The color of transition metal complexes is complementary to the absorbed light; for example, if green light is absorbed, the complex appears red. The wide range of colors arises from the removal of specific wavelengths from white light as it passes through the sample.
How does the color of transition metal complexes relate to the absorption of light in the visible spectrum?
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The color of transition metal complexes is related to the absorption of light in the visible spectrum through the phenomenon of ligand-field theory. Transition metals in complexes exhibit d-d transitions, where electrons in the d orbitals absorb photons and move to higher energy levels. The energy difference between the ground state and the excited state corresponds to a specific wavelength, giving rise to color. The color observed is complementary to the absorbed wavelength. For instance, absorption in the red region results in a green color. The specific color depends on the metal, ligands, and electronic transitions involved, providing a valuable tool in studying complex structures.