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Question
Discuss the nature of bonding in the following coordination entity on the basis of valence bond theory:
[Fe(CN)6]4−
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Solution
The oxidation state of iron in this complex ion is +2.
Electronic configuration of Fe = [Ar] 3d64s2
Electronic configuration of Fe2+ = [Ar] 3d6
The iron (II) ion must provide six vacant orbitals to accommodate the six electron pairs from the six cyanide ions. This can be achieved by the hybridisation method in which the electrons of the d-subshell get paired since the CN– ions are strong field ligands.
Hence, six electron pairs from six cyanide ions occupy six hybrid orbitals of iron (II) ion. Thus, no unpaired electrons are in any orbital, so [Fe(CN)6]4− shows diamagnetism. Hence, [Fe(CN)6]4− is diamagnetic and octahedral.
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