Level 1: Core Concepts Check (Aiming for a Pass - 'S')

1. Define: What is a chemical change?

2. List: Name the four main types of chemical reactions.

3. Identify: What type of reaction is A + B → AB?

4. Identify: What type of reaction is Zn + CuSO₄ → ZnSO₄ + Cu?

5. Recall: What is the activity series of metals?

6. State: What is the chemical test for hydrogen gas?

7. State: What is the chemical test for oxygen gas?

8. Balance: Balance the equation: __H₂ + __O₂ → __H₂O.

9. Recall: Which is more reactive, zinc or copper?

Level 2: Connecting the Dots (Aiming for a Credit - 'C')

1. Explain: Describe the difference between a decomposition reaction and a combination reaction, giving an example of each.

2. Apply: A piece of magnesium ribbon is placed into a solution of copper(II) sulphate. Would you expect a reaction to occur? Explain your answer with reference to the activity series.

3. Describe: Explain how to collect carbon dioxide gas in the lab and why this method is suitable.

4. Balance and Classify: Write the balanced chemical equation for the reaction between sodium hydroxide (NaOH) and hydrochloric acid (HCl) to form sodium chloride (NaCl) and water (H₂O). What type of reaction is this?

5. Explain: Why is electrolysis needed to extract highly reactive metals like sodium, while less reactive metals like iron can be extracted by reduction with carbon?

Level 3: Exam Challenge (Aiming for a Distinction - 'A'/'B')

1. Experimental Analysis: A student performs an experiment by adding a piece of zinc metal to a blue solution of copper(II) sulphate. (a) State two observations the student would make. (b) Write the balanced chemical equation for the reaction that occurs. (c) What type of reaction is this? (d) If the student repeated the experiment by adding copper metal to a colourless solution of zinc sulphate, what would they observe? Explain this result using the activity series.