MCQ
Which of the following is paramagnetic
- A$\left[ {Ni{{\left( {CO} \right)}_4}} \right]$
- B${[Co{(N{H_3})_6}]^{3 + }}$
- C${\left[ {Ni{{\left( {CN} \right)}_4}} \right]^{2 - }}$
- ✓${\left[ {NiC{l_4}} \right]^{2 - }}$
✓
Answer
Correct option: D.
${\left[ {NiC{l_4}} \right]^{2 - }}$
d
In $N i(C O)_{4},$ the oxidation state of $N i$ is zero whereas in $\left[N i C l_{4}\right]^{2-}$, the oxidation state of $N i$ is. The presence of $C O$ ligand, which is a strong ligand, can pair all electrons in $N i(C O)_{4}$ and thus it is diamagnetic in nature but $C l^{-}$ is a weak ligand and is unable to pair up the unpaired electrons and thus $\left[ NiCl _{4}\right]^{2-}$ is paramagnetic in nature.
In $N i(C O)_{4},$ the oxidation state of $N i$ is zero whereas in $\left[N i C l_{4}\right]^{2-}$, the oxidation state of $N i$ is. The presence of $C O$ ligand, which is a strong ligand, can pair all electrons in $N i(C O)_{4}$ and thus it is diamagnetic in nature but $C l^{-}$ is a weak ligand and is unable to pair up the unpaired electrons and thus $\left[ NiCl _{4}\right]^{2-}$ is paramagnetic in nature.
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