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Transition Metal Chemistry
4p
3d
4s
d orbital splitting
in a typical transition
metal atom
Sc
Ti
V
Cr
Mn
4s2d1
4s2d2
4s2d3
4s1d5
4s2d5
Fe 4s2d6
Co 4s2d7
Ni 4s2d8
Cu 4s1d10
Zn 4s2d10
4p
3d
4s
d orbital splitting
in a typical transition
metal atom
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.
4p
4p
3d
4p
4s
4s
3d
4s
3d
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
Coordination Compounds
NH3
Base - electron pair donor
Ligand
Co(NH3)6+3
H
H
N
N
H
H
Co(en)3+3
1,2-diaminoethane
Ethylenediamine
Chelate
Bidentate Ligand
Common Ligands
NH3
H 2O
OHCNCO
NO2FClBrI-
ammine
aqua
hydroxo
cyano
carbonyl
nitro
fluoro
chloro
bromo
iodo
Square Planar
Complexes
trans
cis
Octahedral
Complexes
trans
cis
facial
meridial
Tetrahedral complexes
Optical Isomerism
Porphyrin
N
H
N
N
H
N
Protoporphyrin IX