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Table of Electronegativities (Pauling Scale) Alan D. Earhart 11/22/2016 1 H 2.20 3 Li 0.98 4 Be ... electronegativity-qr-20161107 Author: Alan D. Earhart
Periodic table of electronegativity by Pauling scale. → Atomic radius decreases → Ionization energy increases → Electronegativity increases →. See also: Electronegativities of the elements (data page) There are no reliable sources for Pm, Eu and Yb other than the range of 1.1–1.2; see Pauling, Linus (1960).
The Pauling Electronegativity Scale. The original electronegativity scale, developed in the 1930s by Linus Pauling (1901– 1994) was based on measurements of the strengths of covalent bonds between different elements.
Linus Pauling described electronegativity as “the power of an atom in a molecule to attract electrons to itself.” 1 Basically, the electronegativity of an atom is a relative value of that atom's ability to attract election density toward itself when it bonds to another atom.
This table displays the Linus Pauling derivation of electronegativities. Fluorine, the most electronegative element, has arbitrarily been given a value of 4.0. Every other element's electronegativity has been scaled accordingly.
Using this equation, Pauling found that the largest electronegativity difference was between Cs and F. Pauling set F arbitrarily at 4.0 (today, the value for F is set to 3.98) and this gives a scale in which the values for all other elements are less than 4 but still with a positive number.
Pauling scale. Linus Pauling’s model as a measure of the ionic portion of the bond between two atoms is based on their electronegativity differences. Knowledge of experimentally determined bond dissociation energies is a prerequisite.
