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It is known that molecules at the surface are strongly attached to each other (more attraction less repulsion) than those within the bulk attraction and repulsion are balanced). This is the molecular description of the surface tension and its net direction i.e., parallel to the water surface. Briefly, considering energy (total energy cost) - the cost of excluding a surface molecule is less, than to break a molecule from bulk and evaporate it from the surface! Now, considering evaporation - the question is - why evaporation occurs towards molecules of the surface (the stronger attachment than those of the bulk) and not through molecules from the bulk (like assumed in boiling)?

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It is very unclear what is being asked here. Can you break up your paragraph and re-word things to make what you know versus what you're asking more clear? –  Brandon Enright May 2 '13 at 20:43
Check out this related question: physics.stackexchange.com/questions/10470/… –  Michiel May 6 '13 at 13:59
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