Question

A Balmer series transition is any transition of an electron from some higher energy shell down to the second lowest energy shell (n=2) in hydrogen.
Looking at image (b) above, what is the wavelength of a photon emitted during the Balmer transition from the n=3 shell in hydrogen? (remember nm is short for a nanometer, for example 656 nm = 656 x 10-9 meters)


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Answer 1

Explanation:

The figure that accompanies the question shows the wavelenghts of the photons emitted according to Balmer series transition , from energy levels (n) 3, 4, 5, and 6 to the energy level (n) 2, in  hydrogen atoms.

These are the values shown in the figure

Transition                     wavelength of the photon emitted

                                                nm

from n = 3 to n = 2                  656 <------------- this is the value requested

from n = 4 to n = 2                  486

from n = 5 to n= 2                   434

from n = 6 to n = 2                  410

The wavelength of a photon emitted from the n = 3 shell in hydrogen is the first data of the table, i.e 656 nm.

Using the conversion factor from nm to m that result is:

656 nm * 1 m / (10^9 nm) =  656 * 10 ^ - 9 m.