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Transition metals are known for their ability to exhibit variable oxidation states, which is one of their most notable characteristics. This property arises from the electrons in the d-orbitals of these metals, allowing them to lose different numbers of electrons and form multiple oxidation states.

For example, iron can have oxidation states of +2 and +3, copper can exist in +1 and +2 states, and manganese can have oxidation states ranging from +2 to +7. This variability in oxidation states is essential in many chemical processes, including catalysis and the formation of coordination complexes, which are important in various applications, including biological systems and industrial processes.

In contrast, the other options highlight characteristics that do not align with the nature of transition metals. The formation of only one oxidation state is more typical of certain main group elements rather than transition metals. While some transition metal complexes might appear colorless, many exhibit vibrant colors due to the d-d electron transitions when they are in solution. Lastly, transition metals are metals, not nonmetals. The combination of these traits distinctly separates transition metals from other categories of elements.