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electron affinity
In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as the amount of energy ''released'' when an electron is added to a neutral atom or molecule in the gaseous state to form a negative ion.
::X + e− → X− + energy
In solid state physics, the electron affinity for a surface is defined somewhat differently (see below).
==Measurement and use of electron affinity==
This property is measured for atoms and molecules in the gaseous state only, since in a solid or liquid states their energy levels would be changed by contact with other atoms or molecules only. A list of the electron affinities was used by Robert S. Mulliken to develop an electronegativity scale for atoms, equal to the average of the electron affinity and ionization potential.〔Robert S. Mulliken, Journal of Chemical Physics, 1934, ''2'', 782.〕〔Modern Physical Organic Chemistry, Eric V. Anslyn and Dennis A. Dougherty, University Science Books, 2006, ISBN 978-1-891389-31-3〕 Other theoretical concepts that use electron affinity include electronic chemical potential and chemical hardness. Another example, a molecule or atom that has a more positive value of electron affinity than another is often called an electron acceptor and the less positive an electron donor. Together they may undergo charge-transfer reactions.
抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』
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