Edexcel IGCSE Chemistry 2.4C Group 1 electronic configurations
Practise Group 1 electron-structure questions by comparing shells and explaining why potassium loses its outer electron more easily.
- Syllabus
- First assessment 2019
- Course
- Chemistry 4CH1
Exam points
- Use electronic configurations to compare lithium, sodium or potassium atoms.
- Explain higher reactivity by more shells, weaker attraction and easier outer-electron loss.
- Link similar reactions to each Group 1 atom having one electron in its outer shell.
2.4C Group 1 electronic configurations question 1
[Maximum number: 3]
Iron metal was discovered several thousand years ago. Iron is produced industrially from iron(III) oxide by extraction using carbon.
Sodium is a metal in Group 1 of the Periodic Table. Sodium was discovered by Sir Humphrey Davy in 1807. It is produced industrially by the electrolysis of sodium chloride.
Explain why the reactivity of metals in Group 1 increases from lithium to potassium.
- the outer electron in potassium is further away from the nucleus
- the outer electron in potassium is less strongly attracted by the nucleus
- the outer electron is more easily lost
Allow:
- reverse arguments
- potassium has more electron shells than lithium
- potassium is larger than lithium
- potassium has a greater atomic radius
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