1. Drill: Determine the Ksp for Mn 2 S 3 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. Complex Ion The central element is almost always a positively charged metal

5. Describe or define a Complex Ion

6. Anion Negatively charged ion

7. 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 - H 2 O NH 3 CN - Br - NOO 2 OH -

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

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

13. Bidentate Examples H 2 N-CH 2 -CH 2 -NH 2 - OOC-COO -

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

15. Tridentate Examples H 2 -C-COO - HO-C-COO - H 2 -C-COO -

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

21. Coordination Complex A complex ion and its counter ion

22. 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

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

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

28. H 2 Oaqua NH 3 amine COcarbonyl NOnitrosyl

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

30. 2) Naming Ligands c) name ligands alphabetically

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

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

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

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

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

36. Name the Following: [Pt(NH 3 ) 4 ]Cl 2 [Co(H 2 O) 2 Cl 4 ] -2 [Cu(H 2 O) 2 (en) 2 ]I 2

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

38. Predict # of isomers of each: [Pt(NH 3 ) 4 Cl 2 ] [Co(H 2 O) 3 Cl 3 ]

39. Drill: Name each [Pt (H 2 O) 2 (en) 2 ] +2 [Co(H 2 O) 2 F 2 I 2 ] -2 [ZnNH 3 ClFI] -1

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

41. Geometric Isomers Square planar vs tetrahedral cis vs trans

42. Geometric Isomers Tetra vs Sq Pl

43. Geometric Isomers Square Planer X Y X Y

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 (H 2 O) 2 (en) 2 ] +2 [Co(H 2 O) 2 F 2 I 2 ] -2 [ZnNH 3 ClFI] -1

50. Name & Predict isomer # [FeNH 3 Cl 2 I] -1

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

52. Field Strength CN - > NO 2 - > en > NH 3 > NCS - > H 2 O > F - > Cl -

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

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

55. d level

56. Low field strength (small splitting)

57. d level High field strength (large splitting)

58. d level Low spin High spin

59. Field Strength Large  o yields low spin or diamagnetic compds

60. Field Strength Small  o yields high spin or paramagnetic compds

61. [Pt(NH 3 ) 2 I 4 ] -2 Determine: Name, shape, & possible isomerism

62. Drill: Determine the name, shape & isomers of: [Co(H 2 O) 3 Cl 3 ] -1

63. Determine the name, shape & isomers of: [Cu(NH 3 ) 2 F 2 I 2 ] -2

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

65. [Co(NH 3 ) 6 ] +3 yellow [Co(NH 3 ) 5 NCS] +2 orange [Co(NH 3 ) 5 H 2 O] +2 red [Co(NH 3 ) 5 Cl] +2 purple t-[Co(NH 3 ) 4 Cl 2 ] +1 green

66. Complex Ion Equilibria Cu +2 + 4 NH 3 [Cu(NH 3 ) 4 ] +2 [[Cu(NH 3 ) 4 ] +2 ] [Cu +2 ][NH 3 ] 4 K f =

67. Calculate the ratio of [Cu +2 ]/ [Cu(NH 3 ) 4 ] +2 when Cu +2 is added to a 0.10 M NH 3 solution: K f = 2.0 x 10 12

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

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

70. Common Ion Equilibria K f for [Ag(NH 3 ) 2 ] +1 = 1.7 x 10 7 K f for [Ag(CN) 2 ] -1 = 2.0 x 10 20

71. Common Ion Equilibria CN - will replace NH 3 in the complex with silver

72. Common Ion Equilibria K f for [M(NH 3 ) 2 ] +2 = 1.7 x 10 11 K f for [M(CN) 4 ] -2 = 2.0 x 10 20

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