Dipole-Dipole vs London

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Amina Durrani 3G
Posts: 52
Joined: Sat Jul 20, 2019 12:16 am

Dipole-Dipole vs London

Postby Amina Durrani 3G » Sat Nov 09, 2019 1:04 pm

What’s the difference between Dipole-Dipole and London Forces and what’s an example of each?

Trinity Vu 1D
Posts: 53
Joined: Fri Aug 30, 2019 12:15 am

Re: Dipole-Dipole vs London

Postby Trinity Vu 1D » Sat Nov 09, 2019 2:38 pm

Dipole-dipole forces is an interaction between two polar covalent molecules such as HF. London dispersion forces are temporary induced dipole interactions that happen between non polar covalent molecules as the electron distribution fluctuates leaving one side of the molecule with more electrons and thus more negative than the other at an instant in time. An example of this would be C5H12

Qilan Li 4I
Posts: 54
Joined: Mon Jun 17, 2019 7:23 am

Re: Dipole-Dipole vs London

Postby Qilan Li 4I » Sat Nov 09, 2019 5:46 pm

Dipole-dipole interactions occur when the positively charged part of a molecule interacts with the negatively charged part of another molecule. Induced dipole-induced dipole or London dispersion forces exist between all types of molecules (polar or nonpolar). Electrons constantly move so an atom or molecule can develop a temporary (instantaneous) dipole when its electrons are distributed unevenly around the nucleus (kinda like electrons clump together on one side). A second atom or molecule then can be attracted to the appearance of the dipole in the first atom or molecule.

Rebekah Alfred 1J
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Re: Dipole-Dipole vs London

Postby Rebekah Alfred 1J » Sat Nov 09, 2019 6:06 pm

Examples of Dipole-Dipole Forces:
Image

Image

RobertXu_2J
Posts: 104
Joined: Fri Aug 30, 2019 12:17 am

Re: Dipole-Dipole vs London

Postby RobertXu_2J » Sat Nov 09, 2019 7:06 pm

London dispersion forces occur in all molecules. It refers to how, when electrons are moving randomly around the nucleus, there will always be an ebb and flow in how negatively/positively charged a particular region of that atom is. These slight imbalances that occur attract each other, so all atoms always have london dispersion forces acting between them. Dipole-Dipole on the other hand, refers to when two atoms with a positive end and a negative end, are attracted to each other.


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