Lecture 151 - Wed. Oct. 8, 2003 Todays Lecture Quantum...

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Wed. Oct. 8, 2003 Today’s Lecture Quantum Mechanics and Atomic Theory • 12.4 The Bohr model • 12.5 The quantum mechanical description • 12.6 Particle in a box (review on your own) • 12.7 The Wave Equation
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• The Bohr Model: – Niels Bohr (1885-1962): first quantum model • proposed: electron in a hydrogen atom moves around the nucleus only in certain allowed circular orbits • this was not completely explained by classical physics • it assumes that the e - ’s have restricted values of angular momentum (quantized) (i.e., mass x velocity x orbital radius) Fig 12.10
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• most important equation formulated by Bohr: – energy levels available to the electron in H atom : n = energy levels (integer from 1 to ) Z = nuclear charge ( Z = 1 for H) • Energy difference between two values of n: D E = energy of level n final - energy of level n initial l L - = - 2 2 18 n Z J 10 x 178 . 2 E l L - - = D - 2 initial 2 2 final 2 n Z n Z J 10 x 178 . 2 E
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• for a H atom: • can be used to calculate energy change between two energy levels in hydrogen atom E < 0 when a photon is emitted with: • Bohr’s model also works well for other one-e - species such as He + and Li 2+ • Bohr’s model fails for multielectron atoms l L - - = D - 2 initial 2 final 18 n 1 n 1 J 10 x 178 . 2 E hc E l= D
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This note was uploaded on 01/16/2010 for the course CHEM CHEM 121 taught by Professor Peggy during the Spring '09 term at Simon Fraser.

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Lecture 151 - Wed. Oct. 8, 2003 Todays Lecture Quantum...

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