Imagine vapor pressure as a force that molecules exert as they go from liquid to gas. The higher the temperature of the liquid, the more energy there is for molecules to use to escape from liquid to gas. Remember that boiling point is when vapor pressure equals or exceeds the atmospheric pressure. When you heat water, you increase its vapor pressure until it overcomes atmospheric pressure and boils.
Vapor pressure decreases as intermolecular attraction increases. If the molecules have high attraction to one another, they will not be as willing to enter a gas phase. Compare water and ether: Water can H-bond, and ether can only dipole-dipole bond (which is weaker); comparatively, ether's bp is 35 C and water's is 100 C.
As far as molecular weight is concerned, generally lower MW molecules will have a higher vapor pressure, lower boiling point, etc. but it also depends on the intermolecular attractions (In my water v. ether example, ether has a much higher MW than water, but also has a much higher vapor pressure)