Ionisation energies and electron shells Quiz
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5 questions, one answer each
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1. An element has successive ionisation energies (kJ mol⁻¹) of 590, 1145, 4912, 6491. In which group is it?
- A. Group 2
- B. Group 1
- C. Group 3
- D. Group 4
2. Why is the first ionisation energy of potassium lower than that of sodium?
- A. Potassium has fewer protons
- B. Potassium has a smaller atomic radius
- C. Potassium's outer electron is in a p sub-shell
- D. Potassium's outer electron is further from the nucleus and more shielded
3. Which equation represents the third ionisation energy of aluminium?
- A. Al(g) → Al³⁺(g) + 3e⁻
- B. Al²⁺(g) → Al³⁺(g) + e⁻
- C. Al²⁺(g) + e⁻ → Al⁺(g)
- D. Al(s) → Al³⁺(g) + 3e⁻
4. The first ionisation energy of sulfur is lower than that of phosphorus because
- A. sulfur has fewer protons
- B. sulfur's outer electron is in a 3s sub-shell
- C. repulsion between paired electrons in a 3p orbital makes one easier to remove
- D. sulfur has a smaller atomic radius
5. Which statement about the 10th ionisation energy of sodium is correct?
- A. It is lower than the 9th because the ion is smaller
- B. It is similar to the 9th because both are from the second shell
- C. It is the first to be exothermic
- D. It is much higher than the 9th because the electron is removed from the first shell