College Physics
College Physics
11th Edition
ISBN: 9781305952300
Author: Raymond A. Serway, Chris Vuille
Publisher: Cengage Learning
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Chapter 28, Problem 12CQ
To determine

The list of some concepts of atom pictured by the Bohr Theory in which quantum mechanics altered the view

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The energy levels for a Bohr atom are shown below. Use this diagram to solve problems 7 and 8. 0 eV -2.5 eV -4.0 eV -7.0 eV -12.5 eV 7. What amount of energy is needed for an electron to jump from n = 1 to n = 4? 8. What is the wavelength of the photon needed to make this happen? Is it emission or absorption?
Be sure to answer all parts. Consider the following energy levels of a hypothetical atom: E4-2.51 × 10-19 J E3-5.01 10-19 J E2 -1.25 x 10-18 J E₁-1.85 × 10-18 J (a) What is the wavelength of the photon needed to excite an electron from E₁ to E4? x 10 (b) What is the energy (in joules) a photon must have in order to excite an electron from E₂ to E3? x 10 m x 10 J (c) When an electron drops from the E3 level to the E₁ level, the atom is said to undergo emission. Calculate the wavelength of the photon emitted in this process. m
What is an emission spectrum? Use the Bohr model to explain why the emission spectrum of the hydrogen atom consists of distinct lines at specific wavelengths.
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