One of the most basic things we are taught in school science classes is that water can exist in three different states, either as solid ice, liquid water, or vapor gas. But an international team of scientists have recently found signs that liquid water might actually come in two different states.
Writing in an experimental paper, published in the International Journal of Nanotechnology, the researchers were surprised to find a number of physical properties of water change their behavior between 50℃ and 60℃. This sign of a potential change to a second liquid state could spark a heated discussion in the scientific community. And, if confirmed, it could have implications for a range of fields, including nanotechnology and biology.
States of matter, also called “phases,” are a key concept in the study of systems made from atoms and molecules. Roughly speaking, a system formed from many molecules can be arranged in a certain number of configurations depending on its total energy. At higher temperatures (and therefore higher energies), the molecules have more possible configurations and so are more disorganized and can move about relatively freely (the gas phase). At lower temperatures, the molecules have a more limited number of configurations and so form a more ordered phase (a liquid). If the temperature goes down further, they arrange themselves in a very specific configuration, producing a solid.
This picture is common for relatively simple molecules such as carbon dioxide or methane, which have three clear, different states (liquid, solid, and gas). But for more complex molecules, there is a larger number of possible configurations and this gives rise to more phases. A beautiful illustration of this is the rich behavior of liquid crystals, which are formed by complex organic molecules and can flow like liquids, but still have a solid-like crystalline structure.
Because the phase of a substance is determined by how its molecules are configured, many physical properties of that substance will change abruptly as it goes from one state to another. In the recent paper, the researchers measured several telltale physical properties of water at temperatures between 0℃ and 100℃ under normal atmospheric conditions (meaning the water was a liquid). Surprisingly, they found a kink in properties such as the water’s surface tension and its refractive index (a measure of how light travels through it) at around 50℃.
How can this be? The structure of a water molecule, H₂O, is very interesting and can be pictured like a sort of arrow tip, with the two hydrogen atoms flanking the oxygen atom at the top. The electrons in the molecule tend to be distributed in a rather asymmetric way, making the oxygen side negatively charged relative to the hydrogen side. This simple structural feature leads to a kind of interaction between water molecules known as hydrogen bonding, in which the opposite charges attract each other.
This gives water properties that, in many cases, break the trends observed for other simple liquids. For example, unlike most other substances, a fixed mass of water takes up more room as a solid (ice) than as a (liquid) because of the way it molecules form a specific regular structure. Another example is the surface tension of liquid water, which is roughly twice that of other non-polar, simpler, liquids.
Water is simple enough, but not too simple. This means that one possibility for explaining the apparent extra phase of water is that it behaves a little bit like a liquid crystal. The hydrogen bonds between molecules keep some order at low temperatures, but eventually could take a second, less-ordered liquid phase at higher temperatures. This could explain the kinks observed by the researchers in their data.
If confirmed, the authors’ findings could have many applications. For example, if changes in the environment (such as temperature) cause changes in a substance’s physical properties, then this can potentially be used for sensing applications. Perhaps more fundamentally, biological systems are mostly made of water. How biological molecules (such as proteins) interact with each other likely depends on the specific manner in which water molecules arrange to form a liquid phase. Understanding how water molecules arrange themselves on average at different temperatures could shed light on the workings of how they interact in biological systems.
The discovery is an exciting opportunity for theorists and experimentalists, and a beautiful example of how even the most familiar substance still has secrets hiding within.