[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.
Why does [Co(C₂O₄)₃]³⁻ exhibit diamagnetic behavior, while [CoF₆]³⁻ is paramagnetic despite both having a Co³⁺ ion?
Share
The difference in magnetic behavior between [Co(C₂O₄)₃]³⁻ (diamagnetic) and [CoF₆]³⁻ (paramagnetic) arises from their distinct hybridization schemes. [Co(C₂O₄)₃]³⁻ involves inner orbital complex formation with d²sp³ hybridization, leading to diamagnetism due to the absence of unpaired electrons. In contrast, [CoF₆]³⁻ exhibits outer orbital complex formation with sp³d² hybridization, resulting in paramagnetism due to the presence of four unpaired electrons. The ligand field effects and hybridization patterns in these complexes dictate the distribution of unpaired electrons, influencing their magnetic properties despite both containing Co³⁺ ions.