1. Electron Transfer:
* Metal atoms tend to lose electrons to achieve a stable electron configuration (like a noble gas). They become positively charged ions (cations).
* Non-metal atoms tend to gain electrons to achieve a stable electron configuration. They become negatively charged ions (anions).
2. Electrostatic Attraction:
* The oppositely charged ions are attracted to each other due to electrostatic forces. This attraction forms a strong ionic bond.
3. Formation of a Compound:
* The ions arrange themselves in a specific, repeating pattern called a crystal lattice to maximize electrostatic attraction.
* The resulting compound is neutral overall, as the positive and negative charges balance out.
Example:
* Sodium (Na), a metal, loses one electron to become a sodium ion (Na⁺).
* Chlorine (Cl), a non-metal, gains one electron to become a chloride ion (Cl⁻).
* These ions attract each other and form sodium chloride (NaCl), commonly known as table salt.
Key Characteristics of Ionic Compounds:
* High melting and boiling points due to strong electrostatic attraction.
* Brittle because the ions are tightly packed and any disruption disrupts the lattice structure.
* Conduct electricity when molten or dissolved in water because the ions become free to move.
* Generally soluble in water because water molecules can surround and separate the ions.
Let me know if you want to delve deeper into specific examples or other aspects of ionic bonding!
