Question

the transition metals generally form coloured compound​

Answer 1

Answer:

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:

Answer 2

Answer:

• 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.