Calculate the frequency 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). A) 1.35 * 10^-51 /s B) 1.03 * 10⁸ /s C) 2.06 * 10¹⁴ /s D) 8.22 * 10¹⁴ /s E) 3.08 * 10¹⁵ /s

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Quizplus · Accepted Answer

The energy difference between the levels is calculated using the formula: ΔE = E1 - E4 = -2.18 * 10^-18 J (1/1^2 - 1/4^2). This gives ΔE = 2.04375 * 10^-18 J. The frequency is then found using the relation E = hν, where h = 6.626 * 10^-34 J·s. Solving for ν gives ν = ΔE / h = 3.08 * 10^15 /s.

Calculate the Frequency of the Light Emitted by a Hydrogen