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Journal of Physics & Optics Sciences

Rejection of Rutherford's Planetary Model of the Atom, Bohr's Postulates and the Tunnel Effect

Stanislav Konstantinov, Leo Georgy Sapogin

Published Jan 25, 2021• 2 citations
Publisher

Abstract

The article raises the question of the strange behavior of electrons in an atom, when the electronic orbitals of the P- and d-states of the atom have the form of eights with nodal points in the nucleus of the atom, as well as the discovery of the mysterious K-capture of an electron when the nuclei of atoms of some isotopes of chemical elements someh they sometimes capture an electron from the inner (K- or L-) electron shell of the atom. It has not been possible to explain these phenomena within the framework of the atomic model existing in quantum electrodynamics. In the new model of the atom, proposed by Professor Lev Sapogin in Unitary Quantum Theory, the electron makes quantum leaps within the orbital not randomly, as physicists thought, but through the nucleus of the atom, each time tunneling through it. In this case, the quantization of the energy levels (orbitals) of electrons in an atom is explained by the distribution of nodes and antinodes in a standing wave of an electron, and an integer number of de Broglie wavelengths should be located in the diameter of the electron orbital. The article shows the dependence of the magnitude of the interaction constants in the hydrogen nucleus and, in particular, the fine structure constant, discovered by the CMS cooperation in experiments at the Large Hadron Collider in 2019, during reactions in pp collisions with energies from 1 TeV to 13 TeV and an intranuclear pressure of 10³⁵ Pascal. The value of the fine structure in the near-Earth medium and in a neutron star is given.

DOI
10.47363/jpsos/2021(3)128

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The article raises the question of the strange behavior of electrons in an atom, when the electronic orbitals of the P- and d-states of the atom have the form of eights with nodal points in the nucleus of the atom, as well as the discovery of the mysterious K-capture of an electron when the nuclei of atoms of some isotopes of chemical elements someh they sometimes capture an electron from the inner (K- or L-) electron shell of the atom. It has not been possible to explain these phenomena within the framework of the atomic model existing in quantum electrodynamics. In the new model of the atom, proposed by Professor Lev Sapogin in Unitary Quantum Theory, the electron makes quantum leaps within the orbital not randomly, as physicists thought, but through the nucleus of the atom, each time tunneling through it. In this case, the quantization of the energy levels (orbitals) of electrons in an atom is explained by the distribution of nodes and antinodes in a standing wave of an electron, and an integer number of de Broglie wavelengths should be located in the diameter of the electron orbital. The article shows the dependence of the magnitude of the interaction constants in the hydrogen nucleus and, in particular, the fine structure constant, discovered by the CMS cooperation in experiments at the Large Hadron Collider in 2019, during reactions in pp collisions with energies from 1 TeV to 13 TeV and an intranuclear pressure of 10³⁵ Pascal. The value of the fine structure in the near-Earth medium and in a neutron star is given.
The mere existence of stable atoms, and their arrangement into many-atom nanoscale structures, can only be explained by the laws of quantum mechanics. Indeed, the accumulated evidence regarding the internal structure of atoms motivated the formulation of quantum mechanics at the early twentieth century. Here we focus on single-electron (hydrogen-like) atoms. The dominance of the Coulomb central potential between the electron and nucleus, translates into a simple Schrödinger equation for their relative position distribution. Solving rigorously this equation reveals quantized energy levels, which explains the emission spectra of hydrogen-like atoms (Rydberg formula). The corresponding stationary probability density distributions for the electron around the nucleus are reminiscent of the Bohr model, where classical trajectories (orbits) are replaced by single-electron wave functions (orbitals). The degeneracies of different orbitals, associated with three quantum numbers, will later turn out to be critical for understanding many-electron atoms and the periodic table of the elements.
In 1897, Thomson demonstrated that cathode rays (observed to be emitted from the cathodes of vacuum tubes) were in fact charged particles which he called electrons. Thomson proposed that the atom consisted of a positively charged sphere in which were embedded negatively charged electrons. Rutherford subsequently found in 1911 that the electrons orbited at some distance from a central positively charged nucleus. Rutherford proposed that electrostatic attraction between the nucleus and the electron was balanced by the centrifugal force arising from the orbital motion. However, if this were the case, then the electrons (being accelerated inwards towards the center of rotation) would continuously radiate all their energy as electromagnetic waves and very quickly fall into the nucleus. In 1913, Bohr postulated two important additions to Rutherford’s theory of atomic structure: 1. Electrons can orbit the nucleus in what are called stationary states in which no emission of radiation occurs and in which the angular momentum L is constrained to have values: 2. Electrons can make transitions from one state to another accompanied by the emission or absorption of a single photon of energy E = hf thus leading to absorption and emission spectra.
The basis for the hydrogen atom planetary model, which represents the development of the Rutherford-Bohr atom model, is presented. The measurements of the atom polarizability, radius, electric and magnetic moments, as well as the Stark and Zeeman effects are given as an argument. The central paragraph of the Article is a comparison of the binding energy obtained based on wave measurement data (the Rydberg constant) and the binding energy obtained by calculation according to the data of the electron charge and mass fundamental constants and applying the principle of momentum conservation. The substantiation of the atom stability is given proceeding from the atom planetary model. The nature and mechanism of the optical spectrum formation is discussed. The substantiation of the fine structure of the hydrogen atom spectral lines is presented, proceeding from the fundamental association between the electric field strength of the electron charge and the speed of its velocity. The origin of the optical spectrum hyperfine structure is discussed within the planetary model. The difficulty in constructing an acceptable theory of the electronic structure of atoms is primarily due to the complexity of obtaining direct information on the atoms internal structure. The point is that the outermost electron shell of an atom behaves itself like an effective screen for external probing electrical fields. This circumstance sharply limits the possibilities of experimental methods for studying the intra-atomic structure. On the other hand, it is imperative that the research methods being employed be non-destructive ones in order to obtain reliable information concerning the structure of atoms. This means that the action on the atom during measurement process must meet the condition of the electron shell perturbation smallness of the atom or ion being investigated. Concerns associated with the inaccessibility of the electronic structure of atoms served as a pretext for a conclusion of the limited possibilities of the empirical method of knowing the internal structure of atoms at the proper time.
The hydrogen atom is the Rosetta stone of the early twentieth century atomic physics. The attempt to decipher its structure and properties led to the development of quantum mechanics and the unraveling of many of the mysteries of atomic, molecular, and solid state physics, and a good deal of chemistry and modern biology. Unlike the various one-dimensional model problems that we have been studying in the previous chapters, the hydrogen atom is a real physical system in three dimensions. It consists of an electron moving in a spherically symmetric potential well due to the Coulomb attraction of the positively charged nucleus. In three dimensions, the electron is not constrained to move linearly. It can execute orbital motions and, thus, has angular momentum. Not only is the total energy of the electron in the atom quantized, its angular momentum also has interesting and unexpected quantized properties that cannot possibly be understood on the basis of classical mechanics and electrodynamics. They are, however, the natural and necessary consequences of the basic postulates of quantum mechanics, as will be shown in this chapter. According to classical mechanics and electrodynamics, it is not possible to have a stable structure consisting of a small positively charged nucleus at the center of an electrically neutral atom with an electron sitting in its vicinity. For the electron not to be attracted into the positive charge, it must be orbiting around the nucleus so that the centrifugal force will counter the Coulomb attraction of the nucleus and maintain a constant electron orbit.
The description of the physical and chemical properties of matter is a central issue that has occupied the minds of scientists since the age of the ancient Greeks. In their route to dissect matter down to what cannot be divided any further, they coined the term atom , the indivisible . Matter became then a collection of atoms. More than twenty centuries had to pass until the development of a more precise concept of atom, thanks, amongst others, to the systematic studies of Mendeleyev and the establishment in 1869 of the periodic table of the elements (Mendeleyev, 1869). The discovery of the electron in 1897 and the first modern model of the atomic structure by Sir Joseph Thomson were soon refined by his student, Sir Ernest Rutherford, who in 1910 showed that an atom was made of a positively charged small nucleus and a number of negatively charged electrons that neutralize the nuclear charge. Much in the spirit of planetary systems, and drawing from the analogy between gravitational and electrostatic interactions, scientists in the beginning of the twentieth century built an image of the atom that consisted of a number Z of electrons – of elementary charge – e – orbiting around the nucleus of charge Ze . A number of experimental observations, though, were incompatible with this idea of orbiting electrons. In particular, according to the successful electromagnetic theory, charged electrons in orbital (radially accelerated) motion should radiate energy, thus decelerating and eventually collapsing onto the nucleus. Clearly, such a picture would imply that matter is essentially unstable, in flagrant contradiction with our everyday experience of the very existence of matter.
The Bohr model is historically important in the understanding of quantum physics. It gives many important results for the hydrogen atom including atomic size and ionization energy. It is sometimes referred to as a semi-classical calculation, because it includes the physics of angular momentum quantization without the full quantum mechanical description of an electron wave. It is tremendously useful for gaining physical intuition of the quantum nature of the atom. In the Bohr model of the hydrogen atom, an electron has a circular orbit with speed v and radius r about the proton. The Bohr quantization condition is that an integer number of electron (de Broglie) wavelengths must fit to the atomic circumference.