The electron in a hydrogen atom is excited from the quantum energy level n = 1 to n = 4. (a) How much energy is absorbed by the electron? (b) What are the frequency (v) and wavelength (2., in nanometers) of the photon absorbed by the electron? (c) What is the energy change (AE, in Joule) when this electron jumps from the quantum energy level n =4 to n= 2? (d) Calculate the wavelength (in nm) of the photon emitted by this electronic transition. (E, = -(2.18 x 10-18 J)/n²; h= 6.63 x 10-34 J.s; c = 3.00 x 10° m/s)
The electron in a hydrogen atom is excited from the quantum energy level n = 1 to n = 4. (a) How much energy is absorbed by the electron? (b) What are the frequency (v) and wavelength (2., in nanometers) of the photon absorbed by the electron? (c) What is the energy change (AE, in Joule) when this electron jumps from the quantum energy level n =4 to n= 2? (d) Calculate the wavelength (in nm) of the photon emitted by this electronic transition. (E, = -(2.18 x 10-18 J)/n²; h= 6.63 x 10-34 J.s; c = 3.00 x 10° m/s)
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