[Co(C₂O₄)₃]³⁻ is an inner orbital complex with d²sp³ hybridization, resulting in diamagnetic behavior. In contrast, [CoF₆]³⁻ is an outer orbital complex with sp³d² hybridization, leading to paramagnetism due to the presence of four unpaired electrons.

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, ...

The magnetic data show anomalies in compounds like [Mn(CN)₆]³⁻ and [Fe(CN)₆]³⁻, where [Mn(CN)₆]³⁻ has a magnetic moment of two unpaired electrons, while [Fe(CN)₆]³⁻ exhibits a paramagnetic moment with five unpaired electrons.

In d⁴ (Cr²⁺, Mn³⁺), d⁵ (Mn²⁺, Fe³⁺), and d⁶ (Fe²⁺, Co³⁺) cases, a vacant pair of d orbitals for octahedral hybridization is achieved by pairing 3d electrons, resulting in two, one, and zero unpaired electrons, respectively.

Metal ions like Ti³⁺ (d¹), V³⁺ (d²), Cr³⁺ (d³) exhibit similar magnetic behavior in both free ions and coordination entities as two vacant d orbitals are available for octahedral hybridization with 4s and 4p orbitals.