Lecture24, 3-10-08 H-atom

Lecture24 - Continuous Spectrum Tungsten Filament Line Spectrum H atoms Low Pressure Vapor Phase Emissions of Several Elements Discrete energy

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Unformatted text preview: Continuous Spectrum Tungsten Filament Line Spectrum H atoms Low Pressure Vapor Phase Emissions of Several Elements Discrete energy levels Transitions and the Rydberg Equation ¡ An electron in the lowest energy orbit, n = 1, is in the ground state ¡ An electron in any orbit other than n = 1, is in an excited state ¡ The energy of a line is the difference in the energies of the two orbits involved in the transition Δ E = E final- E initial Δ E = h ν = R H { }- 1 2 n i 1 2 n f Hydrogen atom spectra Visible lines in H atom spectrum are called the BALMER series . High E High E Short Short λ High High ν Low E Low E Long Long λ Low Low ν Energy Ultra Violet Lyman Infrared Paschen Visible Balmer E n = -2.179x10-18 J n 2 6 5 3 2 1 4 n Using The Rydberg Equation Question What is the wavelength of light that corresponds to the transition of the electron from the n = 4 to the n = 2 state of the hydrogen atom. Is the light absorbed or emitted by the atom? Answer: Step 1: Use the Rydberg equation with n i = 4 and n f = 2.-6.17 x 10 14 s-1-6.17 x 10 14 s-1 Δ E = h ν = R H { }- 1 2 n i 1 2 n f R h H ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ { }- 1 2 n i 1 2 n f 2.18 x 10 J 6.63 x J s-18 10 34 − ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ { }- 1 4 2 1 2 2 ν = = = Step 2: Convert to wavelength of light λ = = 4.86 x 10-7 m = 486 nm 486 nm 3.00 x 10 m / s 6.17 x s 8-1 10 14 ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ c ν c = λν c = λν Answer continued = The color of this box is ~ 486 nm Bohr model of the Hydrogen Atom • Duality of matter led to the hypothesis that electrons behave as waves....
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This note was uploaded on 08/06/2008 for the course CHEM 1B taught by Professor Watts during the Winter '08 term at UCSB.

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Lecture24 - Continuous Spectrum Tungsten Filament Line Spectrum H atoms Low Pressure Vapor Phase Emissions of Several Elements Discrete energy

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