Editing Electronegativity (section)

==Correlation of electronegativity with other properties==
[[Image:Sn-119 isomer shifts in hexahalostannates.png|thumb|upright=1.35|The variation of the isomer shift (''y''-axis, in mm/s) of [SnX<sub>6</sub>]<sup>2−</sup> anions, as measured by <sup>119</sup>Sn [[Mössbauer spectroscopy]], against the sum of the Pauling electronegativities of the halide substituents (''x''-axis).]]
The wide variety of methods of calculation of electronegativities, which all give results that correlate well with one another, is one indication of the number of chemical properties that might be affected by electronegativity. The most obvious application of electronegativities is in the discussion of [[bond polarity]], for which the concept was introduced by Pauling. In general, the greater the difference in electronegativity between two atoms the more polar the bond that will be formed between them, with the atom having the higher electronegativity being at the negative end of the dipole. Pauling proposed an equation to relate the "ionic character" of a bond to the difference in electronegativity of the two atoms,<ref name="NOTCB"/> although this has fallen somewhat into disuse.

Several correlations have been shown between [[Infrared spectroscopy|infrared stretching frequencies]] of certain bonds and the electronegativities of the atoms involved:<ref>See, e.g., {{cite book|author=Bellamy, L. J.|year=1958|title=The Infra-Red Spectra of Complex Molecules|location=New York|publisher=Wiley|page=[https://archive.org/details/infraredspectrao0000bell_w1a8/page/392 392]|isbn=978-0-412-13850-8|url=https://archive.org/details/infraredspectrao0000bell_w1a8/page/392}}</ref> however, this is not surprising as such stretching frequencies depend in part on bond strength, which enters into the calculation of Pauling electronegativities. More convincing are the correlations between electronegativity and chemical shifts in [[NMR spectroscopy]]<ref>{{cite journal|author1=Spieseke, H. |author2=Schneider, W. G. |year=1961|journal=Journal of Chemical Physics|volume=35|page=722|doi=10.1063/1.1731992|title=Effect of Electronegativity and Magnetic Anisotropy of Substituents on C13 and H1 Chemical Shifts in CH3X and CH3CH2X Compounds |issue=2 |bibcode = 1961JChPh..35..722S }}</ref> or isomer shifts in [[Mössbauer spectroscopy]]<ref>{{cite journal|author1=Clasen, C. A. |author2=Good, M. L. |year=1970|journal=Inorganic Chemistry|volume=9|pages=817–820 |doi=10.1021/ic50086a025 |title=Interpretation of the Moessbauer spectra of mixed-hexahalo complexes of tin(IV) |issue=4}}</ref> (see figure). Both these measurements depend on the s-electron density at the nucleus, and so are a good indication that the different measures of electronegativity really are describing "the ability of an atom in a molecule to attract electrons to itself".<ref name="definition"/><ref name="NOTCB"/>