Bonding, structure and the properties of matter

• What is an ion?

  A charged particle
• How can an ionic bond be represented?

  Dot and cross diagram
• What is an ionic bond?

  A compound formed from metals combined with non-metals
• What is the structure of an ionic bond?

  Regular lattice structure
• What are the properties of an ionic bond?

  • High melting and boiling points (lots of energy required to break strong bonds)
  • Can conduct electricity when molten or dissolved (ions are free to move around)
• What is the formula of a hydroxide ion?

  $OH^-$
• What is the formula of a sulfate ion?

  $SO4^{2-}$
• What is the formula of a nitrate ion?

  $NO_3^-$
• What is the formula of a carbonate ion?

  $CO3^{2-}$
• What is the formula of an ammonium ion?

  NH4$^+$
• What force acts between ions in an ionic compound?

  Strong electrostatic forces
• How can we draw a covalent bond?

  A dot and cross diagram where elements share electrons
• What is a covalent bond?

  When a non-metal and non-metal bond
• What are some examples of giant covalent structures?

  • Diamond
  • Silicon dioxide
• What are the properties of small covalent molecules?

  • Low melting and boiling point
  • Cannot conduct electricity
• What is the structure of a small covalent molecule?

  • Strong covalent bonds
  • Weak intermolecular forces
• Why do small covalent molecules have a low melting and boiling point?

  There are weak intermolecular forces between the molecules, which do not require a lot of energy to break
• Why can't small covalent molecules conduct electricity?

  They don't have an overall electric charge
• What state are giant covalent structures at room temperature?

  Solid
• What are the properties of giant covalent structures?

  • Insoluble in water
  • High melting and boiling points (many strong covalent bonds)b g
  • Do not conduct electricity
• What are diamonds made from?

  Carbon atoms
• What are the properties of diamonds?

  • Hardness (multiple carbon atoms)
  • High melting and boiling points (strong covalent bonds)
  • Cannot conduct electricity (no free electrons)
• What are the key properties of graphite?

  • Soft and slippery
  • Very high melting and boiling points
  • Good conductor of electricity and heat
• The structure of graphite 


  • Formed from multiple carbon atoms bonded with strong covalent bonds, forming a hexagonal ring
  • Arranged in layers with no covalent bonds (able to slide over each other)
• The uses of graphite

  Lubricants
• Why is graphite able to conduct electricity?

  It contains delocalized electrons
• What is Graphene?

  A single layer of graphite
• Properties of Graphene?

  • Good conductor of electricity
  • Extremely strong
  • High melting and boiling points
• Why is graphene a good conductor of electricity?

  It contains delocalised electrons meaning they can move around the molecule carrying an electric charge
• Why is graphene strong and has a high melting and boiling point?

  It has a large number of strong covalent bonds which require a lot of energy to be broken down
• What is another name for a fullerene?

  Buckminsterfullerene (Bucky ball)
• What is the structure of a buckminsterfullerene?

  • Carbon atoms arranged in a hexagonal shape
  • Hollow in the middle
• What are the uses of fullerenes?

  • Deliver drugs
  • Lubricants
  • Catalysts