understand metallic bonding

• metals are giant structures of atoms held together by metallic bonds. the metal structure is a regular lattice
• metallic bonding is caused because the electrons in the highest energy level of a metal atom has the ability to become delocalised
• delocalised


  electron in an atom that is not connected to a single atom or covalent bond
• they are free to move through the metal in a 'sea' of electrons
• this gives the metal nuclei a positive charge which is attracted to the negative charge on the delocalised electrons
• there is a very strong force of attraction between the positive metal nuclei and the negative delocalised electrons
• non-polar molecule?


  a molecule where the electrons are distributed evenly throughout the molecule eg. covalent bonding in chlorine
• polar molecule


  a molecule with partial positive charge in one part of the molecule and similar negative charge in another part due to an uneven electron distribution