Which property distinguishes metals from nonmetals in reference to electron behavior?

The distinguishing characteristic that separates metals from nonmetals in terms of electron behavior is the tendency of metals to lose electrons. Metals have relatively low electronegativities and ionization energies, making it easier for them to lose electrons and form positive ions (cations) when they undergo chemical reactions. This behavior is a fundamental aspect of metallic bonding and is integral to the formation of metallic compounds.

Nonmetals, on the other hand, tend to gain electrons due to their higher electronegativities, which makes them more likely to form negative ions (anions). The ability to form ionic bonds is, therefore, more indicative of nonmetals but does not specifically capture the electron-losing behavior of metals.

Hybridization characteristics relate to the shapes and bonding capabilities of atoms rather than their fundamental properties concerning electron behavior, which do not capture the distinction between metals and nonmetals in terms of electron loss or gain.

In summary, the tendency of metals to lose electrons is a central property that distinguishes them from nonmetals, reflecting their underlying atomic structure and reactivity.