1. ‘sup? Are you sciencing hard or hardly sciencing? You need: The meaty packet up in the back Your periodic table A fez

3. Stuff and things… Project… Tests back tomorrow or Friday

4. LOOK AT THIS AMAZING THING!

5. LOOK AT IT!

7. Green = solid at room temperature Yellow = gas Blue = liquid

10. Columns: Groups or Families Rows: Periods

11. Periodic Table: Columns = groups or “families” –Elements in the same group share the same characteristics. 18 of them. Rows = periods –Seven of them. The row an element is in corresponds to the energy levels its electrons are arranged on, generally speaking.

12. Bohr Models… How? What do they show?

13. Make Some…

14. Valence Electrons The outermost electrons of an atom How do you know what they are? Figuring our Valence Electrons – “1, 2, skip a few…3, 4, 5, 6, 7, 8.” Everyone wants to have or feel like they have eight valence electrons. This is called the Octet Rule. (Octet = 8)

15. The dots…only show valence electronsThe dots…only show valence electrons Start with a pair on the right, then singles, and then pair them.Start with a pair on the right, then singles, and then pair them.

20. Stuff and things… Project…need to know product by September 18 th (next Friday) Tests back… Test makeups – today after school. Test corrections. Must be done by next Friday. Only corrections on the multiple choice for half the credit back.

21. Remember this?

22. A lie from the pit of hell.

23. And this?

24. Nicer, but still… A lie from the pit of hell.

25. It’s more like this…

26. It’s about the orbitals… s, p, d, and f. Each orbital can hold 2 electrons. s and p – easiest to handle… –H –He What if you’re Be?

27. It’s about the orbitals… What if you’re Be? Where are your electrons? 2 of your electrons are in the 1s orbital 2 of them are in the 2 s orbital Four electrons

28. What if you’re Carbon, though? O.M.G. How many electrons? http://www.youtube.com/watch?v=VfBcfYR1VQo

29. What if you’re Carbon, though? 2 electrons in 1s 2 electrons in 2s 2 electrons in 2p

30. Noticing something? Valence electrons = the outermost s and p electrons of an atom. –An atom can have a maximum of 2 s electrons and a maximum of 6 p electrons, so the maximum number of valence electrons anyone can have is 8.

32. All about the energy…

33. Get your configuration handout ready

34. Stuff and things… Project…need to know product by September 18 th (next Friday) Tests back… Test makeups – today after school. Test corrections. Must be done by next Friday. Only corrections on the multiple choice for half the credit back.

35. So – as a result, then…

36. While we’re on rules… Hund’s rule: Each p, d, or f orbital must receive one electron before it can get its second. (everybody gets an electron before anyone gets seconds) if two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs. Go back in your head to Lewis Dot models... Where were your first two dots? And then what did you do?

37. d and f orbitals – funky, funky.

38. Steps to constructing electron configurations Determine the number of e- in the element. Begin with 1s and follow the arrows for the order of filling energy levels with e-. (Remember that regardless of energy level, the sublevel can only hold a certain number of e-.) Keep a running tally of distributed e-.

40. Example: Sodium (Na) has 11 electrons 1s 2 2s 2 2p 6 3s 1 Example: Gallium (Ga) has 31 electrons 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 1 This method is called long-hand e- configuration

41. Short-Hand e- Configuration Examples: Magnesium (Mg) Previous noble gas  Neon (Ne) Difference in e-  2 e- Answer  [Ne] 3s 2 Holmium (Ho) Previous noble gas  Xe Difference in e-  13 e- Answer  [Xe] 4f 11 6s 2

42. Or – electron filling… To do that, we need to think of the individual electrons in their respective orbits. For example – this is oxygen

43. Practice time…

44. Follow the pattern on your diagonal diagram

45. Stuff and things… Project…need to know product by September 18 th (Friday) Test corrections. Must be done by Friday. Let me know when you’re planning to be here.

46. Smidge of Extra Credit on Unit 2 test: Color the electron “blocks” of the periodic table (s, p, d, f) Cut the periodic table up, and insert the f block where it belongs (look at the numbers!) Tape it together, put it on a larger piece of paper if you want, and turn it in by Tuesday, September 15th

47. Today: Electron Configuration “Lab” –Use full sentences to answer Conclusions E-config quiz Both are due tomorrow, at the start of class.

49. Get ready for:

50. Electrons. Remember?

51. Friggin’ electrons

53. Reviewing – placing electrons..

54. If this is you…. Why? Electron configuration is knocking at the door of quantum mechanics, and without an understanding of quantum mechanics – yeah, even down to the level of where the electrons of atoms are and what they do in stuff, the modern world Does. Not. Exist. This stuff – this s, p, d, and f stuff - is the ground level of making better computers, making lasers better, making better, cheaper cell phones, and tons more, but basically, making a better world. The knowledge of quantum mechanics has literally reshaped the world. Everything that isn’t rocks and sticks tied together concerns quantum mechanics in one way or another. Want in? Don’t be scared. The future is waiting.

55. Today: Periodic Table: Fill in s, p, d and f blocks. Number them as well. You need four colored pencils. Complete the sets of elements on the last page. Complete the Electron Configuration Practice worksheet. Quantum Numbers Practice.

56. Steps to constructing e- configurations Determine the number of e- in the element. Begin with 1s and follow the arrows for the order of filling energy levels with e-. (Remember that regardless of energy level, the sublevel can only hold a certain number of e-.) Keep a running tally of distributed e-.

57. Follow the pattern on your diagonal diagram

59. Turn in your notebooks, quizzes and extra credit.

60. Stuff and things… Project…need to know product by September 18 th (Friday) Test corrections. Must be done by Friday. Let me know when you’re planning to be here.

61. How do you know where people live?

62. Electron filling model

63. Quantum Numbers Electrons’ addresses – four numbers.

64. Every Electron has its own set of 4 unique Quantum Numbers : 1. n = Principal Quantum Number (1-7)  Represents the energy level – if n = 1, 1 st energy level  2n 2 – determines maximum number of electrons that can occupy an energy level 2. ‘ l ’ = orbital or sublevel (1-3) Refers to different energy states in each energy level – orbitals (s=0, p=1, d=2, f=3)

65. 3. m = orbital (m = -‘ l’ to ‘ l ’)  Space occupied by a pair of electrons  s = 1 orbital (0)  p = 3 orbitals (-1,0,1)  d = 5 orbitals (-2, -1, 0, 1, 2)  f = 7 orbitals (-3, -2, -1, 0, 1, 2, 3) 4. s = spin  in order for 2 electrons to occupy the same orbital, they must have opposite spins, up and down. +1/2 goes first. Each arrow represents an electron (+ ½, -½)

66. Rules for placing electrons in orbitals Aufbau Principal –Electrons occupy orbitals of lowest energy first and fully before moving to higher energy levels Hund’s Rule –Within a sublevel, orbitals are half-filled with electrons (one) before they become filled (two) Pauli’s Exclusion Principle - States that no two e- in an atom can have the same set of 4 quantum numbers

67. Now: Quantum Numbers Practice! –Remember: all four numbers give the address of a specific electron in an atom. n = energy level l = orbital type (s, p, d, f) m = orbital orientation (-l to l) s = spin (+1/2 or -1/2)

68. Aluminum’s electrons? Long hand?

69. Aluminum’s electrons? Long hand: 1s 2 2s 2 2p 6 3s 2 3p 1 Electron filling?

70. Aluminum’s electrons? Electron filling? Quantum numbers of this electron?

71. Aluminum’s electrons? Quantum numbers of this electron: n = 3 (it’s in 3p)

72. Aluminum’s electrons? Quantum numbers of this electron: n = 3 (it’s in 3p) l = 1 (it’s a p orbital)

73. Aluminum’s electrons? Quantum numbers of this electron: n = 3 (it’s in 3p) l = 1 (it’s a p orbital) m = -1 (it’s the first p orbital, so it’s the p x orbital)

74. Aluminum’s electrons? Quantum numbers of this electron: n = 3 (it’s in 3p) l = 1 (it’s a p orbital) m = -1 (it’s the first p orbital, so it’s the p x orbital) s = +1/2 (first electron is +1/2 by convention)

75. Aluminum’s electrons? Quantum numbers of this electron: n = 3 l = 1 m = -1 s = +1/2 those 4 numbers are SPECIFIC for that SINGLE electron.

76. You try: Calcium’s 19 th electron

77. Calcium…it’s 19 th electron. –Remember: all four numbers give the address of a specific electron in an atom. n = energy level l = orbital type (s, p, d, f) m = orbital orientation (-l to l) s = spin (+1/2 or -1/2)

78. Calcium…it’s 19 th electron. –Remember: all four numbers give the address of a specific electron in an atom. n = energy level = 4 l = orbital type (s, p, d, f) m = orbital orientation (-l to l) s = spin (+1/2 or -1/2)

79. Calcium…it’s 19 th electron. –Remember: all four numbers give the address of a specific electron in an atom. n = energy level = 4 l = orbital type (s, p, d, f) = 0 m = orbital orientation (-l to l) s = spin (+1/2 or -1/2)

80. Calcium…it’s 19 th electron. –Remember: all four numbers give the address of a specific electron in an atom. n = energy level = 4 l = orbital type (s, p, d, f) = 0 m = orbital orientation (-l to l) = 0 s = spin (+1/2 or -1/2)

81. Calcium…it’s 19 th electron. –Remember: all four numbers give the address of a specific electron in an atom. n = energy level = 4 l = orbital type (s, p, d, f) = 0 m = orbital orientation (-l to l) = 0 s = spin (+1/2 or -1/2) = +1/2

82. The Following is Just Beautiful… The quantum theory of the atom agrees completely with the periodic table, which had been around for 30+ years by the time quantum theory came along and was developed without any knowledge of electron arrangements…. Wait for it…

83. Relationship between the first two quantum numbers and the periodic table:

84. So….last things… States: Ground state: Every electron is where you expect Excited: An electron is somewhere “higher” than it should be, leaving a lower energy level (temporarily) unfilled.

85. Carbon:

86. The Power of What You Now Know Charges of ions can be explained e.g. leadPb: 6s 2 4f 14 5d 10 6p 2 Pb 2+ ion: remove two electrons from 6p Pb 4+ ion: remove two electrons from 6p and two electrons from 6s Magnetism is explained (wtf?)