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  Hydrogen bonding

Hydrogen bonding:

Hydrogen bonding comes into survival as an outcome of dipole-dipole interactions among the molecule in which hydrogen atom is covalently bonded to an extremely electronegative atom. Thus, the conditions for the effective hydrogen bonding are:

1) Very high electro-negativity of the atom bonded to hydrogen atom and hence bond is adequately polar.

2) Small dimension of the atom bonded to hydrogen and hence it is able to attract the bonding electron pair efficiently.

When the atom bonded to hydrogen has low value of electro-negativity and/or big atomic size, dipole-dipole interactions are not strong sufficient to permit efficient hydrogen bonding.

Only oxygen, nitrogen, and fluorine form strong hydrogen bonds since they have high value of electro-negativity and small atomic size.

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Strength of H-bonds:

This is a weak bond since it is merely an electrostatic force and not a chemical bond. Its strength based upon the electro-negativity of atom to which H atom is covalently bonded. Since electro-negativity of F > O > N, the strength of H- bond is in the order of H - F ......... H > H-O.....H > H-N.....H. Hydrogen bonds are too weaker than the covalent bonds. The bond strength of various bonds is in the order: Ionic bond > Covalent bond > Hydrogen bond > dipole-dipole interactions, Vander Waal’s (i.e., London forces).

 

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