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

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(D) To determine the colourless species,we check for the presence of unpaired electrons in the metal ions:$1$. In $TiF_6^{2-}$,$Ti$ is in the $+4$ oxi

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

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(D) To determine the colourless species,we check for the presence of unpaired electrons in the metal ions:$1$. In $TiF_6^{2-}$,$Ti$ is in the $+4$ oxidation state. The electronic configuration of $Ti^{4+}$ is $[Ar] 3d^0$. Since there are no $d$-electrons,it is colourless.$2$. In $CoF_6^{3-}$,$Co$ is in the $+3$ oxidation state. The configuration of $Co^{3+}$ is $[Ar] 3d^6$. It has unpaired electrons,so it is coloured.$3$. In $Cu_2Cl_2$,$Cu$ is in the $+1$ oxidation state. The configuration of $Cu^+$ is $[Ar] 3d^{10}$. Since the $d$-subshell is completely filled,there are no unpaired electrons,making it colourless.$4$. In $NiCl_4^{2-}$,$Ni$ is in the $+2$ oxidation state. The configuration of $Ni^{2+}$ is $[Ar] 3d^8$. It has unpaired electrons,so it is coloured.Therefore,$TiF_6^{2-}$ and $Cu_2Cl_2$ are the colourless species.

Amongst $TiF_6^{2-}$,$CoF_6^{3-}$,$Cu_2Cl_2$,and $NiCl_4^{2-}$ (Atomic numbers: $Ti=22, Co=27, Cu=29, Ni=28$),the colourless species are:

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