2. Alkali Metals Alkali metals are very reactive – even with water! Sodium + Water  EXPLOSION!EXPLOSION

3. Alkaline Earth Metals  Alkaline Earth metals are also very reactive  Shiny solids that are harder than Alkali metals  Alkaline Earth Metal Spotlight: CALCIUM  Calcium is essential for human life, especially in maintaining bones and teeth  Found widely in nature combined with oxygen  Abrasives in toothpaste and emery boards  Magnesium Demo!

4. Boron’s Group  Gallium is a silver metal that literally melts in your hand! Don’t try this yourself!

5. Carbon’s Group  Carbon is one of the most important elements on Earth!  There is a whole branch of chemistry dedicated to studying carbon – ORGANIC CHEMISTRY!  If you are a science major in college, you will most likely take Organic  Silicon is the second most abundant element on Earth!  Use in computer chips and solar cells  Found in quartz, sand, and glass

6. Nitrogen’s Group  Metals, nonmetals, and metalloids!  Nitrogen, which you breathe, can form some of the most explosive compounds known to man  Arsenic is a toxic substance that was used to treat some illnesses back in the day  Bismuth is used in fire sprinklers

7. Oxygen’s Group  Oxygen  We must breathe oxygen to survive…so it’s pretty important  Reacts with some of the noble gases  Sulfur  Hydrogen sulfide smells like rotten egg  Selenium  Used in solar panels because it can convert light into energy

8.  Fluorine (really fluoride) is added to toothpaste  Chlorine gas is a deathly green gas that was first used as a form of chemical WARFARE in WWII Halogens (Fluorine’s Group)

9. Noble Gases (Helium’s Group)  Noble gases do not react with other elements very often – they are already “happy”  They can be called “inert” because they don’t react  Neon is used in neon lights  Helium Voice! Helium Voice

10. Transition Metals  Conduct electricity  Can form different ions (We’ll learn more about ions later!)  Many found in nature – found all over the world (map on page 200)  Uses  Found in alloys, wires, plastics, etc.  Your body needs trace (small) amounts many of them

11. Catalyst – October, 2.009 x 10 3 Put COMPLETED Homework on desk so I can stamp it.  Draw the Bohr model for Aluminum.  Draw the Bohr model for Boron.  What similarities do these two elements have?

12. Today’s Agenda  Catalyst  Go over Homework  Modern Atom Review  Electron Configuration Part 1  Practice, Practice, Practice  Progress Reports  Exit Question

13. Today’s Objectives  SWBAT compare and contrast the Bohr model with the “Modern Atom.”  SWBAT write electron configurations for elements. GUIDED NOTES TODAY!

14. Do we really know where electrons hang out? Key Point #1: The Heisenberg Uncertainty Principle tells us that there are limits to how much we can really know about electrons  Electrons are super tiny and they move very fast!  Can we really know where they are?

15. Heisenberg Uncertainty Principle But! We can make a pretty good guess! Book DefinitionOur Definition The Heisenberg Uncertainty Principle states that it is fundamentally impossible to know precisely both the velocity and the position of a particle at the same time. The Heisenberg Uncertainty Principle tells us that it is impossible to know where an electron is in an atom.

16. How? Schrödinger Equation Key Point #2: The Schrödinger Equation predicts the location of an electron in an atom.  It tells us that electrons hang out in atomic orbitals.

17. Schrödinger Equation and Atomic Orbitals Key Point #3: There are 4 atomic orbitals… s p d f

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

19. The s Orbital – Write notes! One s orbital in each energy level The s orbital is shaped like a sphere

20. The p Orbital – Write notes! Three p orbitals in each energy level (starting in the 2nd energy level!) Shape looks like dumbells or bowties

21. p and s Orbitals Side by Side

22. The d orbital – Write notes! Five d orbitals Start in the 3rd energy level! Shape looks like eggs or flowers

23. The f orbital – Write notes!  Seven f orbitals - start in 4th energy level

24. Quick Review Questions Answer in your notes 1. What are the four atomic orbitals? 2. Draw the s and p orbitals and describe the shape of each. 3. List 2 similarities between the Bohr model and the “Modern Atom.” 4. List 2 differences between the Bohr model and the “Modern Atom.”

25. Electron Configuration  Review: Where do electrons hang out?  Now, we have to know how many electrons can fit into each atomic orbital  Think of each energy level as a type of house  Some houses are big, some small  Some houses have more bedrooms than others

26. Electron Configuration (First Energy Level)  Each orbital (bedroom) can hold two electrons  Review: How many orbitals are on the first energy level?  Good, just one! This is an s orbital!  One bedroom = up to 2 electrons = electron

27. Electron Configuration (Second Energy Level)  Review: Which orbitals are on the second energy level?  Good! s and p  Review: How many p orbitals are there?  Good! Three p orbitals

28. Electron Configuration (Second Energy Level) So….how many electrons could shack up on the second energy level? = electron Eight electrons!

29. Electron Configuration (Third energy level and beyond)  Review: How many d orbitals are there?  Good, five d orbitals! So….how many electrons could shack up in d orbitals? = electron Good! Ten electrons!

30. Electron Configuration (Fourth Energy Level and Beyond)  Review: How many f orbitals are there?  Good! Seven f orbitals So….how many electrons could shack up in f orbitals? = electron Good! Fourteen electrons!

31. 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…

32. Electron Configuration  Key Point #4: Electron configuration helps show 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 Large number = energy level Letter = orbital Small number = Number of electrons

33. Bohr Models and Electron Configuration  Draw the Bohr Models for Hydrogen, Helium, and Lithium on your notes sheet  Then, we’ll write the electron configuration

34. Now, figure it out yourself!!  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 - ?

35. Systematic Way 6s

36. Electron Configuration N – 1s 2 6s

37. Electron Configuration N – 1s 2 2s 2 6s

38. Electron Configuration N – 1s 2 2s 2 2p 3 6s

39. Electron Configuration N – 1s 2 2s 2 2p 3 = 7 e- 6s

40. Electron Configuration Na – 1s 2 6s

41. Electron Configuration Na – 1s 2 2s 2 6s

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

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

44. Electron Configuration Sc – 1s 2 6s

45. Electron Configuration Sc – 1s 2 2s 2 6s

46. Electron Configuration Sc – 1s 2 2s 2 2p 6 6s

47. Electron Configuration Sc – 1s 2 2s 2 2p 6 3s 2 6s

48. Electron Configuration Sc – 1s 2 2s 2 2p 6 3s 2 3p 6 6s

49. Electron Configuration Sc – 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 6s

50. Electron Configuration Sc – 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 1 6s

51. Electron Configuration Sc – 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4s 1 6s = 21 e-

52. Electron Configuration Be: Ne: Br:

53. 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

54. Electron Configuration Backwards!  What elements are represented by the following electron configurations? 1. 1s 2 2s 2 2p 6 3s 2 3p 4 2. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 S Sr

55. Exit Question  Write the electron configuration for the following 2 elements. Also, indicate the number of valence electrons for each: 1. Manganese (Mn) 2. Fluorine (F)

56. Catalyst – October, 20.09 x 10 2 COMPLETED Homework on desk Use your notes/book to help if you need! Write the electron configuration for: 1. Argon (Ar) 2. Iron (Fe)  4s-3d trick!

57. Today’s Agenda  Catalyst  Go over Homework  Electron Configuration Practice  Noble Gas Configuration  Practice/Project Work Time  Exit Question

58. Today’s Objectives  SWBAT write long and noble gas configurations for elements in the periodic table.

59. Electron Configuration The Path to Your Dream Destination! 6s

60. Electron Configuration N – 6s N 1s 2

61. Electron Configuration N – 1s 2 6s N 2s 2

62. Electron Configuration N – 1s 2 2s 2 6s N 2p 3

63. Electron Configuration N – 1s 2 2s 2 2p 3 = 7 e- 6s N

64. Electron Configuration Na – 1s 2 6s

65. Electron Configuration Na – 1s 2 2s 2 6s

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

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

68. Electron Configuration Sc – 1s 2 6s

69. Electron Configuration Sc – 1s 2 2s 2 6s

70. Electron Configuration Sc – 1s 2 2s 2 2p 6 6s

71. Electron Configuration Sc – 1s 2 2s 2 2p 6 3s 2 6s

72. Electron Configuration Sc – 1s 2 2s 2 2p 6 3s 2 3p 6 6s

73. Electron Configuration Sc – 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 6s

74. Electron Configuration Sc – 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 1 6s

75. Electron Configuration Sc – 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4s 1 6s = 21 e-

76. Electron Configuration Be: Ne: Br:

77. 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

78. Electron Configuration Backwards!  What elements are represented by the following electron configurations? 1. 1s 2 2s 2 2p 6 3s 2 3p 4 2. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 S Sr

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

80. 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 5d 1 4f5 Si: Rb:

81. Electron Configuration Key Point #1: Noble Gas Configuration –Start writing your notation from the last noble gas BEFORE the atom you are going to.

82. Electron Configuration Ag

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

84. Electron Configuration Ca

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

86. Electron Configuration S

87. S – [Ne]3s 2 3p 4

88. Project Work TIME!!!  Write electron configurations for the elements in your family  Draw Bohr models for your family

89. Exit Question  Write the noble gas configuration for: 1. Bromine 2. Copper 3. Sodium

90. 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)

91. 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)

92. 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)

93. 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)

94. Valence Electron Trends on the Periodic Table