Absorbed colour of the solutions of the follo | vedclass

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(C) According to the spectrochemical series,the field strength of the ligands is $Cl^- < H_2O < NH_3$. Since the crystal field splitting energy $\Delt

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Violet,Blue and Red

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(C) According to the spectrochemical series,the field strength of the ligands is $Cl^- Since the crystal field splitting energy $\Delta_o$ is directly proportional to the field strength of the ligand,the order of $\Delta_o$ is $[MCl_4]^{2-} The energy of the absorbed light is $E = h
u = \frac{hc}{\lambda}$. As $\Delta_o$ increases,the wavelength of the absorbed light $(\lambda)$ decreases. The order of wavelengths of absorbed light is: $[MCl_4]^{2-} > [M(H_2O)_6]^{2+} > [M(NH_3)_6]^{2+}$. Corresponding to these wavelengths,the absorbed colours follow the order: Red (for $[MCl_4]^{2-}$),Blue (for $[M(H_2O)_6]^{2+}$),and Violet (for $[M(NH_3)_6]^{2+}$). Therefore,the absorbed colours for $[M(NH_3)_6]^{2+}$,$[M(H_2O)_6]^{2+}$ and $[MCl_4]^{2-}$ are Violet,Blue and Red respectively.

List-$I$	List-$II$
$P$. $t_{2g}^6 e_g^0$	$1$. $[Fe(H_2O)_6]^{2+}$
$Q$. $t_{2g}^3 e_g^2$	$2$. $[Mn(H_2O)_6]^{2+}$
$R$. $e^2 t_2^3$	$3$. $[Co(NH_3)_6]^{3+}$
$S$. $t_{2g}^4 e_g^2$	$4$. $[FeCl_4]^{-}$
	$5$. $[CoCl_4]^{2-}$

Absorbed colour of the solutions of the following complexes $[M(NH_3)_6]^{2+}$,$[M(H_2O)_6]^{2+}$ and $[MCl_4]^{2-}$ are respectively (having the same metal ion):

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