What is ionization potential?

Ionization potential, often referred to as ionization energy, is defined as the amount of energy required to remove an electron from an atom or ion in its gaseous state. This fundamental concept plays a crucial role in understanding the reactivity and chemical properties of elements. The higher the ionization potential, the more energy is needed to detach an electron, indicating a stronger attraction between the electrons and the nucleus.

This concept is particularly important in the study of periodic trends; for instance, as one moves across a period in the periodic table, ionization potential generally increases due to the increasing nuclear charge, which pulls electrons closer to the nucleus. Conversely, as one moves down a group, the ionization potential typically decreases because of the increased distance between the nucleus and the outermost electrons, making them easier to remove.

In contrast, the other terms provided do not accurately define ionization potential. Stability refers to an atom's tendency to maintain its state, the mass of an electron is a specific physical property without direct relevance to ionization, and energy released during ion formation addresses a different aspect of atomic interactions concerning ionic bonds and lattice energy.