1. Complex Ions

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

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

4. Describe or define a Complex Ion

5. Negatively charged ion
Anion
Negatively charged ion

6. Positively charged ion
Cation
Positively charged ion

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

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

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

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

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

12. Bidentate Examples
H2N-CH2-CH2-NH2
-O2C-CO2-

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

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

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

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

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

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

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

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

22. 1) Name cations before anions

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

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

25. H2O aqua
NH3 amine
CO carbonyl
NO nitrosyl

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

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

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

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

30. 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 (-)

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

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

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

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

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

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

37. Optical Isomers
Tri-bis mirror images

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

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

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

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

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

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

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

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

46. 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

47. 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

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

49. Common Ion Equilibria
Kf for [M(NH3)2]+2
= 1.7 x 107
Kf for [M(CN)4]-2
= 2.0 x 1020

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

51. [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