Chapter 24 1 Identify the ion that is responsible for the red color

Chemistry: A Molecular Approach, 2e (Tro)

Chapter 24 Transition Metals and Coordination Compounds

Multiple Choice Questions

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

E) [Ar]4s23d6

Answer: B

Diff: 2 Page Ref: 24.2

6) Name the following: Fe[AlF6]

A) ironaluminumhexafluoride

B) iron(II) hexafluoroaluminum

C) iron (III) hexafluoroaluminate

D) iron(I) aluminumhexafluoride

E) aluminumhexafluoroferrate

7) Name the following: [Fe(H2O)4Br2]Cl

A) tetraaquadibromoiron(II) chloride

B) dibromotetrahydroironchloride

C) dibromotetrahydroiron(II)chloride

D) tetraaquadibromoiron(III) chloride

E) iron(II)dibromotetraquachloride

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) triamminetriaquanickel(II)chloride

9) Name the following: [Pt(H2O)4F2]Br2

A) tetraaquadifluoroplatinum(IV) bromide

B) tetraaquadibromodifluoroplatinate

C) platinum(II)bromide

D) platinum(III)tetraaquadifluorobromide

E) platinum (II) dibromodifluorotetrahydride

10) 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

11) Determine the chemical formula for the compound, diamminetetraaquairon(II)chloride.

A) [Fe(NH3)2(H2O)4Cl]

B) [Fe(NH3)2][(H2O)4Cl]

C) [Fe(NH3)2(H2O)4]Cl2

D) [Fe(H2O)4][(NH3)2Cl]

E) [Fe(NH3)2(H2O)4]Cl3

12) Determine the chemical formula for the compound, hexaammineiron(III) hexacyanoferrate(III).

A) [Fe2(NH3)6(CN)6]3+

B) [Fe(NH3)6][Fe(CN)6]2

C) [Fe(NH3)6]3[Fe(CN)6]2

D) [Fe(NH3)6][Fe(CN)6]

E) [Fe2(NH3)3(CN)3]6+

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

A) [PdZn(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]

14) Determine the chemical formula for the compound, potassiumtrisethylenediamine chromate(III).

A) K3[Cr(NH2CH2CH2NH2)3]

B) [K(NH2CH2CH2NH2)3]Cr3+

C) [KCr(NH2CH2CH2NH2)3]3+

D) K2[Cr(NH2CH2CH2NH2)4]

E) [Cr(NH2CH2CH2NH2)2]K2

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

A) [Pt(CO)4]Cl2

B) [Pt(CO)4]Cl4

C) [Pt(CO)4Cl4]2-

D) [PtCl4](CO)4

E) [Pt(CO)4Cl4]4-

16) 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

17) Identify the isomers that have ligands which coordinates to metal in different ways.

A) linkage isomers

B) geometric isomers

C) coordination isomers.

D) optical isomers

E) stereoisomers.

18) Which of the following pairs of coordination compounds or complex ions are examples of

coordination isomers?

A) [Fe(CO)5NO2]2+ and [Fe(CO)5ONO]2+

B) [Fe(NH3)2(H2O)4]Cl2 and [Fe(NH3)2(H2O)4]Br2

C) [Fe(NH3)2(H2O)4]Cl2 and [Fe(NH3)4(H2O)2]Cl2

D) [Cu(CO)5Br]Cl and [Cu(CO)5Cl]Br

E) [MnCl3Br]2- and [MnClBr3]2-

19) 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]Cl2 and [Fe(NH3)4(H2O)2]Cl2

C) [Fe(CO)5NO2]2+ and [Fe(CO)5ONO]2+

D) [Fe(NH3)2(H2O)4]Cl2 and [Fe(NH3)2(H2O)4]Br2

E) [Cr(H2O)6]3+ and [Cr(NH3)6]3+

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

A) [Fe(CO)5NO2]2+

B) [Cu(CO)5Cl]+

C) [MnClBr3]2-

D) [Cr(H2O)6]3+

E) [Ni(CO)2(NH3)2]2+

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

A) [Cr(H2O)4Br2]+

B) [Cu(CO)5Br]+

C) [Fe(CO)3(NH3)3]3+

D) [Fe(CO)5ONO]2+

E) [Fe(NH3)6]2+

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

A) [Cu(CO)5Cl]+

B) [Co(H2O)3(CO)3]3+

C) [Fe(CO)5NO2]2+

D) [Fe(NH3)2(H2O)4]2+

E) [Cr(H2O)4Br2]+

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

A) [Cr(H2O)4Br2]+

B) [Fe(CO)5ONO]2+

C) [Fe(CO)3(NH3)3]3+

D) [Cu(CO)5Br]+

E) [Fe(NH3)4(H2O)2]2+

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24) Which of the following complex ions absorbs light of the longest wavelength?

A) [Cr(CN)6]3-

B) [CrCl6]3-

C) [Cr(en)3]3+

D) [Cr(NH3)6]3+

E) [Cr(NO2)6]3-

25) Which of the following complex ions absorbs light of the shortest wavelength?

A) [FeCl6]3-

B) [Fe(OH)6]3-

C) [Fe(CN)6]3-

D) [Fe(H2O)6]3+

E) [FeI6]3-

26) The complex ion, [Ni(NH3)6]2+, has a maximum absorption near 580 nm. Calculate the crystal

field splitting energy (in kJ/mol) for this ion.

A) 114 kJ/mol

B) 292 kJ/mol

C) 343 kJ/mol

D) 206 kJ/mol

E) 485 kJ/mol

27) 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

28) 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

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

A) 0

B) 5

C) 3

D) 1

E) 2

30) How many unpaired electrons would you expect for the complex ion: [FeCl6]4-?

A) 2

B) 6

C) 4

D) 3

E) 0

31) Identify the shape of the hemoglobin complex.

A) octahedral

B) tetrahedral

C) pentadral

D) hexadral

E) heptadral

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

A) magnesium

B) manganese

C) selenium

D) iron

E) silver

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Algorithmic Questions

1) What is the highest possible oxidation state for manganese?

A) +2

B) +5

C) +6

D) +7

2) Choose the electron configuration for Nb3+.

A) [Kr]5s24d2

B) [Kr]5s2

C) [Kr]4d2

D) [Ar]4s23d104p6

E) [Kr]5s24d4

3) Choose the electron configuration for Ru7+.

A) [Kr]5s14d3

B) [Kr]5s24d2

C) [Kr]5s24d1

D) [Kr]4d3

E) [Kr]5s24d6

4) Choose the electron configuration for Cr3+.

A) [Ne]3s23p6

B) [Ar]4s13d2

C) [Ar]4s23d1

D) [Ar]4s23d7

E) [Ar]3d3

5) Choose the electron configuration for V3+.

A) [Ar]3d2

B) [Ar]4s23d2

C) [Ar]4s23d4

D) [Ar]4s2

E) [Ne]3s23p6

6) What is the ground-state electron configuration for the element chromium (Z = 24)?

A) [Ne] 4s2 3d4

B) [Ar] 4s2 3d4

C) [Ar] 4s1 3d5

D) [Ar] 3d6

7) What is the ground-state electron configuration for Cr3+ (Z = 24)?

A) [Ar] 4s2 3d7

B) [Ar] 4s2 3d1

C) [Ar] 3d3

D) [Ar] 4s1 3d2

8) Which of the following species has the electron configuration [Ar]3d6?

A) Cr

B) Fe3+

C) Co3+

D) Ni3+

9) How many d electrons are there in W O42-?

A) 0

B) 1

C) 2

D) 3

10) Which of the following can function as a bidentate ligand?

A) CO

B) OH –

C) N H3

D) C2O4 2-

11) Which of the following can function as a chelating agent?

A) SH–

B) H2O

C) H2NCH2CO2–

D) SCN –

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12) Choose the bidentate ligand from the substances below.

A) ethylenediamine

B) EDTA

C) chloride ion

D) ammonia

E) carbon monoxide

13) Choose the polydentate ligand from the substances below.

A) oxalate ion

B) EDTA

C) nitrite ion

D) hydroxide ion

E) carbon monoxide

14) Identify the geometry of [PdI4]2-.

A) tetrahedral

B) square planar

C) linear

D) octahedral

E) trigonal planar

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

A) tetrahedral

B) square planar

C) linear

D) bent

E) trigonal pyramidal

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

A) tetrahedral

B) square planar

C) linear

D) octahedral

E) trigonal planar

17) How many moles of aqueous ions will be produced from the dissolution of 1.0 mole of K3[Fe(I)6]

in water?

A) 4

B) 10

C) 2

D) 9

E) 1

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

A) [Rh(CN)6]4-

B) [Rh(CN)6]3-

C) [Rh(H2O)6]2+

D) [Rh(H2O)6]3+

19) Which of the following species is diamagnetic?

A) an isolated, gas-phase Cr3+ ion

B) a high-spin octahedral Cr2+ complex

C) an isolated, gas-phase Cu2+ ion

D) a low-spin octahedral Co3+ complex

20) What type of hybridization (according to valence bond theory) does Fe exhibit in the complex ion,

[Fe(H2O)4(Br)2]+?

A) dsp3

B) sp3

C) d2sp2

D) d2sp3

E) d2sp

21) What type of geometry (according to valence bond theory) does Fe exhibit in the complex ion,

[Fe(H2O)4(Cl)2]+?

A) linear

B) trigonal planar

C) square planar

D) octahedral

E) tetrahedral

22) What type of hybridization (according to valence bond theory) does Pt exhibit in the complex ion,

[Pt(NH3)4]2+?

A) dsp3

B) sp

C) d2sp3

D) d2sp

E) dsp2

23) What type of geometry (according to valence bond theory) does Pt exhibit in the complex ion,

[Pt(NH3)4]2+?

A) square pyramidal

B) see-saw

C) trigonal planar

D) tetrahedral

E) square planar

Diff: 3 Page Ref: 24.5

24) How many unpaired electrons would you expect for the complex ion: [Co(NH3 )6]4+?

A) 1

B) 0

C) 5

D) 2

E) 3

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

A) chromium

B) iron

C) sodium

D) copper

E) silver

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

A) potassium

B) zinc

C) copper

D) manganese

E) chromium

27) Identify the transition metal that is used infat and carbohydrate synthesis in the human body.

A) potassium

B) zinc

C) copper

D) manganese

E) chromium

Matching Questions

Match the following.

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

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

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

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

E) [Cr(en)3]3+

1) linkage

Diff: 2 Page Ref: 24.4

2) coordination

Diff: 2 Page Ref: 24.4

3) cis-trans

Diff: 2 Page Ref: 24.4

4) mer-fac

Diff: 2 Page Ref: 24.4

5) optical

Diff: 2 Page Ref: 24.4

Short Answer Questions

1) What is the Lanthanide contraction?

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

3) What is a coordinate covalent bond?

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

5) Explain how EDTA is used to treat lead poisoning.