2. Catalyst – February 12-5+4, 2010 1. How did Rutherford add to Thompson’s theory? 2. Draw the Bohr model of Chlorine. 3. How many electrons can fit into d orbitals? 4. How many electrons fit in the 2 nd energy level?

3. Catalyst These are the electron configurations for the following elements:  Mg-1s 2 2s 2 2p 6 3s 2  Ne- 1s 2 2s 2 2p 6  Si- 1s 2 2s 2 2p 6 3s 2 3p 2  K- 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1  Find the electron configuration of: 1. Fe 2. O

4. Today’s Agenda  Catalyst  Continue Electron Configuration  Practice!  Review (time left after EC)  Exit Question

5. Today’s Objectives  SWBAT write electron configurations for elements.  SWBAT write noble gas configurations for elements.

6. Electron Configuration Review Fill in the table below on your notes. Orbital Type (s, p, d, or f) Energy Level# of OrbitalsMaximum # of Electrons s p 5 14 1 2 36 d f 7 10 1,2,3,4… 2,3,4… 3,4… 4…

7. Electron Configuration  Key Point #3: Electron configuration shows how the electrons are distributed among the various atomic orbitals and energy levels.  The format consists of a series of numbers, letters, and superscripts as shown below: 1s 2

8. Electron Configuration 1s 2  Large number = energy level  Letter = atomic orbital  Superscript (small) number = number of electrons in atomic orbital

9. Figure it out yourself!! (15 mins)  Look at the tables that have 1s, 2s, 2p on your notes sheet. Below, I have shown 4 correct electron configurations. See if you can figure out how to do the last two.  Mg -1s 2 2s 2 2p 6 3s 2  Ne - 1s 2 2s 2 2p 6  Si - 1s 2 2s 2 2p 6 3s 2 3p 2  K - 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1  S -  B -

10. Before we move on…  Let’s relate this to good ole Bohr Models  Hydrogen  Helium  Lithium

11. Subshells on the Periodic Table s p d f

12. Electron Configuration N – 1s 2

13. Electron Configuration N – 1s 2 2s 2

14. Electron Configuration N – 1s 2 2s 2 2p 3

15. Electron Configuration N – 1s 2 2s 2 2p 3 = 7 e-

16. Electron Configuration Na – 1s 2

17. Electron Configuration Na – 1s 2 2s 2

18. Electron Configuration Na – 1s 2 2s 2 2p 6

19. Electron Configuration Na – 1s 2 2s 2 2p 6 3s 1 = 11 e-

20. Electron Configuration Try these on your own! Be: Ne: Br:

21. Electron Configuration Be: 1s 2 2s 2 Ne: 1s 2 2s 2 2p 6 Br: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5

22. Work Time  Please complete the Independent Practice Problems Part One in your notes  If you finish early, get an extra credit practice sheet from Mr. Jhaveri

23. Electron Configuration Scientists are WAY too lazy to write all that mess!

24. Electron Configuration FIGURE IT OUT YOURSELF!!! (10 mins) Ag – [Kr]5s 2 4d 9 S – [Ne]3s 2 3p 4 Sm – [Ar]4s 2 3d 2 Si- Rb-

25. Electron Configuration Noble Gas Configuration – simply start writing your notation from the last noble gas BEFORE the atom you are going to.

26. Electron Configuration Ag

27. Electron Configuration Ag – [Kr]5s 2 4d 9

28. Electron Configuration Ca

29. Electron Configuration Ca – [Ar]4s 2

30. Electron Configuration S

31. S – [Ne]3s 2 3p 4

32. Electron Configuration and Valence Electrons Each group: Write long electron configurations for first four elements in given family.  Group 1: Alkali Metals (1)  Group 2: Alkaline Earth Metals (2)  Group 3: Boron’s group (13)  Group 4: Nitrogen’s group (15)  Group 5: Halogens (17)  Group 6: Noble Gases (18)

33. Electron Configuration and Valence Electrons Each group: Write long electron configurations for first four elements in given family.  Group 1: Alkali Metals (1)  Group 2: Alkaline Earth Metals (2)  Group 3: Boron’s group (13)  Group 4: Carbon’s group (14)  Group 5: Nitrogen’s group (15)  Group 6: Oxygen’s group (16)  Group 7: Halogens (17)  Group 8: Noble Gases (18)

34. Electron Configuration and Valence Electrons What trends do you see? How many valence electrons are there in each group?  Group 1: Alkali Metals (1)  Group 2: Alkaline Earth Metals (2)  Group 3: Boron’s group (13)  Group 4: Nitrogen’s group (15)  Group 5: Halogens (17)  Group 6: Noble Gases (18)

35. Electron Configuration and Valence Electrons What trends do you see? How many valence electrons are there in each group?  Group 1: Alkali Metals (1)  Group 2: Alkaline Earth Metals (2)  Group 3: Boron’s group (13)  Group 4: Carbon’s group (14)  Group 5: Nitrogen’s group (15)  Group 6: Oxygen’s group (16)  Group 7: Halogens (17)  Group 8: Noble Gases (18)

36. Valence Electron Trends on the Periodic Table

37. Homework/Review Sheet  GAMEDAY TOMORROW!!

38. Exit Question  Write the noble gas configuration for  Bromine  Copper  Sodium

39. Exit Question