Compounds of Sc^3+ are not colored, but those of Ti^3+ and V^3+ are. Why?

Name: Problem 17, Chapter 21: Chemistry
Uploaded: 2020-04-21T20:35:24-08:00
Duration: 1 min 57 s
Channel: Kevin Chimex
Description: Compounds of Sc^3+ are not colored, but those of Ti^3+ and V^3+ are. Why?

step 1 This question says compound of Scandium 3 plus are not colored and compound of Titanium 3 plus a

Compounds of Sc^3+ are not colored, but those of Ti^3+ and...

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Key Concepts

Electron Configuration

This concept refers to the distribution of electrons in an atom's orbitals. In the context of transition metal complexes, the occupancy of d orbitals is crucial because it determines whether electronic transitions can occur. For instance, a d^0 configuration, as found in Sc3+, leaves no electrons in the d orbitals, preventing d–d transitions, while d^1 or d^2 configurations allow such movements.

Crystal Field Theory

Crystal Field Theory explains how the degeneracy of the metal ion's d orbitals is lifted when surrounded by ligands. This splitting creates energy differences between orbitals, and if the energy gap falls within the visible spectrum, specific wavelengths of light are absorbed, leading to color. In complexes of metals like Ti3+ and V3+ (with electrons in d orbitals), this splitting is responsible for the observed coloration.

d–d Transitions

d–d transitions involve the excitation of an electron from a lower-energy d orbital to a higher-energy one within the same metal ion. These transitions are only possible when there are electrons in the d orbitals, and they often correspond to energies that match visible light. The absence of electrons in the d orbitals of Sc3+ prevents these transitions, whereas the presence of electrons in Ti3+ and V3+ allows them, resulting in colored compounds.

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