Which one of the following has the lowest val | vedclass

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(D) The magnetic behavior of a coordination compound depends on the number of unpaired electrons present in the central metal ion.$1$. In $[Cr(CN)_6]^

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$[Co(CN)_6]^{3-}$

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(D) The magnetic behavior of a coordination compound depends on the number of unpaired electrons present in the central metal ion.$1$. In $[Cr(CN)_6]^{3-}$,$Cr^{3+}$ is $3d^3$. Number of unpaired electrons = $3$.$2$. In $[Mn(CN)_6]^{3-}$,$Mn^{3+}$ is $3d^4$. In the presence of a strong field ligand $CN^-$,electrons pair up. Number of unpaired electrons = $2$.$3$. In $[Fe(CN)_6]^{3-}$,$Fe^{3+}$ is $3d^5$. In the presence of a strong field ligand $CN^-$,electrons pair up. Number of unpaired electrons = $1$.$4$. In $[Co(CN)_6]^{3-}$,$Co^{3+}$ is $3d^6$. In the presence of a strong field ligand $CN^-$,all electrons pair up. Number of unpaired electrons = $0$.Since $[Co(CN)_6]^{3-}$ has $0$ unpaired electrons,it is diamagnetic and has the lowest magnetic behavior.

Which one of the following has the lowest value of magnetic behavior?

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