1. Electron Transfer:
* Sodium (Na), an alkali metal, has one valence electron in its outermost shell. It readily loses this electron to achieve a stable electron configuration like that of the noble gas neon (Ne).
* Bromine (Br), a halogen, has seven valence electrons. It needs one more electron to achieve a stable configuration like that of the noble gas krypton (Kr).
2. Formation of Ions:
* Sodium (Na) loses its valence electron, becoming a positively charged ion called a sodium cation (Na+).
* Bromine (Br) gains the electron from sodium, becoming a negatively charged ion called a bromide anion (Br-).
3. Electrostatic Attraction:
* The oppositely charged ions (Na+ and Br-) are now attracted to each other due to electrostatic forces. This attraction is very strong and holds the ions together in a rigid, crystalline structure.
4. Formation of Sodium Bromide (NaBr):
* The resulting compound, sodium bromide (NaBr), is a white crystalline solid. It is formed through the strong electrostatic attraction between the sodium cations and bromide anions.
Key Points:
* Ionic bonding involves the transfer of electrons, unlike covalent bonding which involves electron sharing.
* The formation of ions is essential for the formation of ionic compounds.
* The electrostatic attraction between oppositely charged ions is the driving force behind the formation of ionic compounds.
