Why transition metals are colored?

Answer 1

The 5 orbitals within the 3d subshell have different energies and electrons within the 3d subshell can move up and down these orbitals. The energy transitions within the orbitals of the 3d subshell correspond to the energy of visible light.

Answer 2

Transition metal complexes have colour because the ligands bonding to the central metal atom or ion cause the d-orbitals to have different energies, that is, they are no longer degenerate. In octahedral complexes, the dx2-y2 and the dz2 orbitals are higher in energy than the dxy, dxz and the dyz orbitals. Meanwhile, in tetrahedral complexes, the dxy, dxz and the dyz orbitals are higher in energy than the dx2-y2 and the dz2 orbitals. The energy difference between the orbitals corresponds to some frequency of visible light and the lower energy electrons absorb that energy associated with that frequency of light. When the light is emitted from the substance, the observer sees all the colours except that one absorbed by the substance.

Answer 3

Transition metal compounds exhibit various colors due to the d-d electronic transitions in the d-orbitals. Examples of transition metals are iron, copper, and chromium.

Answer 4

Most transition metals are colored and make some of their ionic compounds colored. This is because they absorb some of the frequencies of white light

Answer 5

It is due to them having partcially filled inner energy levels between groups 2 and 3.

Answer 6

Yes, very many coloured compounds.