What is electronic transition?

Electronic transition refers to the process of an electron moving from one energy level to another within an atom, atom group, or molecule. This transition occurs due to the absorption or emission of electromagnetic radiation, like light, X-rays, or ultraviolet rays. An electron changes its orbit when a photon's energy is equal to the difference between the initial (ground state) and final energy levels (excited state).

The energy of a photon is proportional to its frequency (E = h x ν) and can be used to determine the corresponding wavelength using the speed of light equation (c = λ x ν). Consequently, different wavelengths of light are absorbed or emitted, depending on the energy levels involved in the transition.

Electronic transitions are responsible for a range of phenomena, including the interaction of electrons with matter, the properties of materials, and the colors of light that we see. For instance, the absorption of ultraviolet light by a molecule's electrons leads to the breaking of its chemical bonds, which is why it's harmful to human skin. In contrast, electronic transitions in pigments in the retina allow us to see colors.

In summary, electronic transitions are fundamental to many physical and chemical phenomena that we encounter in our daily life. They help us understand how different systems interact with light and how radiation can affect matter.