* Octet Rule: Nonmetals, like most elements, strive to have a full outer shell of eight electrons (except for hydrogen and helium, which only need two). This arrangement is considered stable and energetically favorable.
* Electronegativity: Nonmetals have high electronegativity, meaning they have a strong attraction for electrons.
* Ionic Bonding: When a nonmetal encounters a metal, it can steal electrons from the metal. This creates negatively charged ions (anions) from the nonmetal and positively charged ions (cations) from the metal. These oppositely charged ions then attract each other and form an ionic bond, like in the case of sodium chloride (NaCl).
* Covalent Bonding: When two nonmetals meet, they share electrons to achieve a full outer shell. This sharing of electrons forms a covalent bond, like in the case of water (H₂O).
Examples:
* Oxygen (O): Oxygen has six electrons in its outer shell. It needs to gain two more electrons to achieve an octet. It can do this by forming covalent bonds with two hydrogen atoms, resulting in water (H₂O).
* Chlorine (Cl): Chlorine has seven electrons in its outer shell. It needs to gain one electron to achieve an octet. It can do this by forming an ionic bond with sodium (Na), resulting in sodium chloride (NaCl).
In summary: Nonmetals achieve stability by gaining electrons through either ionic or covalent bonding, allowing them to complete their outer electron shell and achieve a more stable, lower energy state.
