1. The Basics:
* Metal Cations: Metals tend to lose electrons, becoming positively charged ions (cations).
* Nonmetal Anions: Nonmetals tend to gain electrons, becoming negatively charged ions (anions).
2. Electrostatic Attraction:
The opposite charges of the cation and anion attract each other strongly due to electrostatic forces. This attraction is the basis of the ionic bond.
3. Formation of a Compound:
The electrostatic attraction pulls the ions together, forming a stable, neutral compound called an ionic compound. The compound usually exists as a crystal lattice structure.
4. Examples:
* Sodium Chloride (NaCl): Sodium (Na) loses an electron to become Na+, while chlorine (Cl) gains an electron to become Cl-. The resulting electrostatic attraction forms the ionic compound sodium chloride.
* Magnesium Oxide (MgO): Magnesium (Mg) loses two electrons to become Mg2+, while oxygen (O) gains two electrons to become O2-. This results in the ionic compound magnesium oxide.
5. Properties of Ionic Compounds:
* High Melting and Boiling Points: Due to strong electrostatic forces.
* Solid at room temperature: Ionic compounds are typically hard and brittle.
* Conduct electricity when molten or dissolved: The ions are free to move and carry charge.
In summary: Mixing a metal cation with a nonmetal anion leads to the formation of a stable ionic compound characterized by strong electrostatic attraction between oppositely charged ions.
