Most scientists are fully convinced that the hydrogen atom is described quite well by the Schrödinger wave function. But throughout the existence of quantum mechanics (QM), the

Three-dimensional distribution of extrema of Schrödinger

Y-functions has never been presented.

Why?

Let us turn to the example. Following QM, the density of probability of the presence of a
single electron in the hydrogen atom, at every point and at every instant, is proportional to . Therefore, at *l* = 1 and *m *= 0, extremes
of are in two polar points *s*_{1} and
*s*_{2}, i.e., on the extreme radial sphere determined by the solutions of the radial
equation for the radial function *R _{1}*(

*r*).

The surface (a) and corresponding to it
two polar extremes *s*_{1} and *s*_{2} (b) of on the radial sphere *R _{1}*(

*r*);

*p*is the proton.

Obviously, transitions of the electron between two points, *s*_{1} and
*s*_{2}, separated by the equatorial plane of the zero probability, are impossible. We
arrive at the fact that with the equal probability the electron can be either in *s*_{1}
and *s*_{2}. It means that the electron (being in the state determined by the quantum
numbers *l* = 1 and *m* = 0) "hangs" above the "north" or "south" poles of the proton surface,
forming together with the proton an electric dipole directed along the polar z-axis, and its orbital
(magnetic and mechanical) moments are equal to zero.

Obviously, such a structure of the hydrogen atom,

originated from the QM interpretation, is inconsistent with
experiment.

The similar inconsistency is inherent in all other functions with
different quantum numbers *l* and *m*.

According to the Wave Model

we developed to replace the Standard Model, true atoms are only the simplest hydrogen atoms, to which we refer proton, neutron and protium. The remaining atoms presented in the Periodic Table are elementary molecules of the above hydrogen atoms. They have the shell-nodal structure.

The simplest schematic view of the carbon atom