Among TiF_6^{2-}, CoF_6^{3-}, Cu_2Cl_2 and Ni | vedclass

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(D) The colourless species are $TiF_6^{2-}$ and $Cu_2Cl_2$.$1$. In $TiF_6^{2-}$,the oxidation state of $Ti$ is $+4$. The electronic configuration of $

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$TiF_6^{2-}$ and $Cu_2Cl_2$

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(D) The colourless species are $TiF_6^{2-}$ and $Cu_2Cl_2$.$1$. In $TiF_6^{2-}$,the oxidation state of $Ti$ is $+4$. The electronic configuration of $Ti^{4+}$ is $[Ar]3d^0$. Since there are no $d$-electrons,$d-d$ transition is not possible,making it colourless.$2$. In $Cu_2Cl_2$ (or $CuCl$),the oxidation state of $Cu$ is $+1$. The electronic configuration of $Cu^+$ is $[Ar]3d^{10}$. Since the $d$-subshell is completely filled,$d-d$ transition is not possible,making it colourless.

Among $TiF_6^{2-}, CoF_6^{3-}, Cu_2Cl_2$ and $NiCl_4^{2-}$,the colourless species are:

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