Water and its phases
There is already so much to learn about phases and phase transitions in water
I’m working on a much longer post on phases and phase transitions for next week1, but in the meantime, let me share with you some cool facts about water and its “phases.”
\We all know about solids, liquids, and gases from school. Heat up ice, and you get water; heat up water, and you get vapor. We may even have been slightly baffled if we saw this phase diagram with “pressure” added to the mix
I see here a solid phase, a liquid phase, and a gas phase, but what is this “Critical point”? If you tune your temperature and pressure just right you can smoothly cross over from liquid to gas without ever undergoing a phase transition. Without getting into the molecular details, we can think of phases as particular valleys between mountains, and water wants to reach the absolute lowest point. Sometimes there are two valleys, but one is lower, and sometimes there is just one valley.
In fact, this “number of valleys” is why we see this odd behavior. If we sit at 100 degrees C and decrease or increase the pressure, there are two energy minima2—two valleys. At small pressure, the deepest valley is on the gas side, and at large pressure, the deepest valley is on the liquid side. As you then tune pressure across that one-bar point, one valley gets deeper than the other—it’s the true minimum! Yet, to get from one valley to the next, you need some energy to get you over that mountain in between. That’s the phase transition. However, that's not the only option. As the temperature increases, the mountain in between gets smaller and smaller until, at the critical point, it finally disappears, and the two valleys merge.
Without two distinguished valleys, there is no need to scale the mountain and no need for a phase transition. Liquid smoothly and easily becomes gas. At the temperatures above the critical point, you cannot meaningfully distinguish water and gas. OK, so perhaps we only have two phases?
Not quite; look at this more fleshed-out version of the phase diagram:
When ice forms, it adopts a low-energy crystal structure. However, there are numerous crystal structures to choose from. In fact, as you change pressure and temperature, it can completely reorganize how the ice bonds together into a crystal. This leads to over 20 phases of ice, labeled by some of the Roman numerals above.3
Then what are the phases? Solids undergo their own phase transitions—structural phase transitions. Are these not phases of matter? If they are, then we have already exceeded our three phases of matter just within water. But phases go beyond temperature and pressure. They also possess a multitude of interesting properties, particularly at that critical point. We'll cover some of that in detail next week.
We’ll be making our own phase! Related, of course, to a known phase transition.
For most of the phase diagram, there is one absolute minimum, and the other is a “metastable” or local minimum.
For those interested, this Wikipedia article has a lot of information on the phases of ice.