When an electron goes around an atom, it occupies specific energy levels or orbits known as electron shells or electron energy levels. These energy levels are quantized, meaning they have specific discrete values. The motion of electrons within an atom is described by quantum mechanics, a branch of physics that deals with phenomena on the atomic and subatomic scale.
According to quantum mechanics, the behavior of electrons is better understood in terms of wave-particle duality. Electrons can exhibit both particle-like and wave-like properties simultaneously. Rather than following a well-defined path like a planet orbiting the Sun, electrons are best described by a probability distribution or an electron cloud. This cloud represents the likelihood of finding the electron in a particular region around the nucleus.
The electron's motion around the atom is governed by the laws of quantum mechanics and is described by wave functions or orbitals. These wave functions give the probability amplitude of finding the electron at a particular location around the nucleus. Each electron energy level corresponds to a specific wave function and has a distinct shape and energy associated with it.
When an electron absorbs energy, it can transition to a higher energy level or shell, moving to an orbit that is farther from the nucleus. Conversely, when an electron loses energy, it transitions to a lower energy level, moving to an orbit closer to the nucleus. These transitions can occur through various processes, such as the absorption or emission of photons or interactions with other particles.
It's important to note that the concept of electrons "going around" the atom in a classical sense is an oversimplification. The behavior of electrons is fundamentally quantum in nature, and their precise position and momentum cannot be simultaneously known due to the Heisenberg uncertainty principle. The electron's motion is better described as existing within a probability cloud, where the electron's position can only be determined probabilistically.