Question

Why TETRAHEDRAL complexes are generally more intense in colour THAN octahedral complexes

Answer 1

Answer:

An example occurs in octahedral complexes of manganese (ll).... Tetrahedral complexes have somewhat more intense colour. This is because mixed d and p orbitals is possible when there is no center of symmetry. Therefore transition are not pure d-d transition.

Answer 2

The absorption of different wavelengths of light makes TETRAHEDRAL complexes have a more intense colour THAN octahedral complexes.

Tetrahedral and octahedral complexes.

• In the tetrahedral compound, the central atoms bond with four ligands. Octahedral complexes, on the other hand, bind to 5 ligands through their central atom.

Difference in colour

• The extent of d-orbital splitting is different in the two types of complexes. The crystal field stabilization energy(CFSE) of octahedral and tetrahedral complexes re related by:

                                    Δt = (4/9)Δo

• Here,  Δt= crystal field energy of the tetrahedral field
• Δo= crystal field energy of the octahedral field

       The wavelength of light and CFSE is related by the formula:

                                        Δt = E=hc/λ

Tetrahedral complexes absorb lower wavelength of light than octahedral complexes. Thus, they tend to be of more intense colour than octahedral compounds.