Electrons move around the nucleus in orbits. Why do they not fly away from the atom? Explain what keeps them attracted to the nucleus.
Electrons do not fly away from the atom because they revolve around the positively charged nucleus in fixed circular paths called stationary states, orbits, or shells. Since the electrons are negatively charged, they are attracted to the positive nucleus, which prevents them from flying away.
Furthermore, while moving in these stationary states, the energy of an electron remains constant. Because the electron does not lose energy while in motion, it maintains its fixed orbit without spiraling inward or escaping, ensuring the atom's stability.
Explanation
The textbook context explains that the nucleus contains all the positive charge, while electrons are negatively charged, creating an attraction that keeps electrons bound to the atom. To explain why they don't just spiral in or fly away, Bohr's model is used, which postulates that electrons move in specific 'stationary states' or 'orbits'. In these states, the energy of the electron remains constant, meaning they do not radiate or lose energy as they move, thus maintaining a stable orbit.