If a hydrogen atom in the ground state absorbs a 93.7 nm photon, corresponding to a transition line in the Lyman series, how does this affect the atom's energy and size? How much energy is needed to ionize the atom when it is in this excited state? Give your answers in absolute units, and relative to the ground state. (the Lyman series is a hydrogen spectral series of transitions and resulting ultraviolet emission lines of the hydrogen atom as an electron goes from n ≥ 2 to n = 1 (where n is the principal quantum number), the lowest energy level of the electron.)
If a hydrogen atom in the ground state absorbs a 93.7 nm photon, corresponding to a transition line in the Lyman series, how does this affect the atom's energy and size? How much energy is needed to ionize the atom when it is in this excited state? Give your answers in absolute units, and relative to the ground state. (the Lyman series is a hydrogen spectral series of transitions and resulting ultraviolet emission lines of the hydrogen atom as an electron goes from n ≥ 2 to n = 1 (where n is the principal quantum number), the lowest energy level of the electron.)
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Transcribed Image Text:If a hydrogen atom in the ground state absorbs a 93.7 nm photon, corresponding to a
transition line in the Lyman series, how does this affect the atom's energy and size?
How much energy is needed to ionize the atom when it is in this excited state? Give
your answers in absolute units, and relative to the ground state.
(the Lyman series is a hydrogen spectral series of transitions and resulting ultraviolet emission lines of
the hydrogen atom as an electron goes from n ≥ 2 to n = 1 (where n is the principal quantum number),
the lowest energy level of the electron.)
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