[Fe(H_2O)_6]^{2+} and [Fe(CN)_6]^{4-} differ | vedclass

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Question

(C) In $[Fe(H_2O)_6]^{2+}$, $Fe$ is in $+2$ oxidation state $(3d^6)$. $H_2O$ is a weak field ligand, so no pairing occurs. Hybridization is $sp^3d^2$

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magnetic moment,colour

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(C) In $[Fe(H_2O)_6]^{2+}$, $Fe$ is in $+2$ oxidation state $(3d^6)$. $H_2O$ is a weak field ligand, so no pairing occurs. Hybridization is $sp^3d^2$ (outer orbital complex), it is paramagnetic $(\mu = 4.9 \ B.M.)$, and pale green in colour.
In $[Fe(CN)_6]^{4-}$, $Fe$ is in $+2$ oxidation state $(3d^6)$. $CN^-$ is a strong field ligand, causing pairing of electrons. Hybridization is $d^2sp^3$ (inner orbital complex), it is diamagnetic $(\mu = 0 \ B.M.)$, and yellow in colour.
Both have octahedral geometry and the same number of $d-$ electrons $(6)$.
Therefore, they differ in magnetic moment and colour.

$[Fe(H_2O)_6]^{2+}$ and $[Fe(CN)_6]^{4-}$ differ in

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