Chemistry - Complete d-block Question with Solution | TestHub

In${\text{CuCl}}_2,$${\text{Cu}}^{\text{2+}}$has${\text{d}}^{\text{9}}$configuration, exhibit$\text{d-d}$transition and show colour. Similarly in${\text{VOCl}}_{\text{2}}\text{,}$${\text{V}}^{\text{4+}}$has${\text{d}}^{\text{1}}$configuration, can exhibit$\text{d-d}$transition and show colour.

${\text{MnCl}}_{\text{2}}\text{=}$Pink colour

${\text{Zn}}^{2+}\Rightarrow {\text{3d}}^{10}\left(\text{Colourless}\right)$

${\text{Hg}}^{2+}\Rightarrow {\text{5d}}^{10}\left(\text{Colourless}\right)$

$\text{V}=4{\text{s}}^{2}3{\text{d}}^3$

${\text{V}}^{4+}={\text{4s}}^0{3d}^1$(d - d transition)

${\text{Cu}}^{\text{+2}}\text{=}{\text{d}}^{\text{9}}$configuration =$\text{1}$- unpaired${\text{e}}^{-}$electrons.

Since, in both${\text{CuCl}}_{\text{2}}$and${\text{VOCl}}_{\text{2}},{\text{Cu}}^{\text{2+}}$and${\text{V}}^{\text{4+}}$ion contain 1 unpaired electron each, so their colour may be same.