C1403.2006._Week_Seven.2.POST

C1403.2006._Week_Seven.2.POST - Demonstrations on...

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Demonstrations on Spectroscopy 1. Diffraction 2. Incandescence and continuous (rainbow) spectra 3. Line spectra 4. Spectral colors in the visible from incandescent salts
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Nobels in Families Mother and daughter Husband and wife
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Nobels in Families Father and son
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Nobels in Families Father and son
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Bohr Hydrogen Atom Model Niels Bohr Nobel Prize 1922 “ for the structure of atoms and the radiation emanating from them” E 1 E 2 E 2 E 1 Photon absorbed Photon emitted + h ν - h ν Photon absorbed Photon emitted
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Bohr Hydrogen Atom Model Postulates: 1) Quantization of angular momentum 2) Radiationless motion for electrons in allowed orbits 3) Emission (absorption) of light only during allowed transitions and according to the equation E final - E initial = h ν = hc/ λ
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Bohr Hydrogen Atom Model Bohr radius: Set coulomb force of attraction between the proton nucleus and the electron equal to the force required to maintain circular motion of the orbiting electron: Solve for radial distance r separating charges Ze + ( ) e ! ( ) r 2 = Ze 2 r 2 = m e v 2 r r = Ze 2 m e v 2
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Bohr Hydrogen Atom Model Bohr radius: Quantize angular momentum Bohr radius m e vr = n h 2 ! r = h 2 4 2 m e e 2 n 2 = a o n 2 KEEP IN MIND (as Bohr understood) that h has units of angular momentum Defines a unit of length on the atomic scale r = Ze 2 m e v 2
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Bohr Hydrogen Atom Model The Rydberg equation is derived on considering the energy states themselves. Define the total energy of the system for an electron in its orbit: E total = KE + PE Then take the difference between the two states
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Bohr Hydrogen Atom Model E Total = KE + PE = ! 2 " 2 m e e 4 Z 2 n 2 h 2 E Total # 1 n 2 whenZ = 1 E Total # Z 2
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Bohr Hydrogen Atom Model Bohr’s calculated value of R H was within 0.1% of the empirically derived constant and very close to the
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C1403.2006._Week_Seven.2.POST - Demonstrations on...

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