1. Atomic Structure Ionisation Energies

2. Ionisation Energy The first ionisation energy of an element is the energy required to remove completely one mole of electrons from one mole of gaseous atoms to form one mole of gaseous ions with a single positive charge. Na (g)  Na + (g) + e -

3. Ionisation Energy The second ionisation energy of an element is the energy required to completely remove one mole of electrons from one mole of gaseous singly charged ions to form one mole of gaseous ions with two positive charges. Mg + (g)  Mg 2+ (g) + e -

4. Factors Affecting Ionisation Energy Ionisation energy is a measure of the energy needed to pull a particular electron away from the attraction of the nucleus. A high value of ionisation energy shows a high attraction between the electron and the nucleus.

5. Factors Affecting Ionisation Energy Li First ionisation energy (kJ/mol) 520419 Ionisation energy decreases when the atom becomes larger because the electrostatic attraction between electrons and protons depends on the distance between the two  the larger the distance the weaker the attraction. K

6. Factors Affecting Ionisation Energy First ionisation energy (kJ/mol) 738590 As the atom gets larger it will also have more energy levels that are full of electrons  reduce the electrostatic attraction between protons and electrons.  This is called ELECTRON SHIELDING.  Hence the ionisation energy will decrease Mg Ca

7. Factors Affecting Ionisation Energy ionisation energy (kJ/mol) Ionisation energy increases as the charge on the nucleus increases because the electrostatic attraction between the electrons and protons increases. 10p 20817737 12p

8. Successive ionisation energies Na 2,8,1

9. Successive ionisation energies Na

10. Successive ionisation energies Na

11. Successive ionisation energies Na

12. Successive ionisation energies Na

13. Successive ionisation energies Na

14. Successive ionisation energies Na

15. Successive ionisation energies Na

16. Successive ionisation energies Na

17. Successive ionisation energies Na

18. Successive ionisation energies Na

19. Successive ionisation energies Na

20. Successive ionisation energies Na

21. Successive ionisation energies Na

22. Successive ionisation energies Na

23. Successive ionisation energies Na

24. Successive ionisation energies Na

25. Successive ionisation energies Na

26. Successive ionisation energies Na

27. Successive ionisation energies Na

28. Successive ionisation energies Na

29. Successive ionisation energies Na

30. Successive ionisation energies Na

31. Successive ionisation energies Na 2,8,1

32. Successive ionisation energies Si 2,8,4

33. Successive ionisation energies Si

34. Successive ionisation energies Si

35. Successive ionisation energies Si

36. Successive ionisation energies Si

37. Successive ionisation energies Si

38. Successive ionisation energies Si

39. Successive ionisation energies Si

40. Successive ionisation energies Si

41. Successive ionisation energies Si

42. Successive ionisation energies Si

43. Successive ionisation energies Si

44. Successive ionisation energies Si

45. Successive ionisation energies Si

46. Successive ionisation energies Si

47. Successive ionisation energies Si

48. Successive ionisation energies Si

49. Successive ionisation energies Si

50. Successive ionisation energies Si

51. Successive ionisation energies Si

52. Successive ionisation energies Si

53. Successive ionisation energies Si

54. Successive ionisation energies Si

55. Successive ionisation energies Si

56. Successive ionisation energies Si

57. Successive ionisation energies Si

58. Successive ionisation energies Si

59. Successive ionisation energies Si

60. Successive ionisation energies Si 2,8,4

61. Factors Affecting Ionisation Energy Li First ionisation energy (kJ/mol) 520419 Ionisation energy decreases when the atom becomes larger because the electrostatic attraction between electrons and protons depends on the distance between the two  the larger the distance the weaker the attraction. K

62. Factors Affecting Ionisation Energy First ionisation energy (kJ/mol) 738590 As the atom gets larger it will also have more energy levels that are full of electrons  reduce the electrostatic attraction between protons and electrons.  This is called ELECTRON SHIELDING.  Hence the ionisation energy will decrease Mg Ca

63. Factors Affecting Ionisation Energy ionisation energy (kJ/mol) Ionisation energy increases as the charge on the nucleus increases because the electrostatic attraction between the electrons and protons increases. 10p 20817737 12p

64. Factors Affecting Ionisation Energy- Summary The value of the ionisation energy will: ↑ as Z↑because the electrostatic attraction between the electrons and protons increases. ↓ as size of atom ↑because the larger the distance between electrons and protons the weaker the electrostatic attraction. because more full energy levels (ELECTRON SHIELDING).  reduce the electrostatic attraction between protons and electrons.

65. Variation in 1 st Ionisation Energy Across a Period Question: Predict the trend in value of 1 st IE for period 2 (Li  Ne) by sketching a graph and giving a reason

66. Variation in 1 st Ionisation Energy Across a Period General Trend: As Z increases the 1 st IE increases as the electrons are being removed from the same shell i.e shielding is constant and the size of the atom decreases due to increased nuclear charge. There are 2 exceptions to the general trend: Be  B and N  O

67. Variation in 1 st Ionisation Energy Across a Period Be  B due to the existence of SUB- SHELLS within the energy shells. These are known as s,p,d and f sub-shells. The s sub-shell contains a maximum of 2 electrons The p sub-shell contains a maximum of 6 electrons Beryllium has an electronic configuration of 1s 2 2s 2 Boron has an electronic configuration of 1s 2 2s 2 2p 1 The outer electron in boron is removed from a p- orbital which is higher in energy than the s- orbital outer electron in beryllium Note: higher energy electrons require less energy (i.e.are easier) to remove.

68. Variation in 1 st Ionisation Energy Across a Period N  O Within the sub-shells are found “orbitals” An orbital can only hold a maximum of two electrons The mutual repulsion between the pair of electrons in oxygen means that less energy is required to remove one of them from the atom, hence lowering the first ionisation energy. Nitrogen is 1s 2 2s 2 2p 3 all p electrons are unpaired Oxygen is 1s 2 2s 2 2p 4 pairing occurs for the first time pxpx pypy pzpz ↑↑↑ pxpx pypy pzpz ↑↓↑↑

69. Variation in 1 st Ionisation Energy Across a Period - Summary General Trend: As Z increases the 1 st IE increases as the electrons are being removed from the same shell i.e shielding is constant and the size of the atom decreases due to increased nuclear charge. Be  B The outer electron in boron is removed from a p-orbital which is higher in energy than the s-orbital outer electron in beryllium, therefore, it is easier to remove and the first ionisation energy is lower. N  O Nitrogen is 1s 2 2s 2 2p 3 Oxygen is 1s 2 2s 2 2p 4 The mutual repulsion between the pair of electrons in the 2p orbitals in oxygen means that less energy is required to remove one of them from the atom than the unpaired 2p electrons in nitrogen, hence lowering the first ionisation energy.

70. Variation in 1 st Ionisation Energy Across a Period - Summary Period 3 follows the same pattern as period 2 and is explained in the same way Ionisation energies provide evidence for the presence of shells and orbitals in atoms