How do valence electrons affect the way atoms form compounds?

Valence electrons are the negatively charged particles located in the outermost region of an atom that determine how it interacts with other atoms to form chemical bonds. Because these electrons are more weakly attracted to the atomic nucleus than inner electrons, they can be shared or transferred during the formation of compounds.1

The behavior of valence electrons in bonding is primarily driven by the tendency of atoms to achieve a stable electronic configuration, often resembling that of a noble gas. Atoms achieve this stability in three main ways:23

• Ionic Bonding: Elements with significantly different electronegativities may transfer valence electrons. A metal typically loses its few valence electrons to a nonmetal, creating oppositely charged ions that are held together by electrostatic attraction.456
• Covalent Bonding: When atoms have similar electronegativities—often occurring between nonmetals—they may share pairs of valence electrons to achieve stability. These shared pairs form covalent bonds, which can be single, double, or triple depending on the number of pairs shared.43
• Metallic Bonding: In metals, valence electrons are released in a way that allows them to move freely, facilitating the conduction of electric current.16