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A 2019 study compared how strongly selected cations bind to hydrogen-bond acceptors in solution. It found that lithium and guanidinium formed the most stable complexes in the comparison, but the result is a set of experimentally derived parameters—not a universal ranking that holds regardless of solvent, acceptor, or molecular context.
How the researchers compared cations
Christopher Hunter and co-workers measured equilibrium constants for a selection of cations binding to hydrogen-bond acceptors. They used those binding measurements to derive a hydrogen-bond donor parameter for each cation, creating a way to compare the cations’ interactions in solution.
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The cations included guanidinium; primary, tertiary, and quaternary ammonium; imidazolium; methylpyridinium; and the alkali-metal ions lithium, sodium, potassium, rubidium, and caesium. The team repeated measurements with different acceptors and solvents to check whether the comparisons were consistent across those conditions.
What the reported comparison found
Lithium and guanidinium were highlighted as forming the most stable complexes in the tested comparison. A striking broader finding was that the hydrogen-bonding abilities of charged cations in solution fell within the range observed for neutral hydrogen-bond donors. Some neutral donors could even outcompete fully charged species.
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This is a comparison of measured interactions, not a claim that every cation has one fixed position in an all-purpose ranking. The acceptor and solvent are part of the context for interpreting an interaction; water and the anionic counterion were also examined in the reported systems.
Did water or counterions change the results?
The Chemistry World report says that adding water and changing anionic counterions had negligible effects in the systems tested. That finding is limited to those experimental systems and conditions. It does not establish that water or counterions are irrelevant to cation–acceptor interactions in other solvents, molecular environments, or experimental conditions.
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Why the parameters may be useful
The reported parameters are intended to help estimate the free-energy contribution of cation–acceptor interactions in different solvents and to assess solvation models. That could be useful in supramolecular chemistry, where researchers want to understand how an interaction changes binding affinity, and in catalysis, where transition states are often partially charged. These are potential uses of the parameter set, not a guarantee that it predicts every complex or catalytic system without additional evidence.
What the report does not establish
- A universal order: The findings do not establish a condition-free ranking applicable to every acceptor, solvent, and molecular system.
- Exact parameter values: The Chemistry World report refers to a chart but does not give readable numerical values in its text. No numerical values should be inferred from that passage.
- Universal water or counterion effects: Negligible effects in the tested systems do not mean those variables never matter elsewhere.
The report identifies the underlying paper as S. J. Pike et al., Chemical Science (2019), DOI 10.1039/c9sc00721k. For exact measurements, parameter values, and detailed experimental conditions, consult the paper and its supporting information.
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