Understanding the Basics
* Sodium (Na): Sodium has one valence electron (electron in its outermost shell). It wants to lose this electron to achieve a stable electron configuration like that of a noble gas (neon).
* Chlorine (Cl): Chlorine has seven valence electrons. It wants to gain one electron to achieve a stable electron configuration like that of the noble gas argon.
The Reaction
1. Electron Transfer: The sodium atom transfers its single valence electron to the chlorine atom.
2. Ionic Bonds: The sodium atom, having lost an electron, becomes positively charged (Na+) and is now called a sodium ion. The chlorine atom, having gained an electron, becomes negatively charged (Cl-) and is now called a chloride ion.
3. Electrostatic Attraction: The oppositely charged ions are strongly attracted to each other due to electrostatic forces, forming an ionic bond.
Result
The resulting compound, sodium chloride (NaCl), is a crystal lattice structure. In this structure, each sodium ion is surrounded by six chloride ions, and each chloride ion is surrounded by six sodium ions. This strong electrostatic attraction between the ions gives sodium chloride its high melting point and strong crystal structure.
Key Points
* Ionic Compounds: Sodium chloride is an example of an ionic compound, formed by the electrostatic attraction between oppositely charged ions.
* Octet Rule: Both sodium and chlorine achieve a stable electron configuration by gaining or losing electrons to have eight electrons in their outermost shell (octet rule).
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