Chemistry, 7e (McMurry/Fay)
Chapter 6 Ionic compounds: Periodic Trends and Bonding
6.1 Multiple-Choice Questions
1) What is the ground-state electron configuration of the ion Hg2+?
A) [Xe]4f145d10
B) [Xe]4f145d86s2
C) [Xe]4f145d106s2
D) [Xe]4f145d106s26p2
2) What is the ground-state electron configuration of the ion Cu2+?
A) [Ar] 3d9
B) [Ar] 4s1 3d8
C) [Ar] 4s2 3d7
D) [Ar] 4s2 3d10 4p1
3) Which of the following three sets consist of atoms or ions with the same electron configuration in the
ground state?
(I) O2-, Ne, and Mg2+
(II) Ni, Cu+, and Zn2+
(III) Hg, Tl+, and Pb2+
A) all three sets
B) (II) and (III)
C) (I) and (III)
D) (I)
4) What is the ground-state electron configuration of Se2–?
A) [Ar]3d104s24p2
B) [Ar]3d104s24p4
C) [Ar]3d124s24p4
D) [Ar]3d104s24p6
5) Which ion has the same electron configuration as Kr?
A) Rb+
B) Br–
C) Se2-
D) All of these
6) Consider the following ground state electron configuration: 1s22s22p4. Which of the ions has this
ground state electron configuration?
A) F-1
B) N+1
C) C-2
D) O-2
7) Which ion has the smallest ionic radius?
A) Li+
B) Na+
C) K+
D) Rb+
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8) Which ion has the smallest ionic radius?
A) F–
B) Cl–
C) Br–
D) I–
9) Arrange the ions N3–, O2-, Mg2+, Na+, and F– in order of increasing ionic radius, starting with the
smallest first.
A) Mg2+, Na+, F–, O2-, N3-
B) N3-, Mg2+, O2-, Na+, F–
C) N3-, O2-, Mg2+, F–, Na+
D) N3-, O2-, F–, Na+, Mg2+
10) Which of the following most likely represent the atomic radius of a Cr atom, the ionic radius of a Cr2+
ion, and the ionic radius of a Cr3+ ion?
A) 128 pm for Cr, 167 pm for Cr2+, and 193 pm for Cr3+
B) 128 pm for Cr, 147 pm for Cr2+, and 193 pm for Cr3+
C) 128 pm for Cr, 109 pm for Cr2+, and 63 pm for Cr3+
D) 128 pm for Cr, 89 pm for Cr2+, and 63 pm for Cr3+
11) Consider Li+, F–, and O2-. Which ratio should be the largest?
A) (radius Li+)/(radius F–)
B) (radius Li+)/(radius O2-)
C) (radius F–)/(radius Li+)
D) (radius O2-)/(radius Li+)
12) Which ion has the largest radius?
Ca+2, Ca+1, Br–, K+
A) Ca+2
B) Ca+1
C) Br–
D) K+
13) Of the following, which element has the highest first ionization energy?
A) argon
B) neon
C) helium
D) krypton
14) Of the following, which element has the highest first ionization energy?
A) iodine
B) bromine
C) fluorine
D) chlorine
15) Of the following, which element has the highest first ionization energy?
A) P
B) N
C) Sb
D) As
16) Of the following, which element has the highest first ionization energy?
A) P
B) C
C) Si
D) N
17) Of the following, which element has the highest first ionization energy?
A) Li
B) F
C) Cs
D) At
18) Of the following, which element has the highest first ionization energy?
A) Cl
B) F
C) O
D) S
19) List the elements Na, Ca, Rb, Cl, He in order of decreasing first ionization energy.
A) He > Cl > Ca > Na > Rb
B) He > Na > Ca > Cl > Rb
C) He > Na > Cl > Ca > Rb
D) Rb > Ca > Cl > Na > He
20) List the elements Cs, Ca, Ne, Na, Ar in order of decreasing first ionization energy.
A) Ar > Ca > Cs > Na > Ne
B) Ne > Ar > Ca > Na > Cs
C) Ne > Ar > Na > Cs > Ca
D) Ne > Na > Cs > Ca > Ar
21) Element A has a valence shell configuration of ns2np4 while Element B has a valence shell
configuration of ns2np5 where n = energy level. Which of the following statements is true regarding these
elements?
A) The ionization energy of A is lower than the ionization energy of B.
B) The electron affinity of A is higher than the electron affinity of B.
C) Element A and B are transition metals.
D) Element A and B have the same I.E.
22) Which ionization process requires the most energy?
A) Al(g) → Al+(g) + e–
B) Al+(g) → Al2+(g) + e–
C) Al2+(g) → Al3+(g) + e–
D) Al3+(g) → Al4+(g) + e–
23) Which of the following atoms with the specified electronic configurations would have the lowest first
ionization energy?
A) [He]2s22p3
B) [Ne]3s23p4
C) [Xe]6s1
D) [Xe]6s24f145d106p1
24) Which of the following represents the change in electronic configuration that is associated with the
second ionization energy of magnesium?
A) [Ne]3s2 → [Ne]3s1 + e–
B) [Ne]3s2 → [Ne] + 2 e–
C) [Ne]3s1 → [Ne] + e–
D) [Ne]3s2 + e– → [Ne]3s23p1
25) Consider the following electron configurations for neutral atoms:
atom I = 1s22s22p63s2
atom II = 1s22s22p63s23p4
atom III = 1s22s22p63s23p6
Which atom would be expected to have the largest third ionization energy?
A) atom I
B) atom II
C) atom III
D) All of these atoms would be expected to have the same third ionization energy.
26) Which period 3 element has successive first through seventh ionization energies (kJ/mol) of
Ei1 = 578; Ei2 = 1,817; Ei3 = 2,745; Ei4 = 11,575; Ei5 = 14,830; Ei6 = 18,376; and Ei7 = 23,293?
A) Mg
B) Al
C) S
D) Cl
27) Which period 2 element has successive first through seventh ionization energies (kJ/mol) of
Ei1 = 1,402; Ei2 = 2,856; Ei3 = 4,578; Ei4 = 7,475; Ei5 = 9,445; Ei6 = 53,267; and Ei7 = 64,360?
A) B
B) C
C) N
D) O
28) An element Y, has the following ionization energies
Ei1 = 578 kJ/mol
Ei2 = 1,817 kJ/mol
Ei3 = 2,745 kJ/mol
Ei4 = 11,575 kJ/mol
What is the most likely identity for this element?
A) Na
B) Mg
C) Al
D) Si
29) Which liberates the most energy?
A) Li(g) + e– → Li–(g)
B) Na(g) + e– → Na–(g)
C) K(g) + e– → K–(g)
D) Rb(g) + e– → Rb–(g)
30) Which liberates the most energy?
A) Br(g) + e⁻ → Br⁻(g)
B) Cl(g) + e⁻ → Cl⁻(g)
C) F(g) + e⁻ → F⁻(g)
D) I(g) → I⁻(g)
31) Which electron affinity process would liberate the most energy?
A) [He] 2s2 + e– → [He] 2s2 2p1
B) [He] 2s2 2p2 + e– → [He] 2s2 2p3
C) [He] 2s2 2p3 + e– → [He] 2s2 2p4
D) [He] 2s2 2p6 + e– → [He] 2s2 2p6 3s1
32) Which element has the most favorable (most negative) electron affinity?
A) B
B) C
C) Li
D) N
33) Which element has the most favorable (most negative) electron affinity?
A) K
B) Be
C) I
D) Ne
34) Which of these elements has the most favorable (most negative) electron affinity?
A) Ca
B) N
C) Ne
D) S
35) What is the general trend in ionization energy and electron affinity values?
A) Both decrease as one traverses a period from left to right and both decrease as one descends a group.
B) Both decrease as one traverses a period from left to right and both increase as one descends a group.
C) Both increase as one traverses a period from left to right and both decrease as one descends a group.
D) Both increase as one traverses a period from left to right and both increase as one descends a group.
36) An element that has the valence electron configuration 3s23p3 belongs to which period and group?
A) period 3; group 3A
B) period 3; group 5A
C) period 4; group 3A
D) period 4; group 5A
37) In the reaction of sodium metal with chlorine gas which of the following processes releases energy?
A) Cl2(g) → 2 Cl(g)
B) Cl(g) + e– → Cl–(g)
C) Na(s) → Na(g)
D) Na(g) → Na+(g) + e–
38) Calculate the energy change for the formation of LiCl(s) from its elements in their standard states and
the following tabulated information:
Li(s) + 1/2 Cl2(g) → LiCl(s) ?
Li+(g) + Cl–(g) → LiCl(s) -853 kJ/mol
Li(s) → Li(g) +159.4 kJ/mol
1/2 Cl2(g) → Cl(g) +121.7 kJ/mol
Cl(g) + e– → Cl–(g) -348.6 kJ/mol
Li(g) → Li+(g) + e– +520.2 kJ/mol
A) +1305.7 kJ/mol
B) +296.9 kJ/mol
C) -400.3 kJ/mol
D) -627.2 kJ/mol
39) Calculate the lattice energy for NaCl(s) using a Born-Haber cycle and the following information:
NaCl(s) → Na+(g) + Cl–(g) ?
Na(s) + 1/2 Cl2(g) → NaCl(s) -411.0 kJ/mol
Na(s) → Na(g) +107.3 kJ/mol
Na(g) → Na+(g) + e– +495.8 kJ/mol
1/2 Cl2(g) → Cl(g) +121.7 kJ/mol
Cl(g) + e– → Cl–(g) -348.6 kJ/mol
A) +34.8 kJ/mol
B) +690.3 kJ/mol
C) +787.2 kJ/mol
D) +1512 kJ/mol
40) Calculate the lattice energy for MgCl2(s) using a Born-Haber cycle and the following information:
MgCl2(s) → Mg2+(g) + 2 Cl–(g) ?
Mg(s) + Cl2(g) → MgCl2(s) -641.6 kJ/mol
Mg(s) → Mg(g) +147.1 kJ/mol
Mg(g) → Mg+(g) + e– +737.8 kJ/mol
Mg+(g) → Mg2+(g) + e– +1451.0 kJ/mol
1/2 Cl2(g) → Cl(g) +121.7 kJ/mol
Cl(g) + e– → Cl–(g) -348.6 kJ/mol
A) +641.6 kJ/mol
B) +1240.5 kJ/mol
C) +1882.1 kJ/mol
D) +2523.7 kJ/mol
41) Calculate the energy change for the formation of CaF2(s) from its elements in their standard states and
the following information:
Ca(s) + F2(g) → CaF2(s) ?
Ca(s) → Ca(g) +179.3 kJ/mol
Ca(g) → Ca+(g) + e– +589.9 kJ/mol
Ca+(g) → Ca2+(g) + e– +1145 kJ/mol
1/2 F2(g) → F(g) +79.0 kJ/mol
F(g) + e– → F–(g) -328.0 kJ/mol
CaF2(s) → Ca2+(g) + 2 F–(g) +2630 kJ/mol
A) +4046 kJ/mol
B) -965 kJ/mol
C) -1214 kJ/mol
D) -3286 kJ/mol
42) Calculate the lattice energy for MgO(s) using a Born-Haber cycle and the following information:
MgO(s) → Mg2+(g) + O2-(g) ?
Mg(s) → Mg(g) +147.1 kJ/mol
Mg(g) → Mg+(g) + e– +737.8 kJ/mol
Mg+(g) → Mg2+(g) + e– +1451 kJ/mol
1/2 O2(g) → O(g) +249.0 kJ/mol
O(g) + e– → O–(g) -141.1 kJ/mol
O–(g) + e– → O2-(g) +798.0 kJ/mol
Mg(s) + 1/2 O2(g) → MgO(s) -601.8 kJ/mol
A) +1842 kJ/mol
B) +2444 kJ/mol
C) +3844 kJ/mol
D) +4108 kJ/mol
43) Calculate the energy change in kJ/mol for the reaction using the following
information:
Li(g) → Li+(g) + e– +520 kJ/mol
F(g) + e– → F–(g) -328 kJ/mol
A) -848 kJ/mol
B) -192 kJ/mol
C) +192 kJ/mol
D) +848 kJ/mol
44) Calculate the energy change for the formation of MgBr2(s) from its elements in their standard states:
Mg(s) + Br2(l) → MgBr2(s) ?
Mg(s) → Mg(g) +147.1 kJ/mol
Mg(g) → Mg+(g) + e– +737.8 kJ/mol
Mg+(g) → Mg2+(g) + e– +1451 kJ/mol
Br2(l) → Br2(g) +30.9 kJ/mol
1/2 Br2(g) → Br(g) +112.0 kJ/mol
Br(g) + e– → Br–(g) -325.0 kJ/mol
MgBr2(s) → Mg2+(g) + 2Br–(g) +2440 kJ/mol
A) -150.8 kJ/mol
B) -286.0 kJ/mol
C) -499.2 kJ/mol
D) -5682 kJ/mol
45) Calculate the electron affinity for the formation of the hydride ion from the following information:
H(g) + e– → H–(g) ?
1/2 H2(g) → H(g) +217.9 kJ/mol
Na(s) → Na(g) +107.3 kJ/mol
Na(g) → Na+(g) + e– +495.8 kJ/mol
Na(s) + 1/2 H2(g) → NaH(s) -60.0 kJ/mol
NaH(s) → Na+(g) + H–(g) +810.9 kJ/mol
A) -50.1 kJ/mol
B) -70.1 kJ/mol
C) -816 kJ/mol
D) -1632 kJ/mol
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46) Which chemical process is associated with the lattice energy for sodium chloride?
A) NaCl(s) → Na+(g) + Cl–(g)
B) NaCl(g) → Na+(g) + Cl–(g)
C) Na(s) + 1/2 Cl2(g) → NaCl(s)
D) NaCl(s) + H2O(l) → Na+(aq) + Cl–(aq)
47) Which ionic compound would be expected to have the highest lattice energy?
A) Li2O
B) Na2O2
C) KO2
D) RbO2
48) Which element, indicated by letter on the periodic table above, has a 2+ ion with the electron
configuration [Ar]3d10?
A) A
B) B
C) C
D) D
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49) Which element, indicated by letter on the periodic table above, has a 1+ ion with the electron
configuration
A) A
B) B
C) C
D) D
50) Which element, indicated by letter on the periodic table above, has a 3+ ion with the electron
configuration [Kr]4d5?
A) A
B) B
C) C
D) D
51) Which element, indicated by letter on the periodic table above, has a 3+ ion with the electron
configuration
A) A
B) B
C) C
D) D
52) Which sphere represents the metal atom?
A) A
B) B
C) C
D) D
53) Which sphere represents the nonmetal atom?
A) A
B) B
C) C
D) D
54) Which sphere represents the monatomic anion?
A) A
B) B
C) C
D) D
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55) Which sphere represents the monatomic cation?
A) A
B) B
C) C
D) D
56) The following four spheres represent a Na atom, a Na+ ion, a Cl atom, and a Cl– ion, not necessarily in
that order. Use your knowledge about the relative sizes of atoms, cations, and anions to determine which
of the following sets of reactions is most consistent with the sizes of the atoms and ions shown below.
A) A → B + e– and C → D + e–
B) A → B + e– and D → C + e–
C) B → A + e– and C → D + e–
D) B → A + e– and D → C + e–
57) The following four spheres represent an Mg atom, an Mg2+ ion, a S atom, and a S2– ion, not
necessarily in that order. Use your knowledge about the relative sizes of atoms, cations, and anions to
determine which of the following sets of reactions is most consistent with the sizes of the atoms and ions
shown below.
A) A → B + 2e⁻ and C → D + 2e⁻
B) A → B + 2e⁻ and D → C + 2e⁻
C) B → A + 2e⁻ and C → D + 2e⁻
D) B → A + 2e⁻ and D → C + 2e⁻
The four spheres below represent Na+, Mg2+, F⁻, and O2–, not necessarily in that order.
58) Which sphere most likely represents the Na⁺ ion?
A) A
B) B
C) C
D) D
59) Which sphere most likely represents the Mg2+ ion?
A) A
B) B
C) C
D) D
60) Which sphere most likely represents the F– ion?
A) A
B) B
C) C
D) D
61) Which sphere most likely represents the O2- ion?
A) A
B) B
C) C
D) D