Why do Van der Waals forces hold molecules together?

Van der Waals forces are very weak intermolecular bonds that occur as a result of rapid changes in electron density within a molecule.

Within a molecule, even if there is no overall charge or 'dipole' associated with it, the exact electron distribution will not be perfectly symmetrical and equal across the whole molecule continually. When, for example, electron density shifts from one area of a molecule to another, the original area will end up exhibiting a VERY slight positive charge effect (this is due to to the electron (negative) density moving away from it).

At this brief, almost instantaneous, moment the molecule (lets say 1) has an area of slight negative density and as a result an area of slightly positive density. Now imagine another molecule (2) which also has an area of slight negative density and slight positive density neighbours this original molecule, the area of negative density of molecule 1 will experience attraction to the slightly positive density of molecule 2 and thus the molecules will be 'held' together for that brief moment until their respective electron densities change.

The actual interaction is momentary - it does not last very long AT ALL. However, as interactions are occurring and vanishing all the time across millions of molecules in a substance, the effect is that of constant bonding between molecules.