Van Der Waals

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Michael Du 1E
Posts: 117
Joined: Sun Sep 22, 2019 12:16 am

Van Der Waals

Postby Michael Du 1E » Sat Nov 09, 2019 10:14 pm

How do we know if a lewis structure or molecule has a van der waal intermolecular force? What do we look at?

Jacey Yang 1F
Posts: 101
Joined: Fri Aug 09, 2019 12:17 am

Re: Van Der Waals

Postby Jacey Yang 1F » Sat Nov 09, 2019 10:37 pm

All molecules have van der Waals forces because their electrons are constantly moving around and creating temporary dipoles.

TimVintsDis4L
Posts: 104
Joined: Sat Aug 17, 2019 12:17 am

Re: Van Der Waals

Postby TimVintsDis4L » Sat Nov 09, 2019 10:40 pm

Van Der Waals - the weakest interaction and is present in all compounds, something like Iodine and Argong

Dipole-Dipole - stronger, between more positively charged element and negative. An example being Carbon and Oxygen

Hydrogen Bond- strongest, essentially a super bond between H and C,N,O,F

305416361
Posts: 50
Joined: Fri Aug 09, 2019 12:17 am

Re: Van Der Waals

Postby 305416361 » Sat Nov 09, 2019 11:59 pm

Van Der Waals forces, or London dispersion forces (LDFs), are the weakest form of interactions and are always present in every bond, because all bonds require at least some sort of attraction between atoms/molecules

805422680
Posts: 103
Joined: Sat Sep 14, 2019 12:16 am

Re: Van Der Waals

Postby 805422680 » Sun Nov 10, 2019 12:35 am

All molecules generally possess Van Der Waals forces due to the varying electron density distribution that occurs as a result of the electron cloud moving which temporarily creates a dipole, which can then induce other surrounding molecules to form dipole moments in them.

805291863
Posts: 100
Joined: Sat Sep 14, 2019 12:16 am

Re: Van Der Waals

Postby 805291863 » Sun Nov 10, 2019 10:37 am

As long as a molecule has electrons, it will have Van Der Waals interactions. Therefore, all molecules do


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