How does surface area affect the Van der Waals interactions?

Well, real gases have intermolecular forces, don't they? And thus, we use the van der Waals equation of state to account for such forces: $P = (RT)/(barV...

First off, the van der Waals equation looks like this: $\mathbf(P = (RT)/(barV - b) - a/(barV^2))$ where: $P$ is the pressure in $"bar"$s. $R$ is the universal...

The attractive van der Waals forces between helium atoms are so weak that the normal boiling point of liquid helium is only about 4.2 K, but without them, helium could...

The stronger the Van der Waals forces, the higher the boiling point. To melt or boil a simple molecular substance, we only have to overcome the intermolecular forces. Looked at...

Hydrogen includes inter molecular interactions with permanent dipoles (and partial charges) between hydrogen atoms and a few other . are based on random and instantaneous dipoles which last for fractions...

Van der Walls include any kind of inter- or intra-molecular force other than covalent and ionic bonds, including all interactions between: charges and dipoles dipoles and dipoles monopoles and...

This is one of the wearker intermolecular force which is influence by temporary dipole attractions between the atoms. Usually, non polar molecules are held together by this force. However,...

As you descend the elemental halogens, $X_2$, can you reconcile the statement above with the physical states of each halogen?

This is the conventional order. Ionic bonds are of course non-molecular interactions.

........and the greater the magnitude of Van der Waals forces. The best metric to demonstrate this are the boiling points of the alkanes. As the alkanes increase in size the...