How do the electron orbits work?
Each orbit around the nucleus represents an energy level, and electrons cannot exist in between orbits. Orbits closer to the nucleus have lower energy. If energy is added, an electron can be “excited” to jump to a higher energy level–an orbit farther from the nucleus. Eventually, though, the electron will return to its original state, and the atom will give off energy equal to the difference between the two orbits. In some materials, the energy is given off as X-rays; other materials produce specific colors of visible light, or other types of electromagnetic energy. Each orbit can hold only a certain number of electrons. The lower-energy orbits must fill up first, if the atom is to be at its “ground” state. This is the lowest energy state and therefore most stable state. With more research, scientists discovered that atomic structure is more complex, and that the Rutherford-Bohr model contained serious flaws.
