The concept of electron spin is often misunderstood due to the misleading term "spin." In classical physics, spin typically refers to the literal spinning motion of an object around an axis. However, in the context of quantum mechanics, the term "spin" does not imply actual rotation in space.
Electron spin is an intrinsic property of electrons that is associated with their angular momentum. It is one of the fundamental properties of electrons, along with their charge and mass. The spin of an electron can be thought of as an intrinsic angular momentum, but it does not correspond to a physical rotation of the electron on its axis.
When an electron is bound to an atomic orbital, it occupies a specific quantum state characterized by a set of quantum numbers, such as the principal quantum number, orbital angular momentum, and spin. These quantum numbers describe the behavior and properties of electrons in an atom. The concept of electron spin is crucial for understanding the arrangement of electrons in atomic orbitals and their interactions.
In quantum mechanics, spin is described mathematically using spinors, which are mathematical objects that represent the quantum state of the electron. These spinors have associated probabilities that describe the likelihood of finding the electron in different states when measured.
So, to answer your question, an electron does not physically spin or rotate on its axis in the classical sense, even when it is bound to an atomic orbital. The term "spin" is used to describe the intrinsic angular momentum of the electron. This can be a source of confusion, leading some websites and forums to state that electrons do not spin. However, it's important to understand that spin is a fundamental property of electrons and plays a crucial role in quantum mechanics.