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The amount of energy released when an electron is added to a neutral atom to form an anion is called electron affinity. Electron affinities are difficult to measure. Electron affinity increases going left to right across a period because of increased nuclear attraction.
Unlike electronegativity, electron affinity is a quantitative measurement of the energy change that occurs when an electron is added to a neutral gas atom. The more negative the electron affinity value, the higher an atom's affinity for electrons. Periodic Table showing Electron Affinity Trend
The electron affinity (E ea) of an atom or molecule is defined as the amount of energy released when an electron attaches to a neutral atom or molecule in the gaseous state to form an anion. X(g) + e − → X − (g) + energy
The most common units for electron affinity are kilojoules per mole (kJ/mol) or electronvolts (eV). Electron affinity also applies to molecules, in some cases. Electron affinity is the energy change when an atom gains an electron. For most elements, except noble gases, this is an exothermic process.
Electron affinity is a quantitative measurement of the energy change that occurs when an electron is added to a neutral gaseous atom. The more negative the electron affinity value, the higher the electron affinity and the more easily an electron is added to an atom.
The electron affinity (EA) of an element is the energy change that occurs when an electron is added to a gaseous atom to give an anion. In general, elements with the most negative electron affinities (the highest affinity for an added electron) are those with the smallest size and highest ionization energies and are located in the upper right ...
Electron affinity is the energy change that results from adding an electron to a gaseous atom. For example, when a fluorine atom in the gaseous state gains an electron to form F⁻(g), the associated energy change is -328 kJ/mol.
We tend to liken electron affinity to an atom’s “likelihood,” or “chance,” of gaining an electron. It is the opposite of ionization energy, the energy required to ionize a gaseous atom and consequently remove an electron.
Electron affinity, in chemistry, the amount of energy liberated when an electron is added to a neutral atom to form a negatively charged ion. The electron affinities of atoms are difficult to measure, hence values are available for only a few chemical elements, chiefly the halogens.
Electron affinities are the negative ion equivalent, and their use is almost always confined to elements in groups 6 and 7 of the Periodic Table. Defining first electron affinity. The first electron affinity is the energy released when 1 mole of gaseous atoms each acquire an electron to form 1 mole of gaseous 1- ions.