* Electronegativity: Nonmetals have higher electronegativity than metals. Electronegativity is the ability of an atom to attract electrons towards itself.
* Valence Electrons: Nonmetals typically have nearly full outer electron shells. They want to achieve a stable configuration with eight electrons in their outermost shell (octet rule). Gaining electrons helps them achieve this.
* Formation of Anions: When nonmetals gain electrons, they form negatively charged ions called anions.
Example:
Consider the reaction between sodium (a metal) and chlorine (a nonmetal) to form sodium chloride (NaCl):
* Sodium (Na) has one electron in its outermost shell and tends to lose it to become a positively charged ion (Na+).
* Chlorine (Cl) has seven electrons in its outermost shell and tends to gain one electron to become a negatively charged ion (Cl-).
In this reaction, the nonmetal chlorine gains an electron from the metal sodium, forming an ionic bond between them.
Exceptions:
While nonmetals typically gain electrons, there are some exceptions. For example, in some reactions, nonmetals can share electrons with other nonmetals, forming covalent bonds.
