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Complex Ions

Complex Ions. Complex Ion. An ion formed when a positive central element binds with multiple ions or polar molecules. Complex Ion. The central element is almost always a positively charged metal. Describe or define a Complex Ion. Anion. Negatively charged ion. Cation.

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Complex Ions

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  1. Complex Ions

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

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

  4. Describe or define a Complex Ion

  5. Anion • Negatively charged ion

  6. 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. Polydentate Ligands • Ligands that can bind to more than one point

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

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

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

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

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

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

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

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

  25. H2O aqua • NH3 amine • CO carbonyl • NO nitrosyl

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

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

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

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

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

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

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

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

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

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

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

  44. [Co(NH3)6]+3 yellow [Co(NH3)5NCS]+2 orange [Co(NH3)5H2O]+2 red [Co(NH3)5Cl]+2 purple t-[Co(NH3)4Cl2]+1 green

  45. Complex Ion Equilibria Cu+2 + 4 NH3 [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 0.10 M NH3 solution:Kf = 2.0 x 1012

  47. 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

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