What type of energy change occurs during the formation of ionic bonds?

The formation of ionic bonds is an exothermic process, which means that energy is released. When oppositely charged ions come together to form an ionic compound, the potential energy of the system decreases as the ions stabilize each other through electrostatic attraction. This release of energy typically manifests as heat, which can be observed as an increase in temperature in the surroundings or as energy that could otherwise do work.

In contrast, when ionic bonds are formed, the energy of the enthalpy change is negative, signifying that energy is exiting the system. This is a fundamental concept in understanding ionic bonding, and it indicates that ionic bonds are generally stable and energetically favorable because they lead to a lower energy state compared to the separate ions.

The options that suggest energy is absorbed or that there is no energy change do not reflect the nature of ionic bond formation. Additionally, stating that energy change depends on the type of ions is misleading since, while the magnitude of energy change can vary based on ionic size and charge, the fundamental process still results in energy being released when ionic bonds form.