chem: paper 1, metallic bonding

    Cards (10)

    • what is metallic bonding
      the chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons
    • what holds the atoms in metallic bonding in a regular structure
      strong forces of attraction between the positive metal ions and the shared negative electrons
    • what are the properties of metals
      solid at room temp
      malleable
      good conductors of heat and electricity
      shiny
    • why are metals solid at room temperature
      The electrostatic forces between the delocalised electrons and the positive ions are so strong that a lot of energy is required to break them.

      Energy at room temperature is not sufficient for their breaking.
    • why are metals good conductors of electricity and heat
      delocalised electrons carry electrical current and thermal energy through the structure
    • why are metals malleable
      the layers of atoms can slide over eachother
    • what are alloys
      a mixture of two or more metals or a metal and another element
    • why do we mix pure metals with other metals to make alloys?
      because metals are soft so when they are mixed with different elements with differently sized atoms, the atom with distort the layers of metal atoms, making it harder to slide over eachother
    • describe the structure and bonding of metals
      Metals have a giant structure.
      The metal atoms give up their outer-shell electrons, which become delocalised.
      The metal ions are arranged in a regular lattice structure.
      There are strong electrostatic forces of attraction between the positive metal ions and the negative delocalised electrons.
      These forces are metallic bonds.
    • what does ductile mean
      can be drawn into wires