Contributions to the application of the transferability principle and the multipolar modeling of H atoms: electron-density study of<scp>L</scp>-histidinium dihydrogen orthophosphate orthophosphoric acid. I

Mata, Ignasi; Espinosa, Enrique; Molins, Elı́es; Veintemillas, S.; Maniukiewicz, Waldemar; Lecomte, Claude; Cousson, A.; Paulus, Werner

doi:10.1107/s0108767306025141

Cited by 24 publications

(17 citation statements)

References 38 publications

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“…[35] Outliers or systematic deviations from the expected dependencies should be regarded with special care, as they could be indicative of errors in the determination of 1(r) or of uncommon features in 1(r) that should be analyzed in detail.…”

Section: Resultsmentioning

confidence: 99%

Universal Features of the Electron Density Distribution in Hydrogen‐Bonding Regions: A Comprehensive Study Involving H⋅⋅⋅X (X=H, C, N, O, F, S, Cl, π) Interactions

Mata

Alkorta

Molins

et al. 2010

Chemistry A European J

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Topological analyses of the theoretically calculated electron densities for a large set of 163 hydrogen-bonded complexes show that HX interactions can be classified in families according to X (X=atom or pi orbital). Each family is characterised by a set of intrinsic dependencies between the topological and energetic properties of the electron density at the hydrogen-bond critical point, as well as between each of them and the bonding distance. Comparing different atom-acceptor families, these dependencies are classified as a function of the van der Waals radius r(X) or the electronegativity chi(X), which can be explained in terms of the molecular orbitals involved in the interaction. According to this ordering, the increase of chi(X) leads to a larger range of HX distances for which the interaction is of pure closed-shell type. Same dependencies observed for HO interactions experimentally characterised by means of high-resolution X-ray diffraction data show a good agreement with those obtained from theoretical calculations, in spite of a larger dispersion of values around the expected fitting functions in the experimental case. Theoretical dependencies can thus be applied to the analysis of the experimental electron density for detecting either unconventional hydrogen bonds or problems in the modelling of the experimental electron density.

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Section: Resultsmentioning

confidence: 99%

Universal Features of the Electron Density Distribution in Hydrogen‐Bonding Regions: A Comprehensive Study Involving H⋅⋅⋅X (X=H, C, N, O, F, S, Cl, π) Interactions

Mata

Alkorta

Molins

et al. 2010

Chemistry A European J

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235

124

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“…Anionic complexes of the form (H n-1 AO m -) 2 (8)(9)(10)(11)(12)(13)(14) were obtained after removing one proton from each monomer in 1-7 and optimizing the geometry. Adding one Na + to each monomer in 8-14 and optimizing the geometry, neutral salt complexes of type (NaH n-1 AO m ) 2 were obtained (15)(16)(17)(18)(19)(20)(21).…”

Section: Methodsmentioning

confidence: 99%

The Paradox of Hydrogen-Bonded Anion–Anion Aggregates in Oxoanions: A Fundamental Electrostatic Problem Explained in Terms of Electrophilic···Nucleophilic Interactions

et al. 2014

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A theoretical study of anionic complexes formed by two partly deprotonated oxoacids joined by hydrogen bonds has been carried out at the MP2 computational level. In spite of the ionic repulsion, local energy minima are found both in the gas phase and in aqueous solution. Electrostatic potential and electron density topologies, and the comparison with neutral complexes formed by oxoacids, reveal that the ionization has no significant effect on the properties of the hydrogen bonds. The stability of the complexes in the gas phase is explained by attractive forces localized in a volume situated in the hydrogen bond and defined as the electrostatic attraction region (EAR) and determined by the topological analyses of the electron density and the electrostatic potential, and by the electric field lines. In solution, the strong anionic repulsion is mostly screened by the effect of the surrounding polar solvent, which only leads to a weak destabilizing interaction in the hydrogen bond region and finally favors the overall stability of the complexes. The anion−anion complexes have been compared with the corresponding neutral ones (as salts or protonated forms), showing that EAR remains unchanged along the series.

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“…If any E HB ðpÞ is applied to an experimental case the standard uncertainty of p will affect, by error propagation, to the accuracy of the estimation. Although r 2 q b it is the more informative property for determining the nature of the interaction, it presents also the largest experimental error and is extremely dependent on the quality of the model [38]. In the experimental case, the quality of the estimated G b is affected by the standard uncertainty of q b and r 2 q b , as these quantities are used in the Abramov's functional [32].…”

Section: Comparison Of Interaction Energy Estimatorsmentioning

confidence: 98%

Relationships between interaction energy, intermolecular distance and electron density properties in hydrogen bonded complexes under external electric fields

Mata

Alkorta

Espinosa

et al. 2011

Chemical Physics Letters

323

186

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Contributions to the application of the transferability principle and the multipolar modeling of H atoms: electron-density study ofL-histidinium dihydrogen orthophosphate orthophosphoric acid. I

Cited by 24 publications

References 38 publications

Universal Features of the Electron Density Distribution in Hydrogen‐Bonding Regions: A Comprehensive Study Involving H⋅⋅⋅X (X=H, C, N, O, F, S, Cl, π) Interactions

Universal Features of the Electron Density Distribution in Hydrogen‐Bonding Regions: A Comprehensive Study Involving H⋅⋅⋅X (X=H, C, N, O, F, S, Cl, π) Interactions

The Paradox of Hydrogen-Bonded Anion–Anion Aggregates in Oxoanions: A Fundamental Electrostatic Problem Explained in Terms of Electrophilic···Nucleophilic Interactions

Relationships between interaction energy, intermolecular distance and electron density properties in hydrogen bonded complexes under external electric fields

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