* Metals tend to lose their valence electrons to achieve a stable electron configuration, usually an octet (8 electrons in the outermost shell).
* Nonmetals tend to gain valence electrons to also achieve a stable octet.
Here's how it works:
1. Electron Transfer: When a metal atom interacts with a nonmetal atom, the metal atom *donates* its valence electron(s) to the nonmetal atom.
2. Formation of Ions: This transfer creates two oppositely charged ions:
* The metal atom becomes a cation (positively charged ion) because it has lost electrons.
* The nonmetal atom becomes an anion (negatively charged ion) because it has gained electrons.
3. Electrostatic Attraction: The strong electrostatic attraction between the oppositely charged ions holds them together, forming the ionic bond.
Example: Sodium Chloride (NaCl)
* Sodium (Na) has 1 valence electron. It loses this electron to become a sodium cation (Na+).
* Chlorine (Cl) has 7 valence electrons. It gains one electron to become a chloride anion (Cl-).
* The oppositely charged ions (Na+ and Cl-) are held together by the electrostatic attraction, forming the ionic compound sodium chloride.
Key Points:
* Ionic bonds involve the complete transfer of valence electrons, not sharing.
* The resulting ions have a stable electron configuration, usually an octet.
* The strong electrostatic attraction between the ions is the driving force behind the bond.
