GCSE Combined Science (AQA)

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Properties of Ionic Compounds

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Bonding, structure, and the properties of matter Chemical bonds, ionic, covalent and metallic

Properties of Ionic Compounds

5:21 Ionic Compounds and Formulae
Spec 4.2.1.3 4.2.2.3 4.2.2.1
Previous Naming Ionic Compounds Next Ionic Formulae
  • Ionic compounds consist of many ions in a specific structure.
  • Table salt (NaCl) is a common example of an ionic compound made of sodium and chloride ions.
  • NaCl formula represents trillions of ions arranged in a structure.
  • Ionic compounds have a giant 3D structure of alternating positive and negative ions.
  • This lattice structure gives ionic compounds specific properties.
  • Strong electrostatic forces of attraction between oppositely charged ions form ionic bonds.
  • Electrostatic forces act in all directions in the lattice, making the compound very strong.
  • Ionic compounds have high melting and boiling points due to the strong bonds between ions.
  • Sodium chloride has a melting point of 801��C and a boiling point of 1,465��C.
  • Large amounts of energy are needed to break the strong ionic bonds.
  • Ionic compounds do not conduct electricity in a solid state because ions are fixed in position.
  • In a solid state, no charge can flow through the compound.
  • Ionic compounds can conduct electricity when molten or aqueous.
  • In molten or aqueous states, ions are free to move, allowing charge to flow.
  • Molten ionic compounds have ions no longer arranged in a regular lattice.
  • Aqueous ionic compounds have ions separated by water molecules.
  • Free ions in molten or aqueous states enable the compound to conduct electricity.
  • A circuit with aqueous sodium chloride can conduct electricity and light a bulb.

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