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lecture_12 - CHAPTER 4 Structure of the Atom 4.1 4.2 4.3...

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    4.1 The Atomic Models of Thomson and Rutherford 4.2 Rutherford Scattering 4.3 The Classic Atomic Model 4.4 The Bohr Model of the Hydrogen Atom 4.5 Successes and Failures of the Bohr Model 4.6 Characteristic X-Ray Spectra and Atomic Number 4.7 Atomic Excitation by Electrons CHAPTER 4 Structure of the Atom Structure of the Atom In the present first part of the paper the mechanism of the binding of electrons by a positive nucleus is discussed in relation to Planck’s theory. It will be shown that it is possible from the point of view taken to account in a simple way for the law of the line spectrum of hydrogen. - Niels Bohr, 1913
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    The Correspondence Principle From the previous theoretical value for a 0 we can now calculate a value for the Ryberg constant a 0 = e 2 8 πε 0 hcR H R H = 10 After Bohr had first obtained his solutions to the hydrogen atom problem, he looked to a more fundamental condition to define the permitted orbits, and found in the consideration of angular momentum L (=mvr). F = ma 1 4 0 e 2 r 2 = m v 2 r L 2 = ( mvr ) 2 = me 2 r 4 0 = me 2 n 2 4 0 a 0 = me 2 n 2 4 0 h 2 ε 0 π me 2 = n 2 h 2 4 2 L n = n h where h = h 2
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    The Hydrogen Atom The energies of the stationary states where E 0 = 13.6 eV. Emission of light occurs when the atom is in an excited state and decays to a lower energy state ( n u n l ). where f is the frequency of a photon. R is the Rydberg constant .
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  Transitions in the Hydrogen Atom Lyman series The atom will remain in the excited state for a short time before emitting a photon and returning to a lower stationary state. All hydrogen atoms exist in n = 1 (invisible). Balmer series
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lecture_12 - CHAPTER 4 Structure of the Atom 4.1 4.2 4.3...

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