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Ch 26: More Practice

Total questions: 79

Worksheet time: 40mins

Name
Class
Date
1.

Identify the ion that is responsible for the red color of rubies.

a)

Cr3+

b)

Cr4+

c)

Cr5+

d)

Cr6+

e)

Cr7+

2.

Identify the ion that is responsible for the green color in emeralds.

a)

Cr3+

b)

Cr4+

c)

Cr5+

d)

Cr6+

e)

Cr7+

3.

Identify the ion that is responsible for the blue of turquoise.

a)

Cr2+

b)

Cu+

c)

Cu2+

d)

Cr3+

e)

Fe2+

4.

Identify the ion that is responsible for the red in garnet and the yellow-green of peridot.

a)

Cr2+

b)

Cu+

c)

Cu2+

d)

Cr3+

e)

Fe2+

5.

Choose the electron configuration for Fe3+.

a)

[Ar]4s23d3

b)

[Ar]3d5

c)

[Ar]4s23d9

d)

[Ar]4s13d4

6.

Identify the geometry of [Zn(NH₃)₄]²⁺.

a)

tetrahedral

b)

octahedral

c)

linear

d)

square planar

e)

trigonal planar

7.

Name the following: Fe[AlCl₆]

a)

ironaluminumhexachloride

b)

iron(II) hexachloroaluminum

c)

iron(III) hexachloroaluminate

d)

iron(II) aluminumhexachloride

e)

aluminumhexachloroferrate

8.

Name the following: [Ni(NH₃)₃(H₂O)₃]Cl₂

a)

nickel(II) trihydrotriamminechloride

b)

nickel(I) triamminetrihydrochloride

c)

dichloronickel(II) triamminetrihydride

d)

nickel(III) chloride

e)

triaminetriquanonickel(II) chloride

9.

Name the following: [Fe(CO)6][Ag(CN)2]2

a)

iron(III) hexacarbonylsilverdicyanide

b)

hexacarbonyliron(II) dicyanoargentate

c)

iron(II) carbonyl silvercyanide

d)

hexacarbonyliron(III) dicyanosilvate

e)

iron(II) hexacarbonyl silvercyanide

10.

Determine the chemical formula for the compound, diaquadicarbonylzinc tetrabromopalladate(IV).

a)

Pd[Zn(H2O)2(CO)2]Br4

b)

[Zn(H2O)2(CO)2]2[PdBr4]

c)

Pd(H2O)2[Zn(CO)2]Br4

d)

[Pd(H2O)2]2[Zn(CO)2]3Br4

e)

[Zn(H2O)2(CO)2][PdBr4]

11.

Determine the chemical formula for the compound, lithium tris(ethylenediamine)chromate(III).

a)

Li3[Cr(NH2CH2CH2NH2)3]

b)

[Li(NH2CH2CH2NH2)3]Cr3+

c)

[LiCr(NH2CH2CH2NH2)3]3+

d)

Li2[Cr(NH2CH2CH2NH2)4]

e)

Cr(NH2CH2CH2NH2)2]Li2

12.

Determine the chemical formula for the compound, tetracarbonylplatinum(IV) chloride.

a)

Pt(CO)4Cl2

b)

[Pt(CO)4]Cl4

c)

[Pt(CO)4Cl4]2-

d)

[PtCl4](CO)4

e)

[Pt(CO)4Cl4]4-

13.

Identify the isomers that have ligands with different spatial arrangements about the metal ions.

a)

linkage isomers

b)

geometric isomers

c)

coordination isomers

d)

optical isomers

e)

structural isomers

14.

Identify the isomers that have ligands which coordinate to metal in different ways.

a)

linkage isomers

b)

geometric isomers

c)

coordination isomers

d)

optical isomers

e)

stereoisomers

15.

Identify the isomers that occur when a coordinated ligand exchanges places with the uncoordinated counterion.

a)

linkage isomers

b)

geometric isomers

c)

coordination isomers

d)

optical isomers

e)

stereoisomers

16.

Identify the structure that cis-trans isomerism can occur in.

a)

MA₂B₄

b)

MAB₅

c)

MAB

d)

MA₃B₃

e)

MA₂B

17.

Identify the structure that fac-mer isomerism can occur in.

a)

MA₄B₂

b)

MA₅B

c)

MAB

d)

MA₃B₃

e)

MAB₂

18.

Identify the geometry of the complex ion if the hybridization is dsp².

a)

square planar

b)

octahedral

c)

tetrahedral

d)

linear

e)

trigonal planar

19.

Identify the geometry of the complex ion if the hybridization is d²sp³.

a)

square planar

b)

octahedral

c)

tetrahedral

d)

linear

e)

trigonal planar

20.

How many unpaired electrons would you expect for the complex ion: [Co(OH)6]3-?

a)

1

b)

2

c)

4

d)

0

e)

3

21.

How many unpaired electrons would you expect for the complex ion: [Fe(NH3)6]2+?

a)

5

b)

2

c)

6

d)

4

e)

0

22.

How many unpaired electrons would you expect for the complex ion: [Co(OH)6]4-?

a)

0

b)

5

c)

3

d)

1

e)

2

23.

How many unpaired electrons would you expect for the complex ion: [MnBr6]4-?

a)

2

b)

6

c)

4

d)

3

e)

0

24.

Identify the geometry around the Fe2+ ion in the hemoglobin complex.

a)

octahedral

b)

tetrahedral

c)

pentadral

d)

hexadral

e)

heptadral

25.

Identify the transition metal that is the coordinated metal in chlorophyll.

a)

magnesium

b)

iron

c)

calcium

d)

zinc

e)

chromium

26.

Identify the compound that is used to treat victims of heavy metal poisoning.

a)

KCN

b)

CO

c)

EDTA

d)

carbonic anhydrase

e)

cisplatin

27.

Identify the compound that is an effective anticancer agent.

a)

carbonic anhydrase

b)

CO

c)

EDTA

d)

transplatin

e)

cisplatin

28.

What is the highest possible oxidation state for cobalt?

a)

+2

b)

+7

c)

+6

d)

+4

e)

+5

29.

Choose the electron configuration for Zr²⁺.

a)

[Kr]5s²4d¹

b)

[Kr]5s²

c)

[Kr]4d²

d)

[Ar]5s¹4d¹

e)

[Kr]5s²4d⁵

30.

Choose the electron configuration for Nb4+.

a)

[Kr]5s14d2

b)

[Kr]5s24d3

c)

[Kr]5s24d1

d)

[Kr]4d1

e)

[Kr]5s24d5

31.

Choose the electron configuration for Fe5+.

a)

[Ne]3s23p6

b)

[Ar]4s13d2

c)

[Ar]4s23d1

d)

[Ar]4s23d7

e)

[Ar]3d3

32.

Choose the electron configuration for Ti2+.

a)

[Ar]3d2

b)

[Ar]4s23d2

c)

[Ar]4s23d4

d)

[Ar]4s2

e)

[Ne]3s23p6

33.

What is the ground-state electron configuration for the element vanadium (Z = 23)?

a)

[Ne] 4s1 3d4

b)

[Ar] 4s1 3d4

c)

[Ar] 4s2 3d3

d)

[Ar] 3d5

34.

What is the ground-state electron configuration for Co²⁺ (Z = 27)?

a)

[Ar] 4s² 3d⁹

b)

[Ar] 4s² 3d⁵

c)

[Ar] 3d⁷

d)

[Ar] 4s¹ 3d⁶

35.

Which of the following species has the electron configuration [Ar]3d³?

a)

Sc

b)

Cr³⁺

c)

V³⁺

d)

Fe³⁺

36.

How many d electrons are in CrO₄²⁻?

a)

0

b)

1

c)

2

d)

3

37.

Which of the following can function as a bidentate ligand?

a)

O₂

b)

OH⁻

c)

SCN⁻

d)

H₂NCH₂CH₂NH₂

38.

Which of the following can function as a chelating agent?

a)

SH⁻

b)

CO

c)

H₂NCH₂CO₂⁻

d)

NCS⁻

39.

Choose the bidentate ligand from the substances below.

a)

oxalate ion

b)

EDTA

c)

fluoride ion

d)

ammonia

40.

Choose the polydentate ligand from the substances below.

a)

thiocyanate ion

b)

EDTA

c)

nitrate ion

d)

hydroxide ion

e)

water

41.

Identify the geometry of [PdCl4]2-.

a)

tetrahedral

b)

square planar

c)

linear

d)

octahedral

e)

trigonal bipyramidal

42.

Identify the geometry of [Ag(NH3)2]+.

a)

tetrahedral

b)

square pyramidal

c)

linear

d)

bent

e)

trigonal planar

43.

Identify the geometry of [Cr(H₂O)₆]³⁺.

a)

tetrahedral

b)

square pyramidal

c)

bent

d)

octahedral

e)

trigonal pyramidal

44.

How many moles of aqueous ions will be produced from the dissolution of 1.0 mole of Li₃[FeCl₆] in water?

a)

4

b)

10

c)

2

d)

6

e)

1

45.

Name the following: [Pt(H₂O)₄I₂]Br

a)

tetraaquadiodoplatinum(II) bromide

b)

diiodotetrahydroplatinium bromide

c)

diiodotetrahydroplatinum(II) bromide

d)

tetraaquadiiodoplatinum(II) bromide

e)

platinum(III) diiodotetraaquabromide

46.

Name the following: [Pt(H₂O)₄Br₂]I₂

a)

tetraaquadibromoplatinum(IV) iodide

b)

tetraaquadibromoplatinate diiodide

c)

platinum(II) iodide

d)

platinum(III) tetraaquadibromoiodide

e)

platinum(II) dibromotetrahydride diiodide

47.

Determine the chemical formula for the compound, diaminetetraaquanickel(II) iodide.

a)

[Ni(NH3)2(H2O)4]I

b)

[Ni(NH3)2][(H2O)4I]

c)

[Ni(NH3)2(H2O)4]I2

d)

[Ni(H2O)4][(NH3)2I]

e)

[Ni(NH3)2[(H2O)4]I3

48.

Determine the chemical formula for the compound, hexamminechromium(III) hexacyanochromate(III).

a)

[Cr2(NH3)6(CN)6]3+

b)

[Cr(NH3)6][Cr(CN)6]2

c)

[Cr(NH3)6]3[Cr(CN)6]2

d)

[Cr(NH3)6][Cr(CN)6]

e)

[Cr2(NH3)3(CN)3]6+

49.

Which of the following pairs of coordination compounds or complex ions are examples of coordination isomers?

a)

[Fe(NH3)5NO2]2+ and [Fe(NH3)5ONO]2+

b)

[Fe(NH3)2(H2O)4]F2 and [Fe(NH3)2(H2O)4]I2

c)

[Fe(NH3)2(H2O)4]Br2 and [Fe(NH3)4(H2O)2]Br2

d)

[Cu(CO)5]IF and [Cu(CO)5]FI

e)

[MnClBr3]2- and [MnClBr3]2-

50.

Which of the following pairs of coordination compounds or complex ions are examples of linkage isomers?

a)

[Cu(NH3)5Br]Cl and [Cu(NH3)5Cl]Br

b)

[Fe(NH3)2(H2O)4]Br2 and [Fe(NH3)4(H2O)2]Br2

c)

[Mn(CO)5NO2]2+ and [Mn(CO)5ONO2]2+

d)

[Fe(NH3)2(H2O)4]Br2 and [Fe(NH3)2(H2O)4]I2

e)

[V(H2O)6]3+ and [V(NH3)6]3+

51.

Which of the following compounds can exhibit cis-trans isomerism?

a)

[Cr(CO)5NO2]2+

b)

[Zn(CO)5Br]+

c)

[MnClBr3]2-

d)

[Fe(H2O)6]3+

52.

Which of the following compounds can exhibit cis-trans isomerism?

a)

[Cr(H₂O)₄Br₂]⁺

b)

[Cu(CO)₅Cl]⁺

c)

[Cr(CO)₃(NH₃)₃]³⁺

d)

[Fe(CO)₅ONO]²⁺

e)

[Ni(NH₃)₆]²⁺

53.

Which of the following compounds can exhibit fac-mer isomerism?

a)

[Cu(CO)₅I]⁺

b)

[Ni(H₂O)₃(CO)₃]³⁺

c)

[Co(CO)₅NO₂]²⁺

d)

[Ti(NH₃)₂(H₂O)₄]²⁺

e)

[Cr(H₂O)₄Cl₂]⁺

54.

Which of the following compounds can exhibit fac-mer isomerism?

a)

[Cr(H₂O)₄I₂]⁺

b)

[Fe(CO)₅ONO]²⁺

c)

[Fe(CO)₃(NH₃)₃]³⁺

d)

[Cu(CO)₅F]⁺

e)

[V(NH₃)₄(H₂O)₂]²⁺

55.

Which ion would you expect to have the largest crystal field splitting Δ?

a)

[Co(NO₂)₆]⁴⁻

b)

[Co(NO₂)₆]³⁻

c)

[Co(NH₃)₆]²⁺

d)

[Co(NH₃)₆]³⁺

e)

[Co(Cl)₆]³⁻

56.

Which of the following species is diamagnetic?

a)

an isolated, gas-phase Mn2+ ion

b)

a high-spin octahedral Co2+ complex

c)

an isolated, gas-phase Cu2+ ion

d)

a low-spin octahedral Rh3+ complex

57.

What type of hybridization (according to valence bond theory) does Co exhibit in the complex ion, [Co(H2O)4(Br)2]+?

a)

dsp3

b)

sp3

c)

d2sp2

d)

d2sp3

e)

d2sp

58.

What type of geometry (according to valence bond theory) does Mn exhibit in the complex ion, [Mn(H2O)4I2]+?

a)

linear

b)

trigonal planar

c)

square pyramidal

d)

octahedral

e)

tetrahedral

59.

What type of hybridization (according to valence bond theory) does Pt exhibit in the complex ion, [Pt(NH3)4]2+?

a)

dsp

b)

sp3

c)

d2sp2

d)

d sp

e)

dsp2

60.

What type of geometry (according to valence bond theory) does Ni exhibit in the complex ion, [Ni(NH3)4]2+?

a)

square bipyramidal

b)

see-saw

c)

trigonal planar

d)

bent

e)

square planar

61.

How many unpaired electrons would you expect for the complex ion: [Co(H2O)6]4+?

a)

6

b)

1

c)

4

d)

2

e)

3

62.

Identify the transition metal that is used in oxygen transport in the human body.

a)

zinc

b)

iron

c)

lithium

d)

copper

e)

gold

63.

Identify the transition metal that is used in hemoglobin synthesis in the human body.

a)

potassium

b)

zinc

c)

molybdenum

d)

manganese

e)

silver

64.

Identify the transition metal that is used in fat and carbohydrate synthesis in the human body.

a)

sodium

b)

zinc

c)

copper

d)

manganese

e)

chromium

65.

Which of the following pairs of complexes is an example of linkage isomerism?

a)

[Ni(CN)2(OH)2]2-

b)

[Cu(SCN)4]3- and [Cu(NCS)4]3-

c)

[Zn(NH3)2Cl2]Br2 and [Zn(NH3)2Br2]Cl2

d)

[Cr(NH3)3(CO)3]3+

66.

Which of the following is an example of a coordination isomer?

a)

[Cr(en)3]3+

b)

[Cu(SCN)4]3- and [Cu(NCS)4]3-

c)

[Zn(NH3)2Cl2]Br2 and [Zn(NH3)2Br2]Cl2

d)

[Cr(NH3)3(CO)3]3+

67.

Which of the following complexes exhibits cis-trans isomerism?

a)

[Ni(CN)2(OH)2]2-

b)

[Cu(SCN)4]3- and [Cu(NCS)4]3-

c)

[Zn(NH3)2Cl2]Br2 and [Zn(NH3)2Br2]Cl2

d)

[Cr(NH3)3(CO)3]3+

68.

Which of the following complexes exhibits mer-fac isomerism?

a)

[Cr(en)3]3+

b)

[Cu(SCN)4]3- and [Cu(NCS)4]3-

c)

[Zn(NH3)2Cl2]Br2 and [Zn(NH3)2Br2]Cl2

d)

[Cr(NH3)3(CO)3]3+

69.

Which of the following complexes exhibits optical isomerism?

a)

[Cr(en)3]3+

b)

[Cu(SCN)4]3- and [Cu(NCS)4]3-

c)

[Zn(NH3)2Cl2]Br2 and [Zn(NH3)2Br2]Cl2

d)

[Cr(NH3)3(CO)3]3+

70.

What is the Lanthanide contraction?

a)

It is the explanation for why the 6th period transition elements are about the same size as the 5th period transition elements.

b)

It is the process by which transition metals lose their outer s electrons.

c)

It is the formation of a covalent bond through sharing of electrons.

d)

It is the splitting of d-orbital energies in a complex.

71.

Why is +2 a common oxidation state for transition elements?

a)

Because transition metals lose their outer s electrons before losing any of their d electrons.

b)

Because transition metals gain two electrons in chemical reactions.

c)

Because transition metals have a full d-orbital.

d)

Because transition metals form covalent bonds with two other atoms.

72.

What is a coordinate covalent bond?

a)

A bond formed when one atom donates both electrons to a shared pair in a bond.

b)

A bond formed by the equal sharing of electrons between two atoms.

c)

A bond formed by the transfer of electrons from one atom to another.

d)

A bond formed by the overlap of p-orbitals.

73.

What is the difference between a weak-field complex and a strong-field complex?

a)

In a weak-field complex, d-orbitals split with a small energy difference; in a strong-field complex, d-orbitals split with a large energy difference.

b)

In a weak-field complex, electrons are transferred; in a strong-field complex, electrons are shared.

c)

In a weak-field complex, the central atom is a nonmetal; in a strong-field complex, the central atom is a metal.

d)

In a weak-field complex, the ligands are always neutral; in a strong-field complex, the ligands are always charged.

74.

Explain how EDTA is used to treat lead poisoning.

a)

EDTA forms a complex with calcium, and lead displaces the calcium due to a higher formation constant, allowing the lead/EDTA complex to be excreted.

b)

EDTA directly breaks down lead in the bloodstream.

c)

EDTA increases the absorption of calcium, which then binds to lead.

d)

EDTA oxidizes lead to a less toxic form.

75.

Determine the oxidation state and coordination number of the molybdenum metal ion in the complex ion [Mo(H2O)6]3+.

a)

Oxidation state = +2, coordination number = 6

b)

Oxidation state = +1, coordination number = 1

c)

Oxidation state = +3, coordination number = 6

d)

Oxidation state = +2, coordination number = 2

e)

Oxidation state = +3, coordination number = 4

76.

Determine the oxidation state and coordination number of the ruthenium metal ion in the complex ion [Ru(NH3)3Br3]–.

a)

Oxidation state = +2, coordination number = 6

b)

Oxidation state = +1, coordination number = 1

c)

Oxidation state = +3, coordination number = 6

d)

Oxidation state = +2, coordination number = 2

e)

Oxidation state = +3, coordination number = 4

77.

Determine the oxidation state and coordination number of the copper metal ion in the complex ion [Cu(NH3)2]+.

a)

Oxidation state = +2, coordination number = 2

b)

Oxidation state = +1, coordination number = 2

c)

Oxidation state = +1, coordination number = 2

d)

Oxidation state = +1, coordination number = 1

e)

Oxidation state = +3, coordination number = 2

78.

Determine the oxidation state and coordination number of the osmium metal ion in the complex ion [Os(CN)6]4–.

a)

Oxidation state = +2, coordination number = 6

b)

Oxidation state = +1, coordination number = 5

c)

Oxidation state = +3, coordination number = 6

d)

Oxidation state = +2, coordination number = 5

79.

Determine the oxidation state and coordination number of the platinum metal ion in the complex ion [PtBr4]2–.

a)

Oxidation state = +2, coordination number = 3

b)

Oxidation state = +2, coordination number = 5

c)

Oxidation state = +3, coordination number = 6

d)

Oxidation state = +2, coordination number = 4

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