1. In 1885 Balmer created an equation that described the visible light spectrum for hydrogen. This...

 

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1. In 1885 Balmer created an equation that described the visible light spectrum for hydrogen. This evolved to become the Rydberg equation presented below. Bohr used Balmer's work as an insight into the structure of the hydrogen atom. 1 RH 1 1 2 3 n ng RH = 1.10 x 10 /m (a) The visible portion of the hydrogen spectrum is called the Balmer series. The visible light photons emitted from the hydrogen atom all involve electron transitions from higher (excited) energy levels down to the n = 2 level. Calculate the wavelength of the light emitted from the quantum leap of an electron from the ni= 4 level to the n = 2 level. (b) Use the wave equation, 3= c/f, to calculate the frequency of the light emitted (c = 3.00 x 10³ m/s). (c) Use the Planck equation, E = hf, to calculate the energy of the electron transition and, therefore, the difference in energy between the n₁ = 4 and the n=2 levels (h= 6.63 x 10 J/Hz). -34 1. In 1885 Balmer created an equation that described the visible light spectrum for hydrogen. This evolved to become the Rydberg equation presented below. Bohr used Balmer's work as an insight into the structure of the hydrogen atom. 1 RH 1 1 2 3 n ng RH = 1.10 x 10 /m (a) The visible portion of the hydrogen spectrum is called the Balmer series. The visible light photons emitted from the hydrogen atom all involve electron transitions from higher (excited) energy levels down to the n = 2 level. Calculate the wavelength of the light emitted from the quantum leap of an electron from the ni= 4 level to the n = 2 level. (b) Use the wave equation, 3= c/f, to calculate the frequency of the light emitted (c = 3.00 x 10³ m/s). (c) Use the Planck equation, E = hf, to calculate the energy of the electron transition and, therefore, the difference in energy between the n₁ = 4 and the n=2 levels (h= 6.63 x 10 J/Hz). -34

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