1. Electron Arrangement What do we know?

2. Electron Arrangement What do we know? e- are in the e- cloud

3. Electron Arrangement What do we know? e- are in the e- cloud e- are responsible for the volume of the atom

4. Bohr Model

5. e- move certain distances from the nucleus

6. Bohr Model e- move certain distances from the nucleus – close to nucleus have less E – E increases as e- move away from nucleus

7. e- move with certain speeds due to E

8. – give off E only when they move to a lower E level

9. e- move with certain speeds due to E – give off E only when they move to a lower E level outer most e- are called valence e- and have the most E

10. e- move with certain speeds due to E – give off E only when they move to a lower E level outer most e- are called valence e- and have the most E – valence e- determine behavior of atoms and are involved in bonding

11. Energy state of an e- is described by a set of 4 numbers called quantum numbers

12. Energy state of an e- is described by a set of 4 numbers called quantum numbers QN - describe the most probable location of e- in terms of:

13. Energy state of an e- is described by a set of 4 numbers called quantum numbers QN - describe the most probable location of e- in terms of: 1.distance from the nucleus

14. Energy state of an e- is described by a set of 4 numbers called quantum numbers QN - describe the most probable location of e- in terms of: 1.distance from the nucleus 2.shape of the orbital

15. Energy state of an e- is described by a set of 4 numbers called quantum numbers QN - describe the most probable location of e- in terms of: 1.distance from the nucleus 2.shape of the orbital 3.position of orbital in 3 axis of space

16. Energy state of an e- is described by a set of 4 numbers called quantum numbers QN - describe the most probable location of e- in terms of: 1.distance from the nucleus 2.shape of the orbital 3.position of orbital in 3 axis of space 4.direction of spin of e-

17. I. Principal Quantum Number

18. distance indicates the most probable distance of an e- from the nucleus

19. I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e-

20. I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1 2 3 4 5 6 7

21. I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K 2L 3M 4N 5O 6P 7Q

22. I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K2 2L 3M 4N 5O 6P 7Q

23. I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K2 2L8 3M 4N 5O 6P 7Q

24. I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K2 2L8 3M18 4N 5O 6P 7Q

25. I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K2 2L8 3M18 4N32 5O 6P 7Q

26. I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K2 2L8 3M18 4N32 5O 6P… 7Q…

27. I. Principal Quantum Number can be determined from the period/series number on the periodic table

28. II. Orbital Quantum Number

29. indicates shape of the orbital cloud

30. II. Orbital Quantum Number indicates shape of the orbital cloud 4 orbital shapes, represented by letters

31. II. Orbital Quantum Number s lowest E p d f

32. II. Orbital Quantum Number s lowest E p d f highest E

33. II. Orbital Quantum Number max # e- s 2 p 6 d10 f 14

34. II. Orbital Quantum Number # of orbital shapes is = to the principal QN

35. Principal QN # orbital shapes types of orbitals 1 2 3 4

36. Principal QN # orbital shapes types of orbitals 11 2 3 4

37. Principal QN # orbital shapes types of orbitals 11 s 2 3 4

38. Principal QN # orbital shapes types of orbitals 11 s 22 33 44

39. Principal QN # orbital shapes types of orbitals 11 s 22 s, p 33 44

40. Principal QN # orbital shapes types of orbitals 11 s 22 s, p 33 s, p, d 44

41. Principal QN # orbital shapes types of orbitals 11 s 22 s, p 33 s, p, d 44 s, p, d, f

42. III. Magnetic Quantum Number

43. describes the orbital positions with respect to the 3 axis of space

44. III. Magnetic Quantum Number

45. describes the orbital positions with respect to the 3 axis of space each position, regardless of type can only hold a maximum of 2 e- describes the orbital positions with respect to the 3 axis of space each position, regardless of type can only hold a maximum of 2 e-

46. s orbital/sublevel

47. 1 orbital position for “s”

48. s orbital/sublevel 1 orbital position for “s” spherical shape

49. s orbital/sublevel 1 orbital position for “s” spherical shape lowest possible energy sub-level

50. s orbital/sublevel 1 orbital position for “s” spherical shape lowest possible energy sub-level all energy levels have an s orbital 1s, 2s, 3s, 4s…

51. p orbital/sublevel

52. second energy sublevel… more E

53. p orbital/sublevel second energy sublevel… more E 3 possible “p” orbitals per E Level

54. p orbital/sublevel second energy sublevel… more E 3 possible “p” orbitals per E Level 6 total e- possible in “p” sub-group

55. p orbital/sublevel second energy sublevel… more E 3 possible “p” orbitals per E Level 6 total e- possible in “p” sub-group 2p, 3p, 4p, 5p…

56. d orbital/sublevel

57. 5 possible “d” orbitals per E Level

58. d orbital/sublevel 5 possible “d” orbitals per E Level 10 total e- possible in “d” sub-group

59. d orbital/sublevel 5 possible “d” orbitals per E Level 10 total e- possible in “d” sub-group 3d, 4d, 5d…

60. f orbital/ sublevel

61. 7 possible “f” orbitals per E Level

62. f orbital/sublevel 7 possible “f” orbitals per E Level 14 total e- possible in “f” sub-group

63. f orbital/sublevel 7 possible “f” orbitals per E Level 14 total e- possible in “f” sub-group 4f, 5f

64. Quantum number summary OrbitalsPositionselectrons

65. Magnetic Quantum Number Summary

66. ADD ADD these to your e- in Atoms Questions 13) What is the Octet rule? 14) Describe what happens to e- when atoms absorb energy? 15) How does quantum mechanics differ from classical mechanics?

67. Orbital Filling Chart

68. Order for filling orbitals 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d... Aufbau Principle – e- occupy orbitals of lowest E 1 st * 4s is lower E than 3d

69. Orbital filling chart

70. 1s 2s2p 3s3p3d 4s4p4d4f 5s5p5d5f 6s6p6d6f …

71. Order for filling orbitals 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d...

72. e- configuration

73. Quantum Number Rewind

75. Orbital Filling Chart

76. e- configuration

78. Write the e- configuration for the following: 1.beryllium 2.carbon 3.sodium 4.magnesium 5.aluminum 6.potassium **EC: bromine

79. Quantum Numbers

80. Principle

81. [E level] (n)

82. Principle [E level] (n) Orbital

83. Principle [E level] (n) Orbital [shape] (l)

84. Principle [E level] (n) Orbital [shape] (l) Magnetic

85. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] (m)

86. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital

87. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 )

88. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 )

89. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 2 3 4

90. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 2 3 4

91. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 1 2 3 4

92. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e- 2 3 4

93. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-1 2 3 4

94. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 3 4

95. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 3 4

96. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s p 3 4

97. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 p 3 4

98. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 p 3 3 4

99. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 p 36e- 3 4

100. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 4 p 36e- 3 4

101. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 4

102. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 4

103. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s p 4

104. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s p d 4

105. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- p d 4

106. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- p 36e- d 4

107. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- p 36e- d 510e- 4

108. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 9 p 36e- d 510e- 4

109. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4

110. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s p d

111. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s p d f

112. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e- p d f

113. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e- p 36e- d f

114. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e- p 36e- d 510e- f

115. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e- p 36e- d 510e- f 714e-

116. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e- 16 p 36e- d 510e- f 714e-

117. Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e- 1632 p 36e- d 510e- f 714e-

120. Write the e- configuration for the following: 1.beryllium 2.carbon 3.sodium 4.magnesium 5.aluminum 6.potassium **EC: bromine

122. e- configuration 1.Oxygen 2.fluorine 3.Silicon 4.Copper 5.Arsenic EC: krypton

126. IV. Spin Quantum Number

127. indicates the spin of e- (clockwise & counterclockwise)

128. IV. Spin Quantum Number indicates the spin of e- (clockwise & counterclockwise) Pauli Exclusion Principle – no more than 2 e- per orbital, which must be of opposite spin

129. Hund’s Rule – an e- can not enter a half filled orbital if an empty orbital of the same E is available

130. place 1 e- into each p, d or f orbital before pairing them Pauli Exclusion Principle – no more than 2 e- per orbital, which must be of opposite spin

131. Orbital Notation uses all 4 QN to represent e- arrangement

134. Orbital Notation Practice 1.Fluorine 2.Magnesium 3.Phosphorus 4.Argon 5.Manganese 6.Arsenic **EC: mercury

138. Write e- configuration and orbital diagrams for the following 1)Boron 2)Sulfur 3)Chlorine 4)Potassium 5)Cobalt 6)Copper 7)Iodine 8)barium

139. Pauli Exclusion Principle – no more than 2 e- per orbital, which must be of opposite spin -The 2 Electrons spin in different directions. -Notated as… ___ 1s Principle Energy Level and Orbital or “sub-level” [The 1 st 2 Quantum Numbers] Arrows = electrons