* Electron Configuration: Nonmetals generally have a nearly full outer shell of electrons. They are more stable when they have a full outer shell, which can be achieved by gaining electrons.
* Electronegativity: Nonmetals have higher electronegativity than metals. Electronegativity is a measure of an atom's ability to attract electrons. Nonmetals are "electron hungry" and will readily attract electrons from other atoms.
Examples of nonmetals that gain electrons in bonding:
* Oxygen: Forms an oxide ion (O²⁻) by gaining two electrons.
* Chlorine: Forms a chloride ion (Cl⁻) by gaining one electron.
* Nitrogen: Forms a nitride ion (N³⁻) by gaining three electrons.
Note: While some nonmetals can also share electrons in covalent bonds, their tendency to gain electrons is a defining characteristic.
