Question

Explain the following about transition metals:

Oxidation states

Answer 1

1. Transition metals exhibit variable oxidation states, commonly more than one in their compounds.
2. This variability is due to the involvement of both (n − 1)d and ns electrons in bonding.
3. Lower oxidation states (+1, +2) typically involve ns electrons, while higher states (+3, +4, +5, ...) involve d electrons too.
4. Most first transition series elements show +2 as a common oxidation state due to the loss of two 4s electrons.
5. The stability of oxidation states depends on the electronic configuration; half-filled or filled d-subshells are more stable.
6. Transition metals show the highest oxidation states in oxides and fluorides.