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Unformatted text preview: MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science Fall 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms . _______________________________________________________________________________ ________________________________________________________________________________ 5.111 Lecture Summary #5 Readings for today: Section 1.3 (1.6 in 3 rd ed ) Atomic Spectra, Section 1.7 up to equation 9b (1.5 up to eq. 8b in 3 rd ed ) Wavefunctions and Energy Levels, Section 1.8 (1.7 in 3 rd ed ) The Principle Quantum Number Read for Lecture #6: Section 1.9 (1.8 in 3 rd ed ) Atomic Orbitals. Assignment: Problem set #2 (due Session #8). Topics: The Hydrogen Atom I. Binding energies of the electron to the nucleus (H = E ) II. Verification of hydrogen-atom energy levels A. Photon emission B. Photon absorption III. Wavefunctions (orbitals) for the hydrogen atom (H = E ) THE HYDROGEN ATOM I. BINDING ENERGIES (E n ) OF THE ELECTRON TO THE NUCLEUS The Schrdinger equation for the H atom: m = _____ = ___________________ e = ___________________________ = permittivity constant h = Plancks constant The constants in this equation are can be combined into a single constant: The binding energy (E n ) of the electron to the nucleus for the hydrogen atom : where n = __________________ (an integer) = ________________________________ 1 KEY IDEA Binding energies are quantized! The principal quantum number, n, comes out of solving the Schrdinger equation....
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This note was uploaded on 11/27/2011 for the course CHEMICAL E 20.410j taught by Professor Rogerd.kamm during the Spring '03 term at MIT.

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lecnotes05 - MIT OpenCourseWare http://ocw.mit.edu 5.111...

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