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Author Question: Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron ... (Read 31 times)

caca31

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on: Nov 5, 2023

Question 1

Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level.  Recall that for hydrogen En = –2.18 × 10–18 J(1/n2)
◦ 6.8 × 10–18 nm
◦ 0.612 nm
◦ 82.6 nm
◦ 97.2 nm
◦ 365 nm

Question 2

Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level.  Recall that the energy levels of the H atom are given by
         En = –2.18 × 10–18 J(1/n2)
◦ 9.18 × 10–20 nm
◦ 4.45 × 10–20 nm
◦ 2.16 × 10–6 nm
◦ 2.16 × 103 nm
◦ 1.38 × 1014 nm
Chemistry ¦ Chang, Goldsby ¦ 11th Edition
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Marked as best answer by caca31 on Nov 5, 2023

ElaneShive

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Reply #1 on: Nov 5, 2023
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caca31

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Reply 2 on: Nov 5, 2023
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