In a previous post, we showed the Bohr atom as represented at the Georgia State University Physics Department’s website in the following way:
Is it possible to derive the total energy of electrons in the Bohr model from Schrodinger’s wavefunctions?
In general, we can calculate the total energy, , of the electron as the sum of its Coulombic potential, and kinetic energy, :
With, , we can calculate the average total energy, , using:
So what is the form of ?
The average potential energy, , is calculated using Coulomb’s law:
The average kinetic energy, , can be determined if the electrons travel around the nucleus in a circular fashion.*
From Newton’s second law: and for circular motion
while . Therefore, , so
This means that we have our average total energy for the circulating electron: , and
From here, it is a simple matter of applying the integral we learned earlier: to the and to derive the total energy of the electrons in these Bohr orbits:
The Energy of the 1s electron
The Energy of the 2s electron
Looking at the energy differences between these two energy levels, the can be calculated and compared to the energy levels observed in the hydrogen spectrum (Lymann series):
A wavelength of 121.566 nm corresponds to an energy of: . Not bad agreement! Bohr’s energy levels inversely depend upon the square of the principle quantum number, n. The model is derived from the consideration of a lone electron (of a hydrogen atom or a helium anion) and therefore didn’t work well to describe the spectral lines of the many-electron atoms. This was something that vexed him. As Max Tegmark and John Archibald Wheeler describe in their wonderful “100 Years of Quantum Mysteries”: “Back in Copenhagen, Bohr got a letter from Rutherford telling him he had to publish his results. Bohr wrote back that nobody would believe him unless he explained the spectra of all the elements. Rutherford replied: Bohr, you explain hydrogen and you explain helium, and everyone will believe all the rest.”
In a later post, at some point, it would be interesting to see if we could derive the general square dependence of the Bohr radius on the principle quantum number, n. This has been done for the specific case above, but for a general derivation, it would likely be necessary to determine how the principle quantum number arises from the wave equation. I have never taken a formal quantum course so need to do some reading before I can post about this. Also, it would be fun to try to derive the hydrogen wavefunctions too!
Overall, I think this wraps up my experiments with the overlap between quantum and multivariable calculus and physics for some time. I had a blast and I hope you got to share in the fun too!
*Note: I wonder if we could calculate another version of the kinetic energy using a deBroglie relationship: , treating the electron as a wave.