Balmer equation for the atomic spectral lines was generalized by Rydberg. Here it is shown that 1) while Bohr's theory explains the Rydberg constant in terms of the ground state energy of the hydrogen atom, quantizing the angular momentum does not explain the Rydberg equation, 2) on reformulating Rydberg's equation, the principal quantum numbers are found to correspond to integral numbers of de Broglie waves and 3) the ground state energy of hydrogen is electromagnetic like that of photons and the frequency of the emitted or absorbed light is the difference in the frequencies of the electromagnetic energy levels.
Balmer equation for the atomic spectral lines was generalized by Rydberg. Here it is shown that 1) while Bohr's theory explains the Rydberg constant in terms of the ground state energy of the hydrogen atom, quantizing the angular momentum does not explain the Rydberg equation, 2) on reformulating Rydberg's equation, the principal quantum numbers are found to correspond to integral numbers of de Broglie waves and 3) the ground state energy of hydrogen is electromagnetic like that of photons and the frequency of the emitted or absorbed light is the difference in the frequencies of the electromagnetic energy levels.
Bohr ignored the electromagnetic interaction of moving charges in atoms and only considered Coulomb forces, thus encountering half frequency difficulties. This article considers the Lorentz force to make the classical Bohr model consistent with modern quantum theory, uses de Broglie's standing wave principle instead of Bohr's quantization assumption, derives the energy level formula for hydrogen atoms, and explains the radiation mechanism of hydrogen atomic spectra. The hydrogen atom in a spectral tube emits a photon wave train during one free path, and the wavelength of the photon is the eigen wavelength of its wave train. The head wavelength of the wave train is four thirds of its eigen wavelength, and the tail wavelength of the wave train is two-thirds of its eigen wavelength.
The validity of the de Broglie formula λ=h⁄p for matter waves has been confirmed by numerous experiments such as Davisson-Germer and G. P. Thomson experiments. But there is a major problem here. If λ=h⁄p is valid for matter waves, we must be able to obtain it for these waves using mathematical calculations. But as you will see here, according to de Broglie's hypothesis, which considers matter wave energy equal to E=hf, this work is impossible; and so, we must change the matter wave energy equation to obtain λ=h⁄p. The change in the equation of energy causes two important changes in Schrodinger’s wave equation. These two changes bring us to a new wave equation. In the other part of the article, you will see that, to explain the reason for the quantization of the orbits in Bohr's atomic model, we need a new atomic model for the Hydrogen atom. The new model leads us to new results and findings. In this article, we show what the cause of the quantization of the orbits in the Bohr atomic model is. In this article we have been able to show the reality and nature of Photon and we show that a Photon is an electromagnetic Pulse. In the spectrum of the hydrogen atom, for example, the intensity of Balmer-alpha is greater than Balmer-beta. Here we have been able to explain why this is the case.
The validity of the de Broglie formula λ=h⁄p for matter waves has been confirmed by numerous experiments such as Davisson-Germer and G. P. Thomson experiments. But there is a major problem here. If λ=h⁄p is valid for matter waves, we must be able to obtain it for these waves using mathematical calculations. But as you will see here, according to de Broglie's hypothesis, which considers matter wave energy equal to E=hf, this work is impossible; and so, we must change the matter wave energy equation to obtain λ=h⁄p. The change in the equation of energy causes two important changes in Schrodinger’s wave equation. These two changes bring us to a new wave equation. In the other part of the article, you will see that, to explain the reason for the quantization of the orbits in Bohr's atomic model, we need a new atomic model for the Hydrogen atom. The new model leads us to new results and findings. In this article, we show what the cause of the quantization of the orbits in the Bohr atomic model is. In this article we have been able to show the reality and nature of Photon and we show that a Photon is an electromagnetic Pulse. In the spectrum of the hydrogen atom, for example, the intensity of Balmer-alpha is greater than Balmer-beta. Here we have been able to explain why this is the case.
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.
Abstract The energies, kets and wave functions obtained from the Schrödinger equation for the hydrogen atom are examined in Chapter 9. Three quantum numbers are identified. The energies turn out to be the same as in the Bohr model, and an energy-level diagram appropriate to the quantum description is constructed. Graphs of the probability distributions are interpreted as the electron being in a “cloud” around the proton, rather than at a fixed position: the atom is fuzzy, not sharp-edged. The wavelengths of the five photons of the Balmer series are shown to be in the visible range. These photons are emitted when electrons transition from higher-excited states to the second lowest one, which means that electronic-type transitions underlie the presence of colors in our visible environment. The non-collapse of the atom, required by classical physics, is shown to arise from the structure of Schrödinger’s equation.
The validity of the de Broglie formula λ=h⁄p for matter waves has been confirmed by numerous experiments such as Davisson-Germer and G. P. Thomson experiments. But there is a major problem here. If λ=h⁄p is valid for matter waves, we must be able to obtain it for these waves using mathematical calculations. But as you will see here, according to de Broglie's hypothesis, which considers matter wave energy equal to E=hf, this work is impossible; and so, we must change the matter wave energy equation to obtain λ=h⁄p. The change in the equation of energy causes two important changes in Schrodinger’s wave equation. These two changes bring us to a new wave equation. In the other part of the article, you will see that, to explain the reason for the quantization of the orbits in Bohr's atomic model, we need a new atomic model for the Hydrogen atom. The new model leads us to new results and findings. In this article, we show what the cause of the quantization of the orbits in the Bohr atomic model is. In this article we have been able to show the reality and nature of Photon and we show that a Photon is an electromagnetic Pulse. In the spectrum of the hydrogen atom, for example, the intensity of Balmer-alpha is greater than Balmer-beta. Here we have been able to explain why this is the case.