CHEM 1332 CHAPTER 22
1.
Transition elements and inner transition elements each have a common oxidation state for their
ions. What are they (transition and inner transition, respectively)?
(A)
+2, +3
2.
The ground state electronic configuration of Cr2+ is
(A)
[Ar]4s13d 5
3.
The ground state electronic configuration of Cd2+ is:
(A)
[Kr]5s24d 8
4.
Which of the following atoms has the biggest radius?
(A)
Ti
5.
A certain transition element has the stable oxidation states of +2, +4, +5, and +6. In which state
will the element be most electronegative?
(A)
+2
6.
A certain transition element has the stable oxidation states of +2, +3, +5, and +6. In which state
will the element be most likely to form an ionic bond with chlorine?
(A)
+2
7.
Which of the following transition elements will form an ion with the largest oxidation number?
(A)
(C)
chromium, Cr, Group 6B(6)
iron, Fe, Group 8B(8)
8.
Which of the following ions is most likely to form colored compounds?
(A)
Sc3+
9.
Which of the following ions is least likely to form colored compounds?
(A)
Mn2+
10.
Which of the following will be paramagnetic?
(A)
V5+
11.
What is the highest possible oxidation state for molybdenum, Mo?
(A)
+2
(B)
(B)
(B)
(B)
Cr
(B)
(B)
(B)
(B)
(B)
(B)
+3, +2
(C)
[Ar]4s23d 4
[Kr]5s24d10
(C)
+4
+4
Cu+
Cr5+
Ni2+
+4
Fe
(C)
(C)
(D)
(C)
(C)
(B)
(D)
(C)
(C)
(C)
(C)
+2, +2
[Ar]3d 4
[Kr]5s14d 9
Ni
+5
+5
(E)
(D)
+3, +3
(D)
[Ar]4s13d 3
(D)
[Kr]4d10
Zn
(D)
(D)
+6
+6
manganese, Mn, Group 7B(7)
cobalt, Co, Group 8B(9)
Zn2+
Sc3+
Mn7+
+6
1
(D)
Cr3+
(D)
Fe3+
(D)
Ti4+
(D)
+8
12.
Which of the following will be the strongest oxidizing agent?
(A)
Cr
13.
Which of the oxidation states of chromium has the largest valence-state electronegativity?
(A)
Cr(II)
14.
A certain transition metal complex has the formula MX42+. If the metal ion has a d 8 electron
configuration, what is the shape of the complex?
(A)
octahedral
15.
Which of the following is considered a bidentate ligand?
(A)
(C)
cyanide, CNoxalate, C2O42-
16.
A characteristic of ligands is that
(A)
(C)
they are Lewis acids
they are ions
17.
What is the coordination number of cobalt in the complex ion [Co(en)Cl4]-? (en = ethylene
diamine)
(A)
8
18.
The oxidation and coordination numbers of cobalt in the compound [Co(NH3)5Cl]Cl2 are,
respectively
(A)
2 and 6
19.
In the compound K[Co(C2O4)2(H2O)2] (where C2O42- = oxalate) the oxidation number and
coordination number of cobalt are, respectively:
(A)
-1 and 4
20.
In the compound [Ni(en)2(H2O)2]SO4 (where en = ethylene diamine) the oxidation number and
coordination number of nickel are, respectively:
(A)
2 and 6
21.
Give the systematic name for [Cu(NH3)4]Cl2.
(A)
(C)
dichlorotetraamminecuprate(II)
copper(II)ammonium chloride
(B)
(B)
(B)
(B)
(B)
(B)
(B)
Cr(II)
Cr(III)
(C)
(C)
square planar (C)
2
2 and 8
-1 and 6
4 and 6
Cr(III)
Cr(IV)
tetrahedral
(D)
(D)
(D)
Cr(VI)
Cr(VI)
trigonal pyramid
(B)
(D)
thiocyanate, SCNnitrite, NO2-
(B)
(D)
they are Lewis bases
they are electron pair acceptors
(C)
(C)
(C)
(C)
(B)
(D)
4
3 and 6
3 and 4
6 and 6
(D)
(D)
(D)
(D)
6
3 and 8
3 and 6
2 and 4
tetraamminecopper(II) chloride
tetraaminocopper(II) chloride
2
22.
Give the systematic name for Cr(CO)3(NH3)3.
(A)
(C)
chromiumtriaminotricarbonyl
triamminetricarbonylchromate(0)
23.
Give the systematic name for [CoCl3(H2O)]-.
(A)
(C)
cobalt(II) chloride monohydrate
aquatrichlorocobaltate(II)
24.
Write the formula for pentaamminechlorocobalt(III) chloride.
(A)
(C)
[Co(NH3)5Cl]Cl
[Co(NH3)5Cl]Cl3
25.
Write the formula for diamminedichloroethylenediaminecobalt(III) bromide.
(A)
(C)
[CoCl2(en)(NH3)2]Br
[CoCl2(en)2(NH3)2]Br
26.
Write the formula for sodium tetracyanonickelate(II).
(A)
Na[Ni(CN)4] (B)
27.
Which of the following could not participate in linkage isomerism?
(A)
NO2-
28.
Which of the following species could exist as isomers?
(A)
(C)
[Co(H2O)4Cl2]+
[Pt(en)Cl2]
29.
According to valence bond theory, what would be the set of hybrid orbitals used when a Period 4
transition metal forms a tetrahedral complex?
(A)
d 2 sp
30.
According to Valence Bond theory, in the square planar Ni(CN)42- complex ion, the orbital
hybridization pattern is
(A)
sp3
31.
The crystal field splitting energy, Δ,
(A)
(B)
(C)
(D)
is larger for tetrahedral complexes than for octahedral complexes
depends on the metal but not on the ligand
determines the color of a complex
is larger for ionic ligands like chloride than for molecular ligands like CO
(B)
(B)
(B)
(B)
(D)
(B)
(D)
(B)
(D)
(B)
(D)
Na[Ni(CN)4]2
NCO-
dsp2
aquatrichlorocobalt(II)
aquatrichlorocobaltite(I)
[Co(NH3)5Cl]Cl2
[Co(NH3)5Cl]Cl4
[CoCl2(en)(NH3) 2]Br2
[CoCl2(en)2(NH3) 2]Br2
(C)
(C)
(B)
(D)
dsp2
triamminechromium carbonate
triamminetricarbonylchromium(0)
(C)
(C)
Na2[Ni(CN)4] (D)
OH-
(D)
Na4[Ni(CN)4]
NCS-
[Pt(NH3)Br3][Pt(NH3)3Cl]+
dsp3
d 2 sp
3
(D)
(D)
sp3
d 2 sp3
32.
In the spectrochemical series, which one of the following ligands has the strongest field?
(A)
H2O
33.
Which of the following ions could exist in either the high-spin or low-spin state in an octahedral
complex?
(A)
Sc3+
34.
Which of the following ions could exist in only the high-spin state in an octahedral complex?
(A)
Cr2+
35.
In the presence of a strong octahedral ligand field, the number of unpaired electrons in Co(III) will
be
(A)
0
36.
Which of the following octahedral complexes should have the largest crystal field splitting energy,
Δ?
(A)
[Cr(H2O) 6]3+ (B)
37.
Which of the following ligands is most likely to form a low-spin octahedral complex with
iron(III)?
(A)
Cl-
38.
Which of the following ligands is most likely to form a high spin octahedral complex with
cobalt(II)?
(A)
CN-
39.
Iron(III) forms an octahedral complex with the ligand CN-. How many unpaired electrons are in
the d-orbitals of iron?
(A)
1
40.
In a high-spin octahedral complex, the number of unpaired electrons in Ni(II) will be
(A)
0
41.
If a solution absorbs green light, what is its likely color?
(A)
red
(B)
(B)
(B)
(B)
(B)
(B)
(B)
(B)
(B)
CN-
(C)
Ni2+
(C)
Mn4+
(C)
2
(C)
[Cr(SCN)6]3- (C)
H2O
(C)
I-
(C)
3
(C)
4
violet (C)
(C)
orange
NH3
(D)
Mn2+
(D)
Fe3+
(D)
4
(D)
[Cr(NH3) 6]3+ (D)
CO
(D)
NO2-
(D)
5
(D)
2
(D)
(D)
yellow
OH-
Ti4+
Co3+
6
[Cr(CN) 6]3-
OH-
CO
7
6
(E)
blue
A C D A D |A B D C B | C D D B C | B D C D A| B D C B A | C C A D B | C B C B A |D C B A C | A
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