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Its not the number of electrons a molecule has, its the distribution of those electrons. Any lone pair of electrons and you have created a dipole moment; where there is an electron density usually there is a dipole making it NOT a London dispersion force.

Exceptions to this:

1. Symmetry. Carbon dioxide; look at its Lewis structure; its a carbon with two double bonded oxygens on either side (carbon makes four bonds totaling to 8e). Now oxygen sticks out like two arms there and each of those has two lone pair BUT there are two and like two fat kids on a see-saw they cancel out that dipole making this MOLECULE over all a lazy uninterested self cented and generally non-polarizable.

London dispersion on the other hand is mostly going to be hydrocarbons, like oil. long molecular chains of carbons and hydrogens, the occasional unsaturation but mostly stuff that gets tangled up as viscous non polar material. Not really capable of solubility we would expect between water and alcohol, more like oil in hexane or heptane.

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Q: How is the strength of London dispersion forces related to the number of electrons?
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What determines the strength of dispersion forces?

London dispersion forces are dependent on the motion of electrons, their strength increases with the number of electrons in the interacting atoms or molecules. This means that London forces increase as the atomic or molar mass increases.


How are covalent ionic dipole-dipole and London dispersion arranged in order of increasing strength?

'''''Increasing strength''''' 1.London dispersion 2. dipole-dipole 3. ionic 4. covalent


What is the intermolecular forces present in C3H8?

The only intermolecular forces in this long hydrocarbon will be dispersion forces.


Is Br2 is an induced dipole moment?

No, Br2 is actually a London dispersion. The reason that Br2 is a dispersion is because dispersion forces are weak forces that result from temporary shifts in the density of electrons in the electron clouds.


Which has the larger London dispersion forces O2 or N2?

O2, because it have more electrons than N2


Which Intermolecular forces are present in HSSH?

hydrogen, London dispersion, and dipole - dipole


Is Cl2 a London dispersion?

Cl2 is non polar.So there are london dispersion


Does ch4 have London dispersion?

Yes,CH4 is non polar.So it has london dispersion.


What is the difference between dispersion forces and hydrogen bonding?

Yes, hydrogen bonding may be the strongest force but dispersion forces (London dispersion) increases strength in bonds with size. The greater size the greater strength. Therefore, if you have a huge carbon molecule the forces might be stronger than the H-bond.


Is London dispersion force weak?

Yes, the London dispersion force is very weak.


What is the intermolecular force for CBr4?

Dipole-Dipole and covalent sigma bond forces.


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