Why d block elements show various colours can u explain
Answers
Answered by
0
d block elements show color in both solid and solution form due to their electrons.
Transition 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
Transition 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
Answered by
0
d block elements show color in both solid and solution form due to their electrons. Transition ... This explains why not all transition metal complexes are colourful. For example copper
Similar questions