Practical questions
During the GCSE chemistry course you will complete practical activities from eight Practical Activity Groups (PAGs).
The exams will include questions about some of these experiments. You may also be asked to apply what you know to unfamiliar practical contexts, which will draw on your practical knowledge and understanding.
You could be asked to:
- write or identify a hypothesis or prediction that could be tested in an experiment
- name equipment and measuring instruments, and describe what they do and how they are used
- identify factors that must be controlled, and explain why
- describe how to work safely
- process data by doing calculations and representing them in graphs
- identify patterns and trends in data
- evaluate the accuracy, repeatability and reproducibility of data, and identify possible errors and anomalous results
- suggest improvements to methods
- interpret data and draw conclusions from it
Practical questions will appear throughout both exams papers, and at both foundation tier and higher tier. Practical questions could be multiple choice or free response, and could include calculations. A six-mark question could be asked in a practical context, so practice writing in detail about the practical work you have done.
It's important to look back at your lab book or your notes from the practical activities you have done when revising for your exams.
These questions have been written by Bitesize consultants as suggestions to the types of questions that may appear in an exam paper.
Learn about practicals with Dr Alex Lathbridge
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Sample question 1 - Foundation
Question
Phil is investigating the properties of ionic compounds.
He adds sodium chloride crystals to the bottom of a beaker and dips the electrodes into the crystals.
a) Predict what Phil will observe. [1 mark]
b) Phil now adds water to the beaker. Predict what will change. [1 mark]
c) Explain why you would expect this change. [2 marks]
d) Suggest one safety precaution that Phil should take when carrying out this experiment. [1 mark]
a) The bulb will remain unlit. [1]
b) The bulb will light. [1]
c)
- the sodium chloride is unable to conduct electricity in the solid state as there are no charged particles that are able to move [1]
- when it is dissolved it can conduct electricity because the charged ions are able to move, causing the bulb to light [1]
d) Chlorine is a toxic gas so any precaution to ensure that a large quantity of chlorine is not released is acceptable.
Any one of the following:
- using of low voltages
- only connecting the electricity for a short time
- avoiding use of a high concentration of sodium chloride solution
- ensuring the lab is well ventilated or using a fume hood
[1]