Green light of wavelength 516 nm is absorbed by an atomic gas.

What is the energy difference between the two quantum states involved in the transition?

If the gas absorbed a mole of photons, what is the total energy that would be absorbed?

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Nestor RutherfordLv2

17 Apr 2019

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A certain quantum mechanical system has the energy levels shown in the accompanying diagram. The energy levels are indexed by a single quantum number n that is an integer. (a) As drawn, which quantum numbers are involved in the transition that requires the most energy? (b) Which quantum numbers are involved in the transition that requires the least energy? (c) Based on the drawing, put the following in order of increasing wavelength of the light absorbed or emitted during the transition: (i) n = 1 to n = 2; (ii) n = 3 to n = 2; (iii) n = 2 to n = 4; (iv) n = 3 to n = 1.