Talk:Intermolecular force

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Contents 1 Van der Wall's information incorrect? 2 HCl as an example for a dipole-dipole reaction 3 Van der Waal's Volume? 4 Diagrams 5 Van der Waal's forces and London Dispersion Forces as a synonym 6 Polar molecules not in Symmetrical molecules 7 Intro 8 Merging Keesom force to Intermolecular Force 9 clean up

[edit] Van der Wall's information incorrect?

• 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)

See dipole, there's a short conventional division of weak intermolecular forces. Debye, Keesom, Van der Waals, etc. all studied these phenomenon from slightly different angles prior quantum mechanics, i guess hence the confuse. One could say that the uncertainty principle is working here, as the dipole moments at any given time should be exactly derivable but aren't so...  ;-)

[edit] HCl as an example for a dipole-dipole reaction

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)

[edit] Van der Waal's Volume?

I came here from "van der Waals volume" on the proline page. I found van der Waals, but what's van der Waals volume? —The preceding unsigned comment was added by PierreAbbat (talk • contribs) .

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. —The preceding unsigned comment was added by Mauvila (talk • contribs) .

Two atomic dipoles weakly attract by Van der Waals interaction, bringing the two nuclei closer. When they draw closer together, their electron clouds begin to repel each other. When van der Waals attraction balances this repulsive force, the distance is the Van der Waals radius, and atoms are at their van der Waals volume; in the space-filling molecular models the atoms are usually shown at their van der Waals radii/volumes.

In my opn some of the problems of this argument is that the title "intermolecular interaction" could better be "non covalent interaction" because many interaction are between atoms; van der waals volumes are volumes for atoms inside molecules.

83.103.67.194 13:26, 28 March 2007 (UTC)roberto90967

[edit] Diagrams

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

[edit] Van der Waal's forces and London Dispersion Forces as a synonym

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. —The preceding unsigned comment was added by 68.63.61.216 (talk • contribs) .

[edit] Polar molecules not in Symmetrical molecules

I've been told that in, say CCl4, even though the electro negativities of the Cls cause each C Cl bond to be a dipole, because of it's symmettry, it causes the overall charge to disappear, meaning that the overall molecule isn't polar whatsoever. Now, why? Surely any charge on the outside of a molecule can't cancel a like force also on the outside of a molecule. —The preceding unsigned comment was added by 82.22.102.86 (talk • contribs) .

Don't trust me on this one, but my view is that the symmetry of the dipole bonds makes each bond equally susceptible to outside influences, so would there be an environment that effects to these bonds, the molecule still would rotate, unless it'd be 'anchored' from three points, by an outside &delta+, &delta- , and some London forces. This still wouldn't effect the 4th Cl, since partial charges tend cancel themselves out, because on atomic scale they are intentionally divided parts of an Eigenstate of the molecule in question... see also entropy... Had me thinking for a while. I guess quantum chemists could say something more by some formulas... A good question, hope this helps (somethings can be taken as stated).

symmetric molecules do not have a dipole moment, so they are not polar --Spoon! 19:07, 31 August 2006 (UTC)

[edit] Intro

I reverted this:

Intermolecular forces, the component of the intermolecular bond, are electromagnetic forces...

because the grammar is unsettling and more importantly it adds no useful information. —Keenan Pepper 14:48, 31 January 2006 (UTC)

[edit] Merging Keesom force to Intermolecular Force

I've proposed a merge of the content from Keesom force to Intermolecular Force, because I believe that the term itself is far too unique to be used commonly. The term "Dipole-dipole interaction" has always been used in every textbook I have read, and the term itself redirects here. Keesom force can be made into a redirect. Kareeser|^Talk! 00:56, 13 February 2006 (UTC)

More merging may be done with [intermolecular attraction] perhaps? -Kristan Wifler

[edit] clean up

You bet this article needs a clean up. It coudn't be any more cluttered. I could have made a better article (no I couldn't). Tourskin.