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What is the energy in joules, required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state? The ground state electron energy is -2.18 x 10-11 ergs |
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Answer» Energy of electron in nth orbit of H atom is given by = {-2.18 x 10-11 ergs}/{n2} Thus, E1 = -2.18 x 10-11 ergs = -218 x 10-13 ergs and Es = {-2.18 x 10-11}/{(5)2} ergs = -8.72 x 10-13 ergs Energy required for the electronic transition ΔE = E5 - E1 = -8.72 x 10-13 ergs - (-218 x 10-13 erg) = 2.08 x 10-11 ergs Wavelength of the emitted radiation, λ = ch/ΔE = {3 x 1010 cm x 6.626 x 10-27 ergs}/{2.09 x 10-11 ergs} or, λ = 9.511 x 10-6 cm = 951.1 x 10-8 cm = 956 Å |
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