diamond, graphite, fullerenes and nanoparticles (topic 2) Flashcards
graphite is softer than diamond, explain why (4)
graphite:
- the layers of carbon atoms in graphite can move
- because there are only weak intermolecular forces between layers
diamond:
- each carbon atom is strongly bonded to 4 others
- no carbon atoms are able to move
graphite conducts electricity, but diamond does not, explain why (3)
graphite:
- has delocalised electrons
- which can carry charge
diamond:
- has no delocalised electrons
(3)
- graphite made from layers of carbon atoms
- weak intermolecular forces between layers
- so layers can slide over each other
(3)
- giant structure
- each carbon atom is joined to four others
- by covalent bonds
- bonds are strong
- it takes a lot of energy to break bonds
(3)
- giant lattice
- atoms in graphene are covalently bonded
- covalent bonds are strong
explain why graphene can conduct electricity (2)
- graphene has delocalised electrons
- which can move throughout the structure
suggest why a block of graphite, which has a large number of graphene sheets, could not be used for a touchscreen (1)
- opaque
- layers would slide
explain why carbon nanotubes are very strong (1)
- the carbon atoms are held together by strong covalent bonds
explain why diamond is hard (3)
- giant structure
- each carbon atom forms 4 covalent bonds
- covalent bonds are strong
explain why graphite is slippery (2)
- weak forces of attraction between layers
- layers of atoms can slide over each other
explain why diamond has a high melting point (4)
- large number of covalent bonds
- between atoms
- covalent bonds are strong
- large amount of energy required to break bonds
describe the structure and bonding in diamond (3)
- giant structure
- strong covalent bonds between carbon atoms
- each carbon atom forms 4 bonds
(6)
graphite conducts electricity because (max 3 marks):
- bonds are covalent
- graphite has a giant structure
- three covalent bonds per carbon atom
- so one electron (per carbon atom) is delocalised
- delocalised electrons move freely through the structure
- delocalised electrons carry electrical charge
graphite is soft and slippery because (max 3 marks):
- it has a layered structure
- of (interlocking) hexagonal rings
- weak intermolecular forces between layers
- so layers can slide over each other
suggest why Buckminsterfullerene is a good lubricant (2)
- molecules are spherical
- so molecules will roll