Past paper question

• What type of bonding occurs between atoms in graphene?


  Covalent bonding
• Why is graphene considered strong?

  Because the covalent bonds within its layers are strong
• How does graphene conduct electricity?


  It has delocalized electrons that can move through the structure
• Why is a sheet of graphite unsuitable for touchscreens?

  Because there are weak intermolecular forces between the layers, allowing them to slide
• What property of silver nanoparticles helps stop unpleasant smells?


  They kill bacteria
• Why do silver nanoparticles more effective at preventing unpleasant smells than normal sized silver

  Because they react faster
• Why do silver nanoparticles not get released during washing?

  Because they do not get released during my washing because this could harms fish
• What type of structure does gold have?


  A giant metallic structure
• How are the atoms arranged in gold?


  In a regular pattern with delocalized electrons
• Why can gold conduct electricity?


  Because it has delocalized electrons that can move
• What happens to iron when it corrodes?


  It forms an ionic compound that reduces electrical conductivity
• Why is graphite used as a lubricant?


  Because it has weak intermolecular forces between layers that allow them to slide
• Why are alloys harder than pure metals?

  Because they have different atom sizes that distort the layers
• How many strong covalent bonds does each carbon atom in diamond have?


  Four strong covalent bonds
• What is the difference in bonding between graphite and diamond?

  Graphite has weak intermolecular forces between layers, while diamond has strong covalent bonds
• Why is diamond considered very hard?


  Because it is a giant covalent structure with a large number of strong covalent bonds
• What type of structure does diamond have?

  A giant covalent structure
• How does the bonding in diamond affect its properties?


  Strong covalent bonds make it very hard