As mentioned in this week’s notes on page 4, the electrons of an atom can occupy different energy shells within the atom (simila
r 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
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