1. Transition Metal Chemistry

4. d orbital splitting in a typical transition metal atom

5. Sc 4s 2 d 1 Ti 4s 2 d 2 V 4s 2 d 3 Cr 4s 1 d 5 Mn 4s 2 d 5 Fe 4s 2 d 6 Co 4s 2 d 7 Ni 4s 2 d 8 Cu 4s 1 d 10 Zn 4s 2 d 10

6. d orbital splitting in a typical transition metal atom

7. The 4s an 4p orbitals is much more diffuse in space than are the 3d orbitals. They have a higher quantum number n and the have fewer nodes (0 or 1) versus 2 for the d orbitals. This means that when a transition metal atom bonds to other atoms, the most significant interactions are with the s and p orbitals, not the d orbitals.

9. The 3d orbitals are not as important for bonding as are the 4s and 4p, but the details of what happens to the 3d orbitals determine the properties of transition metal complexes. 3d

11. Coordination Compounds Co(NH 3 ) 6 +3 NH 3 Base - electron pair donor Ligand

12. Co(en) 3 +3 Ethylenediamine 1,2-diaminoethaneChelate Bidentate Ligand

13. Common Ligands NH 3 ammine H 2 Oaqua OH - hydroxo CN - cyano COcarbonyl NO 2 - nitro F - fluoro Cl - chloro Br - bromo I - iodo

14. Square Planar Complexes trans cis

15. Octahedral Complexes cis trans

16. facialmeridial

17. Tetrahedral complexes

18. Optical Isomerism

21. Porphyrin

22. Protoporphyrin IX