Final answer:
As an electron moves closer to the nucleus of an atom, it releases energy, typically in the form of electromagnetic radiation, due to the attraction between its negative charge and the positive charge of protons in the nucleus.
Step-by-step explanation:
As an electron moves closer to the nucleus, it releases energy. This concept is drawn from the principles of atomic physics and quantum mechanics, as described in the Bohr model of the atom. According to Bohr's model, electrons orbit the nucleus at discrete energy levels or shells. Each shell corresponds to a specific energy state, with the energy increasing the further away the electron is from the nucleus.
When an electron moves to a lower energy level closer to the nucleus, it must emit energy, which is often in the form of electromagnetic radiation, to maintain energy conservation. Conversely, moving an electron to a higher energy level away from the nucleus requires the absorption of energy. This interaction between electromagnetic radiation and electrons explains the discrete lines observed in the spectra of elements, which are indicative of quantized electronic energies.
The attraction between the positive charges of the protons and the negative charges of the electrons is a fundamental force in the nucleus-electron relationship within an atom. In other words, the electrostatic force causes negative electrons to be attracted to the positive protons. This attraction means an electron must lose energy to move towards the nucleus, against the electrostatic repulsion of other electrons and the increase in coulomb potential near the nucleus. Consequently, electrons in higher energy orbits (at greater distances from the nucleus) possess higher energy levels thanks to their increased separation from the nuclear positive charge.