1. Drill:
Determine the Ksp for Mn2S3 when the solubility is 1 x 10-20

2. Complex Ions

3. Complex Ion
An ion formed when a positive central element binds with multiple ions or polar molecules

4. The central element is almost always a positively charged metal
Complex Ion
The central element is almost always a positively charged metal

5. Describe or define a Complex Ion

6. Negatively charged ion
Anion
Negatively charged ion

7. Positively charged ion
Cation
Positively charged ion

8. Metal Ion Examples
Cu+2 Cu+ Au+
Ag+ Zn+2 Ni+2
Pt+2 Co+2 Al+3

9. Ligands
The negative ions or polar molecules bound by the central element in a complex ion

10. Ligand Examples
Cl- F- H2O
NH3 CN- Br-
NO O2 OH-

11. Ligands that can bind to more than one point
Polydentate Ligands
Ligands that can bind to more than one point

12. Ligands that can bind to two points in a complex ion
Bidentate Ligands
Ligands that can bind to two points in a complex ion

13. Bidentate Examples
H2N-CH2-CH2-NH2
-OOC-COO-

14. Ligands that can bind to three points in a complex ion
Tridentate Ligands
Ligands that can bind to three points in a complex ion

15. Tridentate Examples
H2-C-COO-
HO-C-COO-

16. Polydentate ligands that bind to metal ions in solution
Chelates
Polydentate ligands that bind to metal ions in solution

17. Coordination Number
The number of points in which ligands bind to the central element in a complex ion

18. Coordinate Covalent Bond
Covalent bonds in which both electrons involved are donated by one atom

19. Drill:
Define:
Complex ion
Ligand
Coordination number

20. The bonds formed in a complex ion are coordinate covalent bonds
Complex Ions
The bonds formed in a complex ion are coordinate covalent bonds

21. A complex ion and its counter ion
Coordination Complex
A complex ion and its counter ion

22. The bonds formed in a complex ion are coordinate covalent bonds
Complex Ions
The bonds formed in a complex ion are coordinate covalent bonds

23. Complex Ion
Because of the type bonding, they are sometimes called coordinate complexes

24. AP CHM HW
Read: Chapter 15
Problems: 3 & 5
Page: 445

25. 1) Name cations before anions
Naming Complexes
1) Name cations before anions

26. 2) Name ligands before metal in the complex ion
Naming Complexes
2) Name ligands before metal in the complex ion

27. a) give neutral compds normal names except:
2) Naming Ligands
a) give neutral compds normal names except:

28. H2O aqua
NH3 amine
CO carbonyl
NO nitrosyl

29. b) change -ide endings to -o for all anions
2) Naming Ligands
b) change -ide endings to -o for all anions

30. c) name ligands alphabetically
2) Naming Ligands
c) name ligands alphabetically

31. d) use geometric prefixes for monodentate ligands
2) Naming Ligands
d) use geometric prefixes for monodentate ligands

32. e) use bis- for 2 & tris- for 3 polydentate ligands
2) Naming Ligands
e) use bis- for 2 & tris- for 3 polydentate ligands

33. a) use the normal name if the complex ion is (+)
3) Naming Metal
a) use the normal name if the complex ion is (+)

34. b) make the metal ending -ate if the complex ion is (-)
3) Naming Metal
b) make the metal ending -ate if the complex ion is (-)

35. d) use Roman numerals in () to indicate metal ox #
3) Naming Metal
d) use Roman numerals in () to indicate metal ox #

36. Name the Following:
[Pt(NH3)4]Cl2
[Co(H2O)2Cl4]-2
[Cu(H2O)2(en)2]I2

37. AP CHM HW
Read: Chapter 15
Name each in Problem 5
Page: 445

38. Predict # of isomers of each:
[Pt(NH3)4 Cl2]
[Co(H2O)3Cl3]

39. Drill: Name each
[Pt (H2O)2(en)2]+2
[Co(H2O)2F2I2]-2
[ZnNH3ClFI]-1

40. Complex Ion Shapes
2-linear
4-tetrahedral or sq pl
6-octahedral

41. Square planar vs tetrahedral
Geometric Isomers
Square planar vs tetrahedral
cis vs trans

42. Geometric Isomers Tetra vs Sq Pl

43. Geometric Isomers Square PlanerX Y Y X

44. Geometric Isomers
Bunched octa-
T-shaped octa-
bis: cis vs trans

45. T-Shaped vs Bunched X X X X X X

46. Optical Isomers
Tri-bis mirror images

47. Cis vs trans

48. Optical isomers

49. Predict isomer #
[Pt (H2O)2(en)2]+2
[Co(H2O)2F2I2]-2
[ZnNH3ClFI]-1

50. Name & Predict isomer #
[FeNH3Cl2I]-1

51. AP CHM HW
Read: Chapter 15
Problem: 13
Page: 445

52. CN- > NO2- > en > NH3 > NCS- > H2O > F- > Cl-
Field Strength
CN- > NO2- > en > NH3 > NCS- > H2O > F- > Cl-

53. Field Strength
CN- is strong field
Cl- is weak field

54. Determines d-level splitting or Do(splitting energy)
Field Strength
Determines d-level splitting or Do(splitting energy)

55. dlevel

56. Low field strength (small splitting)
dlevel

57. High field strength (large splitting)
dlevel

58. Low spin
High spin
dlevel

59. Large Do yields low spin or diamagnetic compds
Field Strength
Large Do yields low spin or diamagnetic compds

60. Small Do yields high spin or paramagnetic compds
Field Strength
Small Do yields high spin or paramagnetic compds

61. Name, shape, & possible isomerism
[Pt(NH3)2I4]-2
Determine:
Name, shape, & possible isomerism

62. Drill: Determine the name, shape & isomers of:
[Co(H2O)3Cl3]-1

63. Drill: Determine the name, shape & isomers of:
[CuCl2I2]-2

64. Determine the name, shape & isomers of:
[ZnBr2Cl2]-2

65. [Co(NH3)6] yellow
[Co(NH3)5NCS] orange
[Co(NH3)5H2O] red
[Co(NH3)5Cl] purple
t-[Co(NH3)4Cl2] green

66. Complex Ion Equilibria
Cu NH [Cu(NH3)4]+2
[[Cu(NH3)4]+2]
[Cu+2][NH3]4
Kf =

67. Calculate the ratio of [Cu+2]/ [Cu(NH3)4]+2 when Cu+2 is added to a 0
Calculate the ratio of [Cu+2]/ [Cu(NH3)4]+2 when Cu+2 is added to a 0.10 M NH3 solution: Kf = 2.0 x 1012

68. AP CHM HW
Read: Chapter 15
Problem: 37
Page: 446

69. The larger the Kf, the more likely the complex will form
Common Ion Equilibria
The larger the Kf, the more likely the complex will form

70. Common Ion Equilibria
Kf for [Ag(NH3)2]+1
= 1.7 x 107
Kf for [Ag(CN)2]-1
= 2.0 x 1020

71. Common Ion Equilibria
CN- will replace
NH3 in the
complex with silver

72. Common Ion Equilibria
Kf for [M(NH3)2]+2
= 1.7 x 1011
Kf for [M(CN)4]-2
= 2.0 x 1020

73. [Zn(NH3)2H2OF]+1 [Co(NH3)3ClFI]-1
Calculate: a) coordination # b) number of isomers c) oxidation # of metal
[Zn(NH3)2H2OF]+1
[Co(NH3)3ClFI]-1