1. Transition Metals and Coordination Chemistry
Chapter 19
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2. Transition Metals and Coordination Chemistry – Ch. 19
1. Define:
a. Lewis acid and Lewis base
b. Ligand
c. Chelate
d. Coordination number
e. Counter ion
f. Isomer

3. Transition Metals and Coordination Chemistry – Ch. 19
2. Rank the following structural isomers by their conductivity in water.
[Cr(H2O)6]Cl3
[Cr(H2O)4Cl2]Cl•(H2O)2
[Cr(H2O)5Cl]Cl2•H2O

4. Transition Metals and Coordination Chemistry – Ch. 19
3. Fill in the following table:
Name
Formula
Diamminedichloroethylendiaminechromium(III) sulfate
lithium hexahydroxoferrate(III)
Bis(ethylenediamine)oxalatomanganese(IV) nitrate
potassium dibromodicyanoplatinate(II)

5. Transition Metals and Coordination Chemistry – Ch. 19
4. Fill in the following table:
Substance/Ion
Ox #
Coord. #
Name
[Pt(NH3)3Br]+
K[CoBrCl3(en)]
[Ni(CO)4] Br2
Na[Mn(C2O4)2(CN)(NO2)]
[Cu(NH3)4(H2O)2][PtI6]

6. Transition Metals and Coordination Chemistry – Ch. 19
5. _____ isomers and _____ isomers are classes of structural isomers.
a. Geometric, optical
b. Coordination, geometric
c. Linkage, geometric
d. Coordination, linkage
e. Geometric, linkage

7. Transition Metals and Coordination Chemistry – Ch. 19
6. Which of the following complexes shows geometric isomerism?
a. [Co(NH3)5Cl]SO4
b. [Co(NH3)6]Cl3
c. Li[Co(NH3)3Cl3]
d. K[Co(NH3)2Cl4]
e. Na3[CoCl6]

8. Transition Metals and Coordination Chemistry – Ch. 19
7. Give the number of geometric isomers for the octahedral compound [MA2B2C2], where A, B, and C represent ligands.
a. 1
b. 2
c. 3
d. 5
e. 6

9. Transition Metals and Coordination Chemistry – Ch. 19
8. For the process Co(NH3)5Cl2+ + Cl– ® Co(NH3)4Cl2+ + NH3, what would be the ratio of cis to trans isomers in the product?
a. 1:1
b. 1:2
c. 1:4
d. 4:1
e. 2:1

10. Transition Metals and Coordination Chemistry – Ch. 19
9. Which of the following statements about the complex ion Co(en)2Cl2+ is true? (en = ethylenediamine, NH2CH2CH2NH2)
a. The complex ion contains Co(I).
b. The complex ion exhibits cis and trans geometric isomers, but no optical isomers.
c. The complex ion exhibits two geometric isomers (cis and trans) and two optical isomers.
d. Because en is a strong field ligand (large Δ), the complex ion is paramagnetic.
e. The geometric isomers of the complex ion have identical chemical properties.

11. Transition Metals and Coordination Chemistry – Ch. 19
10. The compound Co(NH3)4Cl3 (233.44g/mol) has several structural isomers. A solution is made by dissolving g of one of the isomer in 25.0 g of water. The solution freezes at °C. (Kf = 1.86 °C kg/mol)
Which of the following is the correct structural isomer?
a. [Co(NH3)4Cl3]
b. [Co(NH3)4Cl2]Cl
c. [Co(NH3)4Cl]Cl2
d. [Co(NH3)4]Cl3

12. Transition Metals and Coordination Chemistry – Ch. 19
11. An orange complex and a violet complex were both found to have ferric ion as their central metal; which one absorbs light with a longer wavelength?

13. Transition Metals and Coordination Chemistry – Ch. 19
12. Draw the d orbital diagrams according to the crystal field model in order to predict how many unpaired electrons are in each of the following:
a. [ Fe(CN)6]4-
b. [CoBr6]3-
c. [Ni(H2O)4]2+ (tetrahedral)

14. Transition Metals and Coordination Chemistry – Ch. 19

15. Transition Metals and Coordination Chemistry – Ch. 19
13. Solutions of [Co(NH3)6]3+ , [Co(NO2)6]3-and [CoF6]3- are colored. The solutions were red, yellow and blue. Match the solution to the color.

16. Transition Metals and Coordination Chemistry – Ch. 19
14. The complex ion [Zn(H2O)6]2+ is colorless whereas [Ni(H2O)6]2+ is green, explain.

17. Transition Metals and Coordination Chemistry – Ch. 19
1. Define:
a. Lewis acid => electron pair acceptor and Lewis base => electron pair donar
b. Ligand => Lewis base
c. Chelate => Ligand that can form more than one coordination covalent bond
d. Coordination number => Number of coordination covalent bonds per metal atom
e. Counter ion => Oppositely charged ion necessary to neutralize another ion
f. Isomer => Same chemical formula – different properties

18. Transition Metals and Coordination Chemistry – Ch. 19
2. Rank the following 1 M solutions of structural isomers by their conductivity in water.
a. [Cr(H2O)6]Cl3  [Cr(H2O)6]3+ + 3Cl–
(4 ions)
b. [Cr(H2O)4Cl2]Cl•(H2O)2  [Cr(H2O)4Cl2]+ + Cl– + 2H2O
(2 ions)
c. [Cr(H2O)5Cl]Cl2•H2O  [Cr(H2O)5Cl]2+ + 2Cl– + H2O
(3 ions)
Relative conductivity => a > c > b

19. Transition Metals and Coordination Chemistry – Ch. 193.
Name
Formula
lithium hexahydroxoferrate(III)
Li3[Fe(OH)6]
diamminedichloroethylendiaminechromium(III) sulfate
[Cr(NH3)2Cl2(en)]2SO4
bis(ethylenediamine)oxalatomanganese(IV) nitrate
[Mn(en)2(ox)](NO3)2 or
[Mn(NH2CH2CH2NH2)2(C2O4)](NO3)2
potassium dibromodicyanoplatinate(II)
K2[PtBr2(CN)2]

20. Transition Metals and Coordination Chemistry – Ch. 194.
Substance/Ion
Ox # CN
Name
[Pt(NH3)3Br]+ +2 4
triamminebromoplatinum(II) ion
K[CoBrCl3(en)] +3 6
potassium bromotrichloro(ethylenediamine)cobalt(III)
[Ni(CO)4] Br2
tetracarbonylnickel(II) bromide
Na2[Mn(C2O4)2(CN)(NO2)] +4
sodium cyanonitrobisoxalatomanganate(IV)
[Cu(NH3)4(H2O)2][PtI6]
+2, +4
6, 6
tetraamminediaquacopper(II) hexaiodoplatinate(IV)

21. Transition Metals and Coordination Chemistry – Ch. 19
5. _____ isomers and _____ isomers are classes of structural isomers.
a. Geometric, optical
b. Coordination, geometric
c. Linkage, geometric
d. Coordination, linkage
e. Geometric, linkage
6. Which of the following complexes shows geometric isomerism?
a. [Co(NH3)5Cl]SO4
b. [Co(NH3)6]Cl3
c. Li[Co(NH3)3Cl3]
d. K[Co(NH3)2Cl4]
e. Na3[CoCl6]

22. Transition Metals and Coordination Chemistry – Ch. 19
7. Give the number of geometric isomers for the octahedral compound [MA2B2C2], where A, B, and C represent ligands.
a. 1
b. 2
c. 3
d. 5
e. 6 M A B C M C A B M B A C M A B C M B C A

23. Transition Metals and Coordination Chemistry – Ch. 19
8. For the process Co(NH3)5Cl2+ + Cl– ® Co(NH3)4Cl2+ + NH3, what would be the ratio of cis to trans isomers in the product? a. 1:1 b. 1:2 c. 1:4 d. 4:1 e. 2:1 Co Cl N Co Cl N Co Cl N Co Cl N Co Cl N Co Cl N

24. Transition Metals and Coordination Chemistry – Ch. 19
9. Which of the following statements about the complex ion Co(en)2Cl2+ is true? (en = ethylenediamine, NH2CH2CH2NH2) a. The complex ion contains Co(I). b. The complex ion exhibits cis and trans geometric isomers, but no optical isomers. c. The complex ion exhibits two geometric isomers (cis and trans) and two optical isomers. d. Because en is a strong field ligand (large Δ), the complex ion is paramagnetic. e. The geometric isomers of the complex ion have identical chemical properties.

25. Transition Metals and Coordination Chemistry – Ch. 19
10. A solution is made by dissolving g of Co(NH3)4Cl3 in 25.0 g of water. The solution freezes at °C. (Kf = 1.86 °C kg/mol) Calculate the number of ions (i) produced when Co(NH3)4Cl3 is dissolved in water. ΔTf = - kfim -0.56C = -(1.86 Ckg/mol)(i)(0.875g/233.44g/mol)/(0.025kg) i = 2 => [Co(NH3)4Cl2]Cl

26. Transition Metals and Coordination Chemistry – Ch. 19
11. An orange complex and a violet complex were both found to have ferric ion as their central metal; which one absorbs light with a longer wavelength?
The orange complex absorbs blue light and the violet complex absorbs yellow light – λyellow > λblue – so the violet complex absorbs the longer wavelength

27. Transition Metals and Coordination Chemistry – Ch. 19
12. Draw the d orbital diagrams according to the crystal field model in order to predict how many unpaired electrons are in each of the following: a. [ Fe(CN)6]4- b. [CoBr6]3- c. [Fe(H2O)4]3+ (tetrahedral)

28. Transition Metals and Coordination Chemistry – Ch. 19
13. Solutions of [Co(NH3)6]3+ , [Co(NO2)6]3-and [CoF6]3- are colored. The solutions were red, yellow and blue. Match the solution to the color.
Color Seen
Color Absorbed
Relative Wavelength
Relative Energy
Relative Ligand Strength
Ligand
red
green
medium
NH3
yellow
violet
shortest
highest
strongest
NO2-
blue
orange
longest
lowest
weakest F-

29. Transition Metals and Coordination Chemistry – Ch. 19
14. The complex ion [Zn(H2O)6]2+ is colorless whereas [Ni(H2O)6]2+ is green, explain. Zn2+ => [Ar]3d10 => since all of the d orbitals are filled the d electrons if excited would have to absorb an energy outside of the visible spectrum => if the compound doesn’t absorb visible light it will be colorless (with the exception of black which is absorbing all visible colors)