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Physics Experiment on Balmer Spectral Lines of Hydrogen

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Q1: I need to calculate the visible lines that should be seen with a spectroscope. This should correspond to lines in which the final bound energy level is N = 2.

Q2: I need to compare the observed lines to the ones that I calculate.
The observed, recorded wave length lines were:

RED = 650 nanometers
TURQUOISE = 490 nanometers
VIOLET 1 = 435 nanometers
VIOLET 2 = 405 nanometers

(The lines above were observed by looking at the line spectra from hydrogen gas being placed in an electrical discharge tube.)

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Q: I need to calculate the visible lines that should be seen with a spectroscope.

A: Balmer Series is formed due electron transition from n ≥ 3 to n =2 orbits.

So the energy associated with this transition can be written as,

E = 13.6/22 - 13.6/n2] eV
E = [13.6/4 - 13.6/n2] * 1.6 x 10^-19 J
We also know the energy of a photon
E = hf = h c/ ...

Solution Summary

This is a physics laboratory experiment. I have theoretically found the wavelength of spectral lines in Balmer series of Hydrogen. Then I have compared these values with the experimentally found values by finding the percent difference.