Reaction Rate Constant Computations: Theories and Applications (RSC Theoretical and Computational Chemistry) - Hardcover

Buch 5 von 25: Chemical Biology
 
9781849736503: Reaction Rate Constant Computations: Theories and Applications (RSC Theoretical and Computational Chemistry)

Inhaltsangabe

Reaction rate constant plays an essential role in understanding a wide range of processes in chemistry, biochemistry and physics, and thus it is very intuitive for researchers to have a first look at the rate constant of a chemical reaction. This book describes the recent efforts on rate constant computations for reactions in gas phase, solutions and solid-state, covering those on developing new theories, modifying and improving the previously established ones, evaluating the quality of various kinds of theories, mechanistic analyses with rate constant computation, recent interest and the hottest issues in the area. An essential read for all chemists, physicists, biochemists working in the field.

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Über die Autorinnen und Autoren

Prof. Keli Han worked at Dalian Institute of Chemical Physics, Chinese Academy of Sciences (CAS). He received his Ph. D. degree in physical chemistry from Dalian Institute of Chemical Physics, Chinese Academy of Sciences (CAS) in 1990. His research group is mainly interested in molecular reaction dynamics: chemical reaction rate computations, hydrogen-bond dynamics in intermolecular electron transfer, molecular dynamics with attosecond resolution, nonadiabatic dynamics in chemical processes, enzyme dynamics. To date, he has published more than 330 scientific papers with a high citation over 4000. Due to his excellent works, he was invited and published review articles in Int. Rev. Phys. Chem., Phys. Chem. Chem. Phys., J. Comput. Chem., J. Photochem. Photobio. C: Photochem. Rev., Exp. Opin. Drug. Disc. He is recipient of the National Outstanding Youth Foundation. In 1999, he received a first class Natural Science Award from CAS and the Young Chemist Award from the Chinese Chemical Society (CCS). He is the chair of the Virtual Laboratory for Computational Chemistry (VLCC), Supercomputing Center, Computer Network Information Center, CAS. He chaired many international meetings and presented many invited talks. He is a member of the editorial board of the Journal of Physical Chemistry. He is also a member of the advisory editorial board of the Journal of Theoretical & Computational Chemistry, Chinese Journal of Chemical Physics, Acta Physico-Chimica Sinica, Progress in Natural Science, Chinese Science Bulletin, Journal of Atomic and Molecular Physics.

Prof. Tianshu Chu is a visiting scholar in Dalian Institute of Chemical Physics, Chinese Academy of Sciences (CAS) and a professor in Qingdao University, China. She received her Ph. D. degree in physical chemistry from Dalian Institute of Chemical Physics, Chinese Academy of Sciences (CAS) in 2006. Her research interests focused on (i) developing quantum methods and dynamical codes for dynamics investigation of nuclei and electron motions in chemical and physical processes and (ii) growth dynamics of nanoparticles, kinetic and mechanistic analyse of chemical reactions. Worked with Prof. Keli Han, she carried out many rate computations based on quantum dynamics, and published review articles in Int. Rev. Chem. Phys. and Phys. Chem. Chem. Phys., each with a rather high citation of 165 and 94.

Von der hinteren Coverseite

The reaction rate constant plays an essential role a wide range of processes in biology, chemistry and physics. Calculating the reaction rate constant provides considerable understanding to a reaction and this book presents the latest thinking in modern rate computational theory.

The editors have more than 30 years’ experience in researching the theoretical computation of chemical reaction rate constants by global dynamics and transition state theories and have brought together a global pool of expertise discussing these in a variety of contexts and across all phases. This thorough treatment of the subject provides an essential handbook to students and researchers entering the field and a comprehensive reference to established practitioners across the sciences, providing better tools to determining reaction rate constants.

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Reaction Rate Constant Computations

Theories and Applications

By Keli Han, Tianshu Chu

The Royal Society of Chemistry

Copyright © 2014 The Royal Society of Chemistry
All rights reserved.
ISBN: 978-1-84973-650-3

Contents

Chapter 1 Elementary Reactions: Rate Constants and their Temperature-Dependence Ian W. M. Smith, 1,
Chapter 2 Rate Constant Calculation of Benzylperoxy Radical Isomerization S. Canneaux, C. Hammaecher, F. Louis and M. Ribaucour, 34,
Chapter 3 Rate Constants and the Kinetic Isotope Effects in Multi-Proton Transfer Reactions: A Case Study of CIONO2 + HCl [right arrow] HNO3 + Cl2 Reactions with Water Clusters with Canonical Variational Transition State Theory using a Direct Ab Initio Dynamics Approach Yongho Kim, 55,
Chapter 4 Statisticodynamical and Multiscale Modeling of Cluster Dissociation F. Calvo and P. Parneix, 77,
Chapter 5 A Mixed Quantum-Classical View to the Kinetics of Chemical Reactions Involving Multiple Electronic States Aurélien de la Lande, Bernard Lévy and Isabelle Demachy, 99,
Chapter 6 Adiabatic Treatment of Torsional Anharmonicity and Mode Coupling in Molecular Partition Functions and Statistical Rate Coefficients: Application to Hydrogen Peroxide Zeb C. Kramer and Rex T. Skodje, 133,
Chapter 7 Dynamics of Chemical Reaction around a Saddle Point: What Divides Reacting and Non-Reacting Trajectories? Shinnosuke Kawai and Tamiki Komatsuzaki, 154,
Chapter 8 Derivation of Rate Constants from Accurate Quantum Wave Packet Theory for Nonadiabatic and Adiabatic Chemical Reactions Tianshu Chu and Keli Han, 180,
Chapter 9 Understanding Reactivity with Reduced Potential Energy Landscapes: Recent Advances and New Directions Bryan R. Goldsmith, Anthony Fong and Baron Peters, 213,
Chapter 10 Quantum-Classical Liouville Dynamics of Condensed Phase Quantum Processes Gabriel Hanna and Raymond Kapral, 233,
Chapter 11 Free Energetics and Kinetics of Charge Transfer and Shift Reactions in Room-Temperature Ionic Liquids Youngseon Shim and Hyung J. Kim, 260,
Chapter 12 Semi-Classical Treatments of Electron Transfer Rate from Weak to Strong Electronic Coupling Regime Yi Zhao, 283,
Chapter 13 Modified Zusman Equation for Quantum Solvation Dynamics and Rate Processes Hou-Dao Zhang, Jian Xu, Rui-Xue Xu and YiJing Yan, 319,
Chapter 14 Time-Dependent Treatment of SVRT Model for Polyatom–Polyatom Reaction John Z. H. Zhang, 337,
Chapter 15 Role of Water in Radical Reactions: Molecular Simulation and Modelling Dorota Swiatla-Wojcik, 352,
Chapter 16 Molecular Modelling of Proton Transfer Kinetics in Biological Systems Patrick Bertrand, 379,
Chapter 17 Putting Together the Pieces: A Global Description of Valence and Long-Range Forces via Combined Hyperbolic Inverse Power Representation of the Potential Energy Surface A. J. C. Varandas, 408,
Chapter 18 Extension of Marcus Rate Theory to Electron Transfer Reactions with Large Solvation Changes Guillaume Jeanmairet, Daniel Borgis, Anne Boutin and Rodolphe Vuilleumier, 446,
Chapter 19 Theoretical Studies on Mechanism and Kinetics of Atmospheric Chemical Reactions L. Sandhiya and K. Senthilkumar, 462,
Chapter 20 Computation of Intrinsic RRKM and Non-RRKM Unimolecular Rate Constants Amit Kumar Paul, Sujitha Kolakkandy, Subha Pratihar and William L. Hase, 494,
Chapter 21 Molecular Dynamics Simulation of Kinetic Isotope Effects in Enzyme-Catalyzed Reactions Jiali Gao, 530,
Subject Index, 550,


CHAPTER 1

Elementary Reactions: Rate Constants and their Temperature-Dependence


IAN W. M. SMITH


1.1 Introduction

This chapter considers the kinetics of elementary reactions. Unlike complex reactions, elementary reactions cannot be subdivided into processes of lesser molecular complexity, whereas complex reactions proceed through a network of elementary reactions. Elementary reactions necessarily involve the participation of a small integral number of atoms and/or molecules, and one can further define them by saying that the chemical change involves molecular processes which mimic the chemical equation that is used to represent the reaction. Thus, the reaction

F + H2 [right arrow] HF + H (R1)

occurs in binary collisions — though not all binary collisions — between fluorine atoms and molecules of di-hydrogen.

Elementary chemical reactions can be classified as collisional or decay processes. The former, of which reaction (R1) is an example, are generally referred to as bimolecular; two species (e.g. F and H2) collide in each microscopic event that leads to reaction and the formation of products (e.g. HF and H). Decay processes are unimolecular: chemical change occurs in processes where single molecules either dissociate to two new chemical species or isomerise, that is, change to a different form with the same chemical formula.

However, it is necessary to insert a cautionary note in the description of unimolecular processes as elementary since this designation disguises the fact that, although the elementary processes in which chemical change occurs are indeed unimolecular, they involve molecules of reactants that contain high internal energy compared with the great majority. Consequently, collisions in which energy is transferred but no chemical change occurs also play a vital role in the kinetics of these reactions. Finally, I note that association reactions are the reverse of dissociation reactions. They involve two reactant species, frequently two free radicals, coming together to form a collision complex, which is subsequently stabilised against re-dissociation — usually by collision with a third species which removes energy from the energised complex. In the limit of the reactants being atoms, for example, pairs of oxygen atoms, the lifetime of the diatomic complex is very short and the stabilising collision is essentially simultaneous with the radical-radical collision. In this case, the reaction can be considered as termolecular.

Reactions occurring in solution are inevitably affected to a greater or lesser degree by the close proximity of solvent molecules to the reactants. Consequently, one can argue that, by definition, elementary reactions only take place in the gas phase. Certainly, such reactions are simpler to treat theoretically. In this chapter, I shall consider only gas-phase reactions. For such reactions, a continuing synergy between experiment and theory has brought forth a remarkable improvement in our understanding, especially of the factors that influence the magnitude of rate constants and their dependence on temperature, and also of the dynamics of such reactions, that is, what factors control the motions of the atoms as chemical bonds rearrange and reactants are converted to products.

The improvement in our knowledge and understanding of elementary chemical reactions has been stimulated by two principal drivers. The first is the developments in experimental techniques and the ability to apply them over an ever-widening range of temperatures, coupled to a massive increase in computing power which has, inter alia, allowed potential energy surfaces to be calculated accurately for elementary reactions of increasing complexity (see section 1.3). The second driver has been the wish to model complex chemical environments: (a) in planetary atmospheres, especially that of Earth; (b) at high temperatures in pyrolytic and combustion systems; and (c) in interstellar and circumstellar media. The computer models contain a...

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