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Guńka PA, Hapka M, Hanfland M, Dranka M, Chałasiński G, Zachara J. How and Why Does Helium Permeate Nonporous Arsenolite Under High Pressure? Chemphyschem 2018; 19:857-864. [PMID: 29341365 DOI: 10.1002/cphc.201701156] [Citation(s) in RCA: 6] [Impact Index Per Article: 1.0] [Reference Citation Analysis] [Abstract] [Key Words] [Track Full Text] [Journal Information] [Subscribe] [Scholar Register] [Received: 10/24/2017] [Revised: 12/06/2017] [Indexed: 11/06/2022]
Abstract
Investigations into the helium permeation of arsenolite, the cubic, molecular arsenic(III) oxide polymorph As4 O6 , were carried out to understand how and why arsenolite helium clathrate As4 O6 ⋅2 He is formed. High-pressure synchrotron X-ray diffraction experiments on arsenolite single crystals revealed that the permeation of helium into nonporous arsenolite depends on the time for which the crystal is subjected to high pressure and on the crystal history. The single crystal was totally transformed into As4 O6 ⋅2 He within 45 h under 5 GPa. After release of the pressure, arsenolite was recovered and a repeated increase in pressure up to 3 GPa led to practically instant As4 O6 ⋅2 He formation. However, when a pristine arsenolite single crystal was quickly subjected to a pressure of 13 GPa, no helium permeation was observed at all. No neon permeation was observed in analogous experiments. Quantum mechanical computations indicate that there are no specific attractive interactions between He atoms and As4 O6 molecules at the distances observed in the As4 O6 ⋅2 He crystal structure. Detailed analysis of As4 O6 molecular structure changes has shown that the introduction of He into the arsenolite crystal lattice significantly reduces molecular deformations by decreasing the anisotropy of stress exerted on the As4 O6 molecules. This effect and the pΔV term, rather than any specific As⋅⋅⋅He binding, are the driving forces for the formation As4 O6 ⋅2 He.
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Affiliation(s)
- Piotr A Guńka
- Faculty of Chemistry, Warsaw University of Technology, Noakowskiego 3, 00-664, Warszawa, Poland
| | - Michał Hapka
- Faculty of Chemistry, University of Warsaw, Pasteura 1, 02-093, Warszawa, Poland
| | - Michael Hanfland
- European Synchrotron Radiation Facility, 71 avenue des Martyrs, CS 40220, 38043, Grenoble Cedex 9, France
| | - Maciej Dranka
- Faculty of Chemistry, Warsaw University of Technology, Noakowskiego 3, 00-664, Warszawa, Poland
| | - Grzegorz Chałasiński
- Faculty of Chemistry, University of Warsaw, Pasteura 1, 02-093, Warszawa, Poland
| | - Janusz Zachara
- Faculty of Chemistry, Warsaw University of Technology, Noakowskiego 3, 00-664, Warszawa, Poland
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Monteiro NKV, Firme CL. Hydrogen-hydrogen bonds in highly branched alkanes and in alkane complexes: A DFT, ab initio, QTAIM, and ELF study. J Phys Chem A 2014; 118:1730-40. [PMID: 24533436 DOI: 10.1021/jp500131z] [Citation(s) in RCA: 53] [Impact Index Per Article: 5.3] [Reference Citation Analysis] [Abstract] [Track Full Text] [Journal Information] [Subscribe] [Scholar Register] [Indexed: 11/29/2022]
Abstract
The hydrogen-hydrogen (H-H) bond or hydrogen-hydrogen bonding is formed by the interaction between a pair of identical or similar hydrogen atoms that are close to electrical neutrality and it yields a stabilizing contribution to the overall molecular energy. This work provides new, important information regarding hydrogen-hydrogen bonds. We report that stability of alkane complexes and boiling point of alkanes are directly related to H-H bond, which means that intermolecular interactions between alkane chains are directional H-H bond, not nondirectional induced dipole-induced dipole. Moreover, we show the existence of intramolecular H-H bonds in highly branched alkanes playing a secondary role in their increased stabilities in comparison with linear or less branched isomers. These results were accomplished by different approaches: density functional theory (DFT), ab initio, quantum theory of atoms in molecules (QTAIM), and electron localization function (ELF).
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Affiliation(s)
- Norberto K V Monteiro
- Institute of Chemistry, Federal University of Rio Grande do Norte , Natal, Rio Grande do Norte, Brazil , CEP 59078-970
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9
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Gibbs GV, Crawford TD, Wallace AF, Cox DF, Parrish RM, Hohenstein EG, Sherrill CD. Role of Long-Range Intermolecular Forces in the Formation of Inorganic Nanoparticle Clusters. J Phys Chem A 2011; 115:12933-40. [DOI: 10.1021/jp204044k] [Citation(s) in RCA: 16] [Impact Index Per Article: 1.2] [Reference Citation Analysis] [Track Full Text] [Journal Information] [Subscribe] [Scholar Register] [Indexed: 11/30/2022]
Affiliation(s)
| | | | - A. F. Wallace
- Earth Science Division, Lawrence Berkeley National Laboratory, Berkeley, California 94720, United States
| | | | - R. M. Parrish
- Center for Computational Molecular Science and Technology, School of Chemistry and Biochemistry, Georgia Institute of Technology, Atlanta, Georgia 30332-0400, United States
| | - E. G. Hohenstein
- Center for Computational Molecular Science and Technology, School of Chemistry and Biochemistry, Georgia Institute of Technology, Atlanta, Georgia 30332-0400, United States
| | - C. D. Sherrill
- Center for Computational Molecular Science and Technology, School of Chemistry and Biochemistry, Georgia Institute of Technology, Atlanta, Georgia 30332-0400, United States
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11
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Bader RFW. Definition of molecular structure: by choice or by appeal to observation? J Phys Chem A 2010; 114:7431-44. [PMID: 20550157 DOI: 10.1021/jp102748b] [Citation(s) in RCA: 150] [Impact Index Per Article: 10.7] [Reference Citation Analysis] [Abstract] [Track Full Text] [Journal Information] [Subscribe] [Scholar Register] [Indexed: 11/28/2022]
Abstract
There are two schools of thought in chemistry: one derived from the valence bond and molecular orbital models of bonding, the other appealing directly to the measurable electron density and the quantum mechanical theorems that determine its behavior, an approach embodied in the quantum theory of atoms in molecules, QTAIM. No one questions the validity of the former approach, and indeed molecular orbital models and QTAIM play complementary roles, the models finding expression in the principles of physics. However, some orbital proponents step beyond the models to impose their personal stamp on their use in interpretive chemistry, by denying the possible existence of a physical basis for the concepts of chemistry. This places them at odds with QTAIM, whose very existence stems from the discovery in the observable topology of the electron density, the definitions of atoms, of the bonding between atoms and hence of molecular structure. Relating these concepts to the electron density provides the necessary link for their ultimate quantum definition. This paper explores in depth the possible causes of the difficulties some have in accepting the quantum basis of structure beginning with the arguments associated with the acceptance of a "bond path" as a criterion for bonding. This identification is based on the finding that all classical structures may be mapped onto molecular graphs consisting of bond paths linking neighboring atoms, a mapping that has no known exceptions and one that is further bolstered by the finding that there are no examples of "missing bond paths". Difficulties arise when the quantum concept is applied to systems that are not amenable to the classical models of bonding. Thus one is faced with the recurring dilemma of science, of having to escape the constraints of a model that requires a change in the existing paradigm, a process that has been in operation since the discovery of new and novel structures necessitated the extension of the Lewis model and the octet rule. The paper reviews all facets of bonding beginning with the work of Pauling and Slater in their accounting for crystal structures, taking note of Pauling's advocating possible bonding between large anions. Many examples of nonbonded or van der Waals interactions are considered from both points of view. The final section deals with the consequences of the realization that bonded quantum atoms that share an interatomic surface do not "overlap". The time has come for entering students of chemistry to be taught that the electron density can be seen, touched, and measured and that the chemical structures they learn are in fact the tracings of "bonds" onto lines of maximum density that link bonded nuclei. Matter, as we perceive it, is bound by the electrostatic force of attraction between the nuclei and the electron density.
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Affiliation(s)
- Richard F W Bader
- Department of Chemistry, McMaster University, Hamilton, ON, L7L 2T1,Canada
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Gibbs GV, Wallace AF, Zallen R, Downs RT, Ross NL, Cox DF, Rosso KM. Bond Paths and van der Waals Interactions in Orpiment, As2S3. J Phys Chem A 2010; 114:6550-7. [DOI: 10.1021/jp102391a] [Citation(s) in RCA: 22] [Impact Index Per Article: 1.6] [Reference Citation Analysis] [Track Full Text] [Journal Information] [Subscribe] [Scholar Register] [Indexed: 10/19/2022]
Affiliation(s)
- G. V. Gibbs
- Departments of Geosciences, Materials Science and Engineering and Mathematics, Department of Physics, Department of Chemical Engineering, Virginia Tech, Blacksburg, Virginia 24061, U.S.A., Earth Science Division, Lawrence Berkeley National Laboratory, Berkeley, California 94720, Department of Geosciences, University of Arizona, Tucson, Arizona 85721, U.S.A., and Chemical and Materials Science Division, and the W.R. Wiley Environmental Molecular Sciences Laboratory, Pacific Northwest National Laboratory,
| | - A. F. Wallace
- Departments of Geosciences, Materials Science and Engineering and Mathematics, Department of Physics, Department of Chemical Engineering, Virginia Tech, Blacksburg, Virginia 24061, U.S.A., Earth Science Division, Lawrence Berkeley National Laboratory, Berkeley, California 94720, Department of Geosciences, University of Arizona, Tucson, Arizona 85721, U.S.A., and Chemical and Materials Science Division, and the W.R. Wiley Environmental Molecular Sciences Laboratory, Pacific Northwest National Laboratory,
| | - R. Zallen
- Departments of Geosciences, Materials Science and Engineering and Mathematics, Department of Physics, Department of Chemical Engineering, Virginia Tech, Blacksburg, Virginia 24061, U.S.A., Earth Science Division, Lawrence Berkeley National Laboratory, Berkeley, California 94720, Department of Geosciences, University of Arizona, Tucson, Arizona 85721, U.S.A., and Chemical and Materials Science Division, and the W.R. Wiley Environmental Molecular Sciences Laboratory, Pacific Northwest National Laboratory,
| | - R. T. Downs
- Departments of Geosciences, Materials Science and Engineering and Mathematics, Department of Physics, Department of Chemical Engineering, Virginia Tech, Blacksburg, Virginia 24061, U.S.A., Earth Science Division, Lawrence Berkeley National Laboratory, Berkeley, California 94720, Department of Geosciences, University of Arizona, Tucson, Arizona 85721, U.S.A., and Chemical and Materials Science Division, and the W.R. Wiley Environmental Molecular Sciences Laboratory, Pacific Northwest National Laboratory,
| | - N. L. Ross
- Departments of Geosciences, Materials Science and Engineering and Mathematics, Department of Physics, Department of Chemical Engineering, Virginia Tech, Blacksburg, Virginia 24061, U.S.A., Earth Science Division, Lawrence Berkeley National Laboratory, Berkeley, California 94720, Department of Geosciences, University of Arizona, Tucson, Arizona 85721, U.S.A., and Chemical and Materials Science Division, and the W.R. Wiley Environmental Molecular Sciences Laboratory, Pacific Northwest National Laboratory,
| | - D. F. Cox
- Departments of Geosciences, Materials Science and Engineering and Mathematics, Department of Physics, Department of Chemical Engineering, Virginia Tech, Blacksburg, Virginia 24061, U.S.A., Earth Science Division, Lawrence Berkeley National Laboratory, Berkeley, California 94720, Department of Geosciences, University of Arizona, Tucson, Arizona 85721, U.S.A., and Chemical and Materials Science Division, and the W.R. Wiley Environmental Molecular Sciences Laboratory, Pacific Northwest National Laboratory,
| | - K. M. Rosso
- Departments of Geosciences, Materials Science and Engineering and Mathematics, Department of Physics, Department of Chemical Engineering, Virginia Tech, Blacksburg, Virginia 24061, U.S.A., Earth Science Division, Lawrence Berkeley National Laboratory, Berkeley, California 94720, Department of Geosciences, University of Arizona, Tucson, Arizona 85721, U.S.A., and Chemical and Materials Science Division, and the W.R. Wiley Environmental Molecular Sciences Laboratory, Pacific Northwest National Laboratory,
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Abstract
This account takes to task papers that criticize the definition of a bond path as a criterion for the bonding between the atoms it links by mistakenly identifying it with a chemical bond. It is argued that the notion of a chemical bond is too restrictive to account for the physics underlying the broad spectrum of interactions between atoms and molecules that determine the properties of matter. A bond path on the other hand, as well as being accessible to experimental verification and subject to the theorems of quantum mechanics, is applicable to any and all of the interactions that account for the properties of matter. It is shown that one may define a bond path operator as a Dirac observable, making the bond path the measurable expectation value of a quantum mechanical operator. Particular attention is given to van der Waals interactions that traditionally are assumed to represent attractive interactions that are distinct from chemical bonding. They are assumed by some to act in concert with Pauli repulsions to account for the existence of condensed states of molecules. It is such dichotomies of interpretation that are resolved by the experimental detection of bond paths and the delineation of their properties in molecular crystals. Specific criticisms of the stabilization afforded by the presence of bond paths derived from spectroscopic measurements performed on dideuteriophenanthrene are shown to be physically unsound. The concept of a bond path as a "bridge of density" linking bonded atoms was introduced by London in 1928 following the definition of the electron density by Schrödinger in 1926. These papers marked the beginning of the theory of atoms in molecules linked by bond paths.
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Affiliation(s)
- Richard F W Bader
- Department of Chemistry, McMaster University, Hamilton, ON L7L 2T1, Canada
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