Frequently Asked Question

The complex [Co(ox)3]4- is diamagnetic. Here's why:
1. Cobalt(II) Ion: The central cobalt ion, Co2+, has an electronic configuration of [Ar] 3d7.
2. Oxalate Ligand: The oxalate ligand (ox) is a bidentate ligand, meaning it forms two bonds with the cobalt ion. This creates a strong ligand field.
3. Coordination Number: The coordination number of the complex is 6 (three oxalate ligands, each donating two electrons).
4. Strong Field Ligand: The oxalate ligand is a strong field ligand, which means it causes a large splitting of the d-orbitals in the cobalt ion.
5. Pairing of Electrons: Due to the strong field, all six electrons of the cobalt ion are paired in the lower energy d-orbitals, resulting in a diamagnetic complex.
Therefore, the effective magnetic moment (μeff) for [Co(ox)3]4- is zero, since there are no unpaired electrons.