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

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(D) species is colourless if it does not have any unpaired electrons in its $d$-orbitals,preventing $d-d$ transitions.$1$. In $TiF_6^{2-}$,the oxidati

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

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(D) species is colourless if it does not have any unpaired electrons in its $d$-orbitals,preventing $d-d$ transitions.$1$. In $TiF_6^{2-}$,the oxidation state of $Ti$ is $+4$. The electronic configuration of $Ti^{4+}$ is $3d^0$,which has no electrons to undergo $d-d$ transition.$2$. In $Cu_2Cl_2$,the oxidation state of $Cu$ is $+1$. The electronic configuration of $Cu^+$ is $3d^{10}$,which is fully filled,preventing $d-d$ transition.$3$. In $CoF_6^{3-}$,$Co$ is in $+3$ state $(3d^6)$,which has unpaired electrons.$4$. In $NiCl_4^{2-}$,$Ni$ is in $+2$ state $(3d^8)$,which has unpaired electrons.Therefore,$TiF_6^{2-}$ and $Cu_2Cl_2$ are colourless.

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

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