Which of the following ions is paramagnetic?

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Question

(A) To determine if a complex is paramagnetic,we check for the presence of unpaired electrons in the metal ion.$1$. In $[Ni(H_2O)_6]^{2+}$,$Ni$ is in

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$[Ni(H_2O)_6]^{2+}$

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(A) To determine if a complex is paramagnetic,we check for the presence of unpaired electrons in the metal ion.$1$. In $[Ni(H_2O)_6]^{2+}$,$Ni$ is in the $+2$ oxidation state $(3d^8)$. $H_2O$ is a weak field ligand,so the electrons remain unpaired,resulting in $2$ unpaired electrons. Thus,it is paramagnetic.$2$. In $[Fe(CN)_6]^{4-}$,$Fe$ is in the $+2$ oxidation state $(3d^6)$. $CN^-$ is a strong field ligand,causing pairing of electrons,resulting in $0$ unpaired electrons. It is diamagnetic.$3$. In $[Ni(CO)_4]$,$Ni$ is in the $0$ oxidation state $(3d^8 4s^2)$. $CO$ is a strong field ligand,causing pairing,resulting in $0$ unpaired electrons. It is diamagnetic.$4$. In $[Ni(CN)_4]^{2-}$,$Ni$ is in the $+2$ oxidation state $(3d^8)$. $CN^-$ is a strong field ligand,causing pairing,resulting in $0$ unpaired electrons. It is diamagnetic.Therefore,$[Ni(H_2O)_6]^{2+}$ is the paramagnetic species.

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