Différences entre les versions de « ELF abstracts page »
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''Dpto. Química Física y Analítica. Universidad de Oviedo. Spain' | ''Dpto. Química Física y Analítica. Universidad de Oviedo. Spain' | ||
| − | <big>ELF: electron-electron interactions, electron number statistics </big> | + | <big>'''ELF: electron-electron interactions, electron number statistics''' </big> |
The use of lectron localization functions has provided important insights in theoretical chemistry, including | The use of lectron localization functions has provided important insights in theoretical chemistry, including | ||
Version du 21 mai 2010 à 16:08
SPEAKERS : please add below, in your own section, your title talk and abstract :
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- >>> How to insert a picture in your abstract
The order of abstracts follow the program of the workshop.
E. Alikhani
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P. C. Hiberty
Université de Paris-Sud, Laboratoire de Chimie Physique, UMR8000, 91405 Orsay Cédex, France
New Concepts in Chemical Bonding. Charge-Shift Bonding and its Manifestations in Chemistry
Abstract:
Valence bond (VB) theory and electron-localization function (ELF) calculations of various single bonds demonstrate that along the two classical bond families of covalent and ionic bonds, there exists a class of charge-shift bonds (CS-bonds) in which the fluctuation of the electron pair density plays a dominant role. In VB theory, CS-bonding manifests by large covalent-ionic resonance energy, and in ELF by a depleted basin population with large variances (fluctuations).[1]
CS-bonding can be found in homopolar as well as heteropolar bonds. Atoms that are prone to CS-bonding are compact electronegative and/or electron rich species. An extreme case is the single bond in difluorine, where the purely covalent wave function is repulsive at all distances, while the stability of the molecule is entirely due to covalent-ionic resonance.
The difference between covalent and charge-shift bonds, in terms of ELF picture, is illustrated with the examples of ethane and F2 below.
The CS character of such bonds have some experimental consequences, among which the strange stabilities of some cage compounds like the family of propellanes, which display rather strong bonds between “inverted” carbons despite their pyramidalization in the “wrong” direction.[2]
Another experimental consequence, the rarity of silicenium ions in condensed phases,[3] will be addressed if there is some time left.
References
[1] S. Shaik, D. Danovich, B. Silvi, D.L. Lauvergnat, P.C. Hiberty, Chem. Eur. J. 2005, 11, 658.
[2] S. Shaik, D. Danovich, W. Wu, P. C. Hiberty, Nature Chem. 2009, 1, 443.
[3] P. Su, L. Song, W. Wu, S. Shaik, P. C. Hiberty, J. Phys. Chem. A 2008, 112, 2988.
C. Lepetit
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M-M. Rohmer
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B. De Courcy
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H. Jamet
Laboratoire Chimie Théorique, DCM, 301 Rue de la Chimie,Domaine Universitaire, 38041 Grenoble Cedex 9, email: hjamet@ujf-grenoble.fr
ELF and MESP : two efficient methods to validate a QM/MM partition for the modelization of Phosphine ligands
A fundamental question that arises after the decision of using QM/MM methods for a certain problem, is how to partition the system, which atoms are going to be included in the QM region and which atoms are going to be included in the MM region? Chemical knowledge is most of the time the guiding line for this choice, but tests should be run in case of uncertainty. In this study we discuss the modelization of phosphine ligands commonly used in the assymetric Pauson-Khand reaction[1] by means of QM/MM methods. X-ray structures of the ligands bound to the tungsten penta(tetra) carbonyl were used as starting point for all calculations. For the evaluation of the position of the QM/MM border, different approaches were used. Firstly, we compare the results of geometry optimizations obtained from ONIOM method using different QM-MM borders with those obtained from full quantum mechanical calculations. Secondly, we evaluate the molecular electrostatic potential (MESP) and the ELF function for the ligand alone, without optimizing it. More precisely we calculate the minimum value of the MESP around the lone pair region of the phosphorus atom as Suresh et al. done[2] and evaluate the population of the valence phosphorus basin V(P). We show that these two later approaches which have the advantage of being fast and computationally inexpensive reproduce the same trend than results obtained from geometry optimizations of the whole complex.
References
[1] K. Hiroi, T. Watanabe, R. Kawagishi and I. Abe. Tetrahedron: Asymmetry, 2000, 11:1197.
[2] J.Mathew, T. Thomas and C.H.Suresh, Inorg. Chem. 2007, 46(25):10800.
G. A. Cisneros
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X. Assfeld
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H. S. Rzepa
Department of Chemistry, Imperial College London, email: rzepa@imperial.ac.uk
ELF and the Nature of Triple bonds
A recent report of the species HOS≡CH by Schreiner, Mloston and co-workers1 speculated upon the nature of the SC bond; did it have triple significant bond character? Of the various techniques these authors used for the analysis, neither QTAIM nor ELF was employed. I initially filled this gap by a post on my blog2, and followed this by a full article submitted for publication more conventionally3. The results of this investigation will be presented at the workshop, including a rather surprising conclusion regarding the nature of triple bonds themselves in relation to the degree of charge-shift character they display4. The hypothesis so generated was then extended to investigating the nature of metal-metal multiple bonds, particularly Cr-Cr whose compounds are purported to exhibit homonuclear quadruple or quintuple bonds5. These systems also appear to sustain remarkably high charge-shift character and most intriguing ELF behaviour. The issue for discussion in the workshop is therefore whether or not ELF (combined with QTAIM) is indeed revealing something new about the nature of the triple and higher order homonuclear (metal) bond.
The talk will appear @www.ch.ic.ac.uk/rzepa/talks/elf10 and will feature rotatable ELF isosurfaces and models.
References
[1] P. R. Schreiner, H. P. Reisenauer, J. Romanski, and G. Mloston, Angew. Chemie. 2009, 48, 8133-8136. DOI: 10.1002/anie.200903969
[2] H. S. Rzepa, Blog and follow up
[3] H. S. Rzepa, submitted for publication, 2010.
[4] S. Shaik, D. Danovich, W. Wu and P. C. Hiberty, Nature Chem., 2009, 1, 443-449. DOI: 10.1038/nchem.327
[5] For initial speculations, see blog.
M. Yanez
Departamento de Química, C-9. Universidad Autónoma de Madrid. Cantoblanco, 28049-Madrid. Spain
ELF as a useful tool to understand chemical bonding in challenging cases
Quite unexpectedly, substituent effects on the structure of iminoboranes are opposite to those observed for the acetylene derivatives in spite of the fact that both series of compounds are isoelectronic. [1] More importantly these dissimilarities cannot be easily explained in terms of the atoms in molecules (AIM) theory or in terms of the population of the πBN* or πCC* antibonding orbitals. In some molecules a decrease (increase) of the electron density is unexpectedly reflected in a shortening (lengthening) of the bond. Conversely, the ELF analysis offers a clear picture of the substituent effects on the CC and BN bonding. The dissimilarities between acetylene- and iminoborane derivatives are primarily a consequence of the strong electronegativity difference between the B and N atoms in the iminoboranes. This difference is the origin of the significant distortion of the BN bonding electron density in iminoboranes, which is not seen in the corresponding acetylene analogues.
References
[1] O. Mó; M. Yáñez; A. Martín Pendás; J.E. Del Bene; I. Alkorta and J. Elguero, Phys. Chem. Chem. Phys. 9, 3970 (2007)
P. J. MacDougall
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J. Angyan
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M. Causa
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J. Contreras-Garcia
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D. L. Cooper
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A. Lüchow
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E. P. Fowe
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S. Grabowski
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A. Martín Pendás
Dpto. Química Física y Analítica. Universidad de Oviedo. Spain'
ELF: electron-electron interactions, electron number statistics
The use of lectron localization functions has provided important insights in theoretical chemistry, including vivid images of chemically important regions. However, integration of operator densities over ELF basins other than electron populations has not been fully exploited up to now. Here we report two examples of non-standard ELF basin integration. On the one hand we show how the electron repulsion energy between basins is able to recover the Gillespie-Nyholm rule within the VSEPR model. On the other, we show a number of examples of the full statistics of the electron population distribution functions (EDF) computed over ELF basins.
[1] Chem. Phys. Lett. 454, 396 (2008)
E. Matito
Institute of Physics, University of Szczecin, Poland
The Electron Localization Function at the Correlated Level: A Natural Orbital Formulation.
The ELF is nowadays used in a wide context, with applications on aromaticity, chemical bonding or reaction mechanisms. The calculation of the ELF involves the computation of the second-order density matrix (DM2),1 which has a very simple structure in the case of monodeterminantal wavefunctions. In the case of correlated wavefunctions, the structure of the DM2 imposes an important bottleneck for both the calculation of the ELF and the population analysis (variance, covariance) of the ELF basins. Therefore, in practice, the use of the ELF for correlated wavefunctions is limited to very small molecules. However, it is possible to lower the numerical complexity of the calculation of the localization function as well as that of the pair populations using approximated expressions for the calculation of DM2. In this work we propose a correlated version of the ELF where the DM2 has been approximated by the formula for the monodeterminantal wavefunctions (X-HF in the graph below) and the formula of Müller in terms of natural orbitals.3,4 The approximation has been tested in a set of molecules, NH3, CO2, H2O, CO, CN-, NO+, N2, H2O2, F2 and FCl-, which have been calculated using a plethora of methods: HF, B3LYP, MP2, CISD, CCSD and CASSCF. The present approach aims at a correlated version of the ELF which can be used in medium size molecules.
References
[1] Matito E., Silvi B., Duran M. and Solà M., J. Chem. Phys. 125, 024301 (2006)
[2] Feixas F., Matito E., Duran M., Solà M. and Silvi B., in preparation.
[3] Müller A.M.K., Phys. Lett. 105A, 446 (1984)
[4] M. A. Buijse, E. J. Baerends, Mol. Phys., 100, 401 (2002)
D. Borgis
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R. Vuillemier
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J. Cioslowski
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J. Pilmé
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R. Nesper
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Y. Grin
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J-F. Halet
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U. Wedig
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R. Weihrich
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P. Raybaud
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E. Dumont
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N. Chéron
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S. Berski
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L. Joubert
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H. Bolvin
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A. Delalande
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R. Nalewajski
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A. Scemama
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J. Tao
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I. Fourré
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H. Gérard
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N. Russo
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