This is a "sort of" idea. There is a basic idea of chemistry that all substances in a system "try" to achieve chemical equilibrium, to minimize energy of the system. All liquids have a vapor phase concentration that corresponds to the energy level of the liquid. The only question is how much is needed in the adjacent gas phase to make that true. A system where that vapor pressure is lower than the equilibrium condition will see the conversion of some solid or liquid into the gas phase.
Liquid will produce vapor until the amount of vapor returning to liquid gets into balance with the amount of liquid that is converting to vapor (the equilibrium condition). If the pressure of the gas part of the system is lower than that equilibrium pressure, evaporation will occur until the balance is achieved. That is why water may boil in vacuum. It will stop once the vapor pressure gets into equilibrium with the liquid. If you keep removing the vapor, though, the water will continue to try to raise the vapor pressure and continue to evaporate. This does consume some heat energy though, so temperature will drop, making it so the vapor pressure that is in equilibrium with the solid or liquid will drop as well, and eventually, ideally, balance will be achieved.
On earth, the warmer and higher pressure of the lower atmosphere means that more water vapor can be present int he air. That air does not sit still, though, and moves. Eventually it moves up into lower pressure and lower temperature, where there is more water vapor than the air can handle, so we get rain or snow or something. We thus have a cycle: water falls from above, accumulates on the ground, and some evaporates back intot he air to once again migrate and become rain. The system really never gets to equilibrium (the system is not homogeneous in conditions), but it never stops trying to get there.