How does water behave at its surface and the role hydrogen bonding plays in this behavior?

Answer 1

In any pure liquid, the molecules within a few molecular diameters of the surface of the interface of the pure liquid with some other fluid have more average kinetic energy than do those molecules of the pure liquid that are deep within the liquid volume. This phenomenon, often called "surface tension", arises because the attractive forces between molecules that cause a gas to condense into a liquid can not be as strong in molecules at the interface, since a molecule at the interface is in contact with only half as many other molecules of the liquid as are the molecules within its interior.

This effect is particularly strong in water because of its extensive "hydrogen bonding" in liquid phase. The average cohesive energy from hydrogen bonding in water is considerably greater than the average energy of the van der Waals forces that cause most liquids to cohere, so that water has one of the highest quantitative surface tensions known.

Answer 2

Well it is actually quite simple, first you look at the question. Make sure you understand. Then you will open your text book and read about it rather than looking it up, because it helps you if you read and learn about it rather than looking for a quick answer on the internet.