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Bohr Theory Hydrogen Spectrum Pdf
A Brief Description of Bohr's Hydrogen Spectroscopic Theory
Ancient scholars, seeking the way to the microscopic of physics, exploring the principles of all things, and impairing the mystery of nature. Today, there is Bohr's hydrogen spectroscopic theory, which is exquisite, and the analysis is as follows.
The characteristics of the spectral lines of the hydrogen spectrum have always been valued by physicists. Theories of the past, in this explanation, are often inconsistent. Bohr came out, with his insight, and established a theory, which opened up a new way for the solution of hydrogen spectroscopy.
Bohr's theory, the first hypothesis. First, electrons move around the nucleus, and there are no arbitrary orbits. There are only specific orbits. In this orbit, electrons have a certain energy and do not radiate energy. This state is called stationary state. Second, when the electron transitions, if it transitions from the stationary state of the high-energy state to the stationary state of the low-energy state, it will radiate photons, and the energy of the photons is exactly the difference between the two stationary states; conversely, if it absorbs photons of specific energy, it can transition from the low-energy state to the high-energy state.
According to this theory, the orbital radius and energy of the electron in the hydrogen atom can be calculated. The formula of its orbital radius reveals that the quantization characteristics of the electron orbit are non-continuous and variable. The expression of energy is also quantized, which is very different from the concept of continuity in classical physics.
As for the spectral lines of the hydrogen spectrum, Bohr's theory can accurately explain. Different spectral lines correspond to different transition paths of electrons. The Balmer system is the result of the transition of the electron from the high-energy state to the energy state of\ (n = 2\); the Ryman system is the result of the transition to the energy state of\ (n = 1\). The frequency or wavelength of the spectral line obtained by its calculation is quite consistent with the experimental measurements.
Bohr's hydrogen spectroscopy theory, although not complete, has the improvement of quantum mechanics, but it is of great significance in the development of physics. Its application of quantum theory to the study of atomic structure is the first of its kind, which makes our understanding of the atomic world closer to reality, and lays the foundation for the expansion of future theories.
Today's scholars, studying Bohr's hydrogen spectroscopy theory, should think about the difficulty of their original ideas and clarify the way of their exploration, so as to inspire new ideas for future physics research.
Ancient scholars, seeking the way to the microscopic of physics, exploring the principles of all things, and impairing the mystery of nature. Today, there is Bohr's hydrogen spectroscopic theory, which is exquisite, and the analysis is as follows.
The characteristics of the spectral lines of the hydrogen spectrum have always been valued by physicists. Theories of the past, in this explanation, are often inconsistent. Bohr came out, with his insight, and established a theory, which opened up a new way for the solution of hydrogen spectroscopy.
Bohr's theory, the first hypothesis. First, electrons move around the nucleus, and there are no arbitrary orbits. There are only specific orbits. In this orbit, electrons have a certain energy and do not radiate energy. This state is called stationary state. Second, when the electron transitions, if it transitions from the stationary state of the high-energy state to the stationary state of the low-energy state, it will radiate photons, and the energy of the photons is exactly the difference between the two stationary states; conversely, if it absorbs photons of specific energy, it can transition from the low-energy state to the high-energy state.
According to this theory, the orbital radius and energy of the electron in the hydrogen atom can be calculated. The formula of its orbital radius reveals that the quantization characteristics of the electron orbit are non-continuous and variable. The expression of energy is also quantized, which is very different from the concept of continuity in classical physics.
As for the spectral lines of the hydrogen spectrum, Bohr's theory can accurately explain. Different spectral lines correspond to different transition paths of electrons. The Balmer system is the result of the transition of the electron from the high-energy state to the energy state of\ (n = 2\); the Ryman system is the result of the transition to the energy state of\ (n = 1\). The frequency or wavelength of the spectral line obtained by its calculation is quite consistent with the experimental measurements.
Bohr's hydrogen spectroscopy theory, although not complete, has the improvement of quantum mechanics, but it is of great significance in the development of physics. Its application of quantum theory to the study of atomic structure is the first of its kind, which makes our understanding of the atomic world closer to reality, and lays the foundation for the expansion of future theories.
Today's scholars, studying Bohr's hydrogen spectroscopy theory, should think about the difficulty of their original ideas and clarify the way of their exploration, so as to inspire new ideas for future physics research.
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