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).(c = 3.00 × 10⁸ m/s; h = 6.63 × 10^-34 J • s) A)4.45 × 10^-20 nm B)2.16 × 10^-6 nm C)9.18 × 10^-20 nm D)1.38 × 10¹⁴ nm E)2.17 × 10³ nm

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Quizplus · Accepted Answer

The energy difference between the levels is calculated using En = -2.18 × 10^-18 J (1/n^2). The energy difference is converted to wavelength using E = hc/λ. The correct wavelength is approximately 2.17 × 10^3 nm.

Calculate the Wavelength,in Nanometers,of the Light Emitted by a Hydrogen