General Chemistry. Contents. Chapter 9: Electrons in Atoms. Contents. 9-1 Electromagnetic Radiation. EM Radiation. Frequency, Wavelength and Velocity
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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 Contents 9-1 Electromagnetic Radiation 9- 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 00 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 1 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide of 50 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 9-1 Electron Configurations and the Periodic Table Focus on Helium-Neon Lasers 9-1 Electromagnetic Radiation Electric and magnetic fields propagate as waves through empty space or through a medium. A wave transmits energy. Prentice-Hall 00 General Chemistry: Chapter 9 Slide 3 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 4 of 50 EM Radiation Frequency, Wavelength and Velocity Low ν Frequency (ν) in Hertz Hz or s -1. Wavelength (λ) in meters m. cm µm nm D pm (10 - m) (10-6 m) (10-9 m) (10-10 m) (10-1 m) Velocity (c) H 10 8 ms -1. High ν c = λν λ = c/ν ν= c/λ Prentice-Hall 00 General Chemistry: Chapter 9 Slide 5 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 6 of 50
2 Electromagnetic Spectrum ROYGBIV Red Orange Yellow 700 nm 450 nm Green Blue Indigo Violet Prentice-Hall 00 General Chemistry: Chapter 9 Slide 7 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 8 of 50 Constructive and Destructive Interference Prentice-Hall 00 General Chemistry: Chapter 9 Slide 9 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 10 of 50 Refraction of Light 9- Atomic Spectra Prentice-Hall 00 General Chemistry: Chapter 9 Slide 11 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 1 of 50
3 Atomic Spectra 9-3 Quantum Theory Blackbody Radiation: Max Planck, 1900: Energy, like matter, is discontinuous. є = hν Prentice-Hall 00 General Chemistry: Chapter 9 Slide 13 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 14 of 50 The Photoelectric Effect 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 00 General Chemistry: Chapter 9 Slide 15 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 16 of 50 The Photoelectric Effect The Photoelectric Effect At the stopping voltage the kinetic energy of the ejected electron has been converted to potential. 1 mu = ev s At frequencies greater than ν o : V s = k (ν - ν o ) 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 ev s = 1 mu + ev o mu = hν -ev o Prentice-Hall 00 General Chemistry: Chapter 9 Slide 17 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 18 of 50
4 9-4 The Bohr Atom Energy-Level Diagram E = -R H n R H =.179 H J E = E f E i = -R H n f -R H n i 1 1 = R H ( ) = hν = hc/λ ni n f Prentice-Hall 00 General Chemistry: Chapter 9 Slide 19 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 0 of 50 Ionization Energy of Hydrogen Emission and Absorption Spectroscopy 1 1 E = R H ( ) = hν ni As n f goes to infinity for hydrogen starting in the ground state: n f 1 hν = R H ( ni ) = RH This also works for hydrogen-like species such as He + and Li +. hν = -Z R H Prentice-Hall 00 General Chemistry: Chapter 9 Slide 1 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide of 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, 194 Small particles of matter may at times display wavelike properties. debroglie and Matter Waves E = mc hν = mc hν/c = mc = p p = h/λ λ = h/p = h/mu Prentice-Hall 00 General Chemistry: Chapter 9 Slide 3 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 4 of 50
5 X-Ray Diffraction The Uncertainty Principle Werner Heisenberg x p h 4π Prentice-Hall 00 General Chemistry: Chapter 9 Slide 5 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 6 of Wave Mechanics Standing waves. Nodes do not undergo displacement. L λ =, n = 1,, 3 n Wave Functions ψ, psi, the wave function. Should correspond to a standing wave within the boundary of the system being described. Particle in a box. ψ = L nπ x sin L Prentice-Hall 00 General Chemistry: Chapter 9 Slide 7 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 8 of 50 Probability of Finding an Electron Wave Functions for Hydrogen Schrödinger, 197 Eψ = H ψ H(x,y,z) or H (r,θ,φ) ψ(r,θ,φ) = R(r) Y(θ,φ) R(r) is the radial wave function. Y(θ,φ) is the angular wave function. Prentice-Hall 00 General Chemistry: Chapter 9 Slide 9 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 30 of 50
6 Principle Shells and Subshells Orbital Energies Principle electronic shell, n = 1,, 3 Angular momentum quantum number, l = 0, 1, (n-1) l = 0, s l = 1, p l =, d l = 3, f Magnetic quantum number, m l = - l -, -1, 0, 1, +l Prentice-Hall 00 General Chemistry: Chapter 9 Slide 31 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 3 of Interpreting and Representing the Orbitals of the Hydrogen Atom. s orbitals Prentice-Hall 00 General Chemistry: Chapter 9 Slide 33 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 34 of 50 p Orbitals p Orbitals Prentice-Hall 00 General Chemistry: Chapter 9 Slide 35 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 36 of 50
7 d Orbitals 9-9 Electron Spin: A Fourth Quantum Number Prentice-Hall 00 General Chemistry: Chapter 9 Slide 37 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 38 of Multi-electron Atoms Penetration and Shielding Schrödinger equation was for only one e -. Electron-electron repulsion in multielectron atoms. Hydrogen-like orbitals (by approximation). Z eff is the effective nuclear charge. Prentice-Hall 00 General Chemistry: Chapter 9 Slide 39 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 40 of Electron Configurations Orbital Energies 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 00 General Chemistry: Chapter 9 Slide 41 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 4 of 50
8 Orbital Filling Aufbau Process and Hunds Rule Prentice-Hall 00 General Chemistry: Chapter 9 Slide 43 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 44 of 50 Filling p Orbitals Filling the d Orbitals Prentice-Hall 00 General Chemistry: Chapter 9 Slide 45 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 46 of 50 Electon Configurations of Some Groups of Elements 9-1 Electron Configurations and the Periodic Table Prentice-Hall 00 General Chemistry: Chapter 9 Slide 47 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 48 of 50
9 Focus on He-Ne Lasers Chapter 9 Questions 1,, 3, 4, 1, 15, 17, 19,, 5, 34, 35, 41, 67, 69, 71, 83, 85, 93, 98 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 49 of 50 Prentice-Hall 00 General Chemistry: Chapter 9 Slide 50 of 50
Chapter 9: Electrons in Atoms
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
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