A-LevelChemistryChemical periodicity9701/22 · Feb/Mar 2018 · Q19 Marks
The graph shows a sketch of the first ionisation energies of six successive elements in the Periodic Table. The letters are not the symbols of the elements. [Figure 1.1: Bar chart showing first ionisation energy for elements A-F]
- (a)(i)Explain what is meant by the term first ionisation energy.[3]
- (a)(ii)Suggest why the first ionisation energy of B is much less than that of A.[3]
- (b)P–T are successive elements in Period 3 of the Periodic Table. The letters are not the symbols of the elements. On the axes, sketch a graph to show the trend in the atomic radius of the elements P–T. Explain your answer. [Figure 1.2: Graph axes for atomic radius vs element P-T][3]
This question uses a diagram from the original paper, which isn't shown here. Open the full paper from the past papers archive to see it.
Mark scheme
Marking points from the official mark scheme (Feb/Mar 2018). The mark or mark type is shown in brackets.
- [max 3] energy required / energy change
- when one electron is removed
- from each atom in one mole of
- gaseous atoms
- [3] for element B
- (outer electron is removed) from a higher energy level
- more shielding
- less attraction to nucleus
- [3] line on graph decreases P—T
- increasing nuclear charge AND electrons in same shell
- greater attraction between nucleus (and electrons)
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