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Comprehensive Coordination Chemistry Lesson Plan

This lesson plan covers the basics of coordination chemistry, focusing on Lewis acids and bases, complex ions, coordination compounds, and ligands. Learn about coordination numbers, geometries of complexes, and examples like metalloporphyrins.

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Comprehensive Coordination Chemistry Lesson Plan

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  1. INNOVATIVE LESSON PLAN PRASANTH M ST JACOB’S TRAINING COLLEGE

  2. Lewis acid Lewis base Complex ion Lewis acid Lewis base Complex ion Coordination Chemistry • Transition metals act as Lewis acids • Form complexes/complex ions Fe3+(aq) + 6CN-(aq)  [Fe(CN)6]3-(aq) Ni2+(aq) + 6NH3(aq)  [Ni(NH3)6]2+(aq) Complex with a net charge = complex ion Complexes have distinct properties

  3. Coordination Chemistry • Coordination compound • Compound that contains 1 or more complexes • Example • [Co(NH3)6]Cl3 • [Cu(NH3)4][PtCl4] • [Pt(NH3)2Cl2]

  4. Coordination Chemistry • Coordination sphere • Metal and ligands bound to it • Coordination number • number of donor atoms bonded to the central metal atom or ion in the complex • Most common = 4, 6 • Determined by ligands • Larger ligands and those that transfer substantial negative charge to metal favor lower coordination numbers

  5. Coordination Chemistry Complex charge = sum of charges on the metal and the ligands [Fe(CN)6]3-

  6. Coordination Chemistry Complex charge = sum of charges on the metal and the ligands [Fe(CN)6]3- +3 6(-1)

  7. Coordination Chemistry Neutral charge of coordination compound = sum of charges on metal, ligands, and counterbalancing ions [Co(NH3)6]Cl2 neutral compound

  8. Coordination Chemistry Neutral charge of coordination compound = sum of charges on metal, ligands, and counterbalancing ions [Co(NH3)6]Cl2 +2 6(0) 2(-1)

  9. Coordination Chemistry • Ligands • classified according to the number of donor atoms • Examples • monodentate = 1 • bidentate = 2 • tetradentate = 4 • hexadentate = 6 • polydentate = 2 or more donor atoms

  10. Coordination Chemistry • Ligands • classified according to the number of donor atoms • Examples • monodentate = 1 • bidentate = 2 • tetradentate = 4 • hexadentate = 6 • polydentate = 2 or more donor atoms chelating agents

  11. Ligands • Monodentate • Examples: • H2O, CN-, NH3, NO2-, SCN-, OH-, X- (halides), CO, O2- • Example Complexes • [Co(NH3)6]3+ • [Fe(SCN)6]3-

  12. Ligands • Bidentate • Examples • oxalate ion = C2O42- • ethylenediamine (en) = NH2CH2CH2NH2 • ortho-phenanthroline (o-phen) • Example Complexes • [Co(en)3]3+ • [Cr(C2O4)3]3- • [Fe(NH3)4(o-phen)]3+

  13. Ligands oxalate ion ethylenediamine * * * * ortho-phenanthroline * * Donor Atoms

  14. Ligands oxalate ion ethylenediamine H C C O M N M

  15. Ligands

  16. Ligands • Hexadentate • ethylenediaminetetraacetate (EDTA) = (O2CCH2)2N(CH2)2N(CH2CO2)24- • Example Complexes • [Fe(EDTA)]-1 • [Co(EDTA)]-1

  17. Ligands EDTA * * * * * * Donor Atoms

  18. Ligands EDTA O H C N M

  19. Ligands EDTA

  20. Common Geometries of Complexes Coordination Number Geometry 2 Linear

  21. Common Geometries of Complexes Coordination Number Geometry 2 Linear Example: [Ag(NH3)2]+

  22. Common Geometries of Complexes Coordination Number Geometry 4 tetrahedral (most common) square planar (characteristic of metal ions with 8 d e-’s)

  23. Common Geometries of Complexes Coordination Number Geometry 4 tetrahedral Examples: [Zn(NH3)4]2+, [FeCl4]- square planar Example: [Ni(CN)4]2-

  24. Common Geometries of Complexes Coordination Number Geometry 6 octahedral

  25. Common Geometries of Complexes Coordination Number Geometry 6 Examples: [Co(CN)6]3-, [Fe(en)3]3+ octahedral

  26. Porphine, an important chelating agent found in nature

  27. Metalloporphyrin

  28. Myoglobin, a protein that stores O2 in cells

  29. Coordination Environment of Fe2+ in Oxymyoglobin and Oxyhemoglobin

  30. Coordination Environment of Fe2+ in Oxymyoglobin and Oxyhemoglobin

  31. Arterial Blood Strong field large  Bright red due to absorption of greenish light

  32. Venous Blood Weak field small  Bluish color due to absorption of orangish light

  33. End of Presentation

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