Day 1  Day 2  Day 3  Day 4  Day 5  Day 6

Day 1

Question 1

The table below shows the successive ionisation energies (in kJ mol⁻¹) for an unknown element, Q.

By analysing the graph and the data, determine which group element Q belongs to. Explain your reasoning.

Question 2

Write the full electronic configuration (using the 1s, 2s, 2p... notation) for the following atoms and ions: V, Fe³⁺, Br⁻, and Cu.

Day 2

Question 1

An element has the electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁵. Identify the element and state its period and group in the Periodic Table.

Question 2

Predict which element in Period 3 (Na-Ar) will have the largest difference between its first and second ionisation energies. Justify your prediction.

Day 3

Question 1

The graph of first ionisation energy across Period 2 (Li to Ne) shows a general trend but with exceptions at B and O.

• Explain why the first ionisation energy of Boron (B) is lower than that of Beryllium (Be).

• Explain why the first ionisation energy of Oxygen (O) is lower than that of Nitrogen (N).

Day 4

Question 1

Define the first ionisation energy. Write a balanced equation, including state symbols, for the first ionisation energy of aluminium.

Question 2

Sketch a graph showing the general trend in the first ionisation energy across Period 3 (Na to Ar). On your graph, mark and explain the positions of Al and S, which deviate from the general trend.

Day 5

Question 1

A mass spectrum of the element germanium (Ge) shows five peaks, confirming the existence of five stable isotopes. The table below shows the data for three of them.

Day 6

Question 1

Question 2

Element X has the following electronic configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s².

Would you expect the first ionisation energy of X to be greater or less than that of Potassium (K)? Explain.

Would you expect the first ionisation energy of X to be greater or less than that of Magnesium (Mg)? Explain.