Out of TiF_6^{2-},CoF_6^{3-},Cu_2Cl_2 and NiC | vedclass

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(B) To determine if a species is colourless,we check for the presence of unpaired electrons in the $d$-orbitals. If the $d$-orbital is either complete

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

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(B) To determine if a species is colourless,we check for the presence of unpaired electrons in the $d$-orbitals. If the $d$-orbital is either completely empty $(d^0)$ or completely filled $(d^{10})$,the species is colourless due to the absence of $d-d$ transitions.$1$. $TiF_6^{2-}$: $Ti$ is in $+4$ oxidation state. Electronic configuration: $Ti^{4+} = [Ar] 3d^0$. Since it has no $d$-electrons,it is colourless.$2$. $CoF_6^{3-}$: $Co$ is in $+3$ oxidation state. Electronic configuration: $Co^{3+} = [Ar] 3d^6$. It has unpaired electrons,so it is coloured.$3$. $Cu_2Cl_2$: $Cu$ is in $+1$ oxidation state. Electronic configuration: $Cu^{+} = [Ar] 3d^{10}$. Since the $d$-orbital is fully filled,it is colourless.$4$. $NiCl_4^{2-}$: $Ni$ is in $+2$ oxidation state. Electronic configuration: $Ni^{2+} = [Ar] 3d^8$. It has unpaired electrons,so it is coloured.Therefore,$TiF_6^{2-}$ and $Cu_2Cl_2$ are the colourless species.

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

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