Metallic Bonding (Edexcel IGCSE Chemistry)

• Metals consist of giant structures of atoms arranged in a regular pattern 
• Within the metal lattice, the atoms lose their outer electrons and become positively charged metal ions
  • The outer electrons no longer belong to any specific metal atom and are said to be delocalised
  • This means they can move freely between the positive metal ions and act like a “sea of electrons”
• The metallic bond is the strong force of attraction between the positive metal ions and the delocalised electrons
• This type of bonding occurs in metals and metal alloys, which are mixtures of metal

Metallic bonding

Metallic bonds exist between positive metal ions and delocalised electrons

• Most metals have high melting and boiling points 
  • There are strong electrostatic forces of attraction between the positive metal ions and the negative delocalised electrons within the metal lattice structure
  • These needs lots of energy to be broken 
• Metals conduct electricity
  • There are delocalised electrons available to move and carry charge

• Most metals are malleable
  • This means they can be hammered into shape
  • This is because the atoms/ions are arranged in layers which can slide over each other when a force is applied 

The malleability of metals

The atoms are able to slide over each other as they are arranged in layers