unit 1.5 solid structures

• ionic

  • giant ionic lattices
• properties of ionic lattices

  • high melting and boiling points -strong forces of attraction between ions
  • conduct electricity when in solution or molten not when solid- ions are free to move
  • dissolve in polar substances- influtrate lattice and break apart because its charged
• examples of giant ionic lattices

  • NaCl- sodium chloride, co-ordination 6:6
  • each individual is surrounded by 6 chlorides vice versa
  • CsCl- caesium chloride, co-ordination 8:8
• simple molecular

  simple molecules, weak intermolecular forces, strong covalent bonds
• example of simple molecular

  $HCl$, $O_2$, $H_2O$
• properties of simple molecular

  • low melting and boiling point- break van der waals
  • dont conduct electricity- no free charges
  • soluble in non polar substances- like dissolves like
• giant covalent

  covalent bonding between atoms
• examples of giant covalent bonds

  graphite, diamond, silicon dioxide
• properties of giant covalent

  • high melting and boiling points- have to break covalent bonds
  • dont conduct electricity- no free charges
  • insoluble in polar and non-polar- cant break bonds (np) no charges (p)
  • very hard (except graphite, weak van der waals between layers)
• metallic bonding

  metal atoms are ionised and surrounded by a sea of electrons. bonded with a metal
• properties of metallic bonding

  • high melting and boiling point
  • good conductor of electricity
  • malleable and ductile - move the layers of ions
• whats a metallic bond

  bond between a positive ion and delocalised electrons
• graphite

  intermolecular forces, each carbon 1 is delocalised electron.