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Structure and bonding of carbon
This topic compares carbon structures so students can connect bonding arrangement, delocalised electrons, shape and size to properties and applications.
20
Objectives
100
Flashcards
100
Questions
90 min
Study time
AQAGCSEChemistryBonding, structure, and the properties of matter
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Syllabus checklist
What you need to know
20 objective pages available
Diamond5 objectives
- Describe diamond as a giant covalent structure made from carbon atoms.
- Explain that each carbon atom in diamond forms four covalent bonds.
- Explain why diamond is very hard in terms of its bonding and structure.
- Explain why diamond has a very high melting point.
- Explain why diamond does not conduct electricity.
Graphite7 objectives
- Describe graphite as a giant covalent structure made from carbon atoms.
- Explain that each carbon atom in graphite forms three covalent bonds.
- Describe graphite as layers of hexagonal rings with no covalent bonds between the layers.
- Explain that one electron from each carbon atom in graphite is delocalised.
- Explain why graphite conducts electricity.
- Explain why graphite is similar to metals because it contains delocalised electrons.
- Explain graphite's properties using its structure and bonding.
Graphene and fullerenes8 objectives
- Describe graphene as a single layer of graphite.
- Explain the properties of graphene in terms of its structure and bonding.
- Describe fullerenes as hollow molecules made from carbon atoms.
- Explain that fullerene structures are based mainly on hexagonal rings and may include rings with five or seven carbon atoms.
- Identify Buckminsterfullerene, C60, as a spherical fullerene.
- Describe carbon nanotubes as cylindrical fullerenes with very high length to diameter ratios.
- Recognise graphene and fullerenes from diagrams and descriptions of their bonding and structure.
- Give examples of fullerene uses, including carbon nanotubes in nanotechnology, electronics and materials.
Key terms
diamondgiant covalent structureCovalent bondDiamondcovalent bondshigh melting pointelectrical conductivityGraphiteGiant covalent structureHexagonal ringsdelocalised electrongraphite
Exam tips
- Understand Diamond's Structure: Remember to remember that diamond is a giant covalent structure where each carbon atom forms four covalent bonds. Link your answer to Diamond in Structure and bonding of carbon, and keep the biology specific to giant covalent structure.
- Understand Diamond's Bonding: Remember to remember that each carbon atom in diamond forms four covalent bonds, creating a strong network. Link your answer to Diamond in Structure and bonding of carbon, and keep the biology specific to diamond.
Common mistakes
- Misunderstanding Diamond Structure: Emphasize that diamond is a giant covalent structure made from a vast network of carbon atoms bonded together.
- Misunderstanding Carbon Bonds in Diamond: Remember that in diamond, each carbon atom forms four covalent bonds, creating a strong and rigid structure.
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