
Water, the most commonplace of liquids, is also the strangest. It has at least 66 properties that differ from most liquids – high surface tension, high heat capacity, high melting and boiling points and low compressibility. 1 school of thought is that water is not a complicated liquid but ‘2 simple liquids with a complicated relationship’. For some, this statement contradicts the basic principles of physical chemistry; for others it explains just why water behaves in such an anomalous way. Researchers have been searching for this putative liquid–liquid phase transition ever since, and evidence has slowly accumulated that it really exists. New experiments now supply what seems to be a direct observation of such a transformation between liquid states of different density – not in pure water but in solutions of the sugar trehalose. Understanding how such supercold solutions behave could have implications for biology and cryopreservation – where damage to biological tissues by ice crystals must be avoided – as well as for the water-rich states that might exist in the atmospheres of gas giants. Liquids are structurally disordered, so it’s not immediately obvious how they can support 2 distinct structures with different densities. But that does seem to be possible for liquids in which some degree of directional bonding, such as hydrogen bonds between adjacent water molecules, makes distinct local structures possible.




