Which of the following compounds is expected to be coloured?

Transition metal compounds are colored due to the presence of unpaired electrons undergoing $d\text{-}d$ transitions. In ${\text{CuF}}_2$, Copper is in the ${\text{Cu}}^{2+}$ oxidation state with a $3d^9$ electronic configuration, containing an unpaired electron, making it blue/colored. In contrast, ${\text{Ag}}^{+}$ (${\text{Ag}}_2{\text{SO}}_4$) and ${\text{Cu}}^{+}$ ($\text{CuCl}$) have full $3d^{10}$ configurations, and ${\text{Mg}}^{2+}$ (${\text{MgF}}_2$) is an $s$ -block ion with no partially filled $d$ -orbitals, rendering them colorless.