London Dispersion forces

[Neha Gupta 2A]

Just to clarify, do all molecules experience London dispersion forces or only some? I thought that they were present in all molecules but in Sapling I had to choose between London dispersion forces and other types of forces so I wasn't sure.

[Summer_Corona 3L]

I remember in lecture that Lavelle said dispersion interactions are always present/occurring because of electron density fluctuating which causes fluctuating induced dipole- induced dipole moments.

[Kaitlyn Hernandez 3I]

I believe that all molecules have london dispersion forces. The strength of these forces increase with the number of electrons (larger molecules have stronger forces).

[Jaden Haskins 2E]

All molecules do exhibit London dispersion forces! They exist between ionic and covalent molecules, in both polar and non polar molecules. For my sapling question at least, it was dispersion and dipole-dipole, but the answer should be one that has both unless the question asked just for the strongest force.

[Veeda Khan 2E]

As everyone else said above, all molecules experience LDF, but it's pretty weak.

[Chudi Onyedika 3A]

Yes, because electrons will have uneven distribution that results in a temporary dipole.

[Tatyana Bonnet 2H]

Yes all molecules have London dispersion forces, and it is one of the weakest intermolecular forces. When two molecules come in close proximity they "induce" a partial negative/positive on each other instantaneously making it temporary.

[Chris_Butler_1A]

Yes all molecules have London dispersion forces, and it is one of the weakest intermolecular forces. When two molecules come in close proximity they "induce" a partial negative/positive on each other instantaneously making it temporary.

I'm unsure if I am correct on this but I believe it was mentioned that elements further to the lower-right of the periodic table tend to see these kinds of interactions more due to the larger number of electrons present within their shells.

[Joanne Yuh 3I]

Yes, all molecules have London Dispersion Forces. Professor Lavelle said in his lecture that these forces are "always present and attractive." I think this is because the electron densities are always fluctuating, which cause the dipoles to also fluctuate.

[Ayesha Aslam-Mir 3C]

This might be a silly question but are LDF's, dipole induced dipole, and induced dipole-induced dipole the same? My mind is spinning at hte use of the word dipole over and over ahaha.

[joshtully]

All molecules experience London Dispersion Forces.

[Kushaal Madadi 2F]

Would anyone be able to elaborate why the charges are always fluctuating throughout the two molecules so that each atom is delta negative for some time and then delta positive?

[LovepreetSran_3H]

Yes, all molecules do have London dispersion forces.

[Hasan Mirza 3F]

All molecules experience London Dispersion forces. The sapling problem was probably asking you to choose the most apparent force present.

[Geethika Janga 1L]

All molecules do experience London Dispersion Forces but when it comes to problems like that, I think they want us to focus on the stronger intermolecular forces and if there are other forces present, LDFs will always be the weakest.