The correct statement among the following is:

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(C) $1$. For $[Ni(CN)_4]^{2-}$: $Ni^{2+}$ is $3d^8$. $CN^-$ is a strong field ligand,causing pairing of electrons. It forms $dsp^2$ hybridization,maki

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$Ni(CO)_4$ and $[Ni(CN)_4]^{2-}$ are diamagnetic and $[NiCl_4]^{2-}$ is paramagnetic.

Vedclass · Answer

(C) $1$. For $[Ni(CN)_4]^{2-}$: $Ni^{2+}$ is $3d^8$. $CN^-$ is a strong field ligand,causing pairing of electrons. It forms $dsp^2$ hybridization,making it diamagnetic.$2$. For $Ni(CO)_4$: $Ni$ is $3d^8 4s^2$ $(3d^{10})$. $CO$ is a strong field ligand. It forms $sp^3$ hybridization,making it diamagnetic.$3$. For $[NiCl_4]^{2-}$: $Ni^{2+}$ is $3d^8$. $Cl^-$ is a weak field ligand,so electrons do not pair. It forms $sp^3$ hybridization with two unpaired electrons,making it paramagnetic.Therefore,$Ni(CO)_4$ and $[Ni(CN)_4]^{2-}$ are diamagnetic,while $[NiCl_4]^{2-}$ is paramagnetic.

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