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Lyman Series of Electron Transitions in Hydrogen
On the Lyman system of electron transitions in hydrogen atoms
The hydrogen atom is a microscopic wonder. Its electron transitions are changeable, and the Lyman system is particularly peculiar.
The electrons of hydrogen atoms are at different energy levels. When electrons transition from high energy levels to low energy levels, radiation is generated. The Lyman system is a series of electron transitions whose final state is the ground state ($n = 1 $energy level).
Looking at the principle, the energy of electrons follows the rules of quantization. If an electron at a high energy level transitions to a $n = 1 $energy level, the energy of the photons emitted is determined by the energy difference between the two energy levels. According to Bohr's theory, the energy level $E_n = -\ frac {13.6} {n ^ 2} eV $ ($n $is a quantum number).
Let the electron jump from the $n $energy level to the $n = 1 $energy level, and the emitted photon energy $\ Delta E = E_n - E_1 = -\ frac {13.6} {n ^ 2 } - ( - 13.6) = 13.6 (1 -\ frac {1} {n ^ 2}) eV $.
From $E = h\ nu $ ($h $is the Planck constant, $\ nu $is the photon frequency), the photon frequency $\ nu =\ frac {13.6 (1 -\ frac {1} {n ^ 2}) } {h} Hz $can be obtained. The light spectral lines corresponding to this frequency constitute the Lyman system.
The light spectral lines of the Lyman system are mostly in the ultraviolet region. Because of their high photon energy, they can provide important clues for the study of many physical phenomena. In astrophysics, we can use the Lyman spectral lines to explore the state of hydrogen in the atmosphere of stars; in atomic physics, we can also help our generation understand the mystery of atomic structure and electronic behavior.
In conclusion, the Lyman system of electron transitions in hydrogen atoms, although microscopic, is of great significance, providing a bridge for exploring the microscopic world and the macroscopic universe.
The hydrogen atom is a microscopic wonder. Its electron transitions are changeable, and the Lyman system is particularly peculiar.
The electrons of hydrogen atoms are at different energy levels. When electrons transition from high energy levels to low energy levels, radiation is generated. The Lyman system is a series of electron transitions whose final state is the ground state ($n = 1 $energy level).
Looking at the principle, the energy of electrons follows the rules of quantization. If an electron at a high energy level transitions to a $n = 1 $energy level, the energy of the photons emitted is determined by the energy difference between the two energy levels. According to Bohr's theory, the energy level $E_n = -\ frac {13.6} {n ^ 2} eV $ ($n $is a quantum number).
Let the electron jump from the $n $energy level to the $n = 1 $energy level, and the emitted photon energy $\ Delta E = E_n - E_1 = -\ frac {13.6} {n ^ 2 } - ( - 13.6) = 13.6 (1 -\ frac {1} {n ^ 2}) eV $.
From $E = h\ nu $ ($h $is the Planck constant, $\ nu $is the photon frequency), the photon frequency $\ nu =\ frac {13.6 (1 -\ frac {1} {n ^ 2}) } {h} Hz $can be obtained. The light spectral lines corresponding to this frequency constitute the Lyman system.
The light spectral lines of the Lyman system are mostly in the ultraviolet region. Because of their high photon energy, they can provide important clues for the study of many physical phenomena. In astrophysics, we can use the Lyman spectral lines to explore the state of hydrogen in the atmosphere of stars; in atomic physics, we can also help our generation understand the mystery of atomic structure and electronic behavior.
In conclusion, the Lyman system of electron transitions in hydrogen atoms, although microscopic, is of great significance, providing a bridge for exploring the microscopic world and the macroscopic universe.
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