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  2. Electron affinity (data page) - Wikipedia

    en.wikipedia.org/wiki/Electron_affinity_(data_page)

    Electron affinity can be defined in two equivalent ways. First, as the energy that is released by adding an electron to an isolated gaseous atom. The second (reverse) definition is that electron affinity is the energy required to remove an electron from a singly charged gaseous negative ion.

  3. Electron affinity - Wikipedia

    en.wikipedia.org/wiki/Electron_affinity

    Electron capture for almost all non-noble gas atoms involves the release of energy [4] and thus is exothermic. The positive values that are listed in tables of E ea are amounts or magnitudes. It is the word "released" within the definition "energy released" that supplies the negative sign to Δ E .

  4. Electronegativity - Wikipedia

    en.wikipedia.org/wiki/Electronegativity

    Electropositivity is a measure of an element's ability to donate electrons, and therefore form positive ions; thus, it is antipode to electronegativity. Mainly, this is an attribute of metals , meaning that, in general, the greater the metallic character of an element the greater the electropositivity.

  5. Electron configurations of the elements (data page) - Wikipedia

    en.wikipedia.org/wiki/Electron_configurations_of...

    The valence electrons (here 3s 2 3p 3) are written explicitly for all atoms. Electron configurations of elements beyond hassium (element 108) have never been measured; predictions are used below. As an approximate rule, electron configurations are given by the Aufbau principle and the Madelung rule .

  6. Metallic bonding - Wikipedia

    en.wikipedia.org/wiki/Metallic_bonding

    The atoms in metals have a strong attractive force between them. Much energy is required to overcome it. Therefore, metals often have high boiling points, with tungsten (5828 K) being extremely high. A remarkable exception is the elements of the zinc group: Zn, Cd, and Hg.

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  8. Molar ionization energies of the elements - Wikipedia

    en.wikipedia.org/wiki/Molar_ionization_energies...

    This is the energy per mole necessary to remove electrons from gaseous atoms or atomic ions. The first molar ionization energy applies to the neutral atoms. The second, third, etc., molar ionization energy applies to the further removal of an electron from a singly, doubly, etc., charged ion.

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