Final answer:
Non-transition elements have limited and stable oxidation states, while transition metals can display a wide range of oxidation states due to the involvement of their d-orbitals. Transition metals form ionic compounds in lower oxidation states and covalent compounds in higher oxidation states.
Step-by-step explanation:
Non-transition elements typically exhibit fewer and more predictable oxidation states compared to transition elements. For instance, alkali metals have a +1 oxidation state, while alkaline earth metals have a +2 oxidation state. These oxidation states tend to be stable because non-transition elements tend to either lose or gain electrons to achieve a noble gas electron configuration.
In contrast, transition metals have a much more complex chemistry due to the involvement of their d-orbitals. They can exhibit a wide range of oxidation states, often within a single element. For example, manganese can have oxidation states from +2 to +7. Transition metals form ionic compounds in their lower oxidation states and more covalent compounds or polyatomic ions in their higher oxidation states. The higher oxidation states are possible due to the ability of d-orbitals to participate in bonding, which also leads to the variety of possible oxidation states.
Moreover, the nature of bonding in transition metal compounds, such as oxides, changes with the oxidation state. Transition metal oxides with low oxidation states are more ionic, while those with high oxidation states are more covalent. This variation is attributed to the changing electronegativities of the transition metals as their oxidation state changes.