Entry Task: October 16 th -17 th Block 1

1. Entry Task: October 16th -17th Block 1 • Question: What is the shape of the p orbitals? How many electrons can a filled p orbital fill? • You have 5 minutes!

2. Agenda Sign off and discuss section 5-2 Notes on Electron configuration H.W. Section 5-3 ws

9. Break out periodic Table!!

10. s= 2 electrons 1s 1s p= 6 electrons 2p 2s 3p 3s d= 10 electrons 4s 4p 3d 4d 5p 5s 6s 6p 5d 7s 6d f= 14 electrons 4f 5f

11. I can… • Apply the rules to fill in an electron diagram • Write electron configuration for a given element.

12. Electron Configuration

13. How do electrons fill the atomic orbitals? There are rules when filling the atoms orbits with electrons.

14. #1 Aufbau Principle: each electron occupies the lowest energy orbital available. You fill in order of increasing energy. s  p d f Different sublevels have different energy levels. All orbitals in a sublevel have equal energy p > s 2px = 2py = 2pz

16. #2 Pauli Exclusion Principle • A maximum of 2 electrons are allowed in a single atomic orbital, but only if they have opposite spins!

17. #3 Hund’s Rule • Fill each sublevel (i.e. all p-orbitals) with single electrons with parallel spins first. Then come back to put 2nd electrons in. First: 2p Think of it as the school bus rule. Fill up the seats singly first then double.

18. Orbital Shapes

19. Aufbau Diagram s= 2 electrons p= 6 electrons d= 10 electrons f= 14 electrons

20. Order of filling electrons

21. Aufbau Diagram Hydrogen

22. Aufbau Diagram What rule applies here? Pauli Exclusion- 2 different spins Helium

23. Aufbau Diagram Lithium

24. Aufbau Diagram What rule applies here? Aufbau Principle- Fill lower energy levels first Beryllium

25. Aufbau Diagram Boron

26. Aufbau Diagram What rule applies here? Hund’s Rule Fill the sublevel first Carbon

27. Aufbau Diagram Nitrogen

28. Notations of Electron Configurations • Standard • Shorthand

29. Aufbau Diagram Fluorine 2p5 2s2 1s22s22p5 1s2

30. Standard Notation of Fluorine Number of electrons in the sub level 2,2,5 1s22s22p5 Main Energy Level Numbers 1, 2, 2 Sublevels

31. Shorthand Notation • Use the last noble gas that is located in the periodic table right before the element. • Write the symbol of the noble gas in brackets. • Write the remaining configuration after the brackets. • Ex: Fluorine: [He] 2s2 2p5

32. START with Hydrogen= put its Electron configuration in its square H 1s1

33. Helium= put its Electron configuration in its square He 1s2

34. Lithium= put its Electron configuration in its square Li 1s22s1

35. Keep Going- until you reach Neon

36. Neon= put its Electron configuration in its square Ne 1s22s22p6

37. Orbital occupancy for the first 10 elements, H through Ne.

38. Sodium= put its Electron configuration in its square- Noticed I put it into shorthand Na [Ne]3s1

42. Order of filling electrons

43. The relation between orbital filling and the periodic table

44. What’s wrong with this configuration? 1s22s22p63p63s2 Correct: 1s22s22p63s23p6 s orbitals are lower energy than p orbitals.

45. Aufbau Diagram 20 electron Chromium 24 Cr [Ar]4s13d5

46. Aufbau Diagram 20 electron Copper 29 Cu [Ar]4s13d10

47. Exceptions to the rules! Cr [Ar]4s13d5 Cu [Ar]4s13d10 WHY?These electron configurations are more stable for the elements!

48. http://www.chempractice.com/drills/java_AO.php Aufbau Diagram http://www.lon-capa.org/~mmp/period/electron.htm

49. Blocks in the Periodic Table