Semmelweis Chemistry Entrance Practice Exam

Transition metals exhibit versatility primarily through their ability to form variable oxidation states. This characteristic is critical because it allows transition metals to participate in a wide range of chemical reactions and to create a diverse array of compounds. The presence of d electrons enables these metals to lose different numbers of electrons when they interact with other elements, leading to multiple oxidation states. For example, iron can exist in +2 and +3 oxidation states, while manganese can have several states ranging from +2 to +7.

This variability in oxidation states is fundamental in many applications, including catalysis, where transition metals act as catalysts in various chemical reactions by transitioning between different oxidation states to facilitate electron transfer. Their ability to form different bonds and coordination complexes also stems from this versatility, contributing further to their importance in biological systems and industrial processes.

In contrast, forming strong covalent bonds exclusively or having a fixed oxidation state would limit the chemical reactivity and complexity of transition metals. Similarly, the ability to conduct electricity poorly does not directly relate to their versatility in forming different compounds or participating in varied chemical processes. Therefore, the capacity to adopt various oxidation states is the key aspect of their versatility.