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

1. List: Name the three subatomic particles and their respective charges.

2. Define: What is the Atomic Number (Z) of an element?

3. Define: What is the Mass Number (A) of an element?

4. Identify: How many electrons can the first electron shell hold?

5. Recall: What is an isotope?

6. Identify: In the Periodic Table, what are the horizontal rows called?

7. Identify: What are the vertical columns called?

8. List: Give one property of a metal and one property of a non-metal.

9. Define: What is meant by electronic configuration?

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

1. Explain: An atom of Sodium (Na) has an atomic number of 11 and a mass number of 23. Explain how you would find the number of protons, neutrons, and electrons in a neutral atom of Sodium.

2. Connect: The electronic configuration of Magnesium (Mg) is 2, 8, 2. Explain how this information tells you its Group and Period in the Periodic Table.

3. Compare: Describe the difference between a neutral atom and an ion in terms of its subatomic particles.

4. Explain: What makes the Noble Gases (Group VIII/0) so chemically unreactive?

5. Discuss: Explain the periodic trend of electronegativity as you move from left to right across Period 3.

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

1. Problem-Solving: An unknown element 'Y' is in Period 3 and Group VI of the Periodic Table. (a) Write the electronic configuration for an atom of element Y. (b) What is the atomic number of element Y? (c) Is Y a metal or a non-metal? (d) To become stable, would an atom of Y tend to gain or lose electrons? How many? What would be the charge of the ion it forms?