Sodium (Na)
* Initial State: Sodium has 1 electron in its outermost shell (valence shell). It has the electronic configuration 2, 8, 1.
* Desire: Sodium wants to lose this single valence electron to achieve a stable octet (8 electrons) in its outermost shell, like the noble gases.
Chlorine (Cl)
* Initial State: Chlorine has 7 electrons in its outermost shell. Its electronic configuration is 2, 8, 7.
* Desire: Chlorine wants to gain one electron to complete its octet and become stable.
The Reaction:
1. Electron Transfer: When sodium and chlorine react, sodium readily gives up its single valence electron to chlorine.
2. Ion Formation: Sodium, having lost an electron, becomes a positively charged ion (Na⁺). Chlorine, having gained an electron, becomes a negatively charged ion (Cl⁻).
3. Ionic Bond: The oppositely charged ions are strongly attracted to each other, forming an ionic bond. This creates the compound sodium chloride (NaCl).
Final State:
* Sodium (Na⁺): Now has the electronic configuration 2, 8. It has a complete octet and a positive charge.
* Chlorine (Cl⁻): Now has the electronic configuration 2, 8, 8. It has a complete octet and a negative charge.
Key Points:
* The reaction is driven by the desire of both atoms to achieve a stable octet configuration.
* This electron transfer results in the formation of ions with opposite charges.
* The strong electrostatic attraction between these ions creates the ionic bond, holding the sodium chloride compound together.
