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)


​

Answer 1

In the Balmer series, the transition of an electron from n=3 to n=2 in a hydrogen atom emits a photon with a wavelength of 656 nm, which appears as red light.

Step-by-step explanation:

The Balmer series describes transitions in the hydrogen atom from higher energy levels to the second lowest energy level (n=2), which result in the emission of visible light. Specifically, the transition from the n=3 shell to the n=2 shell emits a photon with a wavelength of 656 nanometers (nm), which is visible as red light. This phenomenon is a key part of Bohr's model of the hydrogen atom, reflecting how electrons move to lower energy levels by releasing energy in the form of light.

Answer 2

Step-by-step 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.