zn2+ (aq) Ni2+ (aq) Ni(s)
A) Zn(s) Zn2+ (aq) + 2 eB) Zn2+ (aq) + 2 e- Zn(s)
C) Ni(s) Ni2+ (aq) + 2 eD) Ni2+ (aq) + 2 e- Ni(s)
134)
135) What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand
notation below?
Al(s) Al3+ (aq) Fe2+ (aq) Fe(s)
+ 3 Fe2+ (aq) 2 Al3+ (aq) + 3 Fe(s)
2
Al(s)
A)
B) 3 Al(s) + 2 Fe2+ (aq) 3 Al3+ (aq) + 2 Fe(s)
C) 2 Fe(s) + 3 Al3+ (aq) 2 Fe2+ (aq) + 3 Al(s)
D) 3 Fe(s) + 2 Al3+ (aq) 3 Fe2+ (aq) + 2 Al(s)
135)
136) What is the balanced equation for the galvanic cell reaction expressed using shorthand notation
below?
Ni(s) Ni2+ (aq) Cl2 (g) Cl- (aq) C(s)
A) Ni(s) + 2 Cl- (aq) Ni2+ (aq) + Cl2 (g)
B) Ni(s) + Cl2 (g) Ni2+ (aq) + 2 Cl- (aq)
136)
D) Cu(s) Cu(NO3 )2 (aq) Pb(NO3 )2 (aq) Pb(s)
B) Fe(s) Fe2+(aq) Fe3+(aq) F2 (g) F- (aq) C(s)
C) Pt(s) Fe3+ (aq), Fe2+ (aq), F2 (g) F-(aq) C(s)
D) Pt(s) Fe2+ (aq), Fe3+ (aq) F2(g) F- (aq) C(s)
C) Ni2+ (aq) + 2 Cl- (aq)
D) Ni2+ (aq) + 2 Cl- (aq)
Ni(s) + Cl2 (g)
NiCl2 (s)
137) A galvanic cell consists of a Ni2+ /Ni half-cell and a standard hydrogen electrode. If the Ni2+ /Ni
137)
half-cell standard cell functions as the anode, and the standard cell potential is 0.26 V, what is the
standard reduction potential for the Ni2 +/Ni half-cell?
A) -0.26 V
B) -0.13 V
C) +0.13 V
D) +0.26 V
138) A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that
contains Cu(s) and Cu2+ (aq). What species are produced at the electrodes under standard
conditions?
Ag+ (aq) + e- Ag(s)
E° = +0.80 V
2+
Cu (aq) + 2 e
Cu(s)
E° = +0.34 V
A) Ag(aq) is formed at the cathode and, Cu(s) is formed at the anode.
B) Ag(s) is formed at the cathode, and Cu2+ (aq) is formed at the anode.
C) Cu(s) is formed at the cathode, and Ag+ (aq) is formed at the anode.
D) Cu2+ (aq) is formed at the cathode, and Cu(s) is formed at the anode.
22
138)
139) Consider the following standard reduction potentials,
Ni2+ (aq) + 2 e- Ni(s)
E° = -0.26 V
I2 (s) + 2 e- 2 I- (aq)
E° = +0.54 V
139)
Under standard conditions,
A) Ni2+ (aq) is a stronger oxidizing agent than I2 (s) and I- (aq) is a stronger reducing agent than
Ni(s).
B) I2(s) is a stronger oxidizing agent than Ni2+ (aq) and Ni(s) is a stronger reducing agent than
I-(aq).
C) Ni(s) is a stronger oxidizing agent than I- (aq) and Ni2+ (aq) is a stronger reducing agent than
I2(s).
D) I-(aq) is a stronger oxidizing agent than Ni(s) and I2 (s) is a stronger reducing agent than Ni
2+ (aq).
140) Based on the following information,
Cl2 (g) + 2 e- 2 Cl- (aq)
E° = +1.36 V
2+
Mg (aq) + 2 e
2 Mg(s)
E° = -2.37 V
which of the following chemical species is the strongest reducing agent?
A) Cl2 (g)
B) Mg2+ (aq)
C) Cl- (aq)
140)
D) Mg(s)
141) Using the following standard reduction potentials,
Fe3+(aq) + e- Fe2+ (aq)
E° = +0.77 V
2+
Cd (aq) + 2 e Cd(s)
E° = -0.40 V
calculate the standard cell potential for the cell reaction given below, and determine whether or not
this reaction is spontaneous under standard conditions.
Cd2+ (aq) + 2 Fe2+ (aq) 2 Fe3+ (aq) + Cd(s)
A) E° = -1.17 V, nonspontaneous
B) E° = -1.17 V, spontaneous
C) E° = +1.17 V, nonspontaneous
D) E° = +1.17 V, spontaneous
141)
142) Consider the galvanic cell, Zn(s) Zn2+(aq) Pb2+ (aq) Pb(s). Which one of the following changes to
the cell would cause the cell potential to increase (i.e., become more positive)?
A) increase the [Zn2+ ] concentration
B) increase the [Pb2+ ] concentration
142)
C) increase the mass of Zn(s)
D) decrease the mass of Zn(s)
143) Calculate the value of the reaction quotient, Q, for the galvanic cell expressed using shorthand
notation below.Use the balanced chemical equation that has the smallest, whole number
stoichiometric coefficients.
Zn(s) Zn2+ (aq, 0.0100 M) Ag+ (aq, 1.15 M) Ag(s)
A) 132
B) 115
C) 8.70 × 10-3
D) 7.56 × 10-3
23
143)
144) The gas OF2 can be produced from the electrolysis of an aqueous solution of KF, as shown in the
equation below.
OF2 (g) + 2 H+ (aq) + 4 e- H2 O(l) + 2 F- (aq)
E° = +2.15 V
Using the given standard reduction potential, calculate the amount of OF2 that is produced, and
144)
the electrode at which the OF2 is produced, upon the passage of 0.480 faradays through an
aqueous KF solution.
A) 6.48 g of OF2 at the anode.
C) 6.48 g of OF2 at the cathode.
B) 26.0 g of OF2 at the anode.
D) 26.0 g of OF2 at the cathode.
145) How many grams of chromium metal are plated out when a constant current of 8.00 A is passed
through an aqueous solution containing Cr3+ ions for 320. minutes?
A) 27.6 g
B) 49.2 g
C) 82.4 g
D) 248 g
145)
146) How many grams of nickel metal are plated out when a constant current of 15.0 A is passed
through aqueous NICl2 for 60.0 minutes?
146)
147) How long must a constant current of 50.0 A be passed through an electrolytic cell containing
aqueous Cu2+ ions to produce 5.00 moles of copper metal?
147)
148) Which of the following elements is an inner transition metal?
A) Eu
B) Fe
C) Ru
148)
A) 10.9 g
A) 0.187 hours
B) 16.4 g
C) 32.8 g
B) 0.373 hours
C) 2.68 hours
D) 36.3 g
D) 5.36 hours
D) Sc
149) What is the characteristic outer electron configuration for transition elements?
A) (n - 1)d 10-xns2
B) (n)d 10-xns2
C) (n + 1)d 10-xns1
D) (n - 1)d 10-x(n + 1)s2
149)
150) What is the ground-state electron configuration for the element cobalt (Z = 27)?
A) [Ar] 4s2 3d 7
B) [Ar] 3d 9
C) [Ar] 4s2 4p 6 5s1
D) [Ar] 3d 7
150)
151) Which element is most likely to have an anomalous electron configuration?
A) Y
B) Tc
C) Ag
151)
D) Cd
152) What is the ground-state electron configuration for the element chromium (Z = 24)?
A) [Ne] 4s2 3d 4
B) [Ar] 4s2 3d 4
C) [Ar] 4s1 3d 5
D) [Ar] 3d 6
152)
153) What is the ground-state electron configuration for Cr in Cr2 O7 2- ?
A) [Ar] 4s1 3d 5
B) [Ar] 4s2 3d 6
C) [Ar] 3d 4
153)
154) What is the ground-state electron configuration for Co2+ (Z = 27)?
A) [Ar] 4s2 3d 9
B) [Ar] 4s2 3d 5
C) [Ar] 3d 7
D) [Ar] 3d 0
D) [Ar] 4s1 3d 6
155) Which transition metal has the anomalous ground-state electron configuration: [Kr] 4d 10 ?
A) Rh
B) Pd
C) Ag
D) Cd
24
154)
155)
156) Which of the following species has the ground-state electron configuration [Ar]3d 4 ?
A) Ti
B) V2+
C) Cr2+
D) Fe2+
156)
157) How many d electrons are there in MnO4 - ?
A) 0
B) 1
157)
C) 2
D) 3
158) What is the d orbital-filling diagram for Fe3+ (Z = 26)?
A) (A)
B) (B)
C) (C)
159) How many valence electrons does the element Co have?
A) 2
B) 7
C) 8
158)
D) (D)
D) 9
159)
160) What two transition elements have the highest electrical conductivity of any elements at room
temperature?
A) copper and iron
B) copper and silver
C) iron and chromium
D) silver and gold
160)
161) Which first row transition element has the highest melting point?
A) Sc
B) V
C) Fe
D) Zn
161)
162) Which transition element has the highest melting point?
A) Fe
B) V
C) Mo
D) W
163) Which of the following elements has the highest density?
A) Cr
B) Ni
C) Os
D) Ta
162)
163)
164) For transition elements, which of the following occurs as the effective nuclear charge increases?
A) The atomic radius increases.
B) The density increases.
C) Both the atomic radius and the density increase.
D) The atomic radius decreases and the density increases.
164)
165) Though we would expect an increase in atomic radii going down a group from the second to the
third transition series of elements, the actual radii are nearly identical. The term commonly used to
describe this phenomenon is the ________.
A) atomic disparity
B) effective nuclear charge
C) lanthanide contraction
D) transition default
165)
25
166) Which of the following transition elements (Sc, Ti, V, Mn, and Cu) have positive oxidation
potentials?
A) Sc
B) Cu
C) Sc, Ti, and V
D) Sc, Ti, V, and Mn
166)
167) Which transition element is difficult to oxidize with hydronium ion?
A) Cr
B) Cu
C) Mn
167)
D) Ti
168) What oxidation state(s) is(are) exhibited by all first row transition elements except scandium?
A) +2
B) +3
C) +2 and +3
D) +2, +3 and +4
168)
169) What is the highest possible oxidation state for chromium?
A) +3
B) +4
C) +5
169)
D) +6
170) What statement is most inconsistent with the chemistry of transition elements?
A) Bromide, chloride and iodide stabilize the higher oxidation states of the transition elements.
B) Early transition metal ions with the metal in its lowest oxidation state are good reducing
agents.
C) Ions that have transition metal in their highest oxidation state tend to be good oxidizing
agents.
D) The stability of the higher oxidation states increases down a periodic group.
170)
171) Vanadium in the +5 oxidation is most often found as compounds of ________.
A) bromides
B) chlorides
C) fluorides
171)
D) iodides
172) What is the strongest oxidizing agent of the following set: VCl2 , CrCl3 , KMnO4 , KReO4 ?
A) VCl2
B) CrCl3
C) KMnO4
D) KReO4
172)
173) What is the strongest oxidizing agent of the following set: MnCl2 , Mn(OH)3 , MnO2 , KMnO4 ?
A) MnCl2
B) Mn(OH)3
C) MnO2
D) KMnO4
173)
174) What chemical equation represents the best method for obtaining pure chromium?
A) FeCr2 O4 (s) + 4 C(s) + heat Fe(s) + 2 Cr(s) + 4 CO(g)
B) Cr2 O3 (s) + 2 Al(s) + heat 2 Cr(s) + Al2 O3 (s)
C) Cr2 O3 (s) + 2 Fe(s) + heat Fe2 O3 (s) + 2 Cr(s)
D) Cr2+ (aq) + H2 (g) Cr(s) + 2 H+ (aq)
174)
175) Which is not a characteristic reaction of chromium metal or chromium(II) ion?
A) Cr(s) + 2 H+ (aq) Cr2+ (aq) + H2 (g)
B) 4 Cr2+ (aq) + O2 (g) + 4 H+ (aq) 4 Cr3+ (aq) + 2 H2 O(l)
175)
C) Cr(OH)2 (s) + 2 H3 O+(aq) Cr2+ (aq) + 4 H2 O(l)
D) Cr(OH)2 (s) + OH- (aq) Cr(OH)3 -(aq)
176) Which of the following chromium species is the strongest acid?
A) Cr(OH)2
B) Cr(OH)3
C) CrO2 (OH)2
26
D) CrO4 2-
176)
177) Which chromium species exists only under acidic conditions?
A) Cr(OH)2
B) Cr(OH)4 C) CrO4 2-
D) Cr2 O7 2-
178) Which is the strongest oxidizing agent under acidic conditions?
A) Cr2+
B) Cr3+
C) CrO4 2-
D) Cr2 O7 2-
179) In the two half-reactions shown below, which chromium species is the strongest oxidizing agent?
Cr2 O7 2–(aq) + 14 H+ (aq) + 6 e– 2 Cr3+ (aq) + 7 H2 O(l)
E° = + 1.33 V
A) Cr2 O7 2–
CrO4 2–(aq) + 4 H2 O(l) + 6 e–
B) Cr3+
Cr(OH)3 (s) + 5 OH– (aq)
177)
178)
179)
E° = – 0.13 V
C) CrO4 2–
D) Cr(OH)3
180) What statement is inconsistent with the chemistry of iron?
A) Iron is the fourth most abundant element in the earth's crust.
B) Iron is obtained from the reduction of hematite (Fe2 O3 ) and magnetite (Fe3 O4 ) by carbon in a
blast furnace.
C) Iron is a relatively hard metal and it is relatively unreactive with haloacids.
D) The majority of iron in a healthy human is present in the oxygen-carrying protein
hemoglobin.
180)
181) What are two of the major components of stainless steel?
A) iron and carbon
B) iron and chromium
C) iron and titanium
D) iron and tungsten
181)
182) What statement is most inconsistent about the chemistry of iron?
182)
A) Iron(III) hydroxide is very soluble and reacts readily with hydroxide to form Fe(OH)4 – .
B) Iron reacts with hydrochloric acid in the absence of air to yield iron(II) ion and hydrogen gas.
C) Iron reacts with nitric acid to yield iron(III) ion and nitric oxide.
D) The most common oxidation states of iron are +2 (ferrous) and +3 (ferric).
183) What is the strongest oxidizing agent of the following set: FeO, Fe2 O3 , Fe3 O4 , FeO4 2-?
A) FeO
B) Fe2 O3
C) Fe3 O4
183)
D) FeO4 2-
184) What statement is inconsistent with the chemistry of copper?
A) It has a high electrical conductivity and is widely used to make electrical wiring.
B) It is commonly found in the elemental state.
C) It is a reddish colored metal that accounts for only 0.0068% of the earth's crust by mass.
D) It is used to make corrosion-resistant water pipes because it has a positive oxidation
potential.
184)
185) What is the compound responsible for the green patina seen on bronze monuments?
A) CuCO3
B) Cu2 (OH)2 CO3
C) Cu(OH)2
D) Cu2 (OH)2 SO4
185)
186) Which of the following is a disproportionation reaction?
A) Cu2 S(l) + O2 (g) 2 Cu(l) + SO2 (g)
B) 3 Cu(s) + 2 NO3 -(aq) + 8 H+ (aq) 3 Cu2+ (aq) + 2 NO(g) + 4 H2 O(l)
186)
C) 2 Cu+ (aq) Cu(s) + Cu2+ (aq)
D) Cu2+ (aq) + 4 NH3 (aq) Cu(NH3 )42+ (aq)
27
187) Using the following reduction potentials for copper determine the unstable copper compound.
Cu+ (aq) + e- Cu(s)
E° = +0.52 V
Cu2+ (aq) + e- Cu+ (aq)
E° = +0.15 V
A) CuCl
B) CuCl2
C) CuSO4
D) Cu(OH)2
187)
188) Describe what happens when 3.0 M NH3 is slowly added to an aqueous solution of CuSO4 .
A) A blue precipitate of Cu(OH)2 forms.
B) A royal blue complex of [Cu(NH3 )4 ]2+ is formed.
188)
C) A blue precipitate of Cu(OH)2 is formed which is then converted to the royal blue complex
[Cu(NH3 )4 ]2+ .
D) A royal blue complex of [Cu(NH3 )4 ]2+ is formed which then is converted to a blue precipitate
of Cu(OH)2 .
189) Which one of the following compounds is not consistent with the terminology of a complex?
A) [Cu(NH3 )4 ]2+
B) CuSO4 · 5H2 O
C) K3 [Fe(CN)6 ]
D) [Cr(NH3 )6 ]Cl3
189)
190) Which is a complex ion?
190)
A) CrCl3
B) CrO4 2–
C) [Cr(H2 O)6 ]3+
191) What is the coordination number of the Fe atom in K3 [Fe(C2 O4 )3]?
A) 2
B) 3
C) 4
D) Cr2 O7 2–
191)
D) 6
192) What is the coordination number of the Au atom in K [Au(CN)2 (SCN)2 ]?
A) 2
B) 3
C) 4
192)
D) 6
193) What is the oxidation state of the Cr atom in [Ni(en)3 ]3 [Cr(CN)6 ]2 ?
A) +2
B) +3
C) +4
D) +6
194) What is the oxidation state of the Co atom in [Co(NH3)5 Cl](NO3 )2 ?
A) +2
B) +3
C) +4
D) +6
193)
194)
195) A chromium(III) ion forms a complex ion with two ammonia molecules and four thiocyanate ions.
What is the formula of the complex ion?
A) [Cr(NH3 )2 (NCS)4 ]3+
B) [Cr(NH4 )2 (NCS)4 ]+
195)
196) Which of the following can function as a bidentate ligand?
A) CO
B) OHC) NH3
196)
C) [Cr(NH3 )2 (NCS)4 ]–
D) [Cr(NH3 )2 (NCS)4 ]4–
197) Which of the following can function as a bidentate ligand?
A) CN–
B) NCS–
C) H2 NCH2 CO2 –
D) All of these can function as bidentate ligands.
28
D) C2 O4 2-
197)
198) Ethylenediaminetetraacetate ion (EDTA4-) is commonly referred to as a ________ ligand.
A) monodentate
B) bidentate
C) tetradentate
D) hexadentate
198)
199) Which of the following can function as a chelating agent?
A) CNB) CO
199)
D) NCS-
C) H2 NCH2 CH2 NH2
200) When the oxalate ion, C2 O4 2– is bonded to the iron(III) ion in the complex ion [Fe(C2 O4 )3 ]3–, a
________-membered chelate ring is formed.
A) 3
B) 4
C) 5
201) Which ligand when bonded to a metal would be incorrectly named?
A) H2 O, aqua
B) NH3 , ammonia
C) CO, carbonyl
200)
D) 6
201)
D) F- , fluoro
202) Write the chemical formula for aquabromobis(ethylenediamine)chromium(III) chloride.
A) [CrBr(H2 O)(en)]Cl
B) [CrBr2 (H2 O)(en)]Cl2
C) [CrBr(H2 O)(en)2 ]Cl2
D) [CrBr(H2 O)(en)2 ]Cl3
202)
203) Write the chemical formula for pentaamminenitritocobalt(III) ion.
A) [Co(NO)(NH3 )5 ]3+
B) [Co(NO2 )(NH3 )5 ]2+
C) [Co(ONO)(NH3 )5 ]2+
D) [Co(NH3 )5 (N2 O)]2+
203)
204) What is the correct formula for tetraamminecarbonatoiron(III) chloride?
A) (NH3 )4 [FeCO3 ]Cl
B) [Fe(CO3 )(NH3 )4 ]Cl
C) [Fe(CO3 )(NH3 )4 ]Cl2
D) [Fe(CO3 )Cl(NH3 )4 ]
204)
205) The complex cis-[CoCl(NH3 )(NH2 CH2 CH2 NH2 )2 ]2+ was resolved into optical isomers in 1911 by
Alfred Werner, demonstrating the octahedral geometry of the ion. Name this complex ion.
A) cis-chloroammineethylenediaminecobalt(II) ion
B) cis-amminechloroethylenediaminecobalt(III) ion
C) cis-amminechlorobis(ethylenediamine)cobalt(II) ion
D) cis-amminechlorobis(ethylenediamine)cobalt(III) ion
205)
206) What is the name of the complex [Ni(en)3 ]3 [Cr(CN)6 ]2 ?
A) ethylenediaminenickel(III) hexacyanochromate(II)
B) tris(ethylenediamine)nickel(III) hexacyanochromate(II)
C) tris(ethylenediamine)nickel(II) hexacyanochromate(III)
D) bis(ethylenediamine)nickel(II) hexacyanochromate(III)
206)
207) What is the name of the complex [Ni(H2 O)4 (NH2CH2 CH2 NH2 )]SO4 · 5H2 O?
A) aquaethylenediaminenickel(II) sulfate hydrate
B) tetraaquaethylenediaminenickel(II) sulfate pentahydrate
C) tetraaquabis(ethylenediamine)nickel(II) sulfate pentahydrate
D) tetraaquabis(ethylenediamine)nickel(III) sulfate pentahydrate
207)
29
208) What is the name of the complex ion [AuBrCl(CN)2 ]-?
A) bromochlorodicyanogold(I) ion
B) bromochlorodicyanoaurate(III) ion
C) bromochlorodicyanoargentate(III) ion
D) bromochlorodicyanoaurate(IV) ion
208)
209) In order to form a neutral compound, hexafluoroaluminate would require
A) three K+ ions.
B) three Cl– ions.
C) six Na+ ions.
209)
D) six Br– ions.
210) Identify the classification of isomers illustrated by [Co(NO2 )(NH3 )5 ]2+ and [Co(ONO)(NH3 )5 ]2+ .
A) linkage isomers
B) ionization isomers
C) geometric isomers
D) optical isomers
210)
211) Which pair of isomers illustrates the concept of ionization isomers?
A) [Cr(SCN)(NH3)5 ]2+ and [Cr(NCS)(NH3 )5 ]2+
B) [CoCl(NH3 )5 ]SO4 and [Co(SO4 )(NH3 )5 ]Cl
C) cis -[PtCl2 (NH3 )2 ] and trans -[PtCl2(NH3 )2 ]
D) (+)-[Co(en)3 ]3+ and (-)-[Co(en)3 ]3+
211)
212) The compounds [Cr(H2 O)6 ]Cl3 and [CrCl3 (H2 O)3 ] · 3H2 O are examples of ________.
A) diastereoisomers
B) enantiomers
C) ionization isomers
D) linkage isomers
212)
213) Which ion has cis and trans isomers?
A) [PdCl3 NH3 ]B) [Pt(CN)5 NH3 ]-
213)
C) [PtCl2 (CN)2 ]2-
214) Which complex is optically active?
A) [CoCl4 en]2C) cis-[CrCl2 (en)2 ]+
D) [Pt(C2 O4 )2 ]2-
214)
B) trans-[CrCl2 (en)2 ]+
D) [PtCl2 (NH3 )2 ]
215) Which complex cannot exist as enantiomers?
A) [CoCl2 (H2 O)4 ]+
C) cis-[CrCl2 (C2 O4 )2 ]+
215)
B) [Co(en)3 ]3+
D) [Fe(C2 O4 )2 (en)]-
216) Which definition best describes isomers that are non-superimposable mirror images of each other
that rotate plane polarized light to the same degree but in opposite directions?
A) diastereoisomers
B) enantiomers
C) linkage isomers
D) racemic mixture
216)
217) Which one of the following objects is chiral?
A) a bottle
B) a chair
217)
C) a glass
D) a glove
218) A complex ion that has a broad absorption band at 625 nm in its visible absorption spectrum will
appear to be
A) blue
B) colorless
C) red
D) yellow
218)
219) What hybridization scheme is used for Ni in the square planar complex of [Ni(CN)4 ]2-?
A) sp3
B) dsp2
C) dsp3
D) d 2 sp3
219)
30
220) What type of hybrid orbitals are used by the Ti atom to form chemical bonds in the complex ion
[Ti(H2 O)6 ]3+ ?
A) sp3
B) dsp2
C) dsp3
D) d 2 sp3
220)
221) How many unpaired electrons are present in the high spin form of the [CoF6 ]3- complex and what
metal orbitals are used in bonding?
A) 0 unpaired electrons and 4s, 4p and 4d orbitals to give sp3 d 2
B) 4 unpaired electrons and 4s, 4p and 4d orbitals to give sp3 d 2
C) 0 unpaired electrons and 3d, 4s, and 4p orbitals to give d 2 sp3
D) 4 unpaired electrons and 3d, 4s, and 4p orbitals to give d 2 sp3
221)
222) Which metal ion is most likely to form a square planar complex ion with CN- ?
A) Co2+
B) Cu2+
C) Ni2+
D) Zn2+
222)
223) The complex [Ni(CN)4 ]2- is diamagnetic and the complex [NiCl4 ]2- is paramagnetic. What can
you conclude about their molecular geometries?
A) Both complexes have square planar geometries.
B) Both complexes have tetrahedral geometries.
C) [NiCl4 ]2- has a square planar geometry while [Ni(CN)4]2- has a tetrahedral geometry.
D) [NiCl4 ]2- has a tetrahedral geometry while [Ni(CN)4 ]2- has a square planar geometry.
223)
224) How many d electrons are there on the Fe metal atom in Na3 [Fe(CN)6 ]?
A) 1
B) 3
C) 5
224)
225) Which of the following species is diamagnetic?
A) an isolated, gas-phase V3+ ion
C) an isolated, gas-phase Cu2+ ion
D) 6
B) a high-spin octahedral Fe2+ complex
D) a low-spin octahedral Co3+ complex
226) What is a representative orbital-filling diagram for the cobalt ion in the low spin complex of
[Co(CN)6 ]3- ?
A) (A)
B) (B)
C) (C)
31
D) (D)
225)
226)
227) Which of the following complex ions is colorless?
A) [Co(H2 O)6 ]2+
B) [Mn(CN)6 ]3-
227)
C) [CrCl3 (H2 O)3 ]
228) Which of the following complexes has five unpaired electrons?
A) [Mn(H2 O)6 ]2+
B) [Mn(CN)6 ]3C) CrCl3 (H2 O)3
229) Which of the following complexes are diamagnetic?
[Mn(CN)6 ]3- [Zn(NH3 )4 ]2+
[Fe(CN)6 ]4A) [Zn(NH3 )4 ]2+
D) [Ag(NH3 )2 ]+
228)
D) [Ag(NH3 )2 ]+
229)
[FeF6 ]3-
B) [Zn(NH3 )4 ]2+ and [FeF6 ]3C) [Zn(NH3 )4 ]2+ and [Fe(CN)6 ]4-
D) [Mn(CN)6 ]3- , [Zn(NH3 )4 ]2+ and [Fe(CN)6 ]4230) For an octahedral complex what metal d orbitals are directly towards the ligands?
A) d xy, d xz
B) d xy, d xz, d yz
C) d z², dx²- y²
D) d z², d xz, d yz
230)
231) What is the expected order for increasing octahedral ( 0 ) crystal field splitting for the ligands I- ,
F- , H2 O, NH3 , en, CO?
231)
A) I- < F- < H2O < NH3 < en < CO
C) I- < F- < H2O < CO < NH3 < en
B) F- < I- < NH3 < en < CO < H2 O
D) CO < en < NH3 < H2 O < F- < I-
232) What is the expected order for increasing octahedral ( 0 ) crystal field splitting for ligands?
A) halides < O ligands < N ligands < CNB) halides < CN- < O ligands < N ligands
C) CN- < N ligands < O ligands < halides
D) O ligands < N ligands < CN- < halides
232)
233) What is the crystal field energy level diagram for the complex [Fe(H2 O)6 ]3+ ?
233)
A) (A)
B) (B)
C) (C)
D) (D)
234) What is the crystal field energy level diagram for the complex [Co(CN)6 ]3-?
A) (A)
B) (B)
C) (C)
32
234)
D) (D)
235) Which ion would you expect to have the largest crystal field splitting, ?
A) [Fe(CN)6 ]4B) [Fe(CN)6 ]3C) [Fe(H2 O)6 ]2+
D) [Fe(H2 O)6 ]3+
235)
236) What statement is inconsistent with the crystal field theory of tetrahedral complexes?
A) t is about 4/9's that of 0 .
B) Tetrahedral complexes are nearly all low spin.
C) The d xy, d xz, and dyz orbitals are higher in energy than the d z² and d x²- y² orbitals.
236)
237) Which one of the following complexes is considered to be tetrahedral?
A) [FeCl4 ]B) [Ni(CN)4 ]2C) [PtCl4 ]2-
237)
D) None of the metal d orbitals point directly at the ligands in a tetrahedral environment.
238) How many unpaired electrons will Co have in the complex [CoCl4 ]2- ?
A) 1
B) 3
C) 4
D) [PdCl2 (NH3 )2 ]
238)
D) 5
239) Which group of elements, indicated by letter and shading on the periodic table above, represents
the transition elements?
A) A
B) B
C) C
D) D
239)
240) Which group of elements, indicated by letter and shading on the periodic table above, represents
the inner transition elements?
A) A
B) B
C) C
D) D
240)
241) Which element indicated on the above periodic table has the electron configuration [Kr] 4d 5 5s2 ?
A) element A
B) element B
C) element C
D) element D
241)
33
242) Which element indicated on the above periodic table has the electron configuration [Xe] 4f 7 5d 1
6s2 ?
A) element A
B) element B
C) element C
D) element D
242)
243) Which element indicated on the above periodic table has the electron configuration [Ar] 3d 3 4s2 ?
A) element A
B) element B
C) element C
D) element D
243)
244) Which element indicated on the above periodic table has the electron configuration [Ar] 3d 10 4s1 ?
A) element A
B) element B
C) element C
D) element D
244)
245) Which is the most common ion formed by element B on the above periodic table?
A) B+
B) B2+
C) B3+
D) B4+
245)
246) Which is the most common ion formed by element D on the above periodic table?
A) B+
B) B2+
C) B3+
D) B7+
246)
The first transition series metals are shown below.
247) Which has the highest melting point?
A) Sc
B) V
C) Mn
D) Zn
248) Which has the lowest melting point?
A) Sc
B) V
C) Mn
D) Zn
249) Which has the largest atomic radius?
A) Sc
B) V
C) Ni
D) Zn
250) Which has the smallest atomic radius?
A) Sc
B) V
C) Ni
D) Zn
251) Which has the greatest density?
A) Sc
B) V
C) Cu
D) Zn
252) Which has the most positive standard oxidation potential?
A) Sc
B) V
C) Cu
D) Zn
253) Which has the most negative standard oxidation potential?
A) Sc
B) V
C) Cu
D) Zn
247)
248)
249)
250)
251)
252)
253)
254) Based on the variation in Zeff, which M2+ ion should be the strongest reducing agent?
254)
255) Based on the variation in Zeff, which M2+ ion should be the weakest reducing agent?
255)
A) Ti
A) Ti
B) Cr
C) Fe
B) Cr
C) Fe
34
D) Zn
D) Zn
256) Based on the variation in Zeff, which oxoanion should be the strongest oxidizing agent?
256)
257) Based on the variation in Zeff, which oxoanion should be the weakest oxidizing agent?
257)
258) Which metal exhibits the highest oxidation state in its compounds?
A) Sc
B) Cr
C) Mn
258)
A) VO4 3-
A) VO4 3-
B) CrO4 2-
C) MnO4 2-
B) CrO4 2-
C) MnO4 2-
D) FeO4 2-
D) FeO4 2-
D) Zn
The second transition series metals are shown below.
259) Which has the highest melting point?
A) Y
B) Mo
C) Tc
D) Cd
260) Which has the lowest melting point?
A) Y
B) Mo
C) Tc
D) Cd
261) Which has the largest atomic radius?
A) Y
B) Mo
C) Rh
D) Cd
262) Which has the smallest atomic radius?
A) Y
B) Mo
C) Rh
D) Cd
263) Which has the greatest density?
A) Y
B) Mo
C) Rh
D) Cd
264) Which has the lowest density?
A) Y
B) Mo
C) Rh
D) Cd
265) Which has the highest melting point?
A) La
B) W
C) Os
D) Hg
266) Which has the lowest melting point?
A) La
B) W
C) Os
D) Hg
259)
260)
261)
262)
263)
264)
The third transition series metals are shown below.
267) Which has the largest atomic radius?
A) La
B) W
C) Os
35
D) Hg
265)
266)
267)
268) Which has the smallest atomic radius?
A) La
B) W
C) Os
D) Hg
269) Which has the greatest density?
A) La
B) W
C) Os
D) Hg
270) Which has the lowest density?
A) La
B) W
C) Os
271) Which of the above are bidentate ligands?
A) All are bidentate.
C) (c) and (d)
B) (a) and (b)
D) None are bidentate.
272) Which of the above are monodentate ligands?
A) All are monodentate.
C) (c) and (d)
D) Hg
B) (a) and (b)
D) None are monodentate.
273) Which of the above are ligands that contain two or more donor atoms?
A) All contain two or more donor atoms.
B) (a) and (b)
C) (c) and (d)
D) None contain two or more donor atoms.
36
268)
269)
270)
271)
272)
273)
274) Which of the above are bidentate or tridentate ligands, capable of forming chelate rings?
A) (a) and (c)
B) (b) and (d)
C) (a), (b), and (c)
D) (a), (b), (c), and (d)
274)
275) Which of the above are monodentate ligands?
A) (a) and (c)
C) All are monodentate.
275)
B) (b) and (d)
D) None are monodentate.
Consider the following isomers of [Co(NH3 )4 Br2 ]+ . The black sphere represents Co, gray spheres represent NH3, and
unshaded spheres represent Br.
276) Which are cis-isomers?
A) isomers (1) and (2)
C) isomers (2) and (4)
B) isomers (1) and (3)
D) isomers (3) and (4)
277) Which are trans-isomers?
A) isomers (1) and (2)
C) isomers (2) and (4)
B) isomers (1) and (3)
D) isomers (3) and (4)
37
276)
277)
278) Which structures are identical?
A) None of the structures are identical.
B) structure (1) = structure (2) and structure (3) = structure (4)
C) structure (1) = structure (3) and structure (2) = structure (4)
D) structure (1) = structure (4) and structure (2) = structure (3)
278)
279) Which exist as enantiomers?
A) All exist as enantiomers.
C) isomers (2) and (4)
279)
B) isomers (1) and (3)
D) None exist as enantiomers.
Consider the following ethylenediamine complexes. The black sphere represents Co, gray connected spheres represent
ethylenediamine, NH2 CH2 CH2 NH2 , and unshaded spheres represent Br.
280) Which complexes are chiral?
A) complexes (1), (2), and (3)
C) complexes (1), (3), and (4)
B) complexes (1), (2), and (4)
D) complexes (2), (3), and (4)
281) Which complexes are enantiomers of one another?
A) complexes (1) and (3)
C) complexes (3) and (4)
B) complexes (1) and (4)
D) complexes (1), (3), and (4)
280)
281)
282) Which of the Co(III) complexes above are enantiomers of each other?
A) (A) and (B)
B) (C) and (D)
C) (A), (B), and (C)
D) (A), (B), (C), and (D)
282)
283) Which of the Co(III) complexes above are optically active?
A) (A) and (B)
B) (C) and (D)
C) (A), (B), and (C)
D) (A), (B), (C), and (D)
283)
38
284) Which Pt(II) complexes are geometric isomers of each other?
A) (a) and (f)
B) (b) and (e)
C) (c) and (d)
284)
D) (a) and (b)
285) Using the above schematic of an artist's color wheel, determine the color seen if a substance absorbs
red and yellow light.
A) blue
B) green
C) orange
D) violet
285)
286) Using the above schematic of an artist's color wheel, determine the color seen if a substance absorbs
yellow and blue light.
A) green
B) orange
C) red
D) violet
286)
287) Using the above schematic of an artist's color wheel, determine the color absorbed if a substance is
seen as being green in color.
A) blue
B) orange
C) red
D) violet
287)
39
288) The absorbance spectrum of a complex along with an artist's color wheel is shown below.
Determine the color one might see for this complex.
A) green
B) red
C) red-violet
289) Which is the crystal field energy level diagram for an octahedral ML6 complex?
A) (A)
B) (B)
C) (C)
D) yellow
289)
D) (D)
290) Which is the crystal field energy level diagram for a square pyramidal ML5 complex that contains a
single ligand on the z-axis?
A) (A)
B) (B)
C) (C)
B) (B)
C) (C)
292) Which is the crystal field energy level diagram for a tetrahedral ML4 ?
A) (A)
B) (B)
C) (C)
291)
D) (D)
292)
D) (D)
293) What is the ground-state electron configuration for the element chromium (Z = 24)?
A) [Ne] 4s2 3d 4
B) [Ar] 4s2 3d 4
C) [Ar] 4s1 3d 5
D) [Ar] 3d 6
40
290)
D) (D)
291) Which is the crystal field energy level diagram for a square planar ML4 complex that contains no
ligands on the z-axis?
A) (A)
288)
293)
294) Which of the following elements is an inner transition metal?
A) Eu
B) Fe
C) Ru
295) What is the ground-state electron configuration for Cr3+ (Z = 24)?
A) [Ar] 4s2 3d 7
B) [Ar] 4s2 3d 1
C) [Ar] 3d 3
296) How many d electrons are there in W O4 2- ?
A) 0
B) 1
D) Sc
294)
295)
D) [Ar] 4s1 3d 2
296)
C) 2
D) 3
297) Which of the following species has the electron configuration [Ar]3d 6 ?
A) Cr
B) Fe3+
C) Co3+
D) Ni3+
298) What is the highest possible oxidation state for manganese?
A) +2
B) +5
C) +6
D) +7
299) Which of the following can function as a bidentate ligand?
A) CO
B) OH C) N H3
D) C2 O4 2-
297)
300) Which of the following can function as a chelating agent?
A) SHB) H2 O
C) H2 NCH2 CO2 -
298)
299)
300)
D) SCN -
301) Which of the following species is diamagnetic?
A) an isolated, gas-phase Cr3+ ion
C) an isolated, gas-phase Cu2+ ion
B) a high-spin octahedral Cr2+ complex
301)
D) a low-spin octahedral Co3+ complex
302) Which ion would you expect to have the largest crystal field splitting, ?
A) [Rh(CN)6 ]4B) [Rh(CN)6 ]3C) [Rh(H2 O)6 ]2+
41
D) [Rh(H2 O)6 ]3+
302)
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 SPRING 2015 PRACTICE EXAM 4
1) D
2) B
3) D
4) D
5) D
6) D
7) A
8) B
9) B
10) C
11) B
12) C
13) C
14) A
15) D
16) D
17) A
18) A
19) B
20) B
21) C
22) A
23) D
24) C
25) A
26) C
27) C
28) D
29) D
30) A
31) C
32) D
33) B
34) A
35) B
36) B
37) D
38) A
39) D
40) A
41) B
42) B
43) C
44) C
45) A
46) B
47) D
48) D
49) B
50) C
42
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 SPRING 2015 PRACTICE EXAM 4
51) A
52) C
53) B
54) C
55) B
56) D
57) C
58) B
59) A
60) B
61) C
62) C
63) B
64) A
65) D
66) B
67) D
68) C
69) B
70) C
71) D
72) C
73) D
74) D
75) A
76) C
77) B
78) D
79) B
80) C
81) B
82) C
83) B
84) D
85) A
86) C
87) B
88) B
89) C
90) D
91) D
92) A
93) A
94) A
95) B
96) D
97) D
98) B
99) D
100) C
43
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 SPRING 2015 PRACTICE EXAM 4
101)
102)
103)
104)
105)
106)
107)
108)
109)
110)
111)
112)
113)
114)
115)
116)
117)
118)
119)
120)
121)
122)
123)
124)
125)
126)
127)
128)
129)
130)
131)
132)
133)
134)
135)
136)
137)
138)
139)
140)
141)
142)
143)
144)
145)
146)
147)
148)
149)
150)
A
D
D
B
B
C
B
B
B
C
B
C
D
B
C
D
A
B
A
C
B
C
B
C
A
A
B
B
B
C
C
A
D
D
A
B
A
B
B
D
A
B
D
A
A
B
D
A
A
A
44
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 SPRING 2015 PRACTICE EXAM 4
151)
152)
153)
154)
155)
156)
157)
158)
159)
160)
161)
162)
163)
164)
165)
166)
167)
168)
169)
170)
171)
172)
173)
174)
175)
176)
177)
178)
179)
180)
181)
182)
183)
184)
185)
186)
187)
188)
189)
190)
191)
192)
193)
194)
195)
196)
197)
198)
199)
200)
C
C
D
C
B
C
A
D
D
B
B
D
C
D
C
D
B
A
D
A
C
C
D
B
D
C
D
D
A
C
B
A
D
D
D
C
A
C
B
C
D
C
B
B
C
D
C
D
C
C
45
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 SPRING 2015 PRACTICE EXAM 4
201)
202)
203)
204)
205)
206)
207)
208)
209)
210)
211)
212)
213)
214)
215)
216)
217)
218)
219)
220)
221)
222)
223)
224)
225)
226)
227)
228)
229)
230)
231)
232)
233)
234)
235)
236)
237)
238)
239)
240)
241)
242)
243)
244)
245)
246)
247)
248)
249)
250)
B
C
C
B
D
C
B
B
A
A
B
C
C
C
A
B
D
A
B
D
B
C
D
C
D
B
D
A
C
C
A
A
B
A
B
B
A
B
B
D
C
D
A
B
B
C
B
D
A
C
46
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 SPRING 2015 PRACTICE EXAM 4
251)
252)
253)
254)
255)
256)
257)
258)
259)
260)
261)
262)
263)
264)
265)
266)
267)
268)
269)
270)
271)
272)
273)
274)
275)
276)
277)
278)
279)
280)
281)
282)
283)
284)
285)
286)
287)
288)
289)
290)
291)
292)
293)
294)
295)
296)
297)
298)
299)
300)
C
A
C
A
D
D
A
C
B
D
A
C
C
A
B
D
A
C
C
A
C
B
A
A
B
B
C
C
D
A
A
A
C
C
A
C
C
C
A
B
C
D
C
A
C
A
C
D
D
C
47
Answer Key
Testname: COLLEGE CHEMISTRY II PHS 1035 SPRING 2015 PRACTICE EXAM 4
301) D
302) B
48