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Energy Quantization in Hydrogen
On Quantization of Energy in Hydrogen Atoms
The energy of the hydrogen atom was mostly based on the classical theory, thinking that it can be changed continuously. However, since the theory of quantum, we can only know that it is not.
In the case of a hydrogen atom, an electron spins around the nucleus. According to classical electromagnetism, the movement of an electron generates an electromagnetic field, which must radiate energy, and eventually fall into the nucleus. In fact, the hydrogen atom is stable.
Quantum theory has been developed, thinking that the energy of the electrons in the hydrogen atom is not continuously variable, it is quantized. The electron is in a specific orbit, and each orbit has a specific energy value. The acquisition of this energy value is not arbitrary, and it must comply with specific laws.
Bohr first proposed the hydrogen atom model, determining the rules of the quantization of the angular momentum of the electron orbit. According to this, the radius and energy of the electron orbit have specific values. Electrons transition from high-energy orbitals to low-energy orbitals, radiating photons; conversely, absorbing photons. The energy of a photon is exactly the difference between the two orbitals.
As expressed mathematically, the electron energy of a hydrogen atom is\ (E_n = -\ frac {13.6} {n ^ 2} eV\),\ (n = 1,2,3,\ cdots\). This\ (n\) is also the principal quantum number. Its value is different, and the electron energy is very different.
This image of energy quantization exists not only in hydrogen atoms, but also in all atoms. However, the structure of hydrogen atoms is the simplest, so it is a model for studying energy quantization.
Looking at the image of hydrogen atomic energy quantization, we can see that the principles of the microscopic world are very different from those of the macroscopic world. The classical theory is inferior to this. The quantum theory is the key to uncovering the mysteries of the microscopic world, so that we can have a deeper understanding of the structure of atoms and the causes of spectroscopy. Although its theory is profound, it can also be glimpsed in detail, which will contribute to the progress of science.
The energy of the hydrogen atom was mostly based on the classical theory, thinking that it can be changed continuously. However, since the theory of quantum, we can only know that it is not.
In the case of a hydrogen atom, an electron spins around the nucleus. According to classical electromagnetism, the movement of an electron generates an electromagnetic field, which must radiate energy, and eventually fall into the nucleus. In fact, the hydrogen atom is stable.
Quantum theory has been developed, thinking that the energy of the electrons in the hydrogen atom is not continuously variable, it is quantized. The electron is in a specific orbit, and each orbit has a specific energy value. The acquisition of this energy value is not arbitrary, and it must comply with specific laws.
Bohr first proposed the hydrogen atom model, determining the rules of the quantization of the angular momentum of the electron orbit. According to this, the radius and energy of the electron orbit have specific values. Electrons transition from high-energy orbitals to low-energy orbitals, radiating photons; conversely, absorbing photons. The energy of a photon is exactly the difference between the two orbitals.
As expressed mathematically, the electron energy of a hydrogen atom is\ (E_n = -\ frac {13.6} {n ^ 2} eV\),\ (n = 1,2,3,\ cdots\). This\ (n\) is also the principal quantum number. Its value is different, and the electron energy is very different.
This image of energy quantization exists not only in hydrogen atoms, but also in all atoms. However, the structure of hydrogen atoms is the simplest, so it is a model for studying energy quantization.
Looking at the image of hydrogen atomic energy quantization, we can see that the principles of the microscopic world are very different from those of the macroscopic world. The classical theory is inferior to this. The quantum theory is the key to uncovering the mysteries of the microscopic world, so that we can have a deeper understanding of the structure of atoms and the causes of spectroscopy. Although its theory is profound, it can also be glimpsed in detail, which will contribute to the progress of science.
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