Successive ionisation energies and electronic structure

Last updated: 17/01/2020

WJEC A-Level Chemistry Unit 1.2 – Basic ideas about atoms Successive ionisation energies and electronic structure

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Question 1 of 40

1. Question
Explain the ionisation energy trend across a period.
- The number of protons in the nucleus increases, so there is more nuclear attraction. Electrons are added to the same shell, so the atomic radius decreases. There is the same number of shells so shielding will hardly change. Therefore, the ionisation energy will increase as you go along a period.
- The number of protons in the nucleus decreases, so there is less nuclear attraction. Electrons are added to the same shell, so the atomic radius decreases. There is the same number of shells so shielding will hardly change. Therefore, the ionisation energy will increase as you go along a period.
- The number of protons in the nucleus decreases, so there less nuclear attraction. Electrons are removed from the same shell, so the atomic radius increases. There is the same number of shells so shielding will hardly change. Therefore, the ionisation energy will decrease as you go along a period.
- The number of protons in the nucleus increases, so there is more nuclear attraction. Electrons are removed from the same shell, so the atomic radius increases. There is the same number of shells so shielding will hardly change. Therefore, the ionisation energy will increase as you go along a period.
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Question 2 of 40

2. Question
Which of the following has the lowest first ionisation energy? Rb, Fr, Li, K
- Fr
- K
- Li
- Rb
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Question 3 of 40

3. Question
Write the electronic configuration of a chlorine ion, in its simplest form.
- [Ne] $3s^23p^6$
- [Ne] $3s^23p^4$
- [He] $3s^23p^4$
- [He] $3s^23p^6$
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Question 4 of 40

4. Question
What happens to ionisation energies between groups 2 – 13?
- A slight decrease
- A slight increase
- A significant increase
- A significant decrease
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Question 5 of 40

5. Question
Which of the following has the highest first ionisation energy? Al, Si, P, S, Cl
- Cl
- Si
- S
- P
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Question 6 of 40

6. Question
Write the electronic configuration of a magnesium ion, in its simplest form.
- [Ne]
- [Ne] $3s^2$
- [Ne] $3s^23p^2$
- [Ne] $3s^23p^3$
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Question 7 of 40

7. Question
Explain the pattern change in ionisation energies between groups 2-13.
- The outer electrons in group 13 are in p-orbitals. The outer electrons in group 2 are in s-orbitals. P-orbitals have a higher energy than S-orbitals so are further away from the nucleus and easier to remove so the ionisation energy decreases.
- The outer electrons in group 13 are in p-orbitals. The outer electrons in group 2 are in s-orbitals. P-orbitals have a higher energy than S-orbitals so are further away from the nucleus and easier to remove so the ionisation energy increases.
- The outer electrons in group 13 are in p-orbitals. The outer electrons in group 2 are in s-orbitals. S-orbitals have a higher energy than P-orbitals so are further away from the nucleus and easier to remove so the ionisation energy increases.
- The outer electrons in group 13 are in p-orbitals. The outer electrons in group 2 are in s-orbitals. S-orbitals have a higher energy than P-orbitals so are further away from the nucleus and easier to remove so the ionisation energy decreases.
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Question 8 of 40

8. Question
Write the electronic configuration of calcium, in its simplest form.
- [Ar] $4s^2$
- [Ne] $4s^2$
- [Ar] $4s^1$
- [Ne] $4s^1$
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Question 9 of 40

9. Question
Write the electronic configuration of a calcium ion, in its simplest form. Write the electronic configuration of a calcium ion, in its simplest form.
- [Ar]
- [Ar] $3s^2$
- [Ar] $3s^23p^2$
- [Ar] $3s^23p^3$
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Question 10 of 40

10. Question
Describe the trend in ionisation energy between the end of group 1 and the start of group 2.
- Sharp decrease
- Sharp increase
- Slight increase
- Slight decrease
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Question 11 of 40

11. Question
Write the electronic configuration of bromine, in its simplest form.
- [Ar] $4s^23d^1^04p^5$
- [Ar] $3s^23d^1^04p^5$
- [Ne] $4s^23d^1^04p^5$
- 1s^22s^22p^63s^23p^64s^23d^1^04p^5
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Question 12 of 40

12. Question
Write the electronic configuration of a fluorine ion, in its simplest form.
- [He] $2s^22p^6$
- [He] $3s^23p^6$
- [Ar] $3s^23p^6$
- [Ar] $2s^22p^6$
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Question 13 of 40

13. Question
Explain the pattern change in ionisation energies between the end of group 1 and the start of group 2.
- A new shell is added, increasing the distance of the outer shell from the nucleus and increasing the electron shielding.
- A new shell is removed, decreasing the distance of the outer shell from the nucleus and decreasing the electron shielding.
- A new shell is added, decreasing the distance of the outer shell from the nucleus and decreasing the electron shielding.
- A new shell is removed, increasing the distance of the outer shell from the nucleus and increasing the electron shielding.
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Question 14 of 40

14. Question
Write the electronic configuration of magnesium, in its simplest form.
- [Ne] $3s^2$
- [Ar] $3s^2$
- [Ne] $4s^2$
- [Ar] $4s^2$
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Question 15 of 40

15. Question
Write the electronic configuration of a sulfur ion, in its simplest form.
- [Ne] $3s^23p^6$
- [Ne] $3s^23p^2$
- [He] $3s^23p^2$
- [He] $3s^23p^6$
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Question 16 of 40

16. Question
What is the overall trend in ionisation energies down a group?
- Decreases
- Increases
- Slight increase
- No change to the ionisation energy
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Question 17 of 40

17. Question
Write the electronic configuration of fluorine, in its simplest form.
- [He] 2s^22p^5
- [Ne] 2s^22p^5
- [He] 3s^23p^5
- [Ne] 3s^23p^5
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Question 18 of 40

18. Question
Write the electronic configuration of an aluminium ion, in its simplest form.
- [Ne]
- [Ne] $3s^23p^6$
- [Ne] $3s^23p^4$
- [He] $3s^23p^4$
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Question 19 of 40

19. Question
Explain the ionisation energy trend down a group.
- The number of outer electron shells increases, so the distance of the electrons from the nucleus increases as well as the amount of shielding. Therefore, there is a weaker nuclear attraction. This outweighs the increasing nuclear charge, causing the ionisation energy to decrease
- The number of outer electron shells decreases, so the distance of the electrons from the nucleus decreases as well as the amount of shielding. Therefore, there is a stronger nuclear attraction. This outweighs the increasing nuclear charge, causing the ionisation energy to decrease.
- The number of outer electron shells decreases, so the distance of the electrons from the nucleus increases as well as the amount of shielding. Therefore, there is a weaker nuclear attraction. This outweighs the increasing nuclear charge, causing the ionisation energy to increase.
- The number of outer electron shells increases, so the distance of the electrons from the nucleus decreases as well as the amount of shielding. Therefore, there is a weaker nuclear attraction. This outweighs the increasing nuclear charge, causing the ionisation energy to increase.
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Question 20 of 40

20. Question
Write the electronic configuration of zinc, in its simplest form.
- [Ar] $4s^23d^1^0$
- [Ar] $4s^24d^1^0$
- [Ar] $3s^23d^1^0$
- [Ne] $4s^23d^1^0$
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Question 21 of 40

21. Question
Which of the following has the highest first ionisation energy? Be, Mg, Ca, Sr, Ba, Ra
- Be
- Ba
- Ca
- Ra
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Question 22 of 40

22. Question
Write the electronic configuration of sulfur, in its simplest form.
- [Ne] $3s^23p^4$
- [Ne] $4s^22p^4$
- [Ar] $3s^23p^4$
- [He] $3s^23p^4$
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Question 23 of 40

23. Question
Which of the following has the lowest first ionisation energy? Be, Mg, Ca, Sr, Ba, Ra
- Ra
- Ba
- Ca
- Be
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Question 24 of 40

24. Question
Write the electronic configuration of oxygen, in its simplest form.
- [He] $2s^22p^4$
- [He] $3s^23p^4$
- [Ar] $2s^22p^4$
- [Ne] $2s^22p^4$
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Question 25 of 40

25. Question
Which of the following has the highest first ionisation energy? B,C,N,O,F
- F
- O
- N
- B
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Question 26 of 40

26. Question
Write the electronic configuration of lithium, in its simplest form
- [He] $2s^1$
- [He] $3s^1$
- [Ne] $3s^1$
- [Ne] $2s^1$
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Question 27 of 40

27. Question
Which of the following has the lowest first ionisation energy? B,C,N,O,F
- B
- N
- O
- F
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Question 28 of 40

28. Question
Write the electronic configuration of titanium, in its simplest form.
- [Ar] $4s^23d^2$
- [Ar] $3s^23d^2$
- [Ne] $4s^23d^2$
- [He] $4s^23d^2$
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Question 29 of 40

29. Question
Which of the following has the highest first ionisation energy? Rn, Xe,Kr,Ar
- Ar
- Kr
- Xe
- Rn
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Question 30 of 40

30. Question
Write the electronic configuration of germanium, in its simplest form.
- [Ar] $4s^23d^1^04p^2$
- [Ar] $4s^23d^1^03p^2$
- [Ar] $3s^23d^1^04p^2$
- [Ar] $4s^23d^1^04p^6$
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Question 31 of 40

31. Question
Which of the following has the lowest first ionisation energy? Rn,Xe, Kr, Ar
- Rn
- Xe
- Kr
- Ar
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Question 32 of 40

32. Question
Write the electronic configuration of a bromine ion, in its simplest form.
- [Ar] $4s^23d^1^04p^6$
- [Ar] $4s^23d^1^04p^5$
- [Ar] $3s^23d^1^04p^4$
- [Ar] $3s^23d^1^03p^6$
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Question 33 of 40

33. Question
Which of the following has the highest first ionisation energy? K, Ca, Ga, Ge, As, Se, Br, Kr
- Kr
- Se
- K
- Ca
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Question 34 of 40

34. Question
Write the electronic configuration of a lithium ion, in its simplest form.
- [He]
- [Ne]
- [Ne] $2s^2$
- [He] $2s^1$
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Question 35 of 40

35. Question
Why do the noble gases have the highest ionisation energy out of all the groups?
- They have a full outer shell of electrons and a high positive attraction from the nucleus
- They have an empty outer shell of electrons
- They have a full outer shell of electrons and a low positive attraction from the nucleus
- They have an empty outer shell of electrons and therefore no positive attraction from the nucleus
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Question 36 of 40

36. Question
Which of the following has the lowest first ionisation energy? K, Ca, Ga, Ge, As, Se, Br, Kr
- K
- Ca
- Kr
- Se
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Question 37 of 40

37. Question
Write the electronic configuration of a potassium ion, in its simplest form.
- [Ar]
- [Ne]
- [He] $3s^1$
- [Ar] $4s^1$
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Question 38 of 40

38. Question
What is the overall trend in ionisation energy across a period?
- Increases
- Decreases
- Slight increase
- No change to the ionisation energy
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Question 39 of 40

39. Question
Which of the following has the highest first ionisation energy? Rb, Fr, Li, K
- Li
- K
- Fr
- Rb
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Question 40 of 40

40. Question
Write the electronic configuration of an oxygen ion, in its simplest form.
- [He] $2s^22p^6$
- [He] $2s^22p^2$
- [Ne] $2s^22p^2$
- [Ne] $2s^22p^6$
Correct

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