Notes - Section 6.3-6.6

Notes Section - Paul Jackman Chemistry CHE 106 M029 Section 6.3-6.6 Notes 6.3 Line Spectra and the Bohr Model 1913 Niels Bohr offered a theoretical

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Paul Jackman October 20, 2009 Chemistry CHE 106 – M029 Section 6.3-6.6 Notes 6.3 Line Spectra and the Bohr Model 1913, Niels Bohr offered a theoretical explanation of line spectra Line Spectra Radiation composed of a single wavelength is said to be monochromatic A spectrum is produced when radiation from such sources is separated into its different wavelength components The rainbow of colors, containing light of all wavelengths, is called a continuous spectrum A spectrum containing radiation of only specific wavelengths is called a line spectrum Bohr’s Model Rutherford’s discovery of the nuclear nature of the atom suggests that the atom can be thought of as a “microscopic solar system” in which electrons orbit the nucleus Bohr based his model on three postulates: o Only orbits of certain radii, corresponding to certain definite energies, are permitted for the electron in a hydrogen atom. o An electron in a permitted orbit has a specific energy and is in an “allowed” energy state. An electron in an allowed energy state will not radiate energy and therefore will not spiral into the nucleus o Energy is emitted or absorbed by the electron only as the electron changes from one allowed energy state to another. This energy is emitted or absorbed as a photon, E=hv. The Energy States of the Hydrogen Atom
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This note was uploaded on 02/09/2010 for the course CHE CHE 106 taught by Professor Korter during the Fall '09 term at Syracuse.

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Notes Section - Paul Jackman Chemistry CHE 106 M029 Section 6.3-6.6 Notes 6.3 Line Spectra and the Bohr Model 1913 Niels Bohr offered a theoretical

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