What happens to the energy levels of electrons in an atom when an ionic bond forms?

When an ionic bond forms, it involves the transfer of electrons from one atom to another, resulting in the formation of charged ions. In this process, an atom that loses electrons becomes a positively charged ion, while the atom that gains electrons becomes a negatively charged ion. This transfer alters the energy levels of the electrons because the configuration of the electrons around the nucleus changes significantly.

When an electron moves from one atom to another, it goes from its original energy level to a new energy level in the atom that receives it. The energy levels in an atom are quantized, meaning that electrons can only exist in specific energy states. Therefore, when electrons are transferred, they occupy different energy levels in the new atom, which corresponds to the changes in their potential energy and stability.

This transfer of electrons is a defining characteristic of ionic bonding, demonstrating that electrons do not simply remain at their original energy levels or continue to exist as they did before the bond formed.