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1.4: Fundamental Properties - Electronegativity

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    An issue with ionization potential and electron affinity is that they are defined and measured as reactions in the gas phase. Although values have been determined for molecular fragments it is still difficult to correlate with reaction trends in solution. To overcome this issue the concept of electronegativity was developed.

    Electronegativity is defined as the tendency of an atom in a molecule to attract electrons to itself. Although several electronegativity scales have been developed, that by Linus Pauling (Figure \(\PageIndex{1}\).6) is the most often used. Table \(\PageIndex{1}\).5 provides selected Pauling electronegativity values (unit less).

    Figure \(\PageIndex{1}\).6.png
    Figure \(\PageIndex{6}\): American chemist Linus Carl Pauling (1901 1994).
    Element Pauling Scale
    F 4.0
    O 3.5
    Cl 3.0
    N 3.0
    S 2.5
    C 2.5
    H 2.1
    B 2.0
    Na 0.9
    Table \(\PageIndex{1}\).5: Selected Pauling electronegativity values.

    The advantage of the Pauling electronegativity scale is that it allows the prediction of general behavior. For example, the larger the dierence in electronegativity between two elements the more ionic character or more polar the bonding interaction. Thus, a H-O bond (3.5 - 2.1 = 1.4) is more polar than a H-S bond (2.5 2.1 = 0.4).

    This page titled 1.4: Fundamental Properties - Electronegativity is shared under a CC BY 3.0 license and was authored, remixed, and/or curated by Andrew R. Barron (CNX) via source content that was edited to the style and standards of the LibreTexts platform; a detailed edit history is available upon request.