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9701 · 3.3

Metallic bonding

Metals are giant structures of positive ions held together by a 'sea' of electrons that are free to move. This unique arrangement explains why metals can conduct electricity and be shaped without breaking.

Need to know

What you need to know

  • **High Melting/Boiling Points:** Strong electrostatic attraction requires lots of energy to overcome.
  • **Conductivity:** Mobile delocalised electrons act as charge carriers.
  • **Malleability/Ductility:** Layers of ions can slide without breaking the non-directional bonds.
  • **Insolubility:** The strong metallic bonds are not easily broken by solvent molecules.

Explanation

The Electron Sea

  1. Positive ion lattice in sea of delocalised e⁻.
  2. Conductivity and malleability explained.
  3. Melting point varies with ion charge/size.
  4. Alloys: mixed metals change properties.
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