The Stability of Hydrogen-Bonded Ion-Pair Complex Unexpectedly Increases with Increasing Solvent Polarity
Status PubMed-not-MEDLINE Language English Country Germany Media print-electronic
Document type Journal Article
Grant support
GAČR 22-15374S
Grantová Agentura České Republiky
CZ.10.03.01/00/22_003/0000048
REFRESH- Research Excellence for Region Sustainability and High-tech Industries
CZ.10.03.01/00/22_003/0000048
REFRESH - Research Excellence for Region Sustainability and High-tech Industries
IGA_PrF_2024_017
Univerzita Palackého v Olomouci
- Keywords
- Hydrogen bonding, Micro-solvation, NMR, Slow-growth dynamics, Solvent effect,
- Publication type
- Journal Article MeSH
The generally observed decrease of the electrostatic energy in the complex with increasing solvent polarity has led to the assumption that the stability of the complexes with ion-pair hydrogen bonds decreases with increasing solvent polarity. Besides, the smaller solvent-accessible surface area (SASA) of the complex in comparison with the isolated subsystems results in a smaller solvation energy of the latter, leading to a destabilization of the complex in the solvent compared to the gas phase. In our study, which combines Nuclear Magnetic Resonance, Infrared Spectroscopy experiments, quantum chemical calculations, and molecular dynamics (MD) simulations, we question the general validity of this statement. We demonstrate that the binding free energy of the ion-pair hydrogen-bonded complex between 2-fluoropropionic acid and n-butylamine (CH3CHFCOO-…NH3But+) increases with increased solvent polarity. This phenomenon is rationalized by a substantial charge transfer between the subsystems that constitute the ion-pair hydrogen-bonded complex. This unexpected finding introduces a new perspective to our understanding of solvation dynamics, emphasizing the interplay between solvent polarity and molecular stability within hydrogen-bonded systems.
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