GCSE Chemistry (AQA)

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Ionic Bonding

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

Ionic Bonding

5:27 Different types of Chemical Bonds
Spec 4.2.1.1 4.2.1.2
Previous Transition Elements: Ions & Compounds Next Metallic Bonding
  • Ionic bonding occurs in compounds formed from metals combined with nonmetals.
  • Example: Table salt (NaCl) is an ionic compound.
  • Sodium (Na) is the metal, and chlorine (Cl) is the nonmetal in NaCl.
  • Metals are on the left side of the periodic table; non-metals are on the right.
  • During exams, periodic tables are not color-coded; students must know the positions of metals and non-metals.
  • Ionic compounds form when electrons from the outer shell of metal atoms are transferred to non-metal atoms.
  • Sodium loses an electron to become a positively charged ion (Na+).
  • Chlorine gains an electron to become a negatively charged ion (Cl-).
  • Ionic bond: strong electrostatic force of attraction between oppositely charged ions.
  • Metal atoms lose electrons to achieve the structure of a noble gas.
  • Sodium loses an electron to have the same electronic structure as neon (Ne).
  • Chlorine gains an electron to have the same electronic structure as argon (Ar).
  • The number of electrons lost or gained depends on the number of electrons in the outer shell of the atom.
  • Group numbers in the periodic table indicate the number of electrons in the outer shell.
  • Metals in group 1 lose one electron to form a 1+ charge.
  • Metals in group 2 lose two electrons to form a 2+ charge.
  • Non-metals in group 6 gain two electrons to form a 2- charge.
  • Non-metals in group 7 gain one electron to form a 1- charge.

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