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van der waal

Posted: Tue Oct 29, 2019 12:32 pm
by 005391550
how can we tell which molecules will have a greater dipole-dipole or London force? aka what factors contribute to the strength of dipole-dipole interactions?

Re: van der waal

Posted: Wed Oct 30, 2019 11:35 pm
by DMuth_1J
In most cases, dipole dipole interactions are weaker than London Dispersion Forces as the former uses charges and the latter is the result of temporary dipole moments that occur between molecules.

Re: van der waal

Posted: Thu Oct 31, 2019 11:35 am
by rachel liu 3k
005391550 wrote:how can we tell which molecules will have a greater dipole-dipole or London force? aka what factors contribute to the strength of dipole-dipole interactions?

Addressing the second part of your question, dipole-dipole interactions increase as the polarity of atoms/molecules increase. Polarity is due to unequal sharing of electrons between atoms within the molecule. Hope that helps!

Re: van der waal

Posted: Thu Oct 31, 2019 1:06 pm
by KBELTRAMI_1E
are we supposed to know this already???

Re: van der waal

Posted: Fri Nov 01, 2019 3:03 pm
by BeylemZ-1B
KBELTRAMI_4I wrote:are we supposed to know this already???


This type of bonding was just touched on in lecture recently, so its ok if youre not extremely familiar with it.
These four types of interactions are all pretty much the same if I am not mistaken:
1. dispersion =
2. induced dipole - induced dipole =
3. London =
4. Van Der Waals