Van der Waals

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Emma Scholes 1L
Posts: 62
Joined: Fri Sep 28, 2018 12:18 am

Van der Waals

Postby Emma Scholes 1L » Tue Nov 13, 2018 11:15 am

Do all molecules have Van der Waals forces?

Christopher Wendland 4F
Posts: 30
Joined: Fri Sep 28, 2018 12:29 am

Re: Van der Waals

Postby Christopher Wendland 4F » Tue Nov 13, 2018 11:20 am

Van der Waal's forces are intermolecular forces that are only present between molecules of the same composition and if the molecules are close enough together.

Aria Soeprono 2F
Posts: 64
Joined: Fri Sep 28, 2018 12:27 am

Re: Van der Waals

Postby Aria Soeprono 2F » Tue Nov 13, 2018 12:20 pm

Yes, all molecules display van der waals forces, however, the most prominent example would be in non-polar, because polar and ionic bonds have stronger forces that are more characteristic of those bonds.

Adrienne_4F
Posts: 64
Joined: Fri Sep 28, 2018 12:27 am

Re: Van der Waals

Postby Adrienne_4F » Wed Nov 14, 2018 11:08 pm

Yes, all molecules have this bond. In our notes, it states that all dispersion interactions are always present and active and Van der Waals is just another name for dispersion.

Catherine Kim 3K
Posts: 31
Joined: Fri Sep 28, 2018 12:26 am

Re: Van der Waals

Postby Catherine Kim 3K » Thu Nov 15, 2018 12:53 pm

Yes. Van der Waals forces is a general term used to describe the intermolecular forces between molecules. There are two types of Van der Waals forces - London dispersion forces and dipole-dipole forces.


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