GCSE Chemistry (AQA) chapter 2: Bonding, structure, and the properties of matter MCQs with answers
By Team Megalecture · Updated 4 Nov 2026
29 exam-style questions on Bonding, structure, and the properties of matter, each with the answer and a short explanation. Ten of them are below to try. The chapter test draws ten fresh questions each time and is marked the moment you finish, with your score by topic.
4.2.1 Ionic, covalent and metallic bonding10 questions
4.2.2 How bonding and structure are related to properties10 questions
4.2.3-4.2.4 Structure and bonding of carbon; nanoparticles9 questions
Ten Bonding, structure, and the properties of matter questions with answers
Try each one, then open the answer. These ten stay the same; the test draws new ones every time.
1. Magnesium oxide has a much higher melting point than sodium chloride. What is the best explanation?
A
the ions in MgO have larger charges, so they attract each other more strongly
B
magnesium oxide has stronger intermolecular forces between its molecules
C
magnesium atoms are heavier than sodium atoms, so they are harder to move
D
magnesium oxide has covalent bonds that are much stronger than ionic bonds
Show answer
Answer: A. Mg2+ and O2− attract more strongly than Na+ and Cl−, so more energy is needed to break the lattice. Both are ionic, with no intermolecular forces.
2. Carbon nanotubes are used to reinforce materials such as tennis rackets. Which properties make them suitable?
A
a high length to diameter ratio and high tensile strength
B
solubility in water, so they spread through it
C
a low melting point and a soft, slippery feel
D
ionic bonding, which makes them very hard and brittle
Show answer
Answer: A. Nanotubes are cylindrical fullerenes that are very long compared with their width and very strong when pulled, so they strengthen composites.
3. Why do substances made of small molecules, such as oxygen, not conduct electricity?
A
the molecules are too far apart to touch each other
B
the covalent bonds inside the molecules are too strong
C
the molecules are neutral and have no free electrons
D
the molecules contain ions that are unable to move
Show answer
Answer: C. To conduct there must be charged particles free to move. Small molecules are neutral and have no delocalised electrons.
4. A solid does not conduct electricity when solid or when molten, and it melts at 1710 °C. Which structure is it most likely to have?
A
a giant ionic lattice
B
a simple molecular structure
C
a giant metallic lattice
D
a giant covalent lattice
Show answer
Answer: D. No charged particles can move in either state, so it is not ionic or metallic, and a very high melting point rules out small molecules. Silicon dioxide is an example.
5. The simple particle model shows particles as small, solid spheres. What is a limitation of this model?
A
it shows particles in a liquid as able to move past each other
B
it shows particles in a solid as held in a regular pattern
C
it shows particles as hard spheres with no forces between them
D
it shows particles in a gas as far apart and moving randomly
Show answer
Answer: C. Real particles are not solid spheres and there are forces between them; the model also ignores the space inside atoms. The other statements are useful features of the model.
6. Why does graphite conduct electricity?
A
each carbon atom forms three bonds, held by strong forces between layers
B
it contains positive and negative ions that are free to move
C
each carbon atom forms four bonds, so its layers can slide over each other
D
each carbon uses three electrons in bonds, leaving one delocalised electron
Show answer
Answer: D. In graphite each carbon uses three electrons in bonds; the fourth is delocalised and free to move along the layers.
7. What holds the ions together in solid sodium chloride?
A
strong attraction between oppositely charged ions
B
a sea of delocalised electrons between the ions
C
shared pairs of electrons between sodium and chlorine atoms
D
weak forces between neighbouring sodium chloride molecules
Show answer
Answer: A. Sodium chloride is a giant ionic lattice held by strong electrostatic attraction between Na+ and Cl− ions. There are no molecules.
8. A ball and stick model of sodium chloride shows sticks joining the ions. Why is this misleading?
A
each ion attracts all its neighbours, not just one
B
sodium chloride is really made of small separate molecules
C
the sticks suggest that the ions are joined by weak forces
D
the ions in a real crystal are all exactly the same size
Show answer
Answer: A. The sticks suggest directional bonds between pairs of ions. In reality each ion is attracted electrostatically to every oppositely charged ion around it, and the ions touch.
9. When water boils, what is overcome?
A
the ionic bonds between hydrogen and hydroxide ions
B
the weak intermolecular forces between water molecules
C
the covalent bonds between hydrogen and oxygen atoms
D
the strong forces between the nuclei and the electrons
Show answer
Answer: B. Boiling separates molecules; the covalent bonds inside each H2O molecule stay intact. Steam is still H2O.
10. Why are alloys harder than pure metals?
A
alloys have no delocalised electrons to hold them together
B
the atoms in an alloy are all the same size, so they lock together
C
alloys contain covalent bonds between their atoms
D
different-sized atoms distort the layers so they slide less
Show answer
Answer: D. In a pure metal the layers of identical atoms slide easily. Atoms of a different size disrupt the layers. Alloys still have metallic bonding.
Bonding, structure, and the properties of matter: questions students ask
How many Bonding, structure, and the properties of matter MCQs are there?
29, each with the answer and a short explanation, across 3 topics: 4.2.1 Ionic, covalent and metallic bonding, 4.2.2 How bonding and structure are related to properties, 4.2.3-4.2.4 Structure and bonding of carbon; nanoparticles. Every chapter test draws ten of them, so you can take it many times.
Is the GCSE Chemistry (AQA) chapter 2 test free?
Yes. The test, the answers and the explanations are free and need no sign-up. Sign in only if you want your scores kept across devices.
How is the chapter test marked?
The moment you press Finish: your score, the right answer and an explanation for every question, and the ones you got wrong saved in My mistakes to retry.
