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

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$[NiCl_4]^{2-}$

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(B) The magnetic moment is given by the formula $\mu = \sqrt{n(n+2)} \ BM$,where $n$ is the number of unpaired electrons.For $\mu = 2.82 \ BM$,$n$ must be $2$.In $Ni(CO)_4$,$Ni$ is in $0$ oxidation state $(3d^8 4s^2)$. $CO$ is a strong field ligand,causing pairing of electrons,resulting in $n=0$.In $[NiCl_4]^{2-}$,$Ni$ is in $+2$ oxidation state $(3d^8)$. $Cl^-$ is a weak field ligand,so electrons do not pair up,resulting in $n=2$.In $Ni(PPh_3)_4$,$Ni$ is in $0$ oxidation state,resulting in $n=0$.In $[Ni(CN)_4]^{2-}$,$Ni$ is in $+2$ oxidation state $(3d^8)$. $CN^-$ is a strong field ligand,causing pairing of electrons,resulting in $n=0$.Thus,$[NiCl_4]^{2-}$ has $2$ unpaired electrons and a magnetic moment of $2.82 \ BM$.

Which of the following complex ions will have a magnetic moment of $2.82 \ BM$?

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