1. Electron Configuration Where do the electrons really hang out?? In those crazy orbitals!! EC = The arrangement of electrons around a nucleus.

2. EC--- Things to keep in mind There are seven energy levels (we only worry about the first 4). Within the levels are subshells (s, p, d, f) Each subshell can accommodate a certain number of orbitals Each orbital can contain 2 electrons

3. Electron Configuration 3 Rules:  Aufbau Principle  Pauli Exclusion Principle  Hund’s Rule

4. Aufbau Principle Electrons enter the lowest energy level first Different levels within a principal energy level can overlap the energy levels of an adjacent principal level The filling of atomic orbitals does not follow a simple pattern.

5. Aufbau Principle- Here’s the pattern!! 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f

6. Pauli Exclusion Principle An atomic orbital may describe at most 2 electrons 1 or 2 electrons may occupy an orbital When an orbital contains 2 electrons, they must have an opposite paired spin

7. Pauli Exclusion Principle Because of their magnetic moments, we generally represent electrons using a single barbed arrow. The tip of the arrow points to the magnetic north of the electron

9. Hund’s Rule When electrons occupy orbitals of equal energy (s, p, d, f), one electron enters each suborbital until all orbitals contain 1 electron with the same parallel spin The second electrons then add to each orbital so that their spins are paired.

10. Heisenberg Uncertainty Principle “The more precisely the position is determined, the less precisely the momentum is known in this instant, and vice versa.” It is impossible to know the velocity and position of the electron at the same time.

11. Show them the old fashion way! Practice several on the back. Do WS 1 using the table!1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f

12. Electron Configuration- Level 1 WS- Use the table!

13. Some things to note Valence electrons are those in the outer s and p orbitals. Shared and unpaired electrons can be determined by looking at the outermost, incomplete orbital.

14. We can just use Aufbau– it is a little easier 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f Oxygen Silicon Calcium

15. Work on your Valence electron WS for 10 minutes!

16. Warm Up Can we tell which element by looking at the EC? 1s 2 2s 2 2p 6 3s 2 3p 5 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10

17. How did you do Count the number of electrons 1s 2 2s 2 2p 6 3s 2 3p 5 = 17 electrons, Chlorine 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 = 30 electrons, Zinc

18. Did you write this in your notes? Valence electrons are those in the outer s and p orbitals. Shared and unpaired electrons can be determined by looking at the outermost, incomplete orbital.

19. Molecular Orbital Diagrams- Use lines to show orbitals 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f Li Phosphorus Vanadium

20. Go over some on the Valence electron WS

21. We can also use the periodic table to determine EC. Try some more of the WS using the periodic table method…

22. Get out a half sheet of paper… I will project the quiz as soon as the bell rings. Be sure you write very neat!!

23. Noble Gas Configuration… Write the noble gas in the period above the element… add the rest of the electron configuration. Example: Long form for Phosphorus: 1s 2 2s 2 2p 6 3s 2 3p 3 Noble Gas Configuration for Phosphorus Nobel gas above P = Ne [Ne] 3s 2 3p 3

24. You need to be careful which periodic table you use for this!! The Web-Elements PT works well…

25. Now you try! Write the noble gas configuration for V (atomic #23) La (atomic #57) Lr (atomic #103)

26. Now you try! V (atomic #23) La (atomic #57) Lr (atomic #103)

27. Now you try! Write the noble gas configuration for V [Ar] 4s 2 3d 3 La [Kr]6s 2 4f 1 Lr [Xe] 7s 2 4f 14 6d 1

28. Molybdenum (42) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 4d 5 Th (90) [Rn] 7s 2 5f 2

29. Ground, Excited or Impossible? Ground- If the electrons are in the orbitals that you would expect them to be in. Excited- If some of the electrons are in a higher energy level. Impossible- If the orbital doesn’t exist and/or the EC doesn’t make any sense.

30. Ground, Excited or Impossible? Chlorine- 17 electrons 1s 2 2s 2 2p 6 3s 2 3p 5 1s 2 2s 2 2p 6 3s 1 3p 3 4s 2 4p 1 1s 2 2s 2 2p 6 3s 1 3p 4 2d 2

31. Ground, Excited or Impossible? Zinc- 30 electrons a. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 8 6s 2 b. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 4 4p 7 c. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10

32. You try… Write the electron configuration for carbon… Write an electron configuration for an excited atom. Write an impossible EC… Have your neighbor check your work.

33. Warm Up Think back to unit 3… and the coulombic attraction POGIL. What happens to the size of an atom when it gains electrons? What happens to atomic radius when an atom looses electrons?

34. Questions on the HW?

35. What happens with Ions?? Ions gain or lose electrons… What is the electron configuration for the magnesium cation? What about S 2-

36. When removing electrons … Remove the last electrons that were placed… Unless there are electrons in the d orbital…then remove the last s electrons first.

37. Isoelectronic… Different atoms that have the same electron configuration. Na 1+ Ne F 1-

38. Identify the atoms An element that has a 2- charge that is isoelectronic with Neon.

39. Identify the atoms An atom that has lost 3 electrons and is isoelectronic with He

40. Identify the atoms An atom that has gained one electron and has the same EC as Cu.

41. Identify the atoms An element that has a 2- charge that is isoelectronic with Neon. An atom that has lost 3 electrons and is isoelectronic with He An atom that has gained one electron and has the same EC as Cu.

42. Work on the group activity…

43. Ionization Energy  Energy required to overcome the attraction of the nucleus and remove an electron.

44. Draw the MO diagrams for F, Ne and Na How much energy would it take to remove an electron?

45. The Trend IE decreases as you move down a group because electrons are further away so they are easier to strip off. Ionization energy increases as you move left to right, for representative elements because the attraction by the nucleus is stronger so it is harder to pull electrons away.

46. Ionization Energies 1 st ionization energy- energy to remove the 1 st electron. 2 nd ionization energy- energy to remove the 2nd electron. 3 rd ionization energy- energy to remove the 3rd electron.

47. Warm Up 1. Write the electron configuration for the atom with 43 electrons. 2. Circle the valence electrons. 3. How many shared and unshared electrons? 4. When it becomes an ion, it loses 3 electrons, cross out the 3.

48. Ionization Energy Graph

49. Test