General Science • ChemistryHard
Which statement correctly describes the behavior of transition metal ions in aqueous solution regarding their characteristic coloration?
A. They are invariably colorless because paired electrons absorb no visible light
B. Their color arises primarily from d-d electron transitions facilitated by crystal field splitting caused by surrounding ligands✓ Correct Answer
C. Their color is caused entirely by nuclear radioactive decay within visible wavelengths
D. They exhibit color only in strongly acidic solutions due to protonation of metal orbitals
💡 Solution & Explanation
Transition metal complexes are typically colored because their partially filled d orbitals split into different energy levels when surrounded by coordinating ligands. Absorption of specific wavelengths of visible light promotes electrons from lower to higher d sublevels, an event known as a d-d transition, leaving the complementary color transmitted. Ions with completely empty or completely filled d orbitals, such as scandium three-plus or zinc two-plus, lack d-d transitions and remain colorless. Ligand field strength determines the exact energy gap and corresponding absorbed wavelength.
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