Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Section
Giant covalent structures
19 practice questions
Practice questions
1–8 of 8 · Easy
Question 1
1 mark · Easy
Answer and see the solution →State which form of carbon, out of diamond, graphite, and C60 fullerene, conducts electricity the best.
Question 2
3 marks · Easy
Answer and see the solution →(a)[1 mark]Describe the structure of diamond in terms of the arrangement of its carbon atoms.
(b)[1 mark]Describe the structure of graphite in terms of the arrangement of its carbon atoms.
(c)[1 mark]State the type of structure present in C60 fullerene.
Question 3
2 marks · Easy
Answer and see the solution →Diamond has a melting point of about 3550 °C, while C60 fullerene melts at about 280 °C. Use these values to explain, in terms of bonding, why diamond has such a high melting point compared to C60 fullerene.
Question 4
2 marks · Easy
Answer and see the solution →Explain why C60 fullerene does not conduct electricity as well as graphite, referring to their structures.
Question 5
3 marks · Easy
Answer and see the solution →Bonding and Atomic Arrangement Carbon Allotrope Number of covalent bonds per carbon atom Type of structure Diamond Graphite C60 fullerene Complete the table by filling in the number of covalent bonds per carbon atom and the type of structure for each allotrope.
Question 6
1 mark · Easy
Answer and see the solution →State why graphite is soft.
Question 7
3 marks · Easy
Answer and see the solution →(a)[1 mark]State the electrical conductivity for each of the following carbon structures: diamond, graphite, and C60 fullerene.
(b)[1 mark]Explain why diamond does not conduct electricity.
(c)[1 mark]Explain why graphite conducts electricity.
Question 8
2 marks · Easy
Answer and see the solution →C60 fullerene contains 60 carbon atoms. If each carbon atom forms 3 bonds, calculate the total number of covalent bonds in one C60 molecule.