C2.1.5 - Metallic Bonding

• Metallic Structure

  • Metals consist of giant structures of atoms arranged in a regular pattern
  • Individual metal atoms are held together by strong metallic bonds forming a lattice structure
  • This type of bonding occurs in metals and metal alloys, which are mixtures of metal
  • Within the metal lattice, the atoms lose their valence electrons and become positively charged metal ions
  • The valence 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”

  
• Properties of metallic bonding

  The structure and bonding of metals explains their properties:

  • they are electrical conductors because their delocalised electrons carry electrical charge through the metal
  • they are good conductors of thermal energy because their delocalised electrons transfer energy
  • they have high melting points and boiling points, because the metallic bonding in the giant structure of a metal is very strong - large amounts of energy are needed to overcome the metallic bonds in melting and boiling