The species which has four unpaired electrons | vedclass

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(C) To determine the number of unpaired electrons,we analyze the electronic configuration of the central metal ion in each complex:$1$. In $[Co(CN)_6]

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$[FeCl_4]^{2-}$

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(C) To determine the number of unpaired electrons,we analyze the electronic configuration of the central metal ion in each complex:$1$. In $[Co(CN)_6]^{4-}$,$Co$ is in $+2$ oxidation state $(d^7)$. $CN^-$ is a strong field ligand,causing pairing. Configuration: $t_{2g}^6 e_g^1$,resulting in $1$ unpaired electron.$2$. In $[Cr(H_2O)_6]^{3+}$,$Cr$ is in $+3$ oxidation state $(d^3)$. Configuration: $t_{2g}^3 e_g^0$,resulting in $3$ unpaired electrons.$3$. In $[FeCl_4]^{2-}$,$Fe$ is in $+2$ oxidation state $(d^6)$. $Cl^-$ is a weak field ligand. Configuration: $e^3 t_2^3$,resulting in $4$ unpaired electrons.$4$. In $[Fe(H_2O)_6]^{3+}$,$Fe$ is in $+3$ oxidation state $(d^5)$. $H_2O$ is a weak field ligand. Configuration: $t_{2g}^3 e_g^2$,resulting in $5$ unpaired electrons.Thus,the species with $4$ unpaired electrons is $[FeCl_4]^{2-}$.

The species which has four unpaired electrons is

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