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Apple Academic Press eBooks

Quantum and Wave Characteristics of Spatial-Energy Interactions

Г. А. Кораблев, Gennady Efremovich Zaikov

Published Jul 22, 2013• 1 citation
Publisher

Abstract

Quantum conceptualizations on the composition of atoms and molecules make the foundation of modern natural science theories. Thus, the electronic angular momentum in stationary condition equals the integral multiple from Planck’s constant. This main quantum number and three other combined explicitly characterize the state of any atom. The repetition factors of atomic quantum characteristics are also expressed in spectral data for simple and complex structures.

DOI
10.1201/b15300-11

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The quantum ideas about the structure of atoms and molecules are the foundation of modern scientific theories. So, the steady angular momentum of the electron is an integer multiple of Planck's constant. It is the principal quantum number, and three others in general uniquely characterize the state of any atom. The multiplicity of atomic quantum characteristics is manifested in the spectral data for simple and complex structures. The article shows that in two-particle interactions the principle of summing the inverse quantities of subsystems energetic characteristics is carried out during the processes which occur by potential gradient, and the principle of their algebraic addition during the processes which occur against potential gradient. The authors calculated the equation of dependence of spatial and energetic parameter of free atoms from their wave, spectral and frequency characteristics.

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Quantum conceptualizations on the composition of atoms and molecules make the foundation of modern natural science theories. Thus, the electronic angular momentum in stationary condition equals the integral multiple from Planck’s constant. This main quantum number and three other combined explicitly characterize the state of any atom. The repetition factors of atomic quantum characteristics are also expressed in spectral data for simple and complex structures.
The most simple atom is hydrogen consisting of a positive proton at the center, and one negative electron swarming around it. While the proton is concentrated at the center, the electron swarms in a pattern that depends on its total energy, and its angular momentum. In the lowest energy state of the hydrogen atom, the shape of the pattern is simply a sphere, but in higher energy states the pattern resembles a dumbbell, or a three-dimensional cloverleaf. For atoms with more than one electron, each electron has its own pattern, or state. The fundamental postulate that determines the behavior of atomic electrons is that of de Broglie (1924). This states that an electron of mass, m , and velocity, υ, and therefore with momentum, p = m υ, has a wavelength, λ, associated with it that is given by λ = h / p , where h is Planck's constant. If T = m υ 2 / 2 is the kinetic energy, then the expression for the wavelength can also be written λ = hm / 2 T , so the wavelength depends inversely on the kinetic energy. Thus short wavelengths mean high energies and vice versa. Initially, this seemed to be a rather arbitrary proposal, but it has been verified by many, and differing, experiments, and has led to vast numbers of quantitatively precise interpretations of phenomena.
The foundations of quantum mechanics are analyzed, and some problems that appeared during its crea-tion and remain unsolved today are emphasized. It is shown that the introduction of variable wave number k, depending on electron coordinates, and the omission of the azimuth part of the wave function ̂ ψ, were erro-neous. Including the azimuth factor of the wave function and taking into consideration the constant value of k result in wave-equation solutions showing a discrete nodal structure of intratomic space, and arrives at a peri-odic-nonperiodic law for behavior of atomic structures. Viewing atoms as quasi-spherical neutron molecules makes it possible to understand characteristic features of the periodic table. PACS Numbers: 03.65.Bz, 03.65.Ge 1.
One of the most important developments of modern science was the emergence of the concept of energy quantization which forced its way into our previous classical understanding of matter in nature. Modern day view of matter constituents and present understanding of atomic structure basic to quantum chemistry arose in those first decades of last century. In this line, a key feature for the understanding of microscopic atomic structures and their stability was the concept of angular momentum quantization. To capture the beauty and the power of these concepts is therefore extremely relevant for apprehending the contemporary view of matter, energy and interactions in nature. In this work we present a possible alternative approach of quantizing the atomic orbit for the hydrogen's atom model proposed by Bohr without using his hypothesis of angular momentum quantization from the start. In our approach here we show that when we identify the number of photons and the quantum number for the orbit, we are led to Bohr's hypothesis as a consequence of the Planck's energy quantization.
In its beginning, quantum mechanics was approached in two completely different ways. Schrodinger, reasoning that electronic motions could be treated as waves, developed wave mechanics. The stationary states that an electron or molecule might have were analogues to standing waves set up by applying appropriate boundary conditions. Bohr’s theory could not explain the Stark and Zeeman effect, and the spectra of atoms more complex than alkali metals. In 1927, Heisenberg added one more dimension to the problem through the uncertainty principle. The postulates of any theory are a set of fundamental statements that are asked to be believed and draw conclusions from them. In classical mechanics, all dynamical variables are observables, but there are certain fundamental restrictions placed upon simultaneously measurable quantities in quantum mechanics.
The quantum ideas about the structure of atoms and molecules are the foundation of modern scientific theories. So, the steady angular momentum of the electron is an integer multiple of Planck's constant. It is the principal quantum number, and three others in general uniquely characterize the state of any atom. The multiplicity of atomic quantum characteristics is manifested in the spectral data for simple and complex structures. The article shows that in two-particle interactions the principle of summing the inverse quantities of subsystems energetic characteristics is carried out during the processes which occur by potential gradient, and the principle of their algebraic addition during the processes which occur against potential gradient. The authors calculated the equation of dependence of spatial and energetic parameter of free atoms from their wave, spectral and frequency characteristics.