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

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Question

(A) The colour of coordination compounds arises due to $d-d$ transitions.
The energy gap $(\Delta_o)$ between $t_{2g}$ and $e_g$ orbitals depends on

Vedclass · Accepted Answer

$CN^{-}$ is a strong field ligand and $H_2O$ is a weak field ligand,hence the magnitude of $CFSE$ is different

Vedclass · Answer

(A) The colour of coordination compounds arises due to $d-d$ transitions.
The energy gap $(\Delta_o)$ between $t_{2g}$ and $e_g$ orbitals depends on the strength of the ligand.
$CN^{-}$ is a strong field ligand,which causes a larger splitting $(\Delta_o)$,while $H_2O$ is a weak field ligand,causing smaller splitting.
Since the energy gap is different,they absorb different wavelengths of light from the visible spectrum,resulting in different observed colours.

$[Fe(CN)_6]^{4-}$ and $[Fe(H_2O)_6]^{2+}$ show different colours in dilute solution because

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