Chemical Bonds

• • Ionic bonding: metal and non-metal
  • Covalent bonding: non-metal and non-metal
  • Metallic: metal and metal
• The strength of an ionic bond is due to the electrostatic attraction between oppositely charged ions.
• Ionic bonds involves an attraction between oppositely charged ions.
• Covalent bonding involves sharing electrons to gain a full outer shell.
• Metallic bonding includes an attraction between positive metal ions and delocalised electrons.
• ions: atoms that have gained or lost electrons, so have a different number of electrons
• intermolecular compounds: molecules that are held together by the forces of attraction between the molecules
• bonding: how the atoms are joined together by attraction
• Giant lattice: atoms arranged in a regular patter

  • to melt or boil you need to break a chemical bond, which takes a lot of energy so melting and boiling points are high.
• Ions that have opposite charges are attracted to each other by electrostatic forces
• Properties of Diamond:

  • high melting and boiling points
  • doesn't conduct electricity
  • strong (covalent bonds)
• In order for a material to conduct electricity, it must have delocalised electrons that are free to move.