1. Chapter 7 Atomic Structure pp

3. Electromagnetic Radiation Mutually propagating electric and magnetic fields, at right angles to each other, traveling at the speed of light c

4. Parts of a wave Origin Wavelength Amplitude Crest Trough

6. Parts of a wave  Wavelength Frequency = number of cycles in one second Measured in hertz 1 hertz = 1 cycle/second

9. Frequency = 

10. Figure 7.1 The Nature of Waves

12. Radio waves Microwaves Infrared . Ultra-violet X-Rays Gamma Rays Long Wavelength Short Wavelength Visible Light Low energy High energy Low Frequency High Frequency

13. Electromagnetic Spectrum Which has longer  , ultraviolet or gamma rays? UV rays Which has shorter wavelength, microwave or infrared? Microwave

14. Figure 7.2 Classification of Electromagnetic Radiation

18. Tr 19 Fig 4.3 p. 93 Photoelectric Effect

24. Figure 7.4 Electromagnetic Radiation

29. A wave moves toward a slit.

30. Comes out as a curve

31. with two holes

32. with two holes Two Curves

33. Two Curves with two holes Interfere with each other

34. Two Curves with two holes Interfere with each other crests add up

35. Several waves

36. Several waves Several Curves

37. Several waves Several waves Interference Pattern Several Curves

41. Figure 7.6 A Continuous Spectrum (a) and A Hydrogen Line Spectrum (b)

43. Line emission spectra of H, Hg, and Ne

47. The Bohr Ring Atom n = 3 n = 4 n = 2 n = 1

57. Standing Waves - fixed or “quantized” wavelengths, d = n (  /2) nodes d = (1/2)  d =  d = (3/2) 

58. Figure 7.9 The Standing Waves Caused by the Vibration of a Guitar String Fastened at Both Ends. Each dot represents a node (a point of zero displacement).

60. Figure 7.10 The Hydrogen Electron Visualized as a Standing Wave Around the Nucleus Destructive interference occurs if orbit does not equal a complete wave. So only certain electron energies are allowed.

61. “ allowed” orbit = constructive interference “ forbidden” orbit = destructive interference Standing Waves Quantum Mechanics E. Schrödinger (1927)

67. Moving Electron Photon Before Electron Changes velocity Photon changes wavelength After

69. Heisenberg's Uncertainty Principle We can never SIMULTANEOUSLY know with absolute precision both the exact position (x), and momentum (mass X velocity or mv), of the electron. If one uncertainty gets very small, then the other becomes very large  x •  (mv) > h Uncertainty in momentum Uncertainty in position Planck’s constant

70. If an electron is moving at 1.0 X 10 8 m/s with an uncertainty in velocity of 0.10 %, then what is the uncertainty in position?  x •  (mv) > h and rearranging  x > h /  (mv) or since the mass is fixed  x > h / m  v  x > 7.3 X 10 -9 m or 7300 pm  x > (6.63 X 10 -34 Js) (9.11 X 10 -31 kg)(.001 X 1 X 10 8 m/s)

73. Probability Distance from nucleus

74. Sum of all Probabilities Distance from nucleus

76. We can construct atomic orbitals by drawing a boundary at the place where probability = 90%

83. S orbitals

84. "s" Atomic Orbitals 1s 2s 3s Orbitals are found in 3-D shells instead of 2-D Bohr orbits. The Bohr radius for n=1 was correct, however. + n = 1 n = 2 n = 3

86. P orbitals

87. "p" Atomic Orbitals “ p” orbitals only exist in the 2nd shell and higher (n = 2, 3, ...) + n = 1 n = 2 n = 3 3p x 3p y 3p z 2p x 2p y 2p z

89. P Orbitals

90. D orbitals

91. "d" Atomic Orbitals “ d” orbitals only exist for n = 3, 4, 5…. + n = 1 n = 2 n = 3 3d z 2 3d xz 3d yz 3d xy 3d x2-y2

92. Three F orbitals

93. Other four F orbitals

94. "f" Atomic Orbitals Do not appear until the 4th shell and higher

95. “ The Shell Game” (n = 1) n = 1 n = 2 n = 3 +

96. “ The Shell Game” n = 2 + n = 1 n = 2 n = 3

97. “ The Shell Game” n = 3 + n = 1 n = 2 n = 3

100. Go to application, Atom in a Box pp

103. Figure 7.19 A Picture of the Spinning Electron

107. +11P 11 electrons +11P 10 other electrons e - Z eff

110. Figure 7.18 Orbital Energy Levels for the Hydrogen Atom (degenerate)

111. Figure 7.18 Orbital Energy Levels for the H Atom (degenerate)

113. Increasing energy 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 3d 4d 5d 7p 6d 4f 5f

117. Mendeleev’s Early Periodic Table, Published in 1872 Note the spaces left for missing elements with atomic masses 44, 68, 72 and 100.

123. He with 2 electrons Increasing energy 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 3d 4d 5d 7p 6d 4f 5f

136. Tr23 Aufbau Principle What is the maximum electrons in each box? Two Which is a higher energy level, 4d or 5s? 4d Which is farther from the nucleus, 4d or 5s? 5s

141. The “Extended” Periodic Table pp

151. Remember our simplified atom +11 11 e- Z eff 1 e-

157. Graphically Penetration 2s Radial Probability Distance from nucleus

158. Graphically Radial Probability Distance from nucleus 3s

159. Radial Probability Distance from nucleus 3p

160. Radial Probability Distance from nucleus 3d

161. Radial Probability Distance from nucleus 4s 3d

164. Z eff 1 2 4 5 1

165. Z eff 1 2 4 5 1 If shielding is perfect Z= 1

166. Z eff 1 2 4 5 1 No shielding Z = Z eff

167. Z eff 1 2 4 5 16

171. Symbol First Second Third HHeLiBeBCNO F Ne 1312 2731 520 900 800 1086 1402 1314 1681 2080 5247 7297 1757 2430 2352 2857 3391 3375 3963 11810 14840 3569 4619 4577 5301 6045 6276

172. Symbol First Second Third HHeLiBeBCNO F Ne 1312 2731 520 900 800 1086 1402 1314 1681 2080 5247 7297 1757 2430 2352 2857 3391 3375 3963 11810 14840 3569 4619 4577 5301 6045 6276 Why such increase between the arrows? Special stability of noble gas configuration makes it harder to remove an inner shell electron

173. Summary of Noble Gas Configuration effects on IE

183. First Ionization energy Atomic number H He Li Be B C

184. First Ionization energy Atomic number H He Li Be B C N

186. First Ionization energy Atomic number H He Li Be B C N O F

189. First Ionization energy Atomic number

190. Tr22A Summary of the previous trends

191. Figure 7.31 The Values of First Ionization Energy for the Elements in the First Six Periods

192. Figure 7.32 Trends in Ionization Energies for the Representative Elements

196. Table 5.17 p. 147 Observe period and group trends

203. Tr 26 Fig. 5.13 p. 141 Atomic Radii Mg to Al size gets smaller because same level with more p + s Zn to Ga size jumps because of electron shielding from the d-electrons that makes the increasing nuclear charge less effective, so the electron cloud gets larger.

204. Overall Atomic Number Atomic Radius (nm) H Li Ne Ar 10 Na K Kr Rb

205. Tr21A Fig 5.14 p 142 Atomic Radius vs Atomic Number How does “effective” nuclear charge change left to right Increases Why is there a “peak” in Period 4? Inner 3d sublevel has filled & now in outer 4p sublevel Why is there a U-shape curve across Period 5? As add more 4d electrons, the shielding effect overcomes the effective nuclear charge.

206. Parts of the Periodic Table

214. Ionization energy, Electronegativity, Electron affinity INCREASE

215. Ionization energy, Electronegativity Electron affinity INCREASE

216. Atomic size increases, (shielding constant across a period) Ionic size increases

217. Atomic size increases, (shielding constant across a period) Ionic size increases