2. Catalyst – February -5, 2.011x10 3 FUN GRAPH FRIDAY! 1. What are 2 conclusions you can draw from this pie chart? HW OUT

3. Today’s Agenda  Catalyst  Quiz 2.1 Tracking (Resume)  HW Review  Electron Configuration!!  Practice, Practice, Practice  Work Time!  Reward!  Exit Question HW: STAY WARM AND START STUDYING FOR THE UNIT TEST!

4. Today’s Objectives  SWBAT write electron configurations for elements.

5. QUIZ 2.1 TRACKING!

6. HOMEWORK REVIEW!

7. How? Schrödinger Equation Key Point #1: The Schrödinger Equation predicts the location of an electron in an atom.  It tells us that electrons hang out in atomic orbitals.  Imagine electrons filing into hotels…

8. Schrödinger Equation and Atomic Orbitals Key Point #2: There are 4 atomic orbitals… s p d f

9. A Saying to Remember the Four Atomic Orbitals s ome p irates d ie f iercely!

10. The s Orbital One s orbital in each energy level The s orbital is shaped like a sphere Can hold 2 electrons total

11. So how many electron fit in the FIRST energy level??? 2

12. The p Orbital Three p orbitals in each energy level (starting in the 2nd energy level!) Shape looks like dumbells or bowties Can hold 6 electrons total

13. So how many electron fit in the SECOND energy level??? 2 8

14. The d orbital -Five d orbitals in each energy level (starting in the 3 rd energy level!) -Shape looks like eggs or flowers -Can hold 10 electrons

15. So how many electron fit in the THIRD energy level??? 2 8 18

16. The f orbital  Seven f orbitals (starting in 4th energy level!)  Can hold 14 electrons

17. So how many electron fit in the THIRD energy level??? 2 8 18 32

19. Electron Configuration Rules 1. Pauli Exclusion Principle: An atomic orbital may hold no more than 2 electrons. 2. Aufbau Principle: Electrons enter the lowest energy orbital first. 3. Hund’s Rule: Electrons do not pair up until they have to.

20. 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…

21. 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

22. The Code 1s 2 Large number = energy level Letter = orbital Small superscript number = Number of electrons

23. Figure it out yourself!! (15 mins)  Look at the table that has 1s, 2s, 2p on your notes sheet.  Here I have put a couple 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-

25. Electron Configuration N – 1s 2

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

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

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

29. Electron Configuration Na – 1s 2

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

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

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

33. Electron Configuration Be: Ne: Br:

34. 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

35. Noble Gas Configuration Scientists are WAY too lazy to write all that mess!

36. Electron Configuration FIGURE IT OUT YOURSELF!!! (10 mins) Hg – [Xe]6s 2 4f 14 5d 10 S – [Ne]3s 2 3p 4 Sm – [Xe]6s 2 4f 5 Si- Rb-

37.  Key Point #4: Noble Gas configuration starts with noble gas BEFORE the atom you are going to. Noble Gas Configuration

38. Exit Question  Write the electron configuration for the following element. Then, write how many valence electrons there are. 1. Manganese (Mn)