Electron affinity refers to the energy change that occurs when a neutral gaseous atom gains an electron to form a negatively charged ion. It is a measure of an atom's tendency to accept an electron.
When an atom gains an electron, the electron is added to its outermost electron shell or subshell, resulting in the formation of a negative ion. Electron affinity is quantified as the energy released or absorbed in this process. A positive electron affinity indicates that energy is released when an electron is gained, while a negative electron affinity signifies that energy is absorbed.
Electron affinity is influenced by several factors, including the atomic structure, electronic configuration, and the distance between the nucleus and the electron being added. Elements with high electron affinity have a strong attraction for electrons and readily accept them, whereas elements with low electron affinity have a weaker attraction and are less likely to gain electrons.
Electron affinity is an important concept in understanding chemical reactions and the formation of ionic compounds. It helps predict the behavior of elements when interacting with other elements to form compounds and can provide insights into an element's reactivity and stability.
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