Periodic trends in bonding and structure

• What is metallic bonding?

  The strong electrostatic attraction between positive ions and delocalised electron
• What is the structure in metallic bonding?

  • Positive ions are in a fixed position, maintaining structure and shape of metal
  • Delocalised electrons are able to move around the structure
• What are the properties of metals?

  • High electrical conductivity
  • High melting and boiling points
  • Strong metallic bonds
  • Insoluble
• Why do metals have a high electrical conductivity?

  Because delocalised electrons are able to carry a charge and move through the giant metallic lattice
• Why do metals have high melting and boiling points?

  • Because there are strong electrostatic forces of attraction between positive ions and delocalised electrons
  • So lots of energy is needed to overcome and break the strong bonds
• Why are metals insoluble?

  Because bonds in giant metallic lattice are too strong to be overcome by water
• What are the properties of giant covalent lattices?

  • Do NOT conduct electricity
  • HIGH melting and boiling point
  • INSOLUBLE in water
• Why don't giant covalent lattices conduct electricity?

  Has NO overall charge
• Why do giant covalent lattices have high melting and boiling points?

  They have STRONG covalent bonds that require a LOT of energy to break
• Why are giant covalent lattices insoluble in water?

  Attraction between H2O and covalent bond atoms are NOT strong enough to OVERCOME strong covalent bonnds