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.
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.
'''''Increasing strength''''' 1.London dispersion 2. dipole-dipole 3. ionic 4. covalent
The only intermolecular forces in this long hydrocarbon will be dispersion forces.
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.
O2, because it have more electrons than N2
hydrogen, London dispersion, and dipole - dipole
Cl2 is non polar.So there are london dispersion
Yes,CH4 is non polar.So it has london dispersion.
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.
Yes, the London dispersion force is very weak.
Dipole-Dipole and covalent sigma bond forces.
Dipole-dipole and dispersion