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One free scan finds every outdated or missing driver and matches the right update for your exact hardware.Free scan · exact hardware matchWater molecules can exchange hydrogen-bond partners in a remarkably brief event: a 2010 study of aqueous sodium perchlorate reported that breaking one hydrogen bond and forming another took about 50 femtoseconds. The same study reported an average of about 6 picoseconds with a particular partner and inferred that the molecule rotated roughly 50 degrees as it engaged a new one. These figures describe that specific solution and experiment, not hydrogen bonds universally.
What does hydrogen-bond partner swapping mean?
A hydrogen bond is an interaction between a water molecule and a nearby molecule or ion. In liquid water and other aqueous systems, those interactions are not permanent: a water molecule can leave one partner and form a bond with another. The sequence is simple in outline: the molecule is bonded to one neighbour, that interaction gives way, and molecular motion brings a different partner into reach.
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The 2010 experiment examined water in aqueous sodium perchlorate, where water molecules could be hydrogen-bonded either to other water molecules or to perchlorate ions. It offered experimental evidence about how a hydrogen-bond network reorganizes at the molecular scale.
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How did the researchers observe the exchange?
Led by Kelly Gaffney of Stanford University, the team used laser energy to excite O–H bonds in water and measured their vibrations. Because hydrogen bonding shifts an O–H bond’s vibrational frequency, the researchers could distinguish water bonded to another water molecule from water bonded to a perchlorate anion. Very short-interval absorption measurements tracked the signals. Measurements using polarized light and two lasers were then used to infer how much the molecule rotated as it took up a new partner.
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This distinction matters: the study used vibrational spectroscopy to identify the bonding environment, while the rotation was inferred from polarized-light measurements. The figures below are those reported for this experimental system by Chemistry World on 21 May 2010, in its account of the study by M. Ji, M. Odelius and K. J. Gaffney, published in Science 328, 1003 (2010), DOI 10.1126/science.1187707.
What times and motion did the study report?
| Reported quantity | Value | What it describes |
|---|---|---|
| Average time associated with a particular hydrogen-bond partner | About 6 picoseconds | How long a water molecule remained hydrogen-bonded to a particular partner on average in the aqueous sodium perchlorate study. |
| Bond-exchange interval | About 50 femtoseconds | The reported interval for breaking one hydrogen bond and forming another in that study. |
| Rotation during partner exchange | About 50 degrees | An amount of rotation inferred from polarized-light measurements as the molecule engaged a new partner. |
The residence time and exchange interval describe different parts of the process. The roughly 6-picosecond figure is the average time associated with a particular partner; the roughly 50-femtosecond figure is the much briefer transition in which one bond gives way to another. Keeping those timescales separate helps explain how a molecule can remain associated with a partner for a while yet change partners rapidly once exchange occurs.
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Why is the observation useful?
The work addressed a mechanistic question about hydrogen-bond dynamics: what molecular motion accompanies partner exchange? The picture reported was not a slow, smooth turn. Instead, as one interaction gave way, the water molecule rapidly rotated—about 50 degrees in the account of the experiment—before forming a bond with another partner. That provides a molecular-level description of one way an aqueous hydrogen-bond network can reorganize and gives experimental evidence relevant to theoretical predictions.
Gaffney described the result as an important step toward complementing theoretical predictions with experimental data. Andrew Ellis of the University of Leicester characterized the observation as showing the detaching O–H group swinging around “propeller-like” before it reforms a hydrogen bond with an adjacent molecule. Those descriptions convey the proposed motion; the numerical rotation is an inference from the polarized-light measurements, not a universal angle for every hydrogen-bond exchange.
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What should not be generalized from these numbers?
The values come from one reported experiment on water in aqueous sodium perchlorate. They should not be treated as fixed constants for all water, all liquids, or every molecular environment. The report does not establish cross-study rankings or make a comparison across different chemical systems and measurement methods. Its figures are best read as measurements and an inference tied to the experimental solution and approach.
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