1. Tutorial 1) Using Slater’s rule confirm that the experimentally observed electronic configuration of K (Z = 19), 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1, is energetically more stable than the configuration 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1. 2) Use Slater’s rules to estimate values of Z eff for (a) a 4s and (b) a 3d electron in a V atom. Using your answer, explain why the valence configuration of the ground state of a V + ion is likely to be 3d 3 4s 1 rather than 3d 2 4s 2. 3) Assume three p-block elements A (Z = 6), B (Z = 7) and C (Z = 8) having ground state electronic configuration 1s 2 2s 2 2p 2, 1s 2 2s 2 2p 3 and 1s 2 2s 2 2p 4 respectively. The increase in Z eff between A and B is 0.69 whereas the increase between B and C is only 0.62. Suggest a reason why the increase in Z eff for a 2p electron is smaller between B and C than between A and B given the configurations of the atoms listed above.

3. Transition elements Group Alkali Metal Noble Gas Halogen Alkali Earth Metal Period Inner transition elements f block elements

4. np 1 ns 1 ns 2 f block elements np 2 np 3 np 4 np 5 np 6 d1d1 d2d2 d3d3 s1d5s1d5 d5d5 d6d6 d7d7 d8d8 d 10 s 1 d 10

6. He 2 Ne 10 Ar 18 Kr 36 Xe 54 Rn 86 Noble Gases 1s21s2 1s 2 2s 2 2p 6 1s 2 2s 2 2p 6 3s 2 3p 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6

7. Noble Gases np 6 Noble Gas

8. Noble Gases  Neon (Ne) and the elements below it in Group 18 have eight electrons in their outer energy levels.  Their energy levels are stable, so they do not combine easily with other elements.

9. Alkali Metals H 1 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87 1s11s1 1s 2 2s 1 1s 2 2s 2 2p 6 3s 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 7s 1

10. Alkali Metals ns 1 Alkali Metal

11. Alkali Metals  The alkali metals form compounds that are similar to each other.  Alkali metals each have one outer energy level electron.  It is this electron that is removed when alkali metals react.  The easier it is to remove an electron, the more reactive the atom is.  Unlike halogens, the reactivities of alkali metals increase down the group.

12. ns 1 ns 2 np 4 np 5 np 6 Ionization Energies of Elements

13. Ionization energy increases across a period and decreases down a group. Why ionization energy of N/P is higher than O/S? The variation of first ionization energy (in kilojoules per mole) through the main groups of the periodic table.

14. Ionization Energies of Elements The values of the first ionization energies of the elements up to Rn. Ionization energy increases across a period and decreases down a group.

15. Halogens Noble GasHalogen np 5 np 6

16. Halogens  Fluorine is the most reactive of the halogens because its outer energy level is closest to the nucleus.

17. ELECTRON AFFINITY Electron affinities are highest for elements near fluorine, particularly the halogens. Electronegativity increases across a period and decreases down a group.

18. ELECTRON AFFINITY Electron affinities are highest for elements near fluorine, particularly the halogens. Electronegativity increases across a period and decreases down a group.

19. Periodic Properties

20. Books: 1) INORGANIC CHEMISTRY: Duward Shriver and Peter Atkins. 2) Inorganic Chemistry: Principles of Structure and Reactivity by James E. Huheey, Ellen A. Keiter and Richard L. Keiter. 3) Inorganic Chemistry: Catherine Housecroft, Alan G. Sharpe.