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Energy Levels of Hydrogen Atom Bohr Model
The Bohr model of the energy level of the hydrogen atom explains the theory of the energy level of the hydrogen atom. The Bohr model is very useful. In the past, when classical physics encountered all kinds of difficulties in the analysis of atomic structure, Bohr created this model to solve the confusion. The basis of the Bohr model lies in the quantization assumption. It is said that the electron orbits around the nucleus, which is not any orbit as the classics say, but a specific energy level orbit. This energy level orbit, other than the quantum number\ (n\),\ (n = 1, 2, 3,\ cdots\).
When\ (n = 1\), it is the ground state energy level. At this energy level, the electron has the lowest energy and is the most stable. If an electron gains energy, it can transition to a higher energy orbital, such as the excited state of\ (n = 2,3,\ cdots\).
The energy value of the energy level of a hydrogen atom, according to Bohr's theory, can be calculated by the formula\ (E_n = -\ frac {13.6} {n ^ 2} eV\). Where\ (E_n\) is the energy of the\ (n\) level. From this formula, the larger\ (n\), the smaller the absolute value of\ (E_n\), but the higher the energy.
Electrons transition between energy levels, accompanied by the absorption or release of energy. If you jump from a low energy level to a high energy level, you must absorb photons of a specific frequency, photon energy\ (h\ nu = E_ {high energy level} - E_ {low energy level}\); on the contrary, jumping from a high energy level back to a low energy level, emits photons of a specific frequency, and its frequency is also determined by the energy level difference.
Bohr model uses the idea of quantization to explain the secret of the energy level of the hydrogen atom. Although there are limitations, the progress of atomic physics has inspired future generations to explore and hide, laying a foundation for the rise of atomic structure theory.
When\ (n = 1\), it is the ground state energy level. At this energy level, the electron has the lowest energy and is the most stable. If an electron gains energy, it can transition to a higher energy orbital, such as the excited state of\ (n = 2,3,\ cdots\).
The energy value of the energy level of a hydrogen atom, according to Bohr's theory, can be calculated by the formula\ (E_n = -\ frac {13.6} {n ^ 2} eV\). Where\ (E_n\) is the energy of the\ (n\) level. From this formula, the larger\ (n\), the smaller the absolute value of\ (E_n\), but the higher the energy.
Electrons transition between energy levels, accompanied by the absorption or release of energy. If you jump from a low energy level to a high energy level, you must absorb photons of a specific frequency, photon energy\ (h\ nu = E_ {high energy level} - E_ {low energy level}\); on the contrary, jumping from a high energy level back to a low energy level, emits photons of a specific frequency, and its frequency is also determined by the energy level difference.
Bohr model uses the idea of quantization to explain the secret of the energy level of the hydrogen atom. Although there are limitations, the progress of atomic physics has inspired future generations to explore and hide, laying a foundation for the rise of atomic structure theory.
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