Ionic Bonding

• Ionic bonding occurs between a metal and a non-metal element.
• It involves the transfer of electrons from one atom (metal) to another (non-metal).
• The atom that loses the electrons becomes a positively charged ion (cation), while the atom that gains the electrons becomes a negatively charged ion (anion).
• This transfer of electrons allows both atoms to have a full outer shell of electrons, attaining stable electron configurations.
• These positive and negative ions attract each other, forming a strong ionic bond. This attraction is due to the electrostatic forces between oppositely charged ions.
• Ionic compounds have high melting and boiling points due to the strong forces of attraction between the ions.
• They also conduct electricity when they are dissolved in water or melted, as the ions are free to move and carry the electric charge.
• Ionic compounds generally form crystalline lattices, due to the arrangement of ions in a regular, repeat pattern.
• These crystalline lattices are very hard and brittle, they shatter when stress is applied.
• Dissolving an ionic compound in water can also break apart the ionic bonds, separating the ions and allowing them to move freely in the solution.
• Solubility of ionic compounds in water varies, as it depends on the balance between the strength of the ionic bonds and the attraction between the ions and water molecules.
• In terms of structure, an ionic compound does not consist of separate, discrete molecules. Instead, its formula indicates the ratio of the ions in the crystal lattice.