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'''Electron Affinity''' is a chemical property that quantifies the ability of an atom to accept an electron. It is a measure of the energy change when an electron is added to a neutral atom in the gaseous state to form a negative ion. This property is significant in the study of [[chemical bonding]], [[ionization energies]], and the [[periodic trends]] across the [[Periodic Table]].

==Definition==
Electron affinity is defined as the amount of energy released or spent when an electron is added to a neutral atom or molecule in the gas phase to form a negative ion. It is usually expressed in units of kilojoules per mole (kJ/mol) or electronvolts (eV).

==Trends in the Periodic Table==
Electron affinity varies across the [[Periodic Table]]. Generally, it increases across a period from left to right and decreases down a group. However, there are exceptions to this trend. For instance, the electron affinity of elements in Group 17 (the [[halogens]]) is particularly high due to their one electron shortfall from achieving a stable noble gas electron configuration.

==Factors Affecting Electron Affinity==
Several factors influence the electron affinity of an element:
* '''Atomic Size:''' Smaller atoms tend to have higher electron affinity because the added electron is closer to the nucleus, experiencing a stronger attraction.
* '''Nuclear Charge:''' A higher effective nuclear charge increases electron affinity as the increased charge exerts a stronger pull on the added electron.
* '''Electron Configuration:''' Atoms with a nearly full or half-full valence shell tend to have higher electron affinity because the added electron would lead to a more stable configuration.

==Measurement==
Electron affinity can be difficult to measure directly. It is often determined indirectly through various experimental techniques, such as [[photoelectron spectroscopy]].

==Applications and Significance==
Understanding electron affinity is crucial in fields such as [[quantum chemistry]], [[material science]], and [[electrochemistry]]. It helps in predicting the reactivity of elements, the stability of ions, and the formation of compounds. Electron affinity is also essential in the study of [[semiconductors]] and other materials with electronic applications.

==Examples==
* The halogens have some of the highest electron affinities because they are one electron away from having a full valence shell.
* Noble gases have low electron affinities because they already possess a complete valence shell, making them stable and less likely to accept an electron.

==See Also==
* [[Ionization Energy]]
* [[Chemical Bonding]]
* [[Periodic Trends]]
* [[Valence Electron]]
* [[Halogens]]

[[Category:Chemical Properties]]
[[Category:Physical Chemistry]]
{{Chemistry-stub}}

Electron affinity - Revision history

Prab: CSV import

Prab: CSV import