The number of unpaired electrons responsible | vedclass

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(A) $[Fe(CN)_6]^{3-}$: $Fe^{3+}$ is $3d^5$. $CN^-$ is a strong field ligand,so pairing occurs. $t_{2g}^5, e_g^0$. Unpaired electrons = $1$.$[FeF_6]^{3

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$1, 5, 4, 2$

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(A) $[Fe(CN)_6]^{3-}$: $Fe^{3+}$ is $3d^5$. $CN^-$ is a strong field ligand,so pairing occurs. $t_{2g}^5, e_g^0$. Unpaired electrons = $1$.$[FeF_6]^{3-}$: $Fe^{3+}$ is $3d^5$. $F^-$ is a weak field ligand,so no pairing. $t_{2g}^3, e_g^2$. Unpaired electrons = $5$.$[CoF_6]^{3-}$: $Co^{3+}$ is $3d^6$. $F^-$ is a weak field ligand. $t_{2g}^4, e_g^2$. Unpaired electrons = $4$.$[Mn(CN)_6]^{3-}$: $Mn^{3+}$ is $3d^4$. $CN^-$ is a strong field ligand. $t_{2g}^4, e_g^0$. Unpaired electrons = $2$.

The number of unpaired electrons responsible for the paramagnetic nature of the following complex species are respectively $:$
$[Fe(CN)_6]^{3-}, [FeF_6]^{3-}, [CoF_6]^{3-}, [Mn(CN)_6]^{3-}$

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The number of unpaired electrons responsible for the paramagnetic nature of the following complex species are respectively $:$$[Fe(CN)_6]^{3-}, [FeF_6]^{3-}, [CoF_6]^{3-}, [Mn(CN)_6]^{3-}$