i need help with these 6 questions please i cant figure them out Suppose that an
ID: 1780142 • Letter: I
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i need help with these 6 questions please i cant figure them out
Suppose that an atom is initially in an excited state with an energy of E2 = 5.25 eV where an .eV" is a unit of energy. One Electron-volt (ev) is equivalent to the following: 1 eV = 1.602 x 1019 Joules. If this electron makes a transition to a lower energy state E 3.05 eV, what is the energy (in eV) of the emitted photon of light? The first three energy levels for the hydrogen atom have energies of E1 -13.6 eV, E2 -3.4 eV and E1.5 eV. Draw an Energy Level Diagram (like we did in class) showing these three energy levels. Label each energy level by its energy (remember that-13.6-.3.4 .5). Suppose that the electron in hydrogen is initially in the third energy level Eg. On your Energy Level Diagram, draw all of the possible transitions that this electron can make as it moves downward. Draw downward arrows for each transition. How many possible transitions are there? Submit AnswerTries 0/8 Submit Answer Tries 0/8 What is the frequency (in Hz) ofthe emitted photon of light? Planck's Constant is given by h = 4.136 x 10-15 evs. the electron makes a transition from E3 to E2, what is the frequency (in Hz) of the emitted photon of light? Planck's Constant is given by h = 4.136 x 10-15 evs. Submit Answer Tries 0/8 Submit AnswerTries 0/8 What is the wavelength (in nm) of the emitted photon of light? The speed of light is 3 x 108 m/s. What is the wavelength (in nm) of the emitted photon of light? The speed of light is 3 x 108 m/s. (What color is this?)Explanation / Answer
Energy = 5.35 - 3.05 = 2.3 eV ....Ans
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E = h f
2.3 x 1.6 x 10^-19 = 6.626 x 10^-34 f
f = 5.56 x 10^14 Hz
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wavelength = c / f = 5.39 x 10^-7 m OR 539 nm
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E3 -> E1 , E3 -> E2, E2 -> E1
three transition
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(3.4 - 1.5) = (4.136 x 10^-15)f
f = 4.594 x 10^14 Hz
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wavelength = c / f = 653 x 10^-9 m Or 653 nm
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