1. Transition Metals: The transition metals (groups 3-12) are all multivalent. This is because they have variable oxidation states due to the presence of d-electrons that can participate in bonding. Examples include iron (Fe), copper (Cu), and manganese (Mn).
2. Post-Transition Metals: Some metals in groups 13-15, particularly towards the bottom of the groups, also exhibit multiple oxidation states. This is because their valence electrons are more readily available for bonding. Examples include tin (Sn), lead (Pb), and bismuth (Bi).
Keep in mind that not all metals in these areas are multivalent. For example, zinc (Zn) and cadmium (Cd) are primarily divalent.
