[NiCl₄]²⁻ is paramagnetic while [Ni(CO)₄] is diamagnetic though both are tetrahedral. Why?

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Solution

Though both [NiCl₄]²⁻and [Ni(CO)₄] are tetrahedral, their magnetic characters are different. This is due to a difference in the nature of ligands. Cl⁻ is a weak field ligand and it does not cause the pairing of unpaired 3d electrons. Hence, [NiCl₄]²⁻is paramagnetic.

In Ni(CO)₄, Ni is in the zero oxidation state i.e., it has a configuration of 3d⁸ 4s^2.

But CO is a strong field ligand. Therefore, it causes the pairing of unpaired 3d electrons. Also, it causes the 4s electrons to shift to the 3d orbital, thereby giving rise to sp³ hybridization. Since no unpaired electrons are present in this case, [Ni(CO)₄] is diamagnetic.

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