Which chemical behavior is typical of metals with low electronegativity in reactions?

Metals with low electronegativity tend to lose electrons readily during chemical reactions. This characteristic is due to their atomic structure, which allows them to easily eliminate their outermost electrons, ultimately resulting in the formation of cations. When these metals lose electrons, they achieve a more stable electron configuration, often resembling the nearest noble gas.

This behavior is a fundamental property of metals, as they generally have a tendency to react by losing valence electrons rather than gaining them. Unlike nonmetals, which are more likely to gain electrons to form anions, metals prefer to ionize into positively charged ions, facilitating various types of reactions, such as those in ionic compounds and in metal reactivity with acids or bases.

The tendency to remain unreactive is more characteristic of noble gases, which have a full valence shell, while the formation of anions typically applies to nonmetals. Therefore, the behavior of losing electrons to form cations aligns perfectly with the typical reactions of low electronegativity metals.