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

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(D) To determine the colour of transition metal complexes,we check for the presence of unpaired $d$-electrons. If a complex has a $d^0$ or $d^{10}$ co

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

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(D) To determine the colour of transition metal complexes,we check for the presence of unpaired $d$-electrons. If a complex has a $d^0$ or $d^{10}$ configuration,it is generally colourless.$1$. $TiF_6^{2-}$: $Ti$ 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.$2$. $CoF_6^{3-}$: $Co$ is in the $+3$ oxidation state. The electronic configuration of $Co^{3+}$ is $[Ar] 3d^6$. It has unpaired electrons,so it is coloured.$3$. $Cu_2Cl_2$: $Cu$ is in the $+1$ oxidation state. The electronic configuration of $Cu^+$ is $[Ar] 3d^{10}$. Since the $d$-subshell is completely filled,it is colourless.$4$. $NiCl_4^{2-}$: $Ni$ is in the $+2$ oxidation state. The electronic 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 $NiCl_4^{2-}$,the colourless species are:

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