This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
NG, let's knock this out. The color of transition metal ions in aqueous solution arises from d-d electronic transitions. For these transitions to occur, the metal ion must have partially filled d-orbitals (d^1 to d^9 configuration). Scandium (Sc) has an atomic number of 21, with an electron configuration of [Ar] 3d^1 4s^2. When it forms the Sc^3+ ion, it loses all three valence electrons, resulting in an electron configuration of [Ar] 3d^0. Since there are no d-electrons, no d-d transitions can occur. Zinc (Zn) has an atomic number of 30, with an electron configuration of [Ar] 3d^10 4s^2. When it forms the Zn^2+ ion, it loses its two 4s electrons, resulting in an electron configuration of [Ar] 3d^10. Since the d-orbitals are completely filled, there are no empty d-orbitals for electrons to be promoted to, so no d-d transitions can occur. Because both Sc^3+ and Zn^2+ lack partially filled d-orbitals, they cannot undergo d-d transitions and therefore appear colorless. Send me the next one 📸