How did the Bohr model explain why electrons do not fall into the atomic nucleus?

In the Rutherford model that preceded Niels Bohr’s work, the atom was considered unstable because classical electromagnetic theory predicted that a charged particle moving on a curved path would continuously emit radiation, lose energy, and spiral into the nucleus.1

Bohr resolved this stability problem by proposing that electrons can only exist in specific, "allowed" orbits of fixed size and energy. By requiring that the angular momentum of the electron be quantized, Bohr limited the electrons to these discrete states.21

In this model, an electron cannot lose energy continuously; it can only change its energy level by making a "quantum leap" between these fixed orbits. The atom is completely stable in its lowest energy state (the smallest orbit) because there is no lower energy level available for the electron to occupy, thereby preventing it from falling into the nucleus.231