2. 1 Why is the periodic table shaped like it is and how are the elements arranged?

3. 2

4. 3 Elements are arranged according to atomic # and e - configuration. Li: 3 e - ’s 1s 2 2s 1 Na: 11 e - ’s 1s 2 2s 2 2p 6 3s 1 K: 19 e - ’s 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 Paramagnetic or diamagnetic?

5. 4 Valence orbitals: outer shell orbitals beyond the closest noble-gas configuration Valence electrons: “the ones that can react” (located in the valence orbitals). Elements in a vertical row have the same number of valence electrons. 2s 2 3s 2 4s 2 5s 2 6s 2 7s 2 The other e - ’s are called core electrons and don’t react.

6. 5

7. 6

8. 7 Atomic sizes: Atomic size affects many properties, both physical and chemical

9. 8

10. 9 Li Be B C N O F Na Smaller SmallerSmaller WHY? K

11. 10

12. 11 Ionization Energy: The energy required to completely remove an e - from an atom in its gaseous state. Mg(g)  Mg 1+ + e - 1st ionization energy Mg 1+ (g)  Mg 2+ + e - 2nd ionization energy Question: Which of the above ionizations would have the highest ionization energy and why?

13. 12 electron being lost: 1st 2nd 3rd 4th 5th 6th 7th

14. 13 Increases

15. 14

16. 15 I.E. Overhead

17. 16 Electron Affinites: The energy change that occurs when an electron is added to a gaseous atom. Cl(g) + e -  Cl - (g)  E = - 349 kJ/mol What does the negative value mean?

18. 17 Electron affinity values

19. 18 What is meant by metallic character?

20. 19 Common Oxidation states: note the vertical similarities.

21. 20 I 2 (s) Cl 2 (g) Br 2 (l) The Halogen Family:

22. 21 LiK Na Alkali Metal Family