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This is often expressed in terms of the inverse wavelength or "wave number" as follows:
IndexAtomic structure concepts
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This Bohr model picture of the orbits has some usefulness for visualization so long as it is realized that the "orbits" and the "orbit radius" just represent the most probable values of a considerable range of values. If the radial probabilities for the states are used to make sure you understand the distributions of the probability, then the Bohr picture can be superimposed on that as a kind of conceptual skeleton.
Energy level plotEnergies in eVHydrogen spectrum
Electron energy level diagrams
IndexHydrogen conceptsAtomic structure concepts
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If you look at the hydrogen energy levels at extremely high resolution, you do find evidence of some other small effects on the energy. The 2p level is split into a pair of lines by the spin-orbit effect. The 2s and 2p states are found to differ a small amount in what is called the Lamb shift. And even the 1s ground state is split by the interaction of electron spin and nuclear spin in what is called hyperfine structure.
Electron level calculationEnergies in eV
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This spectrum was produced by exciting a glass tube of hydrogen gas with about 5000 volts from a transformer. It was viewed through a diffraction grating with 600 lines/mm. The colors cannot be expected to be accurate because of differences in display devices.
function sq(x){return x*x}
function tcalc(){fh=document.forms[0];def();zz=fh.z.value;nn2=fh.n2.value;nn1=fh.n1.value;eev=13.605698*sq(zz)*(1/sq(nn1)-1/sq(nn2));fh.h.value=eev;fh.wl.value=1239.842/eev}
function def(){fh=document.forms[0];if (fh.z.value==0)fh.z.value=1;if (fh.n1.value==0)fh.n1.value=2;if (fh.n2.value==0)fh.n2.value=3}
For atomic number Z = ,
a transition from n2 = to n1 =
will have wavelength λ = nm
and quantum energy hν = eV
At left is a hydrogen spectral tube excited by a 5000 volt transformer. The three prominent hydrogen lines are shown at the right of the image through a 600 lines/mm diffraction grating.
An approximate classification of spectral colors:
Violet (380-435nm)
Blue(435-500 nm)Cyan (500-520 nm)Green (520-565 nm)Yellow (565- 590
nm)Orange (590-625 nm)Red (625-740 nm)
Radiation of all the types in the electromagnetic spectrum can come
from the atoms of different elements. A rough classification of some of
the types of radiation by wavelength is:
Infrared > 750 nm
Visible 400 - 750 nm
Ultraviolet 10-400 nm
Xrays < 10 nm
Bohr model Measured hydrogen spectrum Other spectra
IndexGreat experiments of physicsHydrogen conceptsAtomic structure concepts
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The red line of deuterium is measurably different at 656.1065 ( .1787 nm difference).
Illustration of transitions
Hydrogen fine structure (3->2 transition)
More extensive table of spectral lines
IndexHydrogen conceptsAtomic spectra
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