Cambridge IGCSE · Chemistry (0620)

Metallic bonding: Practice Questions

5 multiple-choice questions marked as you go, and 5 written questions with worked solutions. All on Metallic bonding.

10 questions26 marksFree, no account

Question 1

1 mark

Which description best defines metallic bonding?

Question 2

1 mark

Which of the following best describes the bonding in a giant metallic lattice?

Question 3

1 mark

What happens to the structure of a metal when it is stretched into a wire (ductility)?

Question 4

1 mark

Which description best explains the nature of metallic bonding in a giant metallic lattice?

Question 5

1 mark

Which statement best explains why metals are both good electrical conductors and malleable?

Question 6

3 marks

Explain, in terms of their structure, why metals are able to conduct electricity in the solid state.

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Question 7

6 marks

Compare the strength of metallic bonding in Group I metals with that in transition metals, and explain how this affects their respective melting points.

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Question 8

3 marks

In terms of their internal structure, explain why alloys such as brass are significantly harder than pure metals like copper.

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Question 9

4 marks

a) Describe metallic bonding in terms of the arrangement of particles and the nature of the forces involved.
b) Using your description of metallic bonding, explain the following physical properties:
i) Metals are good electrical conductors.
ii) Metals are malleable.

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Question 10

5 marks

Metals are often compared based on their melting points and electrical conductivity. Consider sodium (Group I) and aluminium (Group III).
a) Describe the nature of metallic bonding in these metals.
b) Explain why aluminium has a significantly higher melting point than sodium.
c) Explain why both metals are excellent conductors of electricity in the solid state.

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