Example:An electron in a hydrogen atom drops from energy level E4 to energy levelE2. What is the frequency of the emitted photon, and which line in theemission spectrum corresponds to this event?E6E= -0.378 eVStep 1:EsE = -0.544 eV- E= -0.850 eVFind the energy of the photon. EE = Einitial - EfinalE3E=-1.51 eV= (-0.850 eV) - (-3.40 eV)= 2.55 eVStep 2:Use Plank's equation forfrequency.E₂E= -3.40 eV12EE = hf; f =h(2.55 eV) (1.60 x 10-1916.63 x 10-34 Jsf= 6.15 x 10¹4 HzLine 3 is in the visible partof the electromagneticspectrum and appears tobe blue. The frequency f =6.15 x 10¹4 Hz lies withinthe range of the visiblespectrum and is towardthe violet end, so it isreasonable that light of thisfrequency would be visibleblue light.Step 3:Find the corresponding line in the emission spectrum.Examination of the diagram shows that the electron's jumpfrom energy level E4 to energy level E2 corresponds toLine 3 in the emission spectrum.3IncomingphotonEmittedphoton(a)(b)Figure 4. (a)When a photon is absorbed by an atom, an electronjumps to a higher energy level. (b)When the electron falls back toa lower energy level, the atom releases a photon.Activity:Using the same emission spectrum at the example.Solve for the frequency of the emitted photon when,an electron of a hydrogen atom drops from energylevel Es to energy level E₁ and identify which linecorresponds to this event.

Given Data : Emission spectra for the hydrogen atom are given. To Find : The frequency of photons…

Answered: Activity: Using the same emission…

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Activity: Using the same emission spectrum at the example. Solve for the frequency of the emitted photon when, an electron of a hydrogen atom drops from energy level Es to energy level E₁ and identify which line corresponds to this event.