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(A) The colour of transition metal ions in aqueous solution depends on the presence of unpaired electrons ($d-d$ transition). For $Sc^{3+}$ $(Z=21)$:

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$Sc^{3+}$

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(A) The colour of transition metal ions in aqueous solution depends on the presence of unpaired electrons ($d-d$ transition). For $Sc^{3+}$ $(Z=21)$: Electronic configuration is $[Ar] 3d^0 4s^0$. Since there are $0$ unpaired electrons,$Sc^{3+}$ is colourless. For $Fe^{2+}$ $(Z=26)$: $[Ar] 3d^6$ ($4$ unpaired electrons). For $Ti^{3+}$ $(Z=22)$: $[Ar] 3d^1$ ($1$ unpaired electron). For $Mn^{2+}$ $(Z=25)$: $[Ar] 3d^5$ ($5$ unpaired electrons).

Which one of the following ions will be colourless in an aqueous solution? (Atomic numbers: $Sc = 21, Fe = 26, Ti = 22, Mn = 25$)

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