General Characteristics of Ionic Bond
Ionic bond is a type of chemical bond that involves the electrostatic attraction between oppositely charged ions. Here are the general characteristics of ionic bond:
Formation
Ionic bonds are formed by the complete transfer of one or more electrons from one atom (metal) to another atom (non-metal). Due to this transfer of electrons, positively charged cations and negatively charged anions are formed. The bond is maintained by the strong electrostatic attraction between the oppositely charged ions. The formation of ionic compounds is shown by Born-Haber cycle.
Structure
Ionic compounds generally form a crystalline lattice structure where ions are arranged in a repeating three-dimensional pattern. This lattice is highly ordered and maximizes the attractive forces while minimizing repulsive forces.
Properties
High Melting and Boiling Points: Ionic compounds have high melting and boiling points due to the strong electrostatic forces between the ions.
Hard and Brittle: Ionic compounds are generally hard and brittle. When a force is applied, ions of like charge may be forced close together, resulting in repulsion and the shattering of the crystal.
Electrical Conductivity
In the solid state, ionic compounds do not conduct electricity because the ions are fixed in place within the crystal lattice and cannot move freely but in melted state or when dissolved in water, ionic compounds conduct electricity because the ions are free to move and carry an electric current.
Solubility
Ionic compounds are generally soluble in polar solvents but insoluble in non-polar solvents.
Bond Strength
The strength of an ionic bond is often measured by the lattice energy. Higher the lattice energy, stronger the ionic bond.
Directionality
Ionic bonds are non-directional which means the strength of the bond is equal in all directions around the ion.
Example of Ionic Compounds
Sodium Chloride (NaCl) is Formed by the electrostatic attraction between Na⁺ ion (formed by loss of one electron) ion and Cl⁻ ion (formed by gain of one electron).
