metals

• in a solid metal structure each atom has donated its negative outer-shell electrons to a shared pool of electrons that are delocalised throughout the whole structure
• metallic bonding

  strong electrostatic attraction between cations and delocalised electrons
• cations are fixed in place maintaining the structure and shape of a metal
• the delocalised electrons are mobile and able to move throughout the structure
• properties of metals:

  • strong metallic bonds
  • high electrical conductivity
  • high melting and boiling points
• meals conduct electricity in solid and liquids
• when a voltage is applied across a metal the delocalised electrons can move through the structure carrying a charge
• the meting point depends on the strength of the metallic bonds holding together the atoms in the giant metallic lattice
• at room temperature all metals except mercury are solids
• metals don't dissolve
• any reactions between polar solvents and the charges in a metallic lattice would lead to a reaction