hw13a - MasteringPhysics: Assignment Print View Page 1 of...

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Manage this Assignment: 13a Early Quantum Theroy and the Atomic Model Due: 11:00pm on Sunday, April 11, 2010 Note: To understand how points are awarded, read your instructor's Grading Policy . Print Version with Answers The Bohr Atom Description: The problem applies quantization of angular momentum to the classical model of an electron orbiting a nucleus. Learning Goal: To understand the Bohr model of the hydrogen atom. In 1913 Niels Bohr formulated a method of calculating the different energy levels of the hydrogen atom. He did this by combining both classical and quantum ideas. In this problem, we go through the steps needed to understand the Bohr model of the atom. Part A Consider an electron with charge and mass orbiting in a circle around a hydrogen nucleus (a single proton) with charge . In the classical model, the electron orbits around the nucleus, being held in orbit by the electromagnetic interaction between itself and the protons in the nucleus, much like planets orbit around the sun, being held in orbit by their gravitational interaction. When the electron is in a circular orbit, it must meet the condition for circular motion: The magnitude of the net force toward the center, , is equal to . Given these two pieces of information, deduce the velocity of the electron as it orbits around the nucleus. Express your answer in terms of , , , and , the permittivity of free space. Hint A.1 Electrostatic force Recall that the force between two charged particles is , where and are the charges on the particles, is the separation of the particles, and is the permittivity of free space. This is the force that keeps the electron in a circular orbit, so . ANSWER: = Part B The key insight that Bohr introduced to his model of the atom was that the angular momentum of the electron orbiting the nucleus was quantized. He introduced the postulate that the angular momentum could only come in quantities of , where is Planck's constant and is a nonnegative integer ( ). Given this postulate, what are the allowable values for the velocity of the electron in the Bohr atom? Recall that, in circular motion, angular momentum is given by the formula . Page 1 of 10 MasteringPhysics: Assignment Print View 1/16/2010 http://session.masteringphysics.com/myct/assignmentPrint?assignmentID=1333221
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As the electron orbits the nucleus with a speed at a radius , it has both kinetic energy and electric potential energy. The total energy of the electron can be expressed as . Express your answer in terms of , Planck's constant , , and . ANSWER: = Part C In Parts A and B you found two different expressions to describe the allowed electron velocities . Equate these two values (eliminating ) and solve for the allowable radii in the Bohr model. Express in terms of , , , , and . ANSWER: = Part D In Parts B and C you saw that, according to Bohr's postulate, the electron radius and the electron velocity only have certain allowable values. Plug the values obtained for these two quantities into the energy statement given above to arrive at a new statement for the allowed energy levels in the Bohr atom.
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This note was uploaded on 09/26/2011 for the course PHYSICS 106 taught by Professor Arubi during the Summer '11 term at UCLA.

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hw13a - MasteringPhysics: Assignment Print View Page 1 of...

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