When observed under standard laboratory conditions, which of the following aqueous transition metal — d and f Block Elements Chemistry Question

💡 Solution & Explanation

The colours of transition metal ions heavily depend on the specific $d$ -electron count allowing $d-d$ transitions. $V^{3+}$ ($d^2$) is characteristically green; $Mn^{2+}$ ($d^5$, high spin) is very faintly pink; $Fe^{3+}$ ($d^5$) typically appears yellow-brown in aqueous solution due to hydrolysis complexes. However, $Ti^{4+}$ ($d^0$) possesses no $d$ -electrons to undergo any excitation, rendering it perfectly colourless, not purple.