Electron affinity refers to the energy change that occurs when a neutral atom in the gaseous phase gains an electron to form a negatively charged ion (anion). It quantifies the atom’s willingness to accept an additional electron. When an atom gains an electron, energy is released or absorbed. A higher electron affinity value signifies that more energy is released when the atom accepts an electron, indicating a stronger attraction for an extra electron. Conversely, a lower electron affinity denotes less energy released or sometimes energy absorption, suggesting a weaker attraction for an additional electron. Electron affinity is a crucial factor in understanding the chemical reactivity and behavior of elements, particularly in predicting which elements are likely to gain electrons to form stable ions or compounds. It helps explain trends in the periodic table and influences chemical reactions involving the transfer of electrons.