Cambridge IGCSE · Chemistry (0620)

Ions and ionic bonds: Practice Questions

5 multiple-choice questions marked as you go, and 5 written questions with worked solutions. All on Ions and ionic bonds.

10 questions29 marksFree, no account

Question 1

1 mark

An element X is in Group II and an element Y is in Group VII of the Periodic Table.
What is the formula of the ionic compound formed between X and Y?

Question 2

1 mark

Compound Q is formed from a metal in Group II and a non-metal in Group VI. Which statement about the formation of the ions in Q is correct?

Question 3

1 mark

Which particle has the same electronic configuration as a calcium ion, \(\text{Ca}^{2+}\)?

Question 4

1 mark

Element M is a metal in Period 3 that forms an ion with a \( 3+ \) charge. Element X is a non-metal in Period 2 that forms an ion with a \( 2- \) charge.
What is the formula of the ionic compound formed between M and X, and what is the electronic configuration of the X ion?

Question 5

1 mark

Lithium reacts with fluorine to form the ionic compound lithium fluoride.

Which statement correctly describes what happens to a lithium atom (atomic number 3) during this reaction?

Question 6

2 marks

State two characteristic physical properties of ionic compounds such as sodium chloride, \(NaCl\).

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Question 7

3 marks

Describe the formation of a magnesium ion from a magnesium atom and state its electronic configuration.

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Question 8

6 marks

Describe the structure of a giant ionic lattice and explain why these crystals are typically brittle when a force is applied.

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Question 9

6 marks

Calcium (Group II) reacts with Phosphorus (Group V) to form an ionic compound, calcium phosphide.
a) Describe the formation of a calcium ion from a calcium atom in terms of electrons.
b) Describe the formation of a phosphide ion from a phosphorus atom in terms of electrons.
c) Deduce the chemical formula for calcium phosphide and describe the structure of its solid lattice.

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Question 10

7 marks

Aluminum reacts with oxygen to form the ionic compound aluminum oxide.

a) Describe the formation of the aluminum ion and the oxide ion from their respective atoms in terms of the number of electrons transferred.
b) Deduce the chemical formula of aluminum oxide and describe the structure of its solid lattice.
c) The melting point of aluminum oxide is approximately \(2072^\circ C\), whereas the melting point of sodium chloride is \(801^\circ C\). Explain this difference by referring to the charges on the ions and the strength of the attractive forces.
d) Explain why aluminum oxide conducts electricity when molten but acts as an insulator in the solid state.

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