Assertion : [Fe(CN)_6]^{3-} is weakly paramag | vedclass

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(B) In $[Fe(CN)_6]^{3-}$,$Fe$ is in $+3$ oxidation state ($3d^5$ configuration). Due to the strong field ligand $CN^-$,the electrons pair up,leaving $

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If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.

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(B) In $[Fe(CN)_6]^{3-}$,$Fe$ is in $+3$ oxidation state ($3d^5$ configuration). Due to the strong field ligand $CN^-$,the electrons pair up,leaving $1$ unpaired electron,making it paramagnetic.In $[Fe(CN)_6]^{4-}$,$Fe$ is in $+2$ oxidation state ($3d^6$ configuration). Due to the strong field ligand $CN^-$,all $6$ electrons pair up in the $t_{2g}$ orbitals,leaving $0$ unpaired electrons,making it diamagnetic.Both statements are true,but the magnetic property depends on the number of unpaired electrons resulting from the crystal field splitting and the nature of the ligand,not just the oxidation state. Thus,the Reason is not the correct explanation of the Assertion.

List-$I$ (Complexes)	List-$II$ (Types)
$a$. $[Co(NH_3)_5NO_2]Cl_2$ and $[Co(NH_3)_5ONO]Cl_2$	$i$. Linkage isomerism
$b$. $[Cr(NH_3)_6][Co(CN)_6]$ and $[Cr(CN)_6][Co(NH_3)_6]$	$ii$. Coordination isomerism
$c$. $[Co(NH_3)_5(SO_4)]Br$ and $[Co(NH_3)_5Br]SO_4$	$iii$. Ionisation isomerism
$d$. $[Cr(H_2O)_6]Cl_3$ and $[Cr(H_2O)_5Cl]Cl_2 \cdot H_2O$	$iv$. Solvate isomerism

Assertion : $[Fe(CN)_6]^{3-}$ is weakly paramagnetic while $[Fe(CN)_6]^{4-}$ is diamagnetic.
Reason : $[Fe(CN)_6]^{3-}$ has $+3$ oxidation state while $[Fe(CN)_6]^{4-}$ has $+2$ oxidation state.

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Assertion : $[Fe(CN)_6]^{3-}$ is weakly paramagnetic while $[Fe(CN)_6]^{4-}$ is diamagnetic.Reason : $[Fe(CN)_6]^{3-}$ has $+3$ oxidation state while $[Fe(CN)_6]^{4-}$ has $+2$ oxidation state.