1. Electronic Configuration:
* Sodium has one electron in its outermost shell (valence electron).
* Chlorine has seven electrons in its outermost shell.
2. The Drive for Stability:
* Atoms strive for a full outer shell of electrons for stability. This is the basis of the octet rule (except for hydrogen and helium which aim for a duet, meaning two electrons in their outer shell).
3. Transfer of Electrons:
* Sodium easily loses its single valence electron to become a positively charged ion (Na+).
* Chlorine readily gains one electron to fill its outer shell, becoming a negatively charged ion (Cl-).
4. Electrostatic Attraction:
* The oppositely charged sodium and chloride ions attract each other due to electrostatic forces, forming an ionic bond. This attraction holds the ions together in a crystal lattice structure.
5. Formation of Sodium Chloride (NaCl):
* The strong electrostatic attraction between Na+ and Cl- ions results in the formation of sodium chloride (NaCl), a neutral compound.
In summary: Sodium forms an ionic bond with chlorine by donating its valence electron to chlorine, resulting in the formation of stable ions that attract each other due to their opposite charges. This attraction leads to the formation of sodium chloride (NaCl).
