The diagram above shows three energy levels of a hypothetical atom

The diagram above shows three energy levels of a hypothetical atom

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The diagram above shows three energy levels of a hypothetical atom. The lowest available energy level is E 1 = –5.0 eV. a. Draw arrows on the above diagram showing all possible photon emissions for electrons that begin in the –2.2 eV state. Answer: These electrons can either drop straight to E 1 or drop in two stages, going first to E 2 and then to E 1 . b. What wavelength(s) of visible light can electrons emit that begin in the –2.2 eV state? Answer: The wavelength of the photon emitted by an electron's transition is given by , where hc is 1240 eV • nm and Δ E is the difference between energy levels. The electrons can make any of the three transitions shown in part (a): o Emitting a 1.8 eV photon from E 3 to E 2 o Emitting a 2.8 eV photon from E 3 to E 1 o Emitting a 1.0 eV photon from E 2 to E 1 The wavelengths associated with these transitions are: o 690 nm for the 1.8 eV photon o 440 nm for the 2.8 eV photon o 1240 eV for the 1.0 eV photon Of these, only the 690 nm and 440 nm photons are visible, because the visible spectrum includes wavelengths of approximately 400 to 700 nm. Now visible light is incident upon a photoelectric surface with work function 2.2 eV. c. On the axes below, sketch a graph of the maximum kinetic energy of ejected electrons as a function of the wavelength of the incident light for the range of wavelengths indicated. Label the vertical axis with an appropriate scale and units.
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Answer: d.
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