Part A: Use the energy levels of hydrogen, given by the equation: [E n = (-13.60

Question

Part A:

Use the energy levels of hydrogen, given by the equation: [En = (-13.606/n2)eV] to calculate the energy, E, of the visible Balmer series photons: E = 13.606eV (1/4 - l/n2), where n=3 for the red line, n=4 for the blue-green, and n=5 for the violet; your text shows how to compute the wavelength (in Angstroms) of a photon if its energy is known in eV (electron volts): = 12398/E. Use this formula to compute the wavelenths of the three Balmer lines that you observed; show each step of your work

Part B:

At what angle would you expect to see the second order line for =6562Angstroms in this experiment?

Please any help would be very much appreciated. Thank you.!!

Explanation / Answer

For the visible balmer E = 13.06 eV ( 1/ n^2 - 1/ n_0^2 )           for n = 3 red line     E_3 = - 13.06*1.6*10^-19 J ( 1/ 3^2 -1/1)               = 18.57 *10^-19 J        for n = 4 blue green line     E_4 = - 13.06*1.6*10^-19 J ( 1/ 4^2 -1/1)               = 19.5*10^-19J for n = 5 violet line    E_5 = - 13.06*1.6*10^-19 J ( 1/ 5^2 -1/1)                            = 20.0*10^-19 J             = 20.0*10^-19 J a photon if its energy is known in eV   = 12398/E.     for n = 3 _3 = 12398 / 18.57 *10^-19 J  / 1.6*10^-19 J          = 1068.2 m for n = 4 _4 = 12398 / 19.5 *10^-19 J  / 1.6*10^-19 J            = 1017.4 m            = 1017.4 m   for n = 5 _5 = 12398 /  20.0 *10^-19 J  / 1.6*10^-19 J          = 991.8m _5 = 12398 /  20.0 *10^-19 J  / 1.6*10^-19 J          = 991.8m         

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