New interpretation of the atomic spectra and other quantum phenomena: A mixed mechanism of classical
LC circuits and quantum wave-particle duality
We study the energy conversion laws of the macroscopic harmonic $LC $ oscillator, the electromagnetic wave (photon) and the hydrogen atom. As our analysis indicates that the energies of these apparently different systems obey exactly the same energy conversion law. Based on our results and the wave-particle duality of electron, we find that the atom in fact is a natural microscopic
LC oscillator. In the framework of classical electromagnetic field theory we analytically obtain, for the hydrogen atom, the quantized electron orbit radius. Without the adaptation of any other fundamental principles of quantum mechanics, we present a reasonable explanation of the polarization of photon, the Zeeman effect, Selection rules and Pauli exclusion principle. Particularly, it is found that a pairing Pauli electron can move closely and steadily in a DNA-like double helical electron orbit. Our results also reveal an essential connection between electron spin and the intrinsic helical movement of electron and indicate that the spin itself is the effect of quantum confinement. In addition, a possible physical mechanism of superconductivity and the deeper physical understandings of the electron mass, zero point energy, and the hardness property of electron are also provided. Finally, we show analytically that the Dirac's quantization of magnetic monopole is merely a special handed electron at absolute zero-temperature, which strongly suggests that any efforts to seek for the magneticmonopole in real space will be entirely in vain. Furthermore, it appears that the electron's spin and the magnetic monopole are actually two different concepts for one possible physical phenomenon.
An index is developed for elements and molecules by applying pairwise consistency to relativistic quantum mechanics.This index can be applied to study carcinogenic substances identified in studies on humans or primates.This index is found to be significantly different between carcinogenic and non-carcinogenic chemicals tested on rhesus monkeys.An existing theory of how some chemicals cause damage to living cells is that free radicals can react with other molecules to cause cell damage or DNA mutation.A free radical is any atom or molecule that contains unpaired electrons.Historically, this meant its spin was not zero.In quantum mechanics each molecule under consideration can be thought of as a wave function from a Hilbert space.The Hilbert space of the wave function with odd half spin is shown not to be pairwise consistent.We have previously made the hypothesis that (the spaces of wave functions of) spin zero atoms or molecules are pairwise consistent.Now the lens space L (3, q) is also pairwise consistent if q is relatively prime to 3. Thus we reason that the latter may be a limit or generalization of the Hilbert space (of wave functions of the molecule under consideration).We have defined the above index based on a function that is sensitive to both spin parity and whether it is relatively prime to 3, the space dimensions.The index can be used to extend the theory of how chemicals may cause damage to living cells.Based on the value of the index calculated from a molecule, that molecule can react with other molecules to cause cell damage or DNA mutation.
Motivation You may ask why one needs to know about quantum mechanics. Possibly the simplest answer is that we live in a quantum world! Engineers would like to make and control electronic, opto-electronic, and optical devices on an atomic scale. In biology there are molecules and cells we wish to understand and modify on an atomic scale. The same is true in chemistry, where an important goal is the synthesis of both organic and inorganic compounds with precise atomic composition and structure. Quantum mechanics gives the engineer, the biologist, and the chemist the tools with which to study and control objects on an atomic scale. As an example, consider the deoxyribonucleic acid (DNA) molecule shown in Fig. 1.1. The number of atoms in DNA can be so great that it is impossible to track the position and activity of every atom. However, suppose we wish to know the effect a particular site (or neighborhood of an atom) in a single molecule has on a chemical reaction. Making use of quantum mechanics, engineers, biologists, and chemists can work together to solve this problem. In one approach, laser-induced fluorescence of a fluorophore attached to a specific site of a large molecule can be used to study the dynamics of that individual molecule. The light emitted from the fluorophore acts as a small beacon that provides information about the state of the molecule.