Water behaves in mysterious ways, especially below zero before it turns into ice. Physicists have recently observed the spontaneous first steps of the ice formation process, as tiny crystal clusters as small as 15 molecules start to exhibit the recognizable structural pattern of crystalline ice.
A new study finds that liquid water does not become completely unstable as it becomes supercooled, prior to turning into ice crystals, because of an energy barrier for crystal formation in which supercooled water's compressibility continues to rise. Interestingly, liquid water becomes easier to compress, the colder it gets - unlike other substances, which become harder to compress as temperature drops.
The origin of water's compressibility behavior has been debated for decades. One possible explanation for this unusual phenomenon stems from the presence of a transition, similar to the liquid-gas transition found when water becomes vapor. The difference: in supercooled water the transition is from one phase of liquid to another, very similar, phase of liquid water, upon cooling.
The problem is that in a normal experiment, supercooled water crystallizes under the conditions at which the liquid-liquid phase transition is predicted to occur. Accordingly, the team instead examined a model describing the behavior of supercooled water, in which previous work showed a phase transition. There, they calculated the so-called free energy cost for the formation of small ice crystal nuclei. These findings help explain why water can be found in two very different solid forms that do not exhibit a crystalline structure, unlike ice in a freezer, called low-density and high-density amorphous ice.
Citation: Free energy of formation of small ice nuclei near the Widom line in simulations of supercooled water. Connor R. C. Buhariwalla, Richard K. Bowles, Ivan Saika-Voivod, Francesco Sciortino, and Peter H. Poole (2015), Eur. Phys. J. E 38: 39, DOI 10.1140/epje/i2015-15039-x