1. Formation of Ions:
* Metals tend to lose electrons to achieve a stable electron configuration, becoming positively charged cations.
* Nonmetals tend to gain electrons to achieve a stable electron configuration, becoming negatively charged anions.
2. Electrostatic Attraction:
* Opposite charges attract. When a cation (positive) and an anion (negative) are brought close together, their opposite charges exert a strong electrostatic force of attraction.
3. Formation of the Ionic Bond:
* This electrostatic attraction holds the ions together, forming a chemical bond called an ionic bond.
* The resulting compound is called an ionic compound or salt.
Example: Sodium Chloride (NaCl)
* Sodium (Na) loses one electron to become a positively charged sodium ion (Na+).
* Chlorine (Cl) gains one electron to become a negatively charged chloride ion (Cl-).
* The opposite charges attract, forming an ionic bond between the Na+ and Cl- ions, creating sodium chloride (NaCl), which is table salt.
Key Characteristics of Ionic Bonds:
* Strong attraction: Ionic bonds are relatively strong, resulting in high melting and boiling points.
* Crystalline structure: Ionic compounds typically form a rigid, crystalline structure.
* Solubility: Many ionic compounds are soluble in water because the polar water molecules can surround and separate the ions.
* Conductivity: Ionic compounds conduct electricity when dissolved in water or melted, as the free-moving ions can carry electrical current.
In summary:
Oppositely charged ions attract each other due to electrostatic forces, forming ionic bonds. These bonds hold the ions together in a rigid, crystalline structure, creating ionic compounds.
