Which outer electron configuration would you expect to belong to a reactive metal? a. ns² b. ns²np⁶ c. ns²np⁵ d. ns²np²

Key Concepts

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It is represented using a notation that indicates the energy levels and sublevels occupied by electrons. Understanding electron configuration is crucial for predicting an element's chemical properties, including its reactivity.

Reactivity of Metals

The reactivity of metals is largely determined by their electron configuration, particularly the number of valence electrons. Metals tend to lose electrons to achieve a stable electron configuration, often resembling that of the nearest noble gas. Reactive metals typically have one or two electrons in their outermost shell, making them more likely to participate in chemical reactions.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom and are responsible for an element's chemical behavior. The number of valence electrons influences how an element interacts with others, including its tendency to gain, lose, or share electrons. In the context of the question, the configuration with fewer valence electrons indicates a higher likelihood of reactivity.