Can water (liquid) be hotter than boiling point?

Can a liquid be heated passed its boiling point before converting to its gaseous form? I'm not referring to changing the pressure (suppose we fix the surrounding pressure).
Water boils at 100 deg C, but I guess I'm looking for clarification about how this happens.
Does the water inside (the parts of the liquid that are not at the border of surrounding gas) surpass 100 deg C? I guess I'm just looking for clarification since it's been some time since I've taken chemistry/thermodynamics and was curious.
Is it the water molecules at the edge of surface that will turn to gas once they hit 100 deg C? Are the water molecules in liquid form slightly higher "inside" the liquid?


I was looking at this article: <https://en.wikipedia.org/wiki/Superheating>
and was curious about the statement for "Cause" where it states: "For the bubble to expand, the temperature must be raised slightly above the boiling point to generate enough vapor pressure to overcome both surface tension and ambient pressure."


Thank you!




Yes it can. It is one of the reasons why, performing a distillation, you gently stir the liquid in the lower round bottom flask.


If you distill under reduced pressure, superheating of liquids is even more prominent so that you may add [boiling chips](https://en.wikipedia.org/wiki/Boiling_chip) to the (still cold) stirred liquid, or that you rotate the flask containing the mixture from which you want to remove e.g., the solvent of reaction with a [rotary evaporator](https://en.wikipedia.org/wiki/Rotary_evaporator)


[![enter image description here](https://i.stack.imgur.com/qt1F8.jpg)](https://i.stack.imgur.com/qt1F8.jpg)


(image credit: [Wikipedia](https://en.wikipedia.org/wiki/Rotary_evaporator)).


In the later case, the distillation no longer occurs from the bulk of the solvent, but from the thin film of the liquid on the inner wall of the rotating round bottom flask.


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