In the hydrogen atom, the proton and electron do not revolve around a common axis in a classical sense, as depicted in the outdated Bohr model. Instead, their behavior is described by quantum mechanics.
According to quantum mechanics, the electron in a hydrogen atom occupies certain regions around the proton called orbitals or electron clouds. These orbitals are characterized by specific energy levels, and each energy level can accommodate a specific number of electrons.
The lowest energy orbital in a hydrogen atom is called the 1s orbital, which is spherically symmetric around the proton. It represents the highest probability of finding the electron near the proton, but it does not mean that the electron is located at a fixed distance from the proton.
The electron's behavior is described by a wave function, which provides information about the electron's probable location. The wave function of the electron in the 1s orbital is spread out over space, indicating that the electron can be found at different distances from the proton within a certain probability.
Due to the wave-like nature of electrons, they do not follow a classical trajectory and do not revolve around the proton in a well-defined orbit. The concept of a shared axis or physical contact between the proton and electron is not applicable at the atomic scale.
Instead, the electron's position is described by a probability distribution, and it is more accurate to say that the electron exists in a cloud of probability around the proton. The electron and proton are held together by the electromagnetic attraction between their opposite charges, but they never come into direct contact as classical particles would.