Transition Metal Chemistry

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Transition Metal Chemistry
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d orbital splitting in a typical transition metal
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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d orbital splitting in a typical transition metal
atom
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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.
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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
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Coordination Compounds
NH3
Base - electron pair donor
Ligand
Co(NH3)63
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Co(en)33
1,2-diaminoethane
Chelate
Ethylenediamine
Bidentate Ligand
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Common Ligands
NH3 ammine H2O aqua OH- hydroxo CN- cyano CO
carbonyl NO2- nitro F- fluoro Cl- chloro Br- b
romo I- iodo
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Square Planar Complexes
trans
cis
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Octahedral Complexes
trans
cis
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facial
meridial
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Tetrahedral complexes
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Optical Isomerism
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Porphyrin
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Protoporphyrin IX
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