Physical chemistry

Water's response to the fear of water

Spectroscopic analysis reveals that, at low temperatures, hydrophobic molecules dissolved in water strengthen the hydrogen bonding between nearby water molecules. But at high temperatures, the reverse can be true. See Letter p.582

Water-repellent molecules are said to be hydrophobic — which, literally translated, means they have a fear of water. But unlike human phobias, the effects of the molecular fear of water are difficult to predict. For example, if a nanometre-scale hydrophobic ball is inserted into liquid water, one might expect it to break up the hydrogen bonds between water molecules, thus strongly increasing disorder. The actual outcome, however, is much more complex, and so the effects of hydrophobic solutes on the structure of their hydration shells — the layers of water molecules that surround the solutes — have been a topic of debate for almost 70 years. On page 582 of this issue, Davis et al.1 present an invaluable contribution to the discussion by showing that hydrophobic groups in molecules in fact enhance the ordering of the surrounding hydrogen-bond network of water.

The debate about the effect of hydrophobic molecular groups on water goes back to the work of Frank and Evans2 in the 1940s. They discovered that the hydration of such groups is associated with a decrease of entropy. In addition, they observed that the heat capacity of the resulting solutions becomes anomalously high. Both these effects suggest that a hydrophobic solute induces a strong ordering of the surrounding water. On the basis of these findings, Frank and Evans formulated the 'iceberg' model for hydrophobic hydration2. In this model, hydrophobic solute molecules create ice-like 'clathrate' structures in the surrounding water. The high local order of these structures could explain the observed entropy decreases associated with the hydration of hydrophobic molecules, whereas 'melting' of ice-like hydration shells could account for the large increases in heat capacity.

During the subsequent decades, the iceberg model has been severely challenged, in particular by neutron-diffraction studies. In these studies, the distance between water molecules near hydrophobic solutes was found to be quite similar to that in bulk liquid water, thereby casting serious doubts on the existence of any local ice-like structures3,4. Moreover, theoretical studies have shown that the thermodynamics of hydrophobic-molecule hydration do not require the surrounding water to be different from bulk water — the observed entropy decrease can be explained as the effect of the exclusion of water from the volume taken up by the molecule5. The water around a solute can maintain the same amount of hydrogen bonding as in the bulk liquid, at least for small hydrophobic solutes (less than 1 nanometre in diameter), in the same way that one can create a hole in a loosely woven fabric without breaking the threads.

Davis and colleagues' experiments shed fresh light on the structure of water surrounding hydrophobic solutes, using a spectroscopic method called Raman multivariate curve resolution. This method allows spectral features associated with the vibrational modes of water molecules hydrating the solute to be selectively extracted. Specifically, the authors obtained the spectra of water molecules that were locally hydrating alcohol molecules, for a variety of alcohols bearing hydrophobic groups of different lengths. By focusing on the spectral features corresponding to vibrations of water's hydroxyl (OH) groups, they obtained information about the strength and the distribution of hydrogen bonds around the alcohols' hydrophobic groups. The authors observed that the hydrogen-bond network in this region is significantly enhanced — that is, more ordered than in bulk liquid water.

How should one envisage this enhanced hydrogen-bond structure? It cannot be truly ice-like, because this would contradict the previous neutron-scattering data. The picture that emerges is that the methyl (CH3) and methylene (CH2) groups of the alcohols' hydrophobic groups form ideal templates around which the water network can fold, leading to locally enhanced, tetrahedral order. This network will consist of ridges approximately 0.3 nm in height (the intermolecular distance of the water molecules), with ridge angles of 104.5° (the intramolecular bond angle of the water molecule), as is generally the case for hydrogen-bond networks in water.

Davis et al. further found that the enhanced hydrogen-bond structure vanishes when the temperature of the solution is increased. For instance, they observed that the hydrogen bonding of the hydration shell of n-pentanol (C5H11OH) at 60 °C is similar to that of bulk water. This finding is in line with the original ideas of Frank and Evans: the ordered water structures surrounding hydrophobic groups 'melt' upon an increase in temperature.

The enhanced hydrogen-bond structure of the hydration shell and its disappearance upon heating have counterparts in the shells' dynamics. The molecular reorientation of water primarily proceeds through the transient formation of defects in its hydrogen-bond network — particularly the formation of bifurcated hydrogen bonds6, in which a single hydrogen atom contributes to two hydrogen bonds. The fact that water is excluded from the volume filled by a solute reduces the rate of formation of defects in hydration shells7, an effect that is amplified by the enhancement of the hydrogen-bond network. So, water molecules hydrating a hydrophobic group should undergo slower reorientations than those in the bulk, as is indeed observed in spectroscopic studies8,9,10. As temperature increases, the enhanced hydrogen-bond structure gradually vanishes, which means that the density of weak and/or defective hydrogen bonds also increases. On heating, therefore, the orientational dynamics of water in hydration shells ought to speed up more than the dynamics of bulk water. Again, this effect has been observed8,9,10.

Davis et al. report another interesting effect for alcohols that have hydrophobic chains longer than 1 nm — at temperatures above 80 °C, the water surrounding the hydrophobic chains acquires a structure that is less ordered than bulk liquid water at the same temperature. This phenomenon has been predicted by theory5, and brings us back to the effect of inserting a hydrophobic ball into water: for a large ball with a diameter greater than 1 nm, the curvature of its surface does not fit into the three-dimensional arrangement of the hydrogen bonds of water, and so causes hydrogen bonds near the ball's surface to break up5. There is thus a striking difference between small hydrophobic structures of about 0.5 nm in diameter, which enhance the surrounding hydrogen-bond network, and large hydrophobic structures greater than 1 nm in diameter, which break the hydrogen bonds of nearby water molecules.

These findings contribute to our understanding of the hydrophobic interaction — the tendency of hydrophobic groups to cluster together in liquid water. The hydrophobic interaction is one of the most important driving forces in nature, and is key to processes such as protein folding and the self-assembly of lipid membranes. The present study shows that the interaction of a solute with surrounding water is more than just the sum of local chemical interactions; the water's structure strongly depends on how well the solute fits into the water network. The structure of water surrounding a biomolecular solute will thus be the result of a complex interplay of the sizes and relative positions of the solute's hydrophobic and hydrophilic regions. It is to be hoped that future studies will shed light on these combined effects, and thereby pave the way to a full understanding of the conformational dynamics and aggregation of biomolecules in liquid water.

References

  1. 1

    Davis, J. G., Gierszal, K. P., Wang, P. & Ben-Amotz, D. Nature 491, 582–585 (2012).

    CAS  Article  ADS  Google Scholar 

  2. 2

    Frank, H. S. & Evans, M. W. J. Chem. Phys. 13, 507–532 (1945).

    CAS  Article  ADS  Google Scholar 

  3. 3

    Soper, A. K. & Finney, J. L. Phys. Rev. Lett. 71, 4346–4349 (1993).

    CAS  Article  ADS  Google Scholar 

  4. 4

    Dixit, S., Crain, S. J., Poon, W. C. K., Finney, J. L. & Soper, A. K. Nature 416, 829–832 (2002).

    CAS  Article  ADS  Google Scholar 

  5. 5

    Chandler, D. Nature 437, 640–647 (2005).

    CAS  Article  ADS  Google Scholar 

  6. 6

    Laage, D. & Hynes, J. T. Science 311, 832–835 (2006).

    CAS  Article  ADS  Google Scholar 

  7. 7

    Laage, D., Stirnemann, G. & Hynes, J. T. J. Phys. Chem. B 113, 2428–2435 (2009).

    CAS  Article  Google Scholar 

  8. 8

    Ishihara, Y., Okouchi, S. & Uedaira, H. J. Chem. Soc. Faraday Trans. 93, 3337–3342 (1997).

    CAS  Article  Google Scholar 

  9. 9

    Yoshida, K., Ibuki, K. & Ueno, M. J. Chem. Phys. 108, 1360–1367 (1998).

    CAS  Article  ADS  Google Scholar 

  10. 10

    Petersen, C., Tielrooij, K.-J. & Bakker, H. J. J. Chem. Phys. 130, 214511 (2009).

    CAS  Article  ADS  Google Scholar 

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Correspondence to Huib J. Bakker.

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Bakker, H. Water's response to the fear of water. Nature 491, 533–535 (2012). https://doi.org/10.1038/491533a

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