AQA GCSE Chemistry (8462), Higher tier · Bonding, structure and the properties of matter › Structure and bonding of carbon
Practise Diamond. 12 exam-style questions on this subtopic, at up to four difficulty levels, with full mark schemes and a progress tracker. Free, no account needed.
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How many covalent bonds does each carbon atom form in diamond?
4
Diamond burns when it is heated strongly in oxygen. Name the product.
carbon dioxide
Sample questions
Written for this site in the style of AQA exam questions. They are not taken from real past papers.
Question 1Easy4 marks
Diamond is a form of carbon.
(a) How many covalent bonds does each carbon atom form in diamond?[1]
(b) Diamond is used in the tips of drills. Which property makes diamond suitable for this use? Tick (✓) one box.[1]
It is very hard.
It conducts electricity.
It is shiny.
It dissolves in water.
(c) Why does diamond not conduct electricity? Tick (✓) one box.[1]
It has no delocalised electrons.
It has no covalent bonds.
Its molecules are too small.
Its ions cannot move.
(d) What type of structure does diamond have?[1]
Show the answer and mark scheme
(a)Answer: 4
4
(b)Answer: It is very hard.
(c)Answer: It has no delocalised electrons.
(d)Answer: giant covalent
giant covalent
Question 2Medium6 marks
Diamond is a form of carbon.
(a) Explain why diamond is very hard.[2]
(b) Explain why diamond has a very high melting point.[2]
(c) Explain why diamond does not conduct electricity.[2]
Show the answer and mark scheme
(a)Answer: Each carbon atom is joined to four others by strong covalent bonds in a rigid three-dimensional structure.
each carbon atom is bonded to four other carbon atoms by strong covalent bonds
(in a) rigid / 3D giant structure
(b)Answer: There are many strong covalent bonds, which need a lot of energy to break.
many strong covalent bonds
a lot of energy is needed to break them
(c)Answer: All four outer electrons of each carbon atom are used in covalent bonds, so there are no delocalised electrons.
all four outer electrons (of each carbon atom) are used in covalent bonds
so there are no delocalised electrons / charged particles free to move
Question 3Hard6 marks
Lonsdaleite is a rare form of carbon found at some meteorite impact sites. Every carbon atom in lonsdaleite is covalently bonded to four other carbon atoms in a rigid three-dimensional network, but the atoms are arranged in a slightly different pattern from diamond.
(a) Predict two physical properties of lonsdaleite. Explain each prediction.[4]
(b) Predict whether lonsdaleite conducts electricity. Explain your answer.[2]
Show the answer and mark scheme
(a)Answer: Very hard, because each atom is held rigidly by four strong covalent bonds; very high melting point, because many strong covalent bonds must be broken to melt it.
very hard
because each atom is held firmly in place by four strong covalent bonds in a rigid 3D structure
very high melting point
because many strong covalent bonds must be broken, which needs a lot of energy
(b)Answer: No: each carbon atom uses all four of its outer electrons in covalent bonds, so there are no delocalised electrons.
it does not conduct electricity
each carbon atom uses all 4 outer electrons in covalent bonds, so there are no delocalised electrons (or ions)