Bohr - Bohr's Model Bohr began with the assumption that...

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Bohr's Model Bohr began with the assumption that electrons were orbiting the nucleus, much like the earth orbits the sun. From classical physics, a charge traveling in a circular path should lose energy by emitting electromagnetic radiation If the "orbiting" electron loses energy, it should end up spiraling into the nucleus (which it does not). Therefore, classical physical laws either don't apply or are inadequate to explain the inner workings of the atom Bohr borrowed the idea of quantized energy from Planck o He proposed that only orbits of certain radii, corresponding to defined energies, are "permitted" o An electron orbiting in one of these "allowed" orbits: Has a defined energy state Will not radiate energy Will not spiral into the nucleus If the orbits of the electron are restricted, the energies that the electron can possess are likewise restricted and are defined by the equation: Where R H is a constant called the Rydberg constant and has the value 2.18 x 10 -18 J 'n' is an integer , called the principle quantum number and corresponds to the different allowed orbits for the electron. Thus, an electron in the first allowed orbit (closest to the nucleus) has
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This note was uploaded on 11/22/2011 for the course CHEMISTRY CHM1025 taught by Professor Laurachoudry during the Fall '10 term at Broward College.

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Bohr - Bohr's Model Bohr began with the assumption that...

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