the transition metals generally form coloured compound
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Explanation:
ransition elements are usually characterised by having d orbitals. Now when the metal is not bonded to anything else, these d orbitals are degenerate, meaning that they all have the same energy level.
However when the metal starts bonding with other ligands, this changes. Due to the different symmetries of the d orbitals and the inductive effects of the ligands on the electrons, the d orbitals split apart and become non-degenerate (have different energy levels).
This forms the basis of Crystal Field Theory. How these d orbitals split depend on the geometry of the compound that is formed. For example if an octahedral metal complex is formed, the energy of the d orbitals will look like this:
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- Most of the complexes of transition metals are coloured.
- This is because of the absorption of radiation from visible light region to promote an electron from one of the d−orbitals to another.
- In the presence of ligands, the d-orbitals split up into two sets of orbitals having different energies.
- Therefore, the transition of electrons can take place from one set toanother.
- The energy required for these transitions is quite small and falls in the visible region of radiation.
- The ions of transition metals absorb the radiation of a particular wavelength and the rest is reflected, imparting colour to the solution.
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