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) A)97.2 nm B)82.6 nm C)365 nm D)0.612 nm E)6.8 * 10^-18 nm

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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 energy difference can be converted to wavelength using the formula λ = hc/ΔE, where h is Planck's constant and c is the speed of light. The calculated wavelength is approximately 97.2 nm.

Calculate the Wavelength of the Light Emitted by a Hydrogen