Calculate the difference in magnetic moment of complexes [Ni(CN)4]2− and [Ni(Cl)4]2−.
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Solution
In both complexes, Ni is as Ni2+ that is [Ar]3d8.
In [Ni(CN)4]2−, the ligand is CN− which is a strong field ligand and hence pairing of electrons occur resulting in a square planar complex. Unpaired electrons are 0.
In [NiCl4]2−, the ligand is Cl− which is a weak field ligand and hence pairing of electrons does not occur, resulting in tetrahedral complex. Unpaired electrons are 2.
Magnetic moment = √n(n+2)
For [NiCl4]2−, n = 2 magnetic moment=√2(2+2)=2.828B.M. For [Ni(CN)4]2−, n = 0 magnetic moment = 0 Difference in magnetic moment = 2.828 B.M.