What is the wavelength of light emitted when an electron in a hydrogen atom undergoes a transition from energy level n = 6 to level n = 1? (c = 3.00 × 10⁸ m/s,h = 6.63 × 10^-34 J·s,R_H = 2.179 × 10^-18 J) A) 9.39 × 10^-8 kJ/mol B) 7.06 × 10^-27 kJ/mol C) 1.07 × 10⁷ kJ/mol D) 2.12 × 10^-18 kJ/mol E) 3.2 × 10¹⁵ kJ/mol

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Quizplus · Accepted Answer

The energy of an electron in a hydrogen atom is given by the equation E = -R_H/n², where R_H is the Rydberg constant. The wavelength of light emitted when an electron undergoes a transition from energy level n_i to energy level n_f is given by the equation λ = hc/ΔE, where h is Planck's constant, c is the speed of light, and ΔE is the energy difference between the two levels. In this case, the energy difference between the two levels is ΔE = E_i - E_f = -R_H/n_i² - (-R_H/n_f²) = R_H(1/n_f² - 1/n_i²). Substituting the given values into this equation, we get ΔE = R_H(1/1² - 1/6²) = R_H(5/36) = 3.03 × 10^-19 J. The wavelength of light emitted is then λ = hc/ΔE = (6.63 × 10^-34 J·s)(3.00 × 10⁸ m/s)/(3.03 × 10^-19 J) = 6.56 × 10^-7 m.

What Is the Wavelength of Light Emitted When an Electron