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  Applications of electronegativity

Applications of electronegativity:

1) Nature of bond:

The concept of electronegativity can be utilized to predict whether the bond between alike or unlike atoms is non-polar covalent bond, polar covalent bond or ionic bond.

i) When XA = XB, that is, XA-XB = 0, then A-B bond is non polar covalent bond or just covalent bond and is symbolized as A-B. Example, H-H bond in H2 molecule is a covalent bond and is symbolized as H-H bond.

ii) When XA is slightly bigger than XB, that is, XA - XB is small; the A-B bond is polar covalent bond and is symbolized as Aδ--Bδ+. Example, the O-H bonds in H2O molecule is polar covalent bonds and are symbolized as Oδ--Hδ+, as XO > XH and XO - XH is small.

iii) When XA >> XB, i.e., XA - XB is very big, A-B bond is more ionic or polar bond and is symbolized as A--B+,  as XA >> XB. For illustration Na-Cl bond in Na Cl molecule is an ionic bond and is symbolized as Na+Cl- (Here Cl = A and Na = B).

2. Percentage of ionic character in a polar covalent bond:

Pauling predicted the percentage of ionic character in different Aδ-–Bδ+ polar covalent bonds from recognized (XA–XB) values and has derived the conclusions shown below:

(i) When (XA–XB) = 1.7, the quantity of ionic character in Aδ-– Bδ+ bond is 50% and that of covalent character is also 50%. Therefore A-B bond is 50% ionic and 50% covalent.

(ii) When (XA–XB) < 1.7, the quantity of ionic character in Aδ-– Bδ+ bond is less than 50% and that of covalent character is greater than 50%. Therefore Aδ-– Bδ+ bond is principally covalent and therefore is symbolized as A–B.

(iii) When (XA–XB) > 1.7, the quantity of ionic character in Aδ-– Bδ+ bond is greater than 50% and that of covalent character is lower than 50%. Therefore Aδ-– Bδ+ bond is mostly ionic and therefore is symbolized as A–B+.

 

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