Transition metal colours and various oxidation states:
Coloured compounds have partially filled or incomplete d–orbitals.
Absorption of light energy excites electrons this colour is due to d e– being excited to higher energy d orbital on absorption of certain frequencies of visible light. The colour seen is the colour not absorbed.
Example:
Fe2+ has partially filled d–orbitals It can absorb all light wavelengths except for the green wavelength which it reflects.
Ca2+ no occupied or partly filled d–orbitals so reflects all light wave lengths and so is white.
Zn2+ all d–orbitals are filled. There are no partly filled d orbitals so also reflects all wavelengths of light and so is white.
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