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(A) The colour of metal salts is generally due to $d-d$ transitions,which require the presence of unpaired electrons in the $d$-orbitals.In $TiCl_4$,t

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$Ce(SO_4)_2$

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(A) The colour of metal salts is generally due to $d-d$ transitions,which require the presence of unpaired electrons in the $d$-orbitals.In $TiCl_4$,the oxidation state of $Ti$ is $+4$,which corresponds to a $3d^0$ configuration (no unpaired electrons).In $Cu_2Cl_2$,the oxidation state of $Cu$ is $+1$,which corresponds to a $3d^{10}$ configuration (no unpaired electrons).In $Ce(SO_4)_2$,the oxidation state of $Ce$ is $+4$. Although $Ce^{4+}$ has a $4f^0$ configuration,$Ce(SO_4)_2$ is known to be yellow in colour. This colour arises due to charge transfer transitions rather than $d-d$ transitions.Therefore,$Ce(SO_4)_2$ is the coloured compound among the given options.

Generally,metal ions and their salts are coloured due to the presence of unpaired electrons in the metal ions. Which of the following compounds is coloured?

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