1. Structure of the benzene molecule on the basis of the three-electron bond

Look work at the folder, pdf-file.


Theory of three-electron bond in the four works with brief comments (REVIEW) (full version, p. 91).   http://vixra.org/pdf/1612.0018v1...


This screenshots (foto) (most with explanation) see by this link. 

My ORCID iD: 0000-0002-3725-5571 



Abstract: Using the concept of three-electron bond one can represent the actual electron structure of benzene, explain specificity of the aromatic bond and calculate the delocalization energy. It was shown, that functional relation y = a + b/x + c/x^2 fully describes dependence of energy and multiplicity of chemical bond on bond distance. In this article carbon-to-carbon bonds are reviewed. Using these dependences it is possible to calculate chemical bound energy by different bond distance or different multiplicity of chemical bond, that makes possible to calculate delocalization energy of benzene molecule.

Hückel rule (4n + 2) for aromatic systems can be written in a different form, in the form of 2n where n - unpaired number. So, we have: 2, 6, 10, 14, 18, etc. This is also true for the electron shells in the atom and aromatic systems. The principle of the interaction of fermions always one, everywhere.

The reason for the formation of the chemical bond is still not clear, in fact, there is no physical justification, as it was at the time of Bohr, since the formation of a chemical bond does not follow from the four fundamental interactions. Just imagine, a chemical bond "does not understand" that it can not be explained normally and quietly exists :). A full explanation of the chemical bond can only be provided by quantum mechanics (in the future), classical approaches simply do not work.

To understand this, it is necessary not to forget what L. Pauling did (L. Pauling, "The nature of the chemical bond", and the work of L. Pauling: Chem. Rev. 5, 173 (1928)), namely Pauling analyzed the interaction of the hydrogen atom and the proton in the entire range of lengths (he admitted that the hydrogen atom and H + on the approach are preserved and showed that the bond is not formed in this case (since there is no exchange interaction or resonance by Pauling)). Only one of the above-mentioned facts actually destroys the classical approach (attraction and repulsion by Coulomb) to explaining the chemical bond. There inevitably follows that the chemical bond is a quantum-mechanical effect and no other.

Imagine a system with two protons and one electron, but if it is treated as a hydrogen atom and a proton, then the bond can not form over the whole range of lengths. But, as Burrau showed, the bond in H2 + is formed (if we consider the system as two protons and one electron), and no one particularly doubts this, since H2 + exists. I particularly emphasize that there is only one electron (there is no inter-electronic repulsion, etc.).

After this fact, further discussions can not be continued, they do not make sense (especially to apply this to the explanation of two-electron bond or aromatic, this is a slightly different level of complexity). But nevertheless, it should be noted that quantum mechanics introduced the concept of "exchange interaction", which had no physical justification (since no fundamental interactions are altered in the interchange of electrons, but should, if a bond is formed) explained the chemical bond (more accurately, "disguised" chemical bond into the quantum-mechanical effect of the "exchange interaction"), by this, confirming that the chemical bond is indeed a quantum-mechanical effect.

The science of chemical bonding is only at the beginning of it's journey, and it is for today's students to make the most significant contribution to the theory of chemic