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As mentioned in this week’s notes on page 4, the electrons of an atom can occupy different energy shells within the atom (similar to how the planets all occupy different orbits around the Sun). Electrons prefer to be in the lowest energy shell possible (the ground state); however, they can gain energy and jump to a higher shell by absorbing light or being excited by an electric current. In accordance with the conservation of energy, if an electron drops from a higher energy level to a lower one, this must emit a photon (particle of light) with energy equal to the energy difference of the shells.

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)

A) 656E-9 meters
B) 486E-9 meters
C) 434E-9 meters
D) 410E-9 meters

As mentioned in this weeks notes on page 4 the electrons of an atom can occupy different energy shells within the atom similar to how the planets all occupy dif class=

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jashae2003
The assume that goes with the inquiry demonstrates the wavelenghts of the photons transmitted by Balmer arrangement change , from vitality levels (n) 3, 4, 5, and 6 to the vitality level (n) 2, in  hydrogen particles.

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 discharged from the n = 3 shell in hydrogen is the primary information of the table, i.e 656 nm.

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

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

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