Dipole vs. Hydrogen Bonds

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Sara Sadrolsadat 1G
Posts: 39
Joined: Fri Sep 28, 2018 12:16 am

Dipole vs. Hydrogen Bonds

Postby Sara Sadrolsadat 1G » Thu Nov 08, 2018 8:10 pm

How are dipole interactions weaker than hydrogen bonds, even though dipole interactions involve polar molecules?

Alyssa Wilson 2A
Posts: 65
Joined: Fri Sep 28, 2018 12:18 am

Re: Dipole vs. Hydrogen Bonds

Postby Alyssa Wilson 2A » Thu Nov 08, 2018 8:30 pm

Dipole interactions are weaker since they occur when the partially positively charged part of a molecule interacts with the partially negatively charged part of the neighboring molecule.These intermolecular ion-dipole forces are much weaker than covalent or ionic bonds that are involved in hydrogen bonding. Hydrogen bonding is a special kind of dipole-dipole interaction that occurs specifically between a hydrogen atom bonded to either an oxygen, nitrogen, or fluorine atom. Hydrogen bonding is the strongest of the dipole-dipole interactions.

Xinyi Zeng 4C
Posts: 63
Joined: Fri Sep 28, 2018 12:18 am

Re: Dipole vs. Hydrogen Bonds

Postby Xinyi Zeng 4C » Thu Nov 08, 2018 8:33 pm

I think hydrogen bond is also a type of dipole-dipole interaction, so it is just a strong dipole-dipole interaction, and it usually occurs between polar molecules, too, as it is defined as "electrostatic forces of attraction between the protonic hydrogen of one molecule with a lone pair on a highly electronegative atom of another molecule." For hydrogen bond to be present, the molecule must have at least one H atom directly bonded to a highly electronegative element (N/O/F), and the neighboring molecule must have at least one lone pair of electrons o a highly electronegative atom (N/O/F). Due to this high electronegativity of N/O/F, the H-X (X is N/O/F) bond is usually very polar, and hence hydrogen bond is usually stronger than normal dipole interactions.


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