When an electron moves from the first energy level (also known as the n = 1 energy level or the closest orbit to the nucleus) to the second energy level (n = 2), it undergoes an energy transition. This transition is accompanied by the absorption or emission of electromagnetic radiation in the form of photons.
The energy transition occurs when the electron gains or loses a specific amount of energy. If the electron absorbs energy from an external source, such as through the absorption of light or heat, it can move to a higher energy level. Conversely, if the electron releases energy, it transitions to a lower energy level.
The energy difference between the first and second energy levels corresponds to a specific frequency or wavelength of electromagnetic radiation. According to the equation E = hf, where E represents energy, h is Planck's constant, and f represents frequency, the energy change of the electron is directly proportional to the frequency of the absorbed or emitted photons.
When an electron moves from a higher energy level to a lower one (in this case, the second energy level to the first energy level), it emits a photon. The emitted photon carries away the energy difference between the two levels, and its frequency is directly proportional to that energy difference.
These energy transitions and the accompanying emission or absorption of photons are responsible for various phenomena, including the interaction of atoms with light, the emission spectra of elements, and the absorption and emission of energy in electronic transitions. They form the basis of fields like spectroscopy, which studies the interaction between matter and electromagnetic radiation.
It's worth noting that the behavior of electrons and their energy transitions is more accurately described by quantum mechanics, which takes into account the wave-particle duality of electrons and the probabilistic nature of their behavior.