Answer:
The Balmer series refers to the spectral lines of hydrogen, associated to the emission of photons when an electron in the hydrogen atom jumps from a level [tex]n \geq 3[/tex] to the level [tex]n=2[/tex].
The wavelength associated to each spectral line of the Balmer series is given by:
[tex]\frac{1}{\lambda}=R_H (\frac{1}{2^2}-\frac{1}{n^2})[/tex]
where [tex]R_H[/tex] is the Rydberg constant for hydrogen, and where [tex]n[/tex] is the initial level of the electron that jumps to the level n = 2.
The first few spectral lines associated to this series are withing the visible part of the electromagnetic spectrum, and their wavelengths are:
656 nm (red, corresponding to the transition [tex]3 \rightarrow 2[/tex])
486 nm (green, [tex]4 \rightarrow 2[/tex])
434 nm (blue, [tex]5 \rightarrow 2[/tex])
410 nm (violet, [tex]6 \rightarrow 2[/tex])
All the following lines lie in the ultraviolet part of the spectrum. The limit of the Balmer series, corresponding to the transition [tex]\infty \rightarrow 2[/tex], is at 364.6 nm.
