Oxford AQA IGCSE · Chemistry (9202)

Structure and bonding of carbon: Practice Questions

5 multiple-choice questions marked as you go, and 2 written questions with worked solutions. All on Structure and bonding of carbon.

7 questions16 marksFree, no account

Question 1

1 mark

Which of the following is a fundamental characteristic of the structure of fullerenes?

Question 2

1 mark

Graphite is a non-metal, yet it is an excellent conductor of electricity. Which of the following statements correctly compares the reason for conductivity in both graphite and metals?

Question 3

1 mark

Carbon is a Group 4 element. According to the syllabus, what is the maximum number of covalent bonds that a single carbon atom can form with other atoms?

Question 4

1 mark

In graphite, only three out of four valence electrons of each carbon atom are used in covalent bonds. What is the state and function of the fourth electron?

Question 5

1 mark

Fullerenes are a versatile form of carbon with several industrial and medical applications. Which of the following is not a use of fullerenes specifically mentioned in the syllabus?

Question 6

6 marks

Carbon exists in several forms known as allotropes, including diamond, graphite, and fullerenes. The properties of these substances are determined by their specific bonding and structure.

(a) State the maximum number of covalent bonds a single carbon atom can form.
(b) In diamond, each carbon atom is joined to others in a giant covalent structure. Describe how many bonds each carbon atom forms and explain how this structure affects its hardness.
(c) Graphite is also a form of carbon but, unlike diamond, it can conduct electricity. Explain why graphite is able to conduct electricity by referring to its bonding.
(d) Fullerenes are molecules of carbon atoms with hollow shapes. State the specific arrangement of carbon atoms found in the rings of a fullerene structure.

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Question 7

5 marks

Carbon is a unique element that can form several different giant covalent structures, including diamond and graphite. These different forms have very different physical properties due to their bonding and structure.

(a) Describe the bonding in diamond and explain why it is very hard.
(b) Graphite is much softer than diamond and can conduct electricity. Explain why graphite can conduct electricity, while diamond cannot.
(c) Fullerenes are another form of carbon. State the basic structural feature of fullerenes and give one potential use for these molecules.

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