# How does the process of nucleation work for boiling liquids?

I have a somewhat clear picture how (on the molecular level) a gas turns into a liquids as it cools. When a gas has a certain temperature, its molecules on average have a high enough kinetic energy so that electromagnetic interactions cannot hold the molecules together and they are essentially free. When the gas cools, the kinetic energies are smaller and thus electromagnetic interactions between molecules start to pull the molecules together and the process of turning into a liquid begins. As more molecules lose kinetic energy, initially small numbers of molecules start to cluster up, forming "lumps" that continue growing as more molecules gather up into these clusters. I believe this process is called "nucleation".

I found this video that helps visualize the effect:

But how does the reverse take place? Let's say I'm boiling water. I have a textbook that specifically states:

During nucleation, small droplets of liquid form in gases or gas bubbles form in water as it starts to boil.

As I heat water, the average kinetic energies of the molecules increase. How does nucleation create bubbles in this situation? I understand that a bubble is a "pocket" of gas inside a liquid. If nucleation works the same way in the process of liquid turning into a gas as it works in a gas turning into a liquid, by analogy there should be some "lumps" of gas forming inside the liquid. But what would hold these gas "lumps" together as the molecules in the gas have a higher kinetic energy as the molecules around them (that are still part of the liquid)? And how do these molecules with higher energy "find" each other to start forming clusters/bubbles? Or do I have a completely wrong visualization as to how bubbles form?

Firstly, the average kinetic energy of the water has to be high enough (water obviously doesn't start to boil at room temp. and pressure the moment it is poured into a pan).

As the water gains more and more energy, small bubbles appear but don't fully rise to the surface as the energy of the gas particles is transferred to the surrounding water particles, eventually losing enough energy and becoming liquid again.

But if the energy of the gas particles is lost too slowly for this to occur they fully rise to the surface. This will only occur at a certain temp. difference i.e. the liquid has to be close to boiling temperature if not it will absorb too much energy and the bubble will become a liquid again.

A single bubble can increase in "size" (more molecules inside the bubble compared to when it started not talking about the diameter) as it rises, similar to the cluster effect you mentioned. This will only occur if the energy difference is high enough to vaporise the surrounding water molecules and not just increase their kinetic energy.

This can also not occur depending on how "violently" the water is being heated, or at which temperature the heating element is, therefore the temperature of the bubble being produced.

• Thank you but you start with "..small bubbles appear..". I was interested to know why bubbles appear in the first place as a result of nucleation. Commented Jan 2, 2019 at 20:07
• @S. Rotos it should be the same explanation. How do you select a limit to the size at which a bubble can be called small? Bubble form whenever molecules that are hot enough gather together. Otherwise it will take for ever to leave the liquid. I would have expected further Q on why objects or dirt can act as a bubble seed. I am sure I got or I was told the answer but at the moment I can't answer. Perhaps LR01 can tell us.... Commented Jan 2, 2019 at 20:20

It is difficult for the initial bubbles to appear. If you put pure filtered water in the microwave (don't try this at home), you can make a super-heated liquid that will violently boil when you put a tea bag in it. In boiling organic solvent, you use boiling stones or capillaries to prevent formation of super-heated solutions.

Commonly, bubbles start at a surface or at an impurity (heteronucleation). To start a bubble in pure water, multiple water molecules have to lose all their hydrogen bonds (typically 4) at the same time. This costs energy, lowering the kinetic energy of the molecules or their neighbors. On the other hand, when the water molecule is adjacent to a wall or a piece of dust (hydrophobic), the hydrogen bond network is already disrupted, so it costs less to make a bubble.

On a stove top, bubbles form on the bottom of the pot because the temperature there is the highest. In a microwave, they can form anywhere (not sure whether the top of the liquid is actually hotter than the bottom, depends on the way the microwave oven is built).

Bubbles get bigger as they rise to the top for two reasons: the pressure decreases (not a big difference in a pot of water, you have to go 10 m deep to double the pressure) and the bubble picks up more water molecules if the water has a temperature above the boiling point.

what would hold these gas "lumps" together as the molecules in the gas have a higher kinetic energy as the molecules around them (that are still part of the liquid)? And how do these molecules with higher energy "find" each other to start forming clusters/bubbles?

It is the opposite. If you have - say - four water molecules with very high kinetic energy going in all directions, the space in between will be the newly-formed bubble. Once it is formed, more molecules in the liquid have to separate from it and go into the bubble. And gas molecules have to bounce off the liquid-gas interface to maintain the volume of the bubble.