These numbers are not quite correct. But say that you have F- in the electronic configuration 1s22s22p6: even if you have photons of energy E2p-E1s, there will be no absorption, while you would have absorption for neutral fluorine.ngc2024 said:So that means that a photon with energy corresponding to the energy difference between, say n=1 and n=2, would not be absorbed if n=3 is filled?
Just to be clear: while spectral hole burning is a manifestation of what we are discussing, it applies only to cases where there is initially absorption. In the example I mentioned, the orbitals were already filled.Chandra Prayaga said:The phenomenon is called Spectral Hole Burning.
Yes. All that has happened in your case is that you are half way through the process.DrClaude said:Just to be clear: while spectral hole burning is a manifestation of what we are discussing, it applies only to cases where there is initially absorption. In the example I mentioned, the orbitals were already filled.
Photon excitation to full orbitals refers to the process in which a photon of light is absorbed by an atom or molecule, causing an electron to move from a lower energy level to a higher energy level. This results in the electron occupying a full orbital, which is an energy state defined by the quantum mechanics of the atom or molecule.
Photon excitation to full orbitals occurs when a photon with the appropriate energy level interacts with an atom or molecule. The photon transfers its energy to an electron in the atom or molecule, causing it to move to a higher energy level and occupy a full orbital.
The consequences of photon excitation to full orbitals can vary depending on the specific atom or molecule involved. In some cases, the excited electron may quickly return to its original energy level, emitting a photon of light in the process. In other cases, the electron may remain in its excited state for a longer period of time, leading to different chemical or physical properties for the atom or molecule.
Yes, photon excitation to full orbitals can be controlled through the use of specific wavelengths of light. Different atoms and molecules have different energy levels, so by using a specific wavelength of light, the photon can be matched to the appropriate energy level to cause excitation. This can be useful in various fields such as spectroscopy and optoelectronics.
Studying photon excitation to full orbitals is important in understanding the behavior of atoms and molecules, as well as the properties of light. It is also crucial in various scientific fields such as chemistry, physics, and materials science, as it allows for the manipulation and control of atomic and molecular energy levels. Furthermore, an understanding of this process is essential in developing technologies such as lasers and solar cells.