Transition of hydrogen electron through S-orbits has been studied.Energy levels and frequencies of the emitted spectral lines were computed through new simple atomic model.The equations assume that, the energy and frequency of the emitted lines of six known series are related to enclosed areas of successive orbits and proportionality constants.These constants are strongly related to all spectral lines in all series.The results found from this model will give abroad understanding of quantum mechanics principles.
Transition of hydrogen electron through S-orbits has been studied.Energy levels and frequencies of the emitted spectral lines were computed through new simple atomic model.The equations assume that, the energy and frequency of the emitted lines of six known series are related to enclosed areas of successive orbits and proportionality constants.These constants are strongly related to all spectral lines in all series.The results found from this model will give abroad understanding of quantum mechanics principles.
On the basis of the unconventional concept of the formation of the line spectrum of the hydrogen atom, an equation is obtained that is necessary for computer calculations of the energy emitted by an electron during the transition from a certain current energy level rλ,n to the receiver radius r0. The obtained solution of the energy equation made it possible to derive the formal relations necessary for calculating the values of the radii of the levels of the hydrogen atom and, accordingly, the velocities of the electron in these orbits. The applied aspect of the considered methodology consists in using the results of the performed calculations for the problems of synthesis and analysis of quantum-electronic circuits.
This chapter has provided an alternate method of solving simple problems in atomic physics under Bohr’s model to aid good mental picture of hydrogen atom to scientists. Two values of fundamental physical properties of an electron in the hydrogen atom has been identified. By limiting the orbiting electrons to a series of circular orbits having discrete radii, Bohr could account for the series of discrete wavelengths in the emission spectrum of hydrogen. Light, he proposed, radiated from hydrogen atoms only when an electron made a transition from an outer orbit to one closer to the nucleus. These physical properties (Ve = 174090.938ms-1& Pe = 1.585860888 × 10-25kgms-1) are constant in nature. The aim for the review was to contribute to the solution of disagreement between the Bohr’s wavelength (λ0 = 91.12nm) and the Balmer’s experimental observation (λ0 = 91.18nm) for the emission spectrum of hydrogen atom. There are two other constants δ = 7.199822 × 10-10 eVm and ζ = 1503796277m-1 that were identified in the Bohr’s equation of the hydrogen atom. The four fundamental physical constants can be applied to multi-electron systems because they are inherent characteristics of an electron. They can also be derived from the steady state hydrogen atom Schrodinger's equation. For a deeper understanding, these constants may be scrutinised for their determination. The study recommends that current quantum atomic models and equations governing quantum physics should be revisited for better applications and understanding of the physical world.
The concept of quantized energy lies at the heart of quantum physics. It is shown that the visible spectrum of hydrogen consists of five spectral lines, each with a particular energy. These are shown to correspond to transitions or quantum jumps between particular energy levels of the hydrogen atom. The energy-level diagram for hydrogen is particularly simple, with the values of the energy levels from the ground state to the excited states dependent only on the principal quantum number. Spectral lines in the ultraviolet, visible, and infrared are referred to as the Lyman series, the Balmer series, and the Paschen series respectively. Other quantum numbers including the orbital quantum number, the magnetic quantum number, and the spin quantum number are introduced and the rules for combining them are described. Spectroscopic notation to describe quantum states is also explained. The 21 cm radio emission is shown to be a consequence of the spin-flip transition in hydrogen. Other quantum systems, such as molecules, are briefly described.
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.
The existence of line spectra can be explained bymeans of the first “quantum”model of the atom, developed by Bohr in 1913. Although the Bohr model of the hydrogen atom was eventually replaced, it yields the correct values for the observed spectral lines, and gives a substantial insight into the structure of atoms in general. The following derivation has the objective of obtaining the energy levels of the Bohr atom. If we can obtain the energy levels, we can reproduce the hydrogen atom spectra. The derivation proceeds with three major elements: first, use force balance to relate the velocity to the radius of the electron orbit, then use a quantum assumption to get the radius, then solve for the energies.
Based on the open-loop and closed-loop theory of Daojing, a novel physical mechanism and calculation formula for electronic transitions are proposed. The Bohr radius and the hydrogen atom energy level formula are derived. For a total of 26 hydrogen spectral lines across the Lyman, Balmer, Paschen, Brackett, and Pfund series, the theoretical calculation results are consistent with public experimental data within four significant figures. This demonstrates that quantization is an inevitable result of closed-loop stability, rather than an artificial hypothesis, and that electronic transitions are a continuous transition of closed-loop dynamic periodic modes, rather than an instantaneous quantum jump.