Author Question: Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron ... (Read 86 times)

caca31 · **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 E_n = –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
E_n = –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

ElaneShive · **Reply #1 on:** Nov 5, 2023

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