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.
How does the availability of d orbitals for octahedral hybridization change when more than three 3d electrons are present, as seen in d⁴, d⁵, and d⁶ cases?
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When more than three 3d electrons are present, as in d⁴, d⁵, and d⁶ cases, the availability of d orbitals for octahedral hybridization is influenced by the need to pair electrons. In the d⁴ case (e.g., Cr²⁺, Mn³⁺), a vacant pair of d orbitals is created by pairing one of the 3d electrons. For d⁵ (Mn²⁺, Fe³⁺) and d⁶ (Fe²⁺, Co³⁺) cases, two and three electrons, respectively, need to be paired, creating a vacant pair of d orbitals. This pairing affects the overall magnetic behavior and energy levels in coordination compounds, contributing to their distinct properties.