The complex showing a spin-only magnetic mome | vedclass

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(B) The spin-only magnetic moment $\mu$ is given by $\sqrt{n(n+2)} \ B.M.$,where $n$ is the number of unpaired electrons. For $\mu = 2.82 \ B.M.$,$n=2

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$\left[NiCl_4\right]^{2-}$

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(B) The spin-only magnetic moment $\mu$ is given by $\sqrt{n(n+2)} \ B.M.$,where $n$ is the number of unpaired electrons. For $\mu = 2.82 \ B.M.$,$n=2$.$(A)$ $Ni(CO)_4$: $Ni$ is in $0$ oxidation state. $Ni(0) = 3d^8 4s^2$. $CO$ is a strong field ligand,causing pairing of electrons. All electrons are paired $(n=0)$.$(B)$ $\left[NiCl_4\right]^{2-}$: $Ni$ is in $+2$ oxidation state. $Ni^{2+} = 3d^8$. $Cl^-$ is a weak field ligand,so no pairing occurs. The $3d$ orbitals have $2$ unpaired electrons $(n=2)$. Thus,$\mu = \sqrt{2(2+2)} = \sqrt{8} \approx 2.82 \ B.M.$$(C)$ $Ni\left(PPh_3\right)_4$: $Ni$ is in $0$ oxidation state. $Ni(0) = 3d^8 4s^2$. $PPh_3$ is a strong field ligand,causing pairing. All electrons are paired $(n=0)$.$(D)$ $\left[Ni(CN)_4\right]^{2-}$: $Ni$ is in $+2$ oxidation state. $Ni^{2+} = 3d^8$. $CN^-$ is a strong field ligand,causing pairing. All electrons are paired $(n=0)$.

The complex showing a spin-only magnetic moment of $2.82 \ B.M.$ is

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