04 - Chemistry 1000 Lecture 4: Energy levels and emission...

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Chemistry 1000 Lecture 4: Energy levels and emission spectroscopy of hydrogenic atoms Marc R. Roussel
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Energy levels of hydrogen -1 -0.8 -0.6 -0.4 -0.2 0 E / R H n =1 n =2 n =3 n =4 E n = - Z 2 n 2 R H h ν = E upper - E lower = Z 2 R H ± 1 n 2 lower - 1 n 2 upper ²
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Quantum state terminology The ground state of a quantum system is the lowest possible energy level. For a hydrogenic atom, this is the n = 1 state. The first excited state is the next-lowest possible energy level. For a hydrogenic atom, this is n = 2. The second excited state. . .
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I The emission spectrum of hydrogen (or, in general, of hydrogenic atoms) is organized into series of lines that correspond to a common n lower . I The Lyman series consists of the set of transitions to the ground state ( n = 1). Example: Calculate the wavelength range of the longest wavelength line in the Lyman series of hydrogen. Answer: 121.502 273 nm Note: 122 nm is in the ultraviolet range. All the other lines in the Lyman series will also be in the ultraviolet. (Why?)
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This note was uploaded on 03/03/2012 for the course CHEM 1000 taught by Professor Marc during the Fall '06 term at Lethbridge College.

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04 - Chemistry 1000 Lecture 4: Energy levels and emission...

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