Of the following complex ions,which is diamag | vedclass

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(NONE) To determine the magnetic nature,we analyze the electronic configuration of the central metal ion in each complex:$1$. In $[NiCl_4]^{2-}$,$Ni$

Vedclass · Accepted Answer

$[Co(H_2O)_6]^{3+}$

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(NONE) To determine the magnetic nature,we analyze the electronic configuration of the central metal ion in each complex:$1$. In $[NiCl_4]^{2-}$,$Ni$ is in $+2$ oxidation state $(3d^8)$. $Cl^-$ is a weak field ligand,so it forms a tetrahedral complex with $sp^3$ hybridization,resulting in $2$ unpaired electrons (paramagnetic).$2$. In $[Co(H_2O)_6]^{3+}$,$Co$ is in $+3$ oxidation state $(3d^6)$. $H_2O$ is a weak field ligand,resulting in $4$ unpaired electrons (paramagnetic).$3$. In $[CuCl_4]^{2-}$,$Cu$ is in $+2$ oxidation state $(3d^9)$,resulting in $1$ unpaired electron (paramagnetic).$4$. In $[CoF_6]^{3-}$,$Co$ is in $+3$ oxidation state $(3d^6)$. $F^-$ is a weak field ligand,resulting in $4$ unpaired electrons (paramagnetic).Wait,checking the options again: none of these are diamagnetic. Let us re-evaluate the question. If the question implies a common complex like $[Ni(CN)_4]^{2-}$,it would be diamagnetic. Given the provided options,all are paramagnetic. However,if we must choose,there might be a typo in the provided options. Assuming the question intended to include a diamagnetic complex,but based on the provided list,none are diamagnetic.

Of the following complex ions,which is diamagnetic in nature?

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