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(B) Ions are coloured if they possess unpaired electrons in their $d$-orbitals due to $d-d$ transitions.$Sc^{3+} \rightarrow [Ar] 3d^{0}$ (No unpaired

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$Ni^{2+}, Ti^{3+}$

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(B) Ions are coloured if they possess unpaired electrons in their $d$-orbitals due to $d-d$ transitions.$Sc^{3+} \rightarrow [Ar] 3d^{0}$ (No unpaired electrons,colourless)$Ti^{3+} \rightarrow [Ar] 3d^{1}$ (One unpaired electron,coloured)$Ni^{2+} \rightarrow [Ar] 3d^{8}$ (Two unpaired electrons,coloured)$Cu^{+} \rightarrow [Ar] 3d^{10}$ (No unpaired electrons,colourless)$Co^{2+} \rightarrow [Ar] 3d^{7}$ (Three unpaired electrons,coloured)Comparing the options:$A$: $Ni^{2+}$ (coloured),$Cu^{+}$ (colourless)$B$: $Ni^{2+}$ (coloured),$Ti^{3+}$ (coloured)$C$: $Sc^{3+}$ (colourless),$Ti^{3+}$ (coloured)$D$: $Sc^{3+}$ (colourless),$Co^{2+}$ (coloured)Thus,both ions are coloured in option $B$.

In which of the following pairs are both the ions coloured in aqueous solution?
(At. no. $:$ $Sc = 21, Ti = 22, Ni = 28, Cu = 29, Co = 27$)

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In which of the following pairs are both the ions coloured in aqueous solution?(At. no. $:$ $Sc = 21, Ti = 22, Ni = 28, Cu = 29, Co = 27$)