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Dispersion
A molecule is diamagnetic, if all the electrons are paired.
ethylene glycol and methanol
Yes, water shows all three types of common intermolecular forces, namely dispersion forces, dipole-dipole forces and hydrogen bonds. Dispersion forces are present at any species which consists of movable charges that can be shifted with respect to one another. Thus a dipole emerges which on his part can induce dipoles in close-by molecules. The permanent dipole of water molecules leads to dipole-dipole forces. They can be distinguished from hydrogen bonds as they are present even at angles where no significant hydrogen bonds are expected any more.
Expected based on probability.
Dispersion
methane
dipole-dipole dispersion
Induced dipole forces, or simply, london forces
dipole forces and induced dipole forces
Ammonia form hydrogen bonds.
London Force / van der Waals force
Esters have carbonyl groups which are polar, so there are dipole-dipole attractions. There will also be van der Waals forces.
Amides have some hydrogen bonding, between the lone pair on the nitrogen and the hydrogen on the nitrogen in the next molecule. There will also be van der Waals forces and a little dipole-dipole attraction.
A molecule is diamagnetic, if all the electrons are paired.
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Mercury is the liquid with the strongest surface tension.