|San José State University|
& Tornado Alley
Neils Bohr's model of the hydrogen atom was one of the first great successes of quantum theory. The wavelengths of the hydrogen spectrum are within a few one hundredths of one percent. It failed however in the explanation of the spectra of helium and the higher elements. Nevertheless it is still a valuable theory for providing insights into the mechanism of electron transition phenomena on the subatomic level.
The great success of the Bohr model had been in explaining the spectra of hydrogen-like (single electron around a positive nucleus) atoms. The Schroedinger equation replicated this explanation in a more sophisticated manner and the Bohr analysis was considered obsolete. But the Schroedinger equation approach can be solved for only a very limited number of models. Beyond this limited set the Schroedinger equation approach gives no insights, whereas the Bohr model does provide insights into diverse cases. In particular the Schroedinger equation approach cannot be applied to the case which takes into account the relativistic effects. On the other hand, the Bohr analysis can.
The details of the application of the Bohr analysis to a hydrogen like atom in the
nonrelativistic regime is given here. The significant initial assumption is
that the angular momentum is quantized in units of Planck's constant divided by 2π,
h. The angular momentum of the electron is mvr,
where r is the radius of the elecron's orbit, v is its orbital velocity and m is its mass. Thus
where n is a positive integer which is called the quantum number of the electron.
The potential energy of an electron, V(r), is given by −α/r, where α is a constant equal to the force constant for electrostatic attraction times the square of the charge of an electron. The attractive force is given by −α/r².
In a circular orbit the balance of the attractive force and the centrifugal force requires that:
But from the quantization of angular momentum
Equating the two expressions for v² gives
This is the quantization condition for the orbit radius. The quantization of the other characteristics of the state of the electron follow from that for r.
Orbital velocity is given by
Kinetic energy K is given by
The potential energy V is then
From the expression for K and V it is seen that
If total energy decreases fory ΔT half of the decrease goes into increased kinetic energy and the other half goes into an emitted photon. Thus the energy γ is given by
where nI² is the initial quantum number for the electron and nF² is its final quantum number. The photon energy is converted into wavelenth via the relationships
where c is the speed of light and λ is the wavelength.
|Comparison of Spectral Wavelengths
Computed from Bohr Model
of the Hydrogen Atom with
the Measured Wavelengths
As can be seen in the table the errors are usually a small fraction of one percent.
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