Final answer:
Transition metals possess multiple oxidation states due to their unique electronic configurations, with some nonmetals also exhibiting a range of oxidation states. The number of oxidation states typically increases and then decreases as you move across the transition series. Alkali and alkaline earth metals show more limited oxidation states of +1 and +2, respectively.
Step-by-step explanation:
Transition metals are known for having multiple oxidation states. This is in contrast to alkali and alkaline earth metals which typically exhibit oxidation states of +1 and +2, respectively. Due to the electronic configuration of transition metals, particularly the presence of d-orbital electrons, these metals can lose different numbers of electrons, leading to a variety of possible oxidation numbers. For example, iron commonly exhibits oxidation states of +2 and +3, but can have other states as well. Manganese exhibits a wide range of oxidation states, from +2 to +7. The possibility of synthesizing new oxidation states for these elements remains open, as demonstrated by the creation of a +9 oxidation state for iridium in 2014.
Nonmetals also have common oxidation states which vary depending on the elements they combine with. An element will have a positive oxidation state when combined with a more electronegative element and a negative state when combined with a less electronegative element. Some nonmetals like sulfur, nitrogen, and chlorine have a particularly wide range of possible oxidation states due to their electron configurations and reactivity.