Ionic Structures

Definition

An ionic structure or an ionic compound, is composed of positive and negative ions that are held together by electrostatic forces of attraction.

Ions are formed when atoms lose or gain electrons to achieve a full outer shell and a stable electronic structure.
Ionic bonding is the force of attraction between oppositely charged ions. This kind of bonding usually occurs between a metal and a non-metal.
During the formation of an ionic bond, a metal atom loses electrons to form a positive cation, while a non-metal atom gains those electrons to form a negative anion.

Structures formed by ionic bonding are generally solid and have high melting and boiling points due to the strong electrostatic forces holding the ions together.
Conductivity: Ionic compounds do not conduct electricity in solid state but do conduct when melted or dissolved in water, because the ions become free and can move.
When an ionic compound is dissolved in water or melted, it forms a solution that can conduct electricity as it forms ions that are free to move.

Ionic compounds form a specific type of structure known as an ionic lattice.
In an ionic lattice, each ion is surrounded by ions of the opposite charge, leading to a strong, electrostatic attraction in all directions and a rigid structure.
Due to this lattice structure, ionic compounds are often crystalline solids at room temperature.

Ionic structures are stable due to the full outer shell of electrons for each ion present.
The strong electrostatic forces of attraction between the opposite charges contribute to this stability.

The formation of an ionic structure is exothermic, which means it releases energy. This is because the energy required to form ions is less than the energy released when ions attract each other to form an ionic structure.

Common examples of ionic compounds include Sodium Chloride (NaCl), Potassium iodide (KI) and Magnesium Oxide (MgO).