Which group of elements can demonstrate a range of oxidation states?

The transition elements are known for their ability to exhibit a variety of oxidation states due to their unique electron configurations. These elements, found in the d-block of the periodic table, have partially filled d-orbitals that allow them to lose different numbers of electrons when forming compounds. This flexibility in electron loss leads to a wide range of oxidation states, which is evident in many transition metals like iron, copper, and manganese.

The ability to adopt multiple oxidation states has significant implications in chemistry, particularly in redox reactions, where these elements can act as both oxidizers and reducers. The characteristic variable oxidation states of transition metals also play a crucial role in their complex formation and catalytic activities, making them pivotal in many chemical reactions.

In contrast, other groups of elements, such as halogens, noble gases, and alkaline-earth metals, tend to have more limited oxidation states. Halogens primarily exhibit a -1 oxidation state in ionic compounds, noble gases are mostly inert and do not typically form compounds, and alkaline-earth metals generally show a +2 oxidation state. This stark difference in oxidation state variability is what makes transition elements stand out in this regard.