It is known that in the atom of matter quantum number n determines its kinetic and potential energy, the quantum number l--the shape of the electron orbit
, quantum number [m.sub.l]--the position of the electron orbit
in atomic space and the quantum number [m.sub.s] --its direction of circular rotation around its own axis [4, 7].
In an effort to connect all these facts with the electron orbit
, one could say that the power of each pulse is characteristic of the wave-electron interaction intensity.
As they involve the electron orbits
, as with common chemical reactions, they belong to the chemical realm, yet the evidence suggests that the usual list of properties of elements may be incomplete, and an additional descriptor may be justified: "orbitality" (4).
If the electron orbits
the nucleus at a great distance, there is plenty of space in between for other atoms.
Part I, appearing in July 1913, described the quantum rules for electron orbits
and quantum jumps in the hydrogen atom, explaining the spectrum of colors it emitted.
The fact that the elliptic path s can equal its translation component n  seems to be crucial for forming the stable electron orbits
around the atom nucleus.
Elements get successively heavier and more complex as more protons, neutrons, electrons, and electron orbits
In 1926 an Austrian physicist, Erwin Schrodinger (1887-1961), decided that if the electron was viewed as a wave rather than as a particle, Bohr's electron orbits
(see 1913 and 1915) might make more sense.
Indeed this idea that the electron orbits
at constant radius is a necessary condition for the electron to be considered objectively real.