Metallic Bonding

• Reason for metals high melting and boiling points

  strong electrostatic forces between positive metal ions and negative delocalised electrons
• Reason metals being malleable

  layers of ions can slide over each other
• Reason alloys are harder than pure metals

  Different sized atoms disrupt the layers of ions, preventing layers from sliding
• Usefulness of pure metals

  Too soft for most uses
• Reason metals conduct heat well

  Delocalised electrons can transfer heat energy quickly.
• Reason metals conduct electricity well

  Delocalised electrons can carry electrical charge through the structure.
• Term


  Delocalised electronsDefinitionan electron that is able to move freely throughout a structureLocation
• Term


  Positive metal ionsDefinitionMetal atoms that have lost their outer electronsLocation
• Lattice


  Regular arrangement of particles.
• Giant structure


  A huge 3D network of atoms or ions
• Electrostatic forces of attraction

  Strong forces of attraction between oppositely charged particles
• Metallic bonding


  A lattice of positive metal ions surrounded by delocalised outer electrons, held together by strong electrostatic forces of attraction
• Melting and boiling points of metallic substances

  high
• Reason for metals high melting and boiling points

  Strong electrostatic forces between positive metal ions and negative delocalised electrons
• Reason for metals being malleable


  Layers of metal ions can slide over each other

  
• Reason alloys are harder than pure metals

  Different sized atoms disrupt the layers of ions, preventing layers from sliding