Total number of unpaired electrons in the complex ions and is

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Solution

Q.
Total number of unpaired electrons in the complex ions ${[Co {({NH}_{3})}_{6}]}^{3 +}$ and ${[{NiCl}_{4}]}^{2 -}$ is ______. [2024]

Ans.
(2)

${[Co {({NH}_{3})}_{6}]}^{3 +}$

Oxidation number of Co = +3
${Co}^{3 +} = {}_{18}{[Ar] 3 d^{6}}$

${NH}_{3}$ is a strong field ligand. It pairs up d electrons. After pairing d electrons, two 3d orbitals are vacant. ${Co}^{3 +}$ undergoes $d^{2} {sp}^{3}$ hybridization by using two 3d orbitals. Six $e^{-}$ pairs from six ${NH}_{3}$ are accommodated in these six $d^{2} {sp}^{3}$ orbitals.

Orbital Diagram of ${Co}^{3 +}$ in the presence of ${NH}_{3}$ :

It has no unpaired electrons.

${[{NiCl}_{4}]}^{2 -}$

Oxidation number of Ni = +2

${Ni}^{2 +} = {}_{18}{[Ar] 3 d^{8}}$

${Cl}^{-}$ is a weak field ligand hence does not cause pairing of $3 d^{8}$ electrons. ${Ni}^{2 +}$ undergoes ${sp}^{3}$ hybridization and lone pairs from ${Cl}^{-}$ are accommodated in ${sp}^{3}$ orbitals.

Orbital Diagram of ${Ni}^{2 +}$ in the presence of ${Cl}^{-}$ :

It contains 2 unpaired electrons.

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