What is the preferred behavior of metals in terms of electrons?

Metals are characterized by their tendency to lose electrons during chemical reactions. This behavior is largely due to their electronic structure, as metals typically have few electrons in their outermost shell—usually one to three. By losing these electrons, metals can achieve a more stable electron configuration, often resembling the noble gases.

This tendency to lose electrons allows metals to form positive ions, known as cations. For example, sodium (Na) easily loses one electron to form Na⁺, while magnesium (Mg) can lose two electrons to form Mg²⁺. The propensity to lose electrons is also what gives metals their characteristic properties, such as conductivity and malleability.

In contrast, nonmetals tend to gain electrons to fill their outer shell and attain stability, while metals do not engage in this behavior. Sharing electrons is more typical of covalent bonding, commonly associated with nonmetals rather than metals.

Therefore, the preferred behavior of metals to lose electrons is fundamental to understanding their chemical reactivity and the nature of metallic bonding.