1. Sodium (Na) has 1 valence electron in its outermost shell, making it highly reactive. It wants to lose this electron to achieve a stable electron configuration like its nearest noble gas (Neon).
2. Chlorine (Cl) has 7 valence electrons in its outermost shell. It needs one more electron to achieve a stable electron configuration like its nearest noble gas (Argon).
3. Electron Transfer: The sodium atom readily gives up its valence electron to the chlorine atom. This transfer results in a positively charged sodium ion (Na+) and a negatively charged chloride ion (Cl-).
4. Electrostatic Attraction: Due to their opposite charges, the sodium ion and chloride ion are attracted to each other. This electrostatic attraction forms an ionic bond, holding them together as a molecule of sodium chloride (NaCl).
Key takeaways:
* Ionic bond: This type of bond occurs when a metal (like sodium) loses an electron to a non-metal (like chlorine).
* Stable configuration: Both sodium and chlorine achieve a stable electron configuration after the electron transfer, making the compound more stable than the individual atoms.
* No sharing of electrons: Unlike covalent bonds, in ionic bonds, electrons are completely transferred, not shared.
This exchange of electrons is a fundamental process in chemistry that leads to the formation of many important compounds.
