In quantum mechanics, the behavior of electrons in atomic orbitals is described by probability distributions rather than fixed trajectories. The position of an electron in an atomic orbital is not well-defined but rather represented by a wave function that describes the probability of finding the electron in different regions of space.
The wave function of an electron in an atomic orbital can be thought of as a standing wave, and the probability distribution is given by the square of the wave function (|Ψ|^2). The square of the wave function provides the probability density of finding the electron at a particular location.
The time evolution of an electron in an atomic orbital is governed by the Schrödinger equation, which describes the behavior of quantum systems. The wave function of the electron changes with time, but the rate at which the electron changes position in an atomic orbital can vary depending on the specific orbital and energy level.
In general, electrons in higher energy orbitals tend to have more rapid changes in position compared to those in lower energy orbitals. However, it's important to note that the concept of an electron "changing position" in the classical sense is not applicable in quantum mechanics. Instead, the wave function of the electron evolves over time, reflecting the probability distribution of its location.