metallic bonding

• metals exist as giant metallic lattices
• A metallic bond is the electrostatic attraction between cations and the sea of negatively charged delocalised electrons.
• to melt you need to overcome the strong electrostatic attractions between the cations and delocalized electrons, so have high melting points
• malleable because the layers of cations are able to slide over each other because there are always delocalized electrons between them
• metals have giant metallic structures and are a lattice of cations in a sea of delocalized electrons
• metal conductivity

  conducts electricity because the delocalized electrons are free to move