Bonding and Structure Worksheet - GCSE - Intermediate

Bonding and Structure worksheet for GCSE (Key Stage 4 / GCSE (Ages 14-16)). Intermediate level science practice, aligned to the UK National Curriculum. Print-ready with answer key included.

Science•Key Stage 4 / GCSE (Ages 14-16)•Bonding and Structureintermediate

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Bonding and Structure: GCSE Chemistry Practice

Key Stage 4 | Ages 14–16 | Intermediate

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Instructions: Answer each question using precise chemical vocabulary and the command word as a guide. Show working for calculations and include units where appropriate. The questions progress from recall to applying evidence about bonding and properties.

Bonding: Core Knowledge

Answer each question in a concise, scientifically accurate way. Use the command word to decide how much detail is needed. Include the key particles and forces involved.

1. State the type of particles found in a solid ionic compound. [2 marks]

2. Describe how a sodium atom forms a sodium ion. [2 marks]

3. Define a covalent bond. [2 marks]

4. Explain why metals conduct electricity when solid. [3 marks]

Compare Bonding and Structure

Use the completed comparison table to identify similarities and differences. Then answer each question using evidence from the table and your knowledge of bonding.

Substance	Structure and bonding	Electrical conductivity	Melting point
Magnesium	giant metallic lattice	conducts when solid and liquid	high
Sodium chloride	giant ionic lattice	conducts when molten or dissolved; not solid	high
Carbon dioxide	simple molecular; covalent bonds within molecules; weak forces between molecules	does not conduct	low

1. Which substance has mobile electrons when solid?

2. Explain why solid sodium chloride does not conduct electricity, but molten sodium chloride does. [3 marks]

3. Compare the melting points of magnesium and carbon dioxide in terms of their structures and forces. [3 marks]

Apply Your Knowledge: Ionic and Covalent Bonding

Work through each question, showing electron changes or particle reasoning where relevant. Use the formulae and information given; do not assume that all covalent substances have the same structure.

1. A magnesium atom loses two electrons. State the charge on the ion formed and explain why. [2 marks]

2. Explain why magnesium oxide has a high melting point. [3 marks]

3. A substance consists of small molecules with strong covalent bonds within each molecule and weak forces between molecules. Predict whether it is likely to have a high or low boiling point, and explain your answer. [3 marks]

4. Explain why diamond is hard, although it contains only carbon atoms. [3 marks]

Analyse Property Data

Read the data table carefully. Use the figures as evidence, then connect each observation to the relevant structure and bonding. Give units when quoting temperatures.

Substance	Melting point (°C)	Conducts when solid?	Conducts when molten?
A	801	no	yes
B	−78	no	no
C	660	yes	yes

1. Which substance is most likely to have a giant ionic lattice?

2. Identify the likely bonding in substance C and use the data to support your answer. [2 marks]

3. Explain why substance B has a much lower melting point than substance A. [3 marks]

Explain a Material’s Properties

Build a linked explanation: identify the structure, describe its particles and bonding, then connect these to the stated properties. Use the evidence in the prompt rather than making unsupported claims.

A material is made of layers of carbon atoms. Each carbon atom forms three covalent bonds, and one electron per atom is delocalised. The layers can slide over one another.

Explain why this material conducts electricity and is soft and slippery. [5 marks]

Extended Response: Bonding and Properties

Write one developed comparison, using the evidence in the prompt. Explain how particle arrangement, bonding and the forces between particles account for the properties. Finish with a clear conclusion that directly answers the question.

Compare the structures and properties of sodium chloride and carbon dioxide. Explain the difference in their melting points and electrical conductivity, referring to the particles and forces in each substance. [6 marks]

Answer Key

Activity 1: 1. Positive and negative ions. 2. It loses one electron, forming a Na⁺ ion. 3. A shared pair of electrons, electrostatically attracted to the nuclei of both bonded atoms. 4. It contains delocalised electrons that can move through the metal and carry charge.

Activity 2: 1. Magnesium. 2. In solid sodium chloride, the ions are fixed in a lattice and cannot carry charge. When molten, the ions are mobile and carry charge. 3. Magnesium has a giant metallic lattice with strong metallic bonding throughout, requiring much energy to overcome. Carbon dioxide is simple molecular; only weak intermolecular forces need to be overcome when it melts, so its melting point is low.

Activity 3: 1. Mg²⁺; it loses two negatively charged electrons, leaving two more protons than electrons. 2. It has a giant ionic lattice with strong electrostatic attractions between oppositely charged ions; considerable energy is needed to overcome them. 3. Low; only the weak forces between molecules need to be overcome, which requires relatively little energy. 4. Each carbon atom is strongly covalently bonded to other carbon atoms in a giant network, making diamond very hard.

Activity 4: 1. A. 2. Metallic bonding; it conducts when solid and molten, consistent with mobile delocalised electrons. 3. A is ionic, with strong electrostatic attractions in a giant lattice, whereas B is simple molecular, with weak forces between molecules; much less energy is needed to melt B.

Activity 5: Graphite. Delocalised electrons can move along the layers and carry charge. Each layer consists of strongly covalently bonded carbon atoms, but the forces between layers are weak, so the layers slide over one another; this makes graphite soft and slippery.

Activity 6: Sodium chloride has a giant ionic lattice of positive and negative ions held by strong electrostatic attractions. A large amount of energy is needed to overcome these attractions, so it has a high melting point. Its ions are fixed in the solid and cannot carry charge, but become mobile when molten, allowing it to conduct. Carbon dioxide consists of small molecules with strong covalent bonds within each molecule but weak intermolecular forces between molecules. Relatively little energy is needed to overcome these weak forces, so it has a low melting point. It does not conduct because it has no mobile ions or delocalised electrons. Conclusion: their contrasting structures and mobile particles account for their different melting points and conductivity.