Valence Bond Theory attributes the anomalies to the formation of inner orbital and outer orbital coordination entities. Inner orbital complexes like [Mn(CN)₆]³⁻ and [Fe(CN)₆]³⁻, with d²sp³ hybridization, are paramagnetic, while outer orbital complexes like [MnCl₆]³⁻ and [FeF₆]³⁻, with sp³d² hybridization, are paramagnetic due to four, five, and four unpaired electrons.
How does valence bond theory explain the anomalous magnetic behavior in certain coordination compounds, considering inner and outer orbital complexes?
Share
Valence Bond Theory (VBT) explains the anomalous magnetic behavior in coordination compounds by considering inner and outer orbital complexes. Inner orbital complexes, such as [Mn(CN)₆]³⁻ and [Fe(CN)₆]³⁻, involve d²sp³ hybridization, leading to diamagnetic and paramagnetic behavior, respectively. The distribution of unpaired electrons deviates from conventional expectations due to ligand effects. In outer orbital complexes, like [MnCl₆]³⁻ and [FeF₆]³⁻, with sp³d² hybridization, the paramagnetic behavior corresponds to the expected number of unpaired electrons. VBT emphasizes the influence of ligand-field effects on electron distribution, providing insights into the magnetic properties of coordination compounds.