Chem_215_week001_Summer_2011_final-emission

Chem_215_week001_Summer_2011_final-emission - The Bohr...

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The Bohr Model of the Hydrogen Atom Bohr used Planck’s and Einstein’s ideas about quantized energy and proposed three postulates: 1. The H atom has only certain allowable energy levels, which Bohr called stationary states . Each of these states is associated with a fixed circular orbit of the electron around the nucleus. 2. The atom does not radiate energy while in one of its stationary states. That is, even though it violates the ideas of classical physics, the atom does not change energy while the electron moves within an orbit. 3. The atom changes to another stationary state (the electron moves to another orbit) only by absorbing or emitting a photon whose energy equals the difference in energy between the two states: E photon = E state A - E state B = h ν
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Fig. 7-8, p.281 The Bohr Model; Energy States of the Hydrogen Atom
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Valid for one-electron species Z 2 n 2 E n = - 2.18 x 10 -18 J Better Scale
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Fig. 7-8, p.281 The Bohr Model; Energy States of the Hydrogen Atom Valid for one-electron species Z 2 n 2 E n = - 2.18 x 10 -18 J
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Fig. 7-8, p.281 Using the Bohr model to calculate ionization energy. Valid for one-electron species Z 2 n 2 E n = - 2.18 x 10 -18 J IE = E - E n IE = - E n
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Ionization Energy of Hydrogen Atom Valid for one-electron species Z 2 n 2 E = - 2.18 x 10 -18 J IE = E - E n IE = - E n
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This note was uploaded on 09/23/2011 for the course CHEM 215 taught by Professor Staff during the Spring '11 term at S.F. State.

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Chem_215_week001_Summer_2011_final-emission - The Bohr...

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