Transition metal compounds are usually coloured because
Correct answer: A. electrons move between d orbitals split by the ligands, absorbing part of the visible spectrum
- A. electrons move between d orbitals split by the ligands, absorbing part of the visible spectrum
- B. the metals reflect all wavelengths equally
- C. they contain water of crystallisation
- D. their ions are very large
Explanation
Ligands split the five d orbitals into groups of slightly different energy, and the small energy gap corresponds to visible light, so the complex absorbs one part of the spectrum and appears in the complementary colour. Ions with an empty or completely full d subshell, such as Sc3+ and Zn2+, have no such transition available and their compounds are white. Changing the ligand changes the gap, and hence the colour.
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About Electronic Structure of d-Block Elements
The electronic structure of d-block elements covers the filling of the (n-1)d and ns orbitals, general electronic configurations, and the exceptions shown by chromium and copper. It explains how partially filled d orbitals produce variable oxidation states, coloured ions, magnetic behaviour and complex formation, while distinguishing transition elements from elements with completely filled d subshells.
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