The electron in a hydrogen atom moves around the nucleus due to the electromagnetic force of attraction between the positively charged nucleus (containing the proton) and the negatively charged electron. This force is governed by the laws of quantum mechanics.
In quantum mechanics, electrons are described by wavefunctions that represent the probability distributions of their positions. These wavefunctions determine the likelihood of finding the electron in different regions around the nucleus. The behavior of electrons in atoms is described by the Schrödinger equation, which is a fundamental equation in quantum mechanics.
The Schrödinger equation allows us to calculate the allowed energy states, or orbitals, of the electron in the hydrogen atom. These orbitals describe the three-dimensional regions where the electron is likely to be found. The lowest energy orbital is called the 1s orbital, which is spherically symmetric around the nucleus. Higher energy orbitals have more complex shapes.
The electron moves around the nucleus by occupying these different orbitals or energy states. However, it's important to note that the motion of the electron in an orbital is not the same as the motion of a planet around the sun. Electrons do not follow classical trajectories but exist in a superposition of states with different probabilities.
The electron's movement can be thought of as existing in a cloud of probability, where the electron is more likely to be found in certain regions compared to others. The exact location of the electron within an orbital is uncertain and is described by its wavefunction.
Overall, the electron's movement around the nucleus in a hydrogen atom is a consequence of the attractive electrostatic force between the positively charged nucleus and the negatively charged electron, as described by the principles of quantum mechanics.