Ionic bond

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An ionic bond is the bonding (agg) between a non-metal and a metal, that occurs when charged atoms (ions) attracted. This happens after a metal atom loses one or more of its electrons to the non-metal atom. This makes the bond stronger and harder to break. A maximum of 3 electrons can be transferred in the process.

When this happens, the metal becomes a positive cation, and the non-metal becomes a negative anion. This occurs, for example, when sodium and chlorine join to form common table salt, NaCl.

In other bonds, an ionic bond is the electrostatic force of attraction between two oppositely charged ions.[1] The positive ion is called a cation, and the negative ion is the anion.

Features of ionic bonds[change | change source]

  • Three dimensional structures called an ionic lattice.[1]
  • Soluble in water.
  • In a solid state they do not conduct electricity. However, in a liquid state or when dissolved in water, they will conduct electricity well because the ions are free to move.
  • They contrast to the characteristics of a covalent bonds.
  • Sometimes if they do not have a spare valence electron to create a complete shell one will act as two and spin in a figure of eight around both atoms.
  • Ionic bonds are a lot weaker than covalent bonds.
  • High melting/boiling point.

References[change | change source]

  1. 1.0 1.1 Curtis, Cliff (2011). Edexcel IGCSE Chemistry Revision Guide. Pearson Education. p. 21. ISBN 9780435046729.