60) Which of the following cannot form both high- and low-spin octahedral complexes?
A) MN2+
B) V2+
C) Co3+
D) Cr2+
E) All of the above can form both high- and low-spin complexes.
61) Which of the following can form both high- and low-spin octahedral complexes?
A) Cr2+
B) Cr3+
C) Zn2+
D) Cu+
E) All of the above can form either high- or low-spin complexes.
62) How many d electrons are associated with the metal ion in [Cr(NH3)6]3+?
A) 1
B) 2
C) 3
D) 4
E) 5
23.2 Bimodal Questions
1) The coordination numbers of cobalt(III) and of chromium(III) in their complexes are always
__________.
A) 4
B) 5
C) 2
D) 3
E) 6
15
2) The coordination number of platinum in complexes is always __________.
A) 4
B) 5
C) 2
D) 3
E) 6
3) During the formation of a coordination compound, the metal acts as a __________.
A) Lewis acid
B) Br∅nsted acid
C) Arrhenius acid
D) Br∅nsted base
E) Lewis base
4) During the formation of a coordination compound, ligands act as __________.
A) Lewis bases
B) Arrhenius bases
C) Br∅nsted bases
D) Lewis acids
E) Arrhenius acids
5) The coordination sphere of a complex consists of __________.
A) the central metal ion only
B) the ligands
C) the central metal ion and the ligands bonded to it
D) the primary and secondary valencies
E) coordination and steric numbers
6) In the following reaction, Ni2+ is acting as a(n) __________.
Ni2+ (g) + 6H2O (l) → Ni(H2O)62+ (aq)
A) oxidizing agent
B) Lewis acid
C) precipitating agent
D) solvent
E) ligand
7) How many d electrons are in the cobalt ion of K3[Co(CN)6]?
A) 3
B) 5
C) 6
D) 7
E) 4
8) What is the charge on the complex ion in Mg2[FeCl6]?
A) 2-
B) 2+
C) 3-
D) 3+
E) 4-
9) What is the oxidation number of chromium in [Cr(NH3)4Cl2]Cl?
A) -3
B) +3
C) +2
D) -2
E) 0
10) What is the ligand in Ca3[Fe(CN)6]2?
A) Ca2+
B) Fe3+
C) CN–
D) Fe(CN)63-
E) Fe2+
11) What is the charge of the central metal ion in Ca3[Fe(CN)6]2?
A) 0
B) 1+
C) 2+
D) 3+
E) 6+
12) What is the oxidation number of cobalt in [Co(NH3)4F2]?
A) -3
B) +2
C) +1
D) +3
E) +6
13) The charge of the complex ion in [Zn(H2O)3Cl]Cl is __________.
A) 0
B) 1-
C) 2+
D) 1+
E) 2-
14) The coordination number for [Zn(H2O)3Cl]Cl is __________.
A) 5
B) 4
C) 2
D) 1
E) 6
15) What is the oxidation state of iron in CaNa[Fe(CN)6]?
A) 0
B) +2
C) +3
D) +4
E) +6
16) What is the oxidation state of iron in K3[Fe(CN)6]?
A) 0
B) +2
C) +3
D) +4
E) +6
18
17) What is the coordination number of iron in CaNa[Fe(CN)6]?
A) 2
B) 8
C) 4
D) 6
E) 12
18) What is the coordination number of cobalt in [Co(NH3)5Cl](NO3)2?
A) 12
B) 8
C) 4
D) 2
E) 6
19) What is the oxidation state of cobalt in [Co(NH3)5Cl](NO3)2?
A) 0
B) 2
C) 3
D) 4
E) 6
20) What is the oxidation state of chromium in [Cr(H2O)4Cl2]+?
A) 0
B) +2
C) +3
D) -2
E) -3
21) What is the coordination number of chromium in [Cr(H2O)4Cl2]+?
A) 8
B) 6
C) 4
D) 2
E) 12
22) The “dentation” of a ligand is defined by __________.
A) how many “dents” or “deceptions” there are in the coordination sphere of a complex species it forms
B) how many electron donor atoms it utilizes to form coordinate bonds to the central metal ion
C) the total number of lone pairs of electrons it possesses
D) how many metal ions it can sequester from solution
E) none of the above
23) EDTA is __________-dantate ligand.
A) mono
B) bi
C) tri
D) tetra
E) hexa
24) What is the metal ion in the porphyrin of heme?
A) iron
B) calcium
C) molybdenum
D) magnesium
E) chlorophyll
25) How many iron atoms are coordinated in a hemoglobin molecule?
A) 1
B) 2
C) 3
D) 4
E) 5
26) The correct name for [Ni(NH3)6](NO3)3 is __________.
A) dinitrohexaamminenickel (II)
B) hexaamminenickel (III) trinitrate
C) dinitrohexaamminenickelate (III)
D) hexaamminenickel (II) nitrate
E) hexaamminenickel (III) nitrate
27) The correct name for [Cu(NH3)4(H2O)2]+2 is __________.
A) diwaterquatraamminecopper (II)
B) tetraamminediaquacopper (II)
C) diaquatetraammoniumcopper (II)
D) tetraamminecopper (II) dihydrate
E) none of the above
28) The correct name for [Al(H2O)2(OH–)4]– is __________.
A) diwaterquatrahydroxyaluminum
B) tetrahydroxydiaquaaluminum (III)
C) diaquatetrahydroxoaluminate
D) aluminum (IV) hydroxide dihydrate
E) none of the above
29) The correct name for [Co(NH3)5Cl]Cl2 is __________.
A) pentaaminechlorocobalt(III) chloride
B) chloropentaammoniacobalt (II) chloride
C) pentaammoniachlorocobalt(II) chloride
D) cobalt(III) pentaamino trichloride
E) none of the above
30) The names of complex anions end in __________.
A) -o
B) -ium
C) -ate
D) -ous
E) –ic
31) The correct name for Na3[CoF6] is __________.
A) trisodium hexakisfluorocobalt(III)
B) trisodium hexakisfluorocobalt(II)
C) trisodium hexakisfluorocobalt(IV)
D) sodium hexafluorocobaltate(III)
E) sodium hexafluorocobaltate(IV)
21
32) Triphenylphosphine is often given the abbreviated formula PPh3. The correct name for
Rh(PPh3)3Cl is __________.
A) chlorotriphenylphosphinerhodium
B) chlorotriphenylphosphinerhodium(I)
C) tris(triphenylphosphine)chlororhodium(I)
D) chlorotris(triphenylphosphine)rhodium(I)
E) chlorotris(triphenylphosphine)rhodate(-I)
33) In __________, the bonds are the same but the spatial arrangement of the atoms is different.
A) structural isomers
B) linkage isomers
C) coordination-sphere isomers
D) stereoisomers
E) resonance structures
34) A geometrical isomer with like groups located on opposite sides of the metal atom is denoted with
the prefix __________.
A) cis-
B) trans-
C) bis-
D) tetrakis-
E) d-
35) The complex [Zn(NH3)2Cl2]2+ does not exhibit cis-trans isomerism. The geometry of this complex
must be __________.
A) tetrahedral
B) trigonal bipyramidal
C) octahedral
D) square planar
E) either tetrahedral or square planar
36) How many isomers exist for the octahedral complex ion [Co(NH3)4F2]+?
A) 1
B) 2
C) 3
D) 4
E) 5
37) Trans-[Fe(H2O)2Cl4]2- must be __________.
A) tetrahedral
B) octahedral
C) square planar
D) trigonal bipyramidal
E) linear
38) Linkage isomerism can only occur __________.
A) in cis-isomers of octahedral complexes
B) with cobalt complexes
C) with coordination number 6
D) with tetrahedral complexes
E) with ligands that have more than one possible donor atom
39) Metals with __________ electron configurations characteristically form diamagnetic, square planar
complexes.
A) d0
B) d9
C) d6
D) d8
E) d10
23.3 Short Answer Questions
1) Draw a diagram of the short-hand ground state electron configuration of zinc.
2) Most transition metal ions contain partially occupied __________ subshells.
3) A substance is __________ if its ions or atoms have one or more unpaired electrons.
4) The two more common oxidation states of chromium are __________ and __________.
5) __________ arises when the unpaired electrons of the atoms or ions in a solid are influenced by the
orientations of the electrons of their neighbors.
6) What is the oxidation state of the iron atom in CaNa[Fe(CN)6]?
7) The most common coordination numbers are __________.
8) What is the coordination number of the iron atom in CaNa[Fe(CN)6]?
9) Six-coordinate complexes generally have __________ geometry.
10) The number of “free” chloride ions in an ionic coordination compound can be determined by treating
the compound with __________.
11) The secondary valence in metal ion complexes is called the __________.
12) Werner’s theory of primary and secondary valences for transition metal complexes has given us the
concepts of __________ and __________.
13) Transition metal ions with empty valence orbitals act as __________.
14) What is the oxidation number of the central metal in [Mo(H2O)5NO3]Cl2
15) Define the chelate effect.
16) The chelate effect is enhanced by polydentate ligand binding because of the change in __________.
17) List three of the ten transition metals required for human life.
18) Myoglobin has __________ heme group(s) that bind(s) __________.
19) In photosynthesis, __________ moles of photons are required to form one mole of __________.
20) In the leaves of plants, visible light is absorbed by a compound known as __________, and is aided
by a __________ ion bonded to a porphyrin ring.
21) What is the mechanism used in humans to combat blood bacterial growth via deprivation of iron?
22) A large difference in formation constant (Kf) of a poly- versus monodentate ligand is called
__________.
23) A compound that can occupy two coordination sites is a (an) __________.
24) The porphyrin compound that contains Mg(II) is called __________.
25) The transport of iron into bacteria is facilitated by the formation of the complex __________.
26) Name the compound: K2[Cr(H2O)4(CO3)2]
27) Name Na[Ru(H2O)2(C2O4)2].
28) Two compounds have the same formula and contain an SCN– ligand. In one compound the SCN–
ligand is bonded to the metal atom via the N atom and in the other it is bonded via the S atom. These
two compounds are examples of __________ isomers.
29) Non superimposable isomers are __________ isomers.
30) How can high-spin and low-spin transition metal complexes be distinguished from each other?
23.4 True/False Questions
1) If chloride is a ligand to a transition metal it will not be precipitated by silver nitrate.
2) The chelate effect must always occur with positive enthalpy change.
3) The color of hemoglobin changes from purple to red when water displaces oxygen on the molecule.
4) The heme unit of myoglobin is bound to the protein via a nitrogen-containing ligand.
5) To separate racemic mixtures the isomers must be in a chiral environment.
6) Green and orange are complementary colors.
7) The energy of a metal ligand complex is higher than the energy of the separated components.
23.5 Essay Questions
1) What is the purpose of adding sodium tripolyphosphate to a detergent?
2) What colors of light does chlorophyll-a absorb?
3) How does an elevated body temperature deprive some bacteria in the body of iron?
4) What is a siderophore?
5) What is meant by the prefix tetrakis-, and when is it used?
6) Name the compound, Ca[AlH4]2.
7) Name the compound, [Os(en)3]2[NiCl2Br2]3.
8) Name the compound, Cu(H2O)42+.
9) In what two ways can an object appear blue?