The arrangement of electrons orbiting around protons in an atom, rather than the other way around, can be explained by the interplay of two fundamental forces in nature: the electromagnetic force and the gravitational force.
The electromagnetic force is much stronger than the gravitational force at atomic scales. It is responsible for the attraction between negatively charged electrons and positively charged protons, as described by Coulomb's law. This electrostatic attraction causes the electrons to be pulled towards the positively charged nucleus.
On the other hand, the gravitational force is relatively weak compared to the electromagnetic force, especially at the scale of individual atoms. The gravitational force between the electrons and protons is negligible in comparison to the electromagnetic force, which is why it does not significantly influence the electron-proton interaction in atoms.
Furthermore, the behavior of electrons in atoms is governed by quantum mechanics, specifically by the principles of wave-particle duality and the Heisenberg uncertainty principle. Electrons are described by wave functions that determine their probability distributions within specific regions around the nucleus called orbitals. These orbitals represent the allowed energy levels and spatial distributions of electrons in an atom.
In quantum mechanics, the concept of "orbiting" is different from the classical idea of planets orbiting the Sun. Electrons do not follow well-defined circular paths around the nucleus but exist in a superposition of multiple possible states, with different probabilities of being found at various distances from the nucleus. The specific distribution of electrons in an atom's orbitals is determined by the quantum mechanical solutions to the Schrödinger equation.
In summary, the electromagnetic force, the strength of the forces involved, and the principles of quantum mechanics govern the arrangement of electrons around protons in atoms. The electrostatic attraction between electrons and protons keeps electrons near the nucleus, while the quantum mechanical nature of electrons determines their distribution in orbitals rather than distinct circular orbits.