metallic

• metallic definition

  strong electrostatic attraction of positive metal ions surrounded by negative delocalised electrons. Has structure of a giant metallic lattice.
• factors affect strength/ metallic

  • The larger the charge on the ions, the stronger the electrostatic attraction
  • The smaller the ion, the stronger the electrostatic attraction
  • The larger the number of delocalised electrons, the stronger the electrostatic attraction
• conductivity/ metallic

  • metals are good electrical and thermal conductors
  • delocalised electrons help transfer energy through the metal
  • delocalised electrons can also flow and hence metals can also conduct electricity very well
• strength of metal

  • very strong as there is a strong electrostatic attraction between the positive metal ions and delocalised electrons
  • strongest metals have ions which are small, have a large positive charge and many delocalised electrons
• malleable and ductile

  • Metals can be hammered into shape (are malleable) and can be pulled into wires (are ductile) because rows of metals ions can slide past one another without metallic bonds breaking
  • ion lattice changes shape the delocalised electrons will still move with the ions to continue holding them together
• melting and boiling point/ metallic

  • The stronger they are, the higher the melting point and boiling point will be as more energy is needed to break the metallic bonds.