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Questions
Discuss the nature of bonding in the following coordination entity on the basis of valence bond theory:
[FeF6]3−
Explain the structure of [FeF6]3− on the basis of valence bond theory.
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Solution
- In this complex, the oxidation state of Fe is +3.
- Orbitals of Fe+3 ion:
- The complex ion [FeF6]3− is explained on the basis of valence bond theory as follows: Iron in this complex is in the +3 oxidation state, so the electronic configuration of Fe3+ is [Ar] 3d5. The fluoride ion (F−) is a weak field ligand and does not cause the pairing of electrons in the d-orbitals.
- As a result, the five 3d electrons in Fe3+ remain unpaired. Since there are six ligands, the geometry of the complex is octahedral, requiring six hybrid orbitals.
- Due to the weak field nature of F−, the complex uses outer d-orbitals (4d) for bonding, resulting in sp3d2 hybridization.
- The [FeF6]3− complex is an outer orbital octahedral complex. Because of the presence of five unpaired electrons, the complex is paramagnetic in nature.
- The sp3d2 hybridized orbitals of Fe are:
Hence, the geometry of the complex is found to be octahedral.
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