Key Characteristics:
* Formation: Metals lose electrons (forming positively charged cations) and nonmetals gain electrons (forming negatively charged anions). The electrostatic attraction between these oppositely charged ions creates the ionic bond.
* Structure: Ionic compounds are usually arranged in a regular, repeating pattern called a crystal lattice. This structure maximizes the attraction between ions.
* Properties:
* High melting and boiling points: The strong electrostatic forces require a lot of energy to break.
* Good conductors of electricity when dissolved in water or molten: The ions are free to move and carry an electric current.
* Brittle: The rigid crystal lattice structure makes them prone to breaking when force is applied.
* Usually solid at room temperature: The strong forces hold the ions tightly together.
Examples:
* Sodium chloride (NaCl): Sodium (Na) loses an electron to become Na+, while chlorine (Cl) gains an electron to become Cl-. These ions attract each other, forming table salt.
* Magnesium oxide (MgO): Magnesium (Mg) loses two electrons to become Mg2+, while oxygen (O) gains two electrons to become O2-.
* Potassium bromide (KBr): Potassium (K) loses an electron to become K+, while bromine (Br) gains an electron to become Br-.
In Summary:
Ionic compounds are formed by the electrostatic attraction between positively charged metal cations and negatively charged nonmetal anions. They exhibit characteristic properties due to their strong ionic bonds and crystal lattice structure.
