Abstract
This article introduces potential wells around nuclei and their roles in chemical bonds. The approach uses one-electron Bohr atomic model concept. Multi-electron atoms are converted to one-electron atoms by grounding all inactive, non-reacting electrons using the Apparent Nuclear Charge (ANC) and Electron Shielding Effect (ESE) concepts introduced in earlier publications. Then, the resulting two one-electron atoms and their potential wells are utilized to obtain the related chemical bond length. The methodology is applicable to all elements of periodic table without a need for any additional tool. To test the concept, calculated bond lengths were compared to experimental ones for about 90 different bonds, which showed an average error of less than 5%. The article discusses some nontraditional views for chemical bonds which may contradict the traditional beliefs in chemistry. Hopefully, readers would consider the calculated results in support of the presented views. Attached to this article is a computer software program which was prepared with sample input and output files for readers. The software can be utilized to obtain any interested bond length. The software is applicable to all elements in the periodic table up to the element Hassium with the atomic number of 108. Nuclear potential well associated with the electron of hydrogen atom.
Highlights
The primary objective of this article is to introduce a new approach to estimate chemical bonds within molecules
As the center of gravity of Bohr-like orbital sphere moves away from the nucleus, we would see a drop in the coulombic potential energy which would continue to decrease until the center of gravity of electronic sphere arrives at 0.370468 Ȧ distance of the nucleus
Software: This article accompanies a computer software program that might be helpful to readers to find or estimate an unknown chemical bond length using the methodology outlined in this article
Summary
The primary objective of this article is to introduce a new approach to estimate chemical bonds within molecules. To better understand the concept presented in this article, a review of earlier works seems to be essential and necessary. Bohr Atomic Model [14,15,16,17,18,19,20,21,22,23]: Niels Bohr and Ernest Rutherford atomic model presented in 1913 is a simple wellunderstood one-electron atomic model using classical mechanics. It assumes circular orbit for the electron in equilibrium under two forces. One force is the centripetal force acting on the electron due to its rotational speed which is assumed to be equal to the attracting coulombic force acting on electron by the nucleus (Eq.1)
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