Physical Properties

• Simple molecular:

  1. Low melting point as little energy required to overcome weak van der Waals forces between the molecules
  2. No free delocalised electrons - Do not conduct
• Metallic:

  1. High melting and boiling points as lots of energy required to overcome strong electrostatic forces of attraction between + metal ions and sea of delocalised electrons
  2. Malleable - Delocalised electrons can slide over each other (can be bent, shaped)
  3. Good Conductors - Delocalised electrons carry the charge through substance
• Giant Covalent:

  1. High melting and Boiling point, as lots of energy required to overcome strong covalent bonds
  2. No free delocalised electrons - so does not conduct
• Diamond Properties:

  1. In diamond Carbon atoms form 4 covalent bonds arranged in a pyramid structure meaning it is very hard

  2. High melting/Boiling points as strong covalent bonds require lots of energy to overcome

  3. No free electrons- Does not conduct
• Graphite

  1. Has 1 delocalised electron which is free to move and carry the charge through the substance