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Energy of Photon Emitted by Hydrogen Atom
The exploration of the photon energy emitted by hydrogen atoms
The hydrogen atom is a wonderful thing in the microscopic world. Its energy level transition is related to the emission of photons, and the photon energy is really the key to physical investigation.
The energy level of the hydrogen atom, according to Bohr's theory, has the characteristics of quantization. When the hydrogen atom transitions from the high energy level to the low energy level, it must emit photons. This photon energy is exactly the difference between the two energy levels.
Let the hydrogen atom be initially at the\ (n_1\) energy level and the final state is at the\ (n_2\) energy level (\ (n_1 > n_2\)). According to Bohr's theory, the energy expression of the hydrogen atom is\ (E_n = -\ frac {13.6} {n ^ 2} eV\).
Then the energy of the emitted photon\ (E\) is:\ (E = E_ {n_1} - E_ {n_2} = -\ frac {13.6} {n_1 ^ 2} eV - (-\ frac {13.6} {n_2 ^ 2} eV) = 13.6 (\ frac {1} {n_2 ^ 2} -\ frac {1} {n_1 ^ 2}) eV\).
For example, if a hydrogen atom transitions from the\ (n = 3\) energy level to the\ (n = 2\) energy level, at this time\ (n_1 = 3\),\ (n_2 = 2\). The emission photon energy\ (E = 13.6\ times (\ frac {1} {2 ^ 2} -\ frac {1} {3 ^ 2}) eV = 13.6\ times (\ frac {1} {4} -\ frac {1} {9}) eV = 13.6\ times\ frac {5} {36} eV\ approx 1.89eV\).
It can be seen that the energy of the photon emitted by the transition energy level of the hydrogen atom varies according to the transition energy level. Clarifying this principle is of great benefit to understanding the atomic structure and the essence of light.
The hydrogen atom is a wonderful thing in the microscopic world. Its energy level transition is related to the emission of photons, and the photon energy is really the key to physical investigation.
The energy level of the hydrogen atom, according to Bohr's theory, has the characteristics of quantization. When the hydrogen atom transitions from the high energy level to the low energy level, it must emit photons. This photon energy is exactly the difference between the two energy levels.
Let the hydrogen atom be initially at the\ (n_1\) energy level and the final state is at the\ (n_2\) energy level (\ (n_1 > n_2\)). According to Bohr's theory, the energy expression of the hydrogen atom is\ (E_n = -\ frac {13.6} {n ^ 2} eV\).
Then the energy of the emitted photon\ (E\) is:\ (E = E_ {n_1} - E_ {n_2} = -\ frac {13.6} {n_1 ^ 2} eV - (-\ frac {13.6} {n_2 ^ 2} eV) = 13.6 (\ frac {1} {n_2 ^ 2} -\ frac {1} {n_1 ^ 2}) eV\).
For example, if a hydrogen atom transitions from the\ (n = 3\) energy level to the\ (n = 2\) energy level, at this time\ (n_1 = 3\),\ (n_2 = 2\). The emission photon energy\ (E = 13.6\ times (\ frac {1} {2 ^ 2} -\ frac {1} {3 ^ 2}) eV = 13.6\ times (\ frac {1} {4} -\ frac {1} {9}) eV = 13.6\ times\ frac {5} {36} eV\ approx 1.89eV\).
It can be seen that the energy of the photon emitted by the transition energy level of the hydrogen atom varies according to the transition energy level. Clarifying this principle is of great benefit to understanding the atomic structure and the essence of light.
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