AQA GCSE Chemistry
AQA GCSE Chemistry 4.2.3 Structure and Bonding of Carbon Exam Questions
Free AQA GCSE Chemistry exam questions for 4.2.3 Structure and Bonding of Carbon, with a mark scheme for every pack. Covers diamond, graphite, graphene, fullerenes including buckminsterfullerene and carbon nanotubes, linking structure to properties and uses.
4.2.3 Structure and Bonding of Carbon exam questions
1 question pack of real past exam questions, each with its mark scheme. Do not stop after a few: answer as many as you can without notes, then mark every answer with the mark scheme. The more questions you do, the more quickly you will spot how examiners ask about each idea.
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About AQA GCSE Chemistry 4.2.3 Structure and Bonding of Carbon
AQA GCSE Chemistry 4.2.3 looks at the different forms of carbon and why such similar atoms produce very different materials. You compare diamond, graphite, graphene and the fullerenes, including buckminsterfullerene (C60) and carbon nanotubes, and explain their properties from their structure and bonding. It is in section 4.2, assessed on Paper 1, and builds on giant covalent structures from 4.2.2. Examiners frequently ask why graphite conducts but diamond does not, why graphite is soft and slippery, and how the structure of nanotubes or graphene makes them suitable for electronics, nanotechnology and composite materials.
What you need to know
- Diamond Each carbon atom forms four covalent bonds in a giant covalent structure. It is very hard, has a very high melting point and does not conduct electricity because there are no delocalised electrons.
- Graphite Each carbon atom forms three covalent bonds, making layers of hexagonal rings with no covalent bonds between layers. The layers slide over each other, so graphite is soft and slippery; one electron per atom is delocalised, so graphite conducts electricity and thermal energy, similar to metals.
- Graphene A single layer of graphite, one atom thick. It is very strong and conducts electricity, making it useful in electronics and composites.
- Fullerenes Molecules of carbon atoms with hollow shapes, based on hexagonal rings but sometimes with rings of five or seven atoms. Buckminsterfullerene, C60, was the first discovered and is spherical.
- Carbon nanotubes Cylindrical fullerenes with very high length to diameter ratios. Their high tensile strength, high electrical and thermal conductivity make them useful in nanotechnology, electronics and materials such as reinforcing sports equipment.
- Uses of fullerenes Fullerenes can be used for drug delivery into the body, as lubricants and as catalysts, helped by their large surface area.
Common mistakes in 4.2.3 Structure and Bonding of Carbon
- Saying graphite is soft because covalent bonds between layers are weak. There are no covalent bonds between the layers; the forces between layers are weak, so they slide.
- Saying graphite conducts because of free ions. It conducts because each carbon has one delocalised electron.
- Describing diamond as having 'strong intermolecular forces'. Diamond is a giant covalent structure, so its hardness comes from many strong covalent bonds, not intermolecular forces.
- Confusing graphene (one layer of graphite) with fullerenes (hollow molecules such as C60).
- Forgetting that C60 is a molecule, so it has a much lower melting point than diamond or graphite.
Try three 4.2.3 Structure and Bonding of Carbon exam-style questions
1. Explain why graphite conducts electricity but diamond does not. (3 marks)
Show the mark scheme answer
In graphite each carbon forms three covalent bonds; one electron from each carbon is delocalised and free to move through the structure; in diamond each carbon forms four bonds so there are no delocalised electrons.
2. Explain why diamond has a very high melting point. (3 marks)
Show the mark scheme answer
Giant covalent structure; many strong covalent bonds; lots of energy needed to break them.
3. Give one property of carbon nanotubes and a use that depends on it. (2 marks)
Show the mark scheme answer
High tensile strength, used to reinforce materials such as tennis rackets; or high electrical conductivity, used in electronics; (property 1, matching use 1).
4.2.3 Structure and Bonding of Carbon FAQs
What does AQA GCSE Chemistry 4.2.3 cover?
It covers the structures, properties and uses of diamond, graphite, graphene and fullerenes, including buckminsterfullerene and carbon nanotubes.
Which paper is 4.2.3 examined in?
It is part of section 4.2 and is assessed on AQA GCSE Chemistry Paper 1.
How should I compare diamond and graphite in a 6 mark question?
Compare bonds per carbon atom (four versus three), structure (rigid 3D lattice versus layers), hardness (very hard versus soft and slippery) and conductivity (none versus conducts due to delocalised electrons). Say that both have very high melting points because of many strong covalent bonds.
