* Sodium (Na) has one electron in its outermost shell. It readily loses this electron to achieve a stable, full outer shell.
* Chlorine (Cl) has seven electrons in its outermost shell. It needs one more electron to achieve a stable, full outer shell.
The Exchange:
1. Sodium loses its single valence electron, becoming a positively charged ion called a sodium cation (Na+).
2. Chlorine gains this electron, becoming a negatively charged ion called a chloride anion (Cl-).
Ionic Bond Formation:
The opposite charges of the sodium cation and chloride anion attract each other strongly, forming an ionic bond. This electrostatic attraction holds the ions together in a crystal lattice structure, forming sodium chloride.
Key Points:
* Ionic bonds are formed between metals (like sodium) and nonmetals (like chlorine).
* The transfer of electrons results in the formation of charged ions (cations and anions).
* The electrostatic attraction between oppositely charged ions is what holds the compound together.
* Sodium chloride is a classic example of an ionic compound, and its formation through electron transfer is a fundamental concept in chemistry.
