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What is the diff. between H-bonding and dipole-dipole forces (between HCl molecules) ?

What is the diff. between H-bonding and dipole-dipole forces (between HCl molecules) ?


1 Answers

AskiitianExpert Shine
10 Points
12 years ago


A hydrogen bond is the attractive force between one electronegative atom and a hydrogen covalently bonded to another electronegative atom. It results from a dipole-dipole force with a hydrogen atom bonded to nitrogen, oxygen or fluorine (thus the name "hydrogen bond", which must not be confused with a covalent bond to hydrogen). The energy of a hydrogen bond (typically 5 to 30 kJ/mole) is comparable to that of weak covalent bonds (155 kJ/mol), and a typical covalent bond is only 20 times stronger than an intermolecular hydrogen bond. These bonds can occur between molecules (intermolecularly), or within different parts of a single molecule (intramolecularly). The hydrogen bond is a very strong fixed dipole-dipole van der Waals-Keesom force, but weaker than covalent, or ionic bonds. The hydrogen bond is somewhere between a covalent bond and an electrostatic intermolecular attraction.

Dipole-dipole interactions, also called Keesom interactions or Keesom forces after Willem Hendrik Keesom, who produced the first mathematical description in 1921, are the forces that occur between two molecules with permanent dipoles. They result from the dipole-dipolemolecules. An example of this can be seen in hydrochloric acid interaction between two

Therefore, in case of HCl, H bonding and dipole dipole interactions means just the same, but not always incase of other elements too.


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