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 when force is applied 

The malleability of metals

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