Amongst 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 $Cu_2Cl_2$. In $TiF_6^{2-}$,the oxidation state of $Ti$ is $+4$,which corresponds to a $d^0$ configura

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

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(D) The colourless species are $TiF_6^{2-}$ and $Cu_2Cl_2$. In $TiF_6^{2-}$,the oxidation state of $Ti$ is $+4$,which corresponds to a $d^0$ configuration. Since there are no $d$-electrons,$d-d$ transitions are not possible,making it colourless. In $Cu_2Cl_2$,the oxidation state of $Cu$ is $+1$,which corresponds to a $d^{10}$ configuration. Since the $d$-subshell is completely filled,$d-d$ transitions are not possible,making it colourless.

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

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