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  Paulings scale

Pauling’s scale (1932):

Pauling’s scale is based on an empirical relation among the energy of a bond and the electro-negativities of bonded atoms.

Assume a bond A-B between two dissimilar atoms A and B of a molecule AB. Let the bond energies of A-A, B-B and A-B bonds be symbolized as EA-A, EB-B and EA-B correspondingly. It might be seen that the bond dissociation energy of A-B is approximately higher than the geometric mean of the bond dissociation energies of A-A and B-B bonds that is,

EA-B > √ EA-A X EB-B

Their difference (Δ) is linked to the difference in the electro-negativities of A and B according to the equation as shown below:

Δ = EA-B - √ EA-A X EB-B
   = (XA -XB)2
 (or)
0.208 Δ =XA – XB

Here, XA and XB are the electro-negativities of A and B correspondingly.

The factor 0.208 occurs from the conversion of Kcals to electron volt.

Considering arbitrarily the electro-negativity of hydrogen to be 2.1, Pauling computed electro-negativities of other elements with the help of the above equation.

1283_paulings scale.jpg


Disadvantage of Pauling scale:

The demerits of Pauling’s scale are that bond energies are not acknowledged with any degree of accurateness for many solid elements.

 

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