Bohr's Atom

Koshun Suto

Bohr assumed a quantum condition when deriving the energy levels of a hydrogen atom. This famous quantum condition was not derived logically, but it beautifully explained the energy levels of the hydrogen atom. Therefore, Bohr’s quantum condition was accepted by physicists. However, the energy levels predicted by the eventually completed quantum mechanics do not match perfectly with the predictions of Bohr. For this reason, it cannot be said that Bohr’s quantum condition is a perfectly correct assumption. Since the mass of an electron which moves inside a hydrogen atom varies, Bohr’s quantum condition must be revised. However, the newly derived relativistic quantum condition is too complex to be assumed at the beginning. The velocity of an electron in a hydrogen atom is known as the Bohr velocity. This velocity can be derived from the formula for energy levels derived by Bohr. The velocity v of an electron including the principal quantum number n is given by αc/n. This paper elucidates the fact that this formula is built into Bohr’s quantum condition. It is also concluded in this paper that it is precisely this velocity formula that is the quantum condition that should have been assumed in the first place by Bohr. From Bohr’s quantum condition, it is impossible to derive the relativistic energy levels of a hydrogen atom, but they can be derived from the new quantum condition. This paper proposes raising the status of the previously-known Bohr velocity formula.

Changyong Chen

Generalized Bohr hydrogen atomic theory is gained by putting forward to generalized Bohr angular momentum quantumlized condition and energy level transmission condition,in which the hydrogen atomic spectra can be explained perfectly and of which the Bohr hydrogen atomic theory is only a special case.

V. P. Milant’ev

The history of the creation and development of Bohr's atomic theory is discussed. Even now, with a consistent quantum theory available, Bohr's theory is not simply the property of history, of methodological interest only. To this day, the ideas of the theory not only provide an excellent introduction to atomic physics, but are also used successfully in treating atomic Rydberg states, exotic atoms, etc.

J. D. Main Smith