Chapter 9: Electrons in Atoms

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1 General Chemistry Principles and Modern Applications Petrucci Harwood Herring 8 th Edition Chapter 9: Electrons in Atoms Philip Dutton University of Windsor, Canada N9B 3P4 Prentice-Hall 2002 Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 1 of 49

2 Contents 9-1 Electromagnetic Radiation 9-2 Atomic Spectra 9-3 Quantum Theory 9-4 The Bohr Atom 9-5 Two Ideas Leading to a New Quantum Mechanics 9-6 Wave Mechanics 9-7 Quantum Numbers and Electron Orbitals Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 2 of 49

3 Contents 9-8 Quantum Numbers 9-9 Interpreting and Representing Orbitals of the Hydrogen Atom 9-9 Electron Spin 9-10 Multi-electron Atoms 9-11 Electron Configurations 9-12 Electron Configurations and the Periodic Table Focus on Helium-Neon Lasers Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 3 of 49

4 9-1 Electromagnetic Radiation Electric and magnetic fields propagate as waves through empty space or through a medium. A wave transmits energy. Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 4 of 49

5 EM Radiation Low ν High ν Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 5 of 49

6 Frequency, Wavelength and Velocity Frequency (ν) in Hertz Hz or s -1. Wavelength (ë) in meters m. cm µm nm D pm (10-2 m) (10-6 m) (10-9 m) (10-10 m) (10-12 m) Velocity (c) H 10 8 m s -1. c = ëν ë = c/ν ν= c/ë Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 6 of 49

7 Electromagnetic Spectrum Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 7 of 49

8 ROYGBIV Red Orange Yellow 700 nm 450 nm Green Blue Indigo Violet Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 8 of 49

9 Constructive and Destructive Interference Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 9 of 49

10 Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 10 of 49

11 Refraction of Light Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 11 of 49

12 9-2 Atomic Spectra Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 12 of 49

13 Atomic Spectra Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 13 of 49

14 9-3 Quantum Theory Blackbody Radiation: Max Planck, 1900: Energy, like matter, is discontinuous. º = hν Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 14 of 49

15 The Photoelectric Effect Light striking the surface of certain metals causes ejection of electrons. ν > ν o e - % I e k % ν threshold frequency Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 15 of 49

16 The Photoelectric Effect Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 16 of 49

17 The Photoelectric Effect At the stopping voltage the kinetic energy of the ejected electron has been converted to potential. 1 2 mu 2 = ev s At frequencies greater than ν o : V s = k (ν - ν o ) Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 17 of 49

18 The Photoelectric Effect E k = ev s E o = hν o ν o = ev o h ev o, and therefore ν o, are characteristic of the metal. Conservation of energy requires that: E photon = E k + E binding E k = E photon - E binding hν = 1 2 ev s = 2 1 mu 2 + ev o mu 2 = hν - ev o Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 18 of 49

19 9-4 The Bohr Atom E = -R H n 2 R H = H J Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 19 of 49

20 Energy-Level Diagram ÄE = E f E i = -R H n f 2 -R H n i 2 1 = R H ( ni 2 1 n f 2 ) = hν = hc/ë Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 20 of 49

21 Ionization Energy of Hydrogen 1 ÄE = R H ( ni 2 1 n f 2 ) = hν As n f goes to infinity for hydrogen starting in the ground state: 1 hν = R H ( ni 2 ) = RH This also works for hydrogen-like species such as He + and Li 2+. hν = -Z 2 R H Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 21 of 49

22 Emission and Absorption Spectroscopy Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 22 of 49

23 9-5 Two Ideas Leading to a New Quantum Mechanics Wave-Particle Duality. Einstein suggested particle-like properties of light could explain the photoelectric effect. But diffraction patterns suggest photons are wave-like. debroglie, 1924 Small particles of matter may at times display wavelike properties. Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 23 of 49

24 debroglie and Matter Waves E = mc 2 hν = mc 2 hν/c = mc = p p = h/ë ë = h/p = h/mu Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 24 of 49

25 X-Ray Diffraction Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 25 of 49

26 The Uncertainty Principle Werner Heisenberg Äx Äp h 4ð Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 26 of 49

27 Standing waves. 9-6 Wave Mechanics Nodes do not undergo displacement. 2L ë =, n = 1, 2, 3 n Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 27 of 49

28 Wave Functions ø, psi, the wave function. Should correspond to a standing wave within the boundary of the system being described. Particle in a box. ø = 2 L sin nπ L x Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 28 of 49

29 Probability of Finding an Electron Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 29 of 49

30 Wave Functions for Hydrogen Schrödinger, 1927 Eø = H ø H (x,y,z) or H (r,è,ö) ø(r,è,ö) = R(r) Y(è,ö) R(r) is the radial wave function. Y(è,ö) is the angular wave function. Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 30 of 49

31 Principle Shells and Subshells Principle electronic shell, n = 1, 2, 3 Angular momentum quantum number, l = 0, 1, 2 (n-1) l = 1, s l = 2, p l = 3, d l = 4, f Magnetic quantum number, m l = 0, 1, 2 (±l ) Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 31 of 49

32 Orbital Energies Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 32 of 49

33 9-8 Interpreting and Representing the Orbitals of the Hydrogen Atom. Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 33 of 49

34 s orbitals Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 34 of 49

35 p Orbitals Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 35 of 49

36 p Orbitals Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 36 of 49

37 d Orbitals Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 37 of 49

38 9-9 Electron Spin: A Fourth Quantum Number Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 38 of 49

39 9-10 Multi-electron Atoms Schrödinger equation was for only one e -. Electron-electron repulsion in multielectron atoms. Hydrogen-like orbitals (by approximation). Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 39 of 49

40 Penetration and Shielding Z eff is the effective nuclear charge. Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 40 of 49

41 9-11 Electron Configurations Aufbau process. Build up and minimize energy. Pauli exclusion principle. No two electrons can have all four quantum numbers alike. Hund s rule. Degenerate orbitals are occupied singly first. Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 41 of 49

42 Orbital Energies Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 42 of 49

43 Orbital Filling Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 43 of 49

44 Aufbau Process and Hunds Rule Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 44 of 49

45 Filling p Orbitals Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 45 of 49

46 Filling the d Orbitals Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 46 of 49

47 Electon Configurations of Some Groups of Elements Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 47 of 49

48 9-12 Electron Configurations and the Periodic Table Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 48 of 49

49 Focus on He-Ne Lasers Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 49 of 49

50 Chapter 9 Questions Prentice-Hall 2002 General Chemistry: Chapter 9 Slide 50 of 49

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