This document summarizes Crystal Field Theory, which considers the electrostatic interactions between metal ions and ligands. It describes ligands and metal ions as point charges that can have attractive or repulsive forces. This causes the d orbitals of the metal ion to split into two sets with different energies - t2g and eg orbitals. The type of splitting and whether complexes are high or low spin depends on the ligand field stabilization energy and pairing energy. Color in coordination compounds is also explained by d-d transitions under ligand influence. Factors like the metal ion, ligands, and complex geometry affect crystal field splitting. However, the theory has limitations like not accounting for other metal orbitals or fully explaining ligand strengths.

1. Presented by
Dr. Neelam
Department of chemistry

2. Crystal Field Theory
This theory considers only electrostatic interactions between the central
metal ion (C.M.A.) and the ligand.
It considers the ligands and the C.M.A. as point charges:
C.M.A. = +ve point charges
Ligands = - ve point charges
Attractive forces = decreases energy
Repulsive forces = increases energy
To form a complex compound with the –ve charged ligand molecules
approach the C.M.A.

3. dxy dyz dzx
t2g
Lobes lying between the axis
Lobes lying along the axis
dx
2 - y
2 dz
2
eg
The five d orbitals in an isolated gaseous metal atom/ion have same energy,
i.e., they are degenerate.
dxy dyz dzx dx
2 - y
2 dz
2

4. Splitting of d orbital into two different set of orbitals in presence of the repulsive
field created by the approaching ligands .

7. The two possibilites are :
(i) If Δ0 < P weak field ligands and form high spin complexes.
(ii) If Δ0 > P stong field ligands and form low spin complexes.
COLOUR IN COORDINATION COMPOUNDS
According to the crystal field theory the colour is due to the d-d transition
of electron under the influence of ligands.

8. Factors affecting CFSE
nature of the metal ion
CFSE ∝ principle quantum no. Of metal
oxidation state of metal
CFSE ∝ oxidation state of C.M.A.
nature of the ligands
CFSE ∝ strength of ligand
nature of the complex
Octahedral complex > tetrahedral complex

9. Limitations of crystal field theory
(1) It considers only the metal ion d-orbitals and gives no consideration at
all to other metal orbitals (such as s, px, py and pz orbitals).
(2) It is unable to account satisfactorily for the relative strengths of
ligands. For example it gives no explanation as to why H2O is a stronger
ligand than OH– in the spectrochemical series.
(3) Account to this theory, the bond between the metal and ligands are
purely ionic. It gives no account on the partly covalent nature of the metal
ligand bonds.
(4) The CFT cannot account for the π-bonding in complexes.
(5) The theory failed to explain color in compound having d0 configuration
For ex. KMnO4 , K2Cr2O7

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