Metallic Bonding

• Metallic bonding refers to the electrostatic attraction between positive metal ions and delocalised electrons

  
  

  In a metallic bond, metals effectively lose their valence electrons, leading to the formation of a 'sea' of electrons that move freely around the metal cations.
• Delocalised electrons can also explain the high thermal conductivity of metlas, as vibrations can pass quickly through the structure
• The 'free' or 'delocalised' electrons in a metal can move throughout the structure, leading to the property of electrical conductivity.

  These mobile electrons originate from the outermost shell of the metal atoms, they are the valence electrons
• This 'sea' of electrons, gives rise to metallic properties such as malleability and ductility.

  The 'sea' allows the metal ions to roll over each other into new positions without breaking the metallic bonds