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

1. Define: What is Relative Atomic Mass (Ar)?

2. Calculate: Find the Relative Molecular Mass (Mr) of water (H₂O). (Ar: H=1, O=16).

3. Define: What is a mole?

4. Recall: What is the value of the Avogadro Constant?

5. Define: What is Molar Mass, and what are its units?

6. Identify: What is the mass of one mole of Carbon (C)? (Ar: C=12).

7. List: How many molecules are in one mole of any substance?

8. Calculate: Find the Relative Formula Mass of Sodium Chloride (NaCl). (Ar: Na=23, Cl=35.5).

9. State the formula: Write the equation that connects mass, moles, and molar mass.

10. True or False: The Relative Molecular Mass of O₂ is 16.

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

1. Explain: Explain the difference between the Relative Atomic Mass of Chlorine (35.5) and the Mass Number of its most common isotope (35).

2. Calculate: How many moles are there in 88 g of carbon dioxide (CO₂)? (Ar: C=12, O=16).

3. Calculate: What is the mass of 3 moles of sulphuric acid (H₂SO₄)? (Ar: H=1, S=32, O=16).

4. Explain: Two balloons are filled with 1 mole of Helium gas and 1 mole of Oxygen gas respectively. Which balloon is heavier? Explain why, even though they contain the same number of particles.

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

1. Multi-step Problem: A student is given a 90 g sample of glucose (C₆H₁₂O₆). (Ar: C=12, H=1, O=16). (a) Calculate the Molar Mass of glucose. (b) Calculate the number of moles of glucose in the 90 g sample. (c) Calculate the total number of molecules of glucose in the sample. (d) Calculate the total number of carbon atoms in the sample.