Which of the following is paramagnetic?

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Question

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

Vedclass · Accepted Answer

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

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(A) To determine paramagnetism,we check for the presence of unpaired electrons in the central metal ion.$1$. In $[Ni(H_2O)_6]^{2+}$,$Ni$ is in the $+2$ oxidation state ($3d^8$ configuration). $H_2O$ is a weak field ligand,so the electrons remain unpaired in the $3d$ orbitals,resulting in $2$ unpaired electrons. Thus,it is paramagnetic.$2$. In $[Ni(CO)_4]$,$Ni$ is in the $0$ oxidation state $(3d^8 4s^2)$. $CO$ is a strong field ligand,causing pairing of electrons,resulting in $0$ unpaired electrons. Thus,it is diamagnetic.$3$. In $[Zn(NH_3)_4]^{2+}$,$Zn$ is in the $+2$ oxidation state ($3d^{10}$ configuration). All electrons are paired. Thus,it is diamagnetic.$4$. In $[Co(NH_3)_6]^{3+}$,$Co$ is in the $+3$ oxidation state ($3d^6$ configuration). $NH_3$ is a strong field ligand,causing pairing of electrons,resulting in $0$ unpaired electrons. Thus,it is diamagnetic.

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