MuonMinus said:How would you explain, on a basic level, why only one photon (as opposed to two, three...) is emitted when an electron in an atom changes its energy level? This is for students with only introductory Physics background.
Photon emission in electronic transitions refers to the process in which an electron in an atom or molecule moves from a higher energy state to a lower energy state, emitting a photon of light in the process. This is a fundamental process in the field of quantum mechanics and is responsible for the emission of light in various phenomena such as fluorescence and phosphorescence.
Photon emission occurs when an electron in an excited energy state loses energy and transitions to a lower energy state. This loss of energy is emitted as a photon of light with a specific wavelength that corresponds to the energy difference between the two states.
The energy of the emitted photon is determined by the energy difference between the initial and final energy states of the electron. This difference in energy is dependent on the specific atom or molecule and the electronic configuration of the electron.
The color of light emitted in an electronic transition is determined by the energy of the photon. Light with shorter wavelengths (higher energy) appears blue or violet, while light with longer wavelengths (lower energy) appears red or orange. Therefore, the color of light emitted in electronic transitions can provide information about the energy states of the electron and the substance emitting the light.
Photon emission in electronic transitions has numerous applications in everyday life, including fluorescent lighting, LED displays, and laser technology. It is also essential in fields such as spectroscopy, where the emitted photons can provide valuable information about the molecular structure of a substance.