Which one of the following complex ions is di | vedclass

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(B) To determine the magnetic nature,we analyze the electronic configuration of the central metal ion in each complex:$1$. In $[CoF_6]^{3-}$,$Co$ is i

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$[Co(ox)_3]^{3-}$

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(B) To determine the magnetic nature,we analyze the electronic configuration of the central metal ion in each complex:$1$. In $[CoF_6]^{3-}$,$Co$ is in $+3$ oxidation state $(3d^6)$. $F^-$ is a weak field ligand,so electrons remain unpaired. It is paramagnetic.$2$. In $[Co(ox)_3]^{3-}$,$Co$ is in $+3$ oxidation state $(3d^6)$. $ox^{2-}$ (oxalate) is a strong field ligand,causing pairing of electrons in $t_{2g}$ orbitals. The configuration becomes $t_{2g}^6 e_g^0$,meaning all electrons are paired. Thus,it is diamagnetic.$3$. In $[Mn(CN)_6]^{3-}$,$Mn$ is in $+3$ oxidation state $(3d^4)$. It has unpaired electrons. It is paramagnetic.$4$. In $[Fe(CN)_6]^{3-}$,$Fe$ is in $+3$ oxidation state $(3d^5)$. It has one unpaired electron. It is paramagnetic.Therefore,the correct option is $B$.

Which one of the following complex ions is diamagnetic in nature?

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