Transition Metal Chemistry. d orbital splitting in a typical transition metal atom.
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Transcript of Transition Metal Chemistry. d orbital splitting in a typical transition metal atom.
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Transition Metal Chemistry
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4p
3d
4s
d orbital splittingin a typical transitionmetal atom
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Sc 4s2d1
Ti 4s2d2
V 4s2d3
Cr 4s1d5
Mn 4s2d5
Fe 4s2d6
Co 4s2d7
Ni 4s2d8
Cu 4s1d10
Zn 4s2d10
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4p
3d
4s
d orbital splittingin a typical transitionmetal atom
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The 4s an 4p orbitals is much more diffusein space than are the 3d orbitals. They havea higher quantum number n and the havefewer nodes (0 or 1) versus 2 for the d orbitals.
This means that when a transition metalatom bonds to other atoms, the most significant interactions are with the s andp orbitals, not the d orbitals.
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4p
4s
3d
4p
4s
3d
4p
3d
4s
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The 3d orbitals are not as important forbonding as are the 4s and 4p, but the details of what happens tothe 3d orbitals determine the propertiesof transition metal complexes.
3d
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Coordination Compounds
Co(NH3)6+3
NH3
Base - electron pair donorLigand
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Co(en)3+3
NNH
H
H
H
Ethylenediamine1,2-diaminoethane Chelate
Bidentate Ligand
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Common LigandsNH3 ammineH2O aquaOH- hydroxoCN- cyanoCO carbonylNO2
- nitroF- fluoroCl- chloroBr- bromoI- iodo
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Square Planar Complexes
trans
cis
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OctahedralComplexes
cis
trans
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facial meridial
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Tetrahedral complexes
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Optical Isomerism
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Porphyrin
N
N
N
NH
H
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Protoporphyrin IX
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