Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen E_n = -2.18 * 10^-18 J(1/n²). A) 1.82 * 10^-19 /s B) 9.13 * 10¹³ /s C) 2.74 * 10¹⁴/s D) 3.65 * 10¹⁴ /s E) 1.64 * 10¹⁵ /s

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Quizplus · Accepted Answer

The energy difference between the levels is calculated using E = E₆ - E₃. The frequency is then found using E = hν, where h is Planck's constant (6.626 x 10^-34 J·s). The correct frequency is approximately 3.65 x 10^14 /s.

Calculate the Frequency of the Light Emitted by a Hydrogen