Metallic bonding

• Metallic bonding is the electrostatic attractions between positive metal cations and sea of delocalised electrons
• The strength of a metallic bond depends on

  • the number of electrons in the sea of delocalised electrons. The higher the number of delocalised electrons the stronger the metallic bond
  • the size of the ion. The smaller the ion the stronger the metallic bond
  • the charge of the ion. The higher/ lower the charge the stronger the metallic bond
• Metals can conduct electricity because of the sea of delocalised electrons are free to move and carry charge
• Metals are good heat conductors because the sea of delocalised electrons allows for heat energy to be transfers across the substance as kinetic energy between the delocalised electrons
• increasing the number of delocalised electrons increases the heat and electrical conductivity
• Mercury has low melting point and is liquid at room temperature
• Francium and caesium are liquid at room temperature but because they have a small charge, small number of delocalised electrons and are large in size so have a low melting point
• Malleability is the ability to be made into different shapes
• Ductility is the ability to be made into wire