The red line in the hydrogen emission spectrum is 656 nm.If the energy of the nth level is -13.6/n ² eV,then calculate the transition between n levels that this emitted photon comes from. A)n = 2 to n = 3 B)n = 4 to n = 3 C)n = 5 to n = 2 D)n = 3 to n = 2 E)n = 2 to n = 4

Question

Quizplus · Accepted Answer

The energy of the photon emitted during the transition from level n to level m is given by the formula E = (13.6/n^2 - 13.6/m^2) eV. Substituting the wavelength of the emitted photon (656 nm) into the equation E = hc/λ (where h = Planck's constant and c = speed of light), we can find the energy of the emitted photon to be approximately 1.89 eV.

Using the formula for energy, we can find the transitions that lead to this emitted photon. By trying different combinations of n and m and checking if the energy difference matches the calculated energy of the emitted photon, we find that the transition from level n = 3 to level m = 2 is the only one that matches with our calculated energy. Therefore, the correct choice is D.

The Red Line in the Hydrogen Emission Spectrum Is 656