Talk:Intermolecular force: Difference between revisions

Content deleted Content added

Inline

Revision as of 15:59, 24 November 2005

Van der Waal's information here has a contrast to what I learnt at school.

What I learnt was Van der Waal's forces occur because of assymetrical distribution of electron clouds due to movement of electrons, instead of polarity. jynx 15:59, 24 November 2005 (UTC)[reply]

Might it be a good idea to use a different polar molecule for dipole-dipole interaction than HCl? Namely something without hydrogen. maybe Acetone or CO or any other aprotic polar molecule? Fett0001 02:13, 1 November 2005 (UTC)[reply]

I came here from "van der Waals volume" on the proline page. I found van der Waals, but what's van der Waals volume?

I believe van der Waals forces and "van der Waals volume" relate back to the van der Waals equation, which compensates for intermolecular forces and volume. I believe van der Waals volume would be the volume of a gas molecule that is accounted for by the equation. Don't hold me to that.

This page would really benefit from some real diagrams. - Omegatron 19:59, May 26, 2004 (UTC)

I don't think the Van der Waals forces should be used as a synonym for London dispersion forces. In its true definition, Van der Waals forces are those which contribute to the non-volume part of the Van der Waals equation.

@@ Line 1: / Line 1: @@
+* Van der Waal's information here has a contrast to what I learnt at school.
+What I learnt was Van der Waal's forces occur because of assymetrical distribution of electron clouds due to movement of electrons, instead of polarity. [[User:Jynx|jynx]] 15:59, 24 November 2005 (UTC)
 Might it be a good idea to use a different polar molecule for dipole-dipole interaction than HCl? Namely something without hydrogen. maybe Acetone or CO or any other aprotic polar molecule? [[User:Fett0001|Fett0001]] 02:13, 1 November 2005 (UTC)
 ----