Barrier, reaction

The rearrangment of nitromethane to aei-nitromethane via the postulated 1,3-intramolecular hydrogen shift is a high barrier reaction (barrier height of 310 kJ/mol), in agreement with the predietion based on the higher tension of four-membered ring and orbital symmetry considerations. [Pg.425]

From the point of view of associative desorption, this reaction is an early barrier reaction. That is, the transition state resembles the reactants.46 Early barrier reactions are well known to channel large amounts of the reaction exoergicity into product vibration. For example, the famous chemical-laser reaction, F + H2 — HF(u) + H, is such a reaction producing a highly inverted HF vibrational distribution.47-50 Luntz and co-workers carried out classical trajectory calculation on the Born-Oppenheimer potential energy surface of Fig. 3(c) and found indeed that the properties of this early barrier reaction do include an inverted N2 vibrational distribution that peaks near v = 6 and extends to v = 11 (see Fig. 3(a)). In marked contrast to these theoretical predictions, the experimentally observed N2 vibrational distribution shown in Fig. 3(d) is skewed towards low values of v. The authors of Ref. 44 also employed the electronic friction theory of Tully and Head-Gordon35 in an attempt to model electronically nonadiabatic influences to the reaction. The results of these calculations are shown in... [Pg.393]

For many chemical reactions with high sharp barriers, the required time dependent friction on the reactive coordinate can be usefully approximated as the tcf of the force with the reacting solute fixed at the transition state. That is to say, no motion of the reactive solute is permitted in the evaluation of (2.3). This restriction has its rationale in the physical idea [1,2] that recrossing trajectories which influence the rate and the transmission coefficient occur on a quite short time scale. The results of many MD simulations for a very wide variety of different reaction types [3-12] show that this condition is satisfied it can be valid even where it is most suspect, i.e., for low barrier reactions of the ion pair interconversion class [6],... [Pg.245]

In general, the lower the activation energy the faster the reaction. In the limit of a zero barrier , reaction rate will be limited entirely by how rapidly molecules can move. Such limiting reactions have come to be known as diffusion controlled reactions. [Pg.11]

Theory may play two particularly important roles in rationalizing and predicting chemical reaction dynamics. As noted in the last section, the first step to understanding the dynamical behavior of a complex chemical system is breaking down the overall system into its constituent elementary processes. From a theoretical standpoint, the likely importance of various processes may be qualitatively assessed from the potential energy surfaces of putative reactions. Reactions with very high barriers will be less likely to play an important role, while low-barrier reactions will be more likely to do so. [Pg.522]

B. Barrier Reactions Saddle-Point Transition State... [Pg.6]

Barrier reactions Electron transfer Vander Waals reactions Rydberg reactions Exchange reactions Cleavage/addition Norrish reactions... [Pg.8]

The simplest system for addressing the dynamics of barrier reactions is of the type [ABA] — AB + A. This system is the half-collision of the A + BA full collision (see Fig. 14). It involves one symmetrical stretch (Qs), one asymmetrical stretch (QA), and one bend (q) it defines a barrier along the reaction coordinate. [Pg.25]

Figure 14. (a) Potential-energy surfaces, with a trajectory showing the coherent vibrational motion as the diatom separates from the I atom. Two snapshots of the wavepacket motion (quantum molecular dynamics calculations) are shown for the same reaction at / = 0 and t = 600 fs. (b) Femtosecond dynamics of barrier reactions, IHgl system. Experimental observations of the vibrational (femtosecond) and rotational (picosecond) motions for the barrier (saddle-point transition state) descent, [IHgl] - Hgl(vib, rot) + I, are shown. The vibrational coherence in the reaction trajectories (oscillations) is observed in both polarizations of FTS. The rotational orientation can be seen in the decay of FTS spectra (parallel) and buildup of FTS (perpendicular) as the Hgl rotates during bond breakage (bottom). [Pg.26]

Absolute Free Energy Barriers, Reaction Mechanisms, and Kinetic Isotope Effects... [Pg.351]

Finally, it should be mentioned that self-poisoning due to erroneous integer folded depositions is only one manifestation of a productive reaction, which leads to thermodynamic stability, being retarded by a competing lower barrier reaction which almost leads to a stable product. The observations of a crystallization rate minimum in an aromatic polyketone [88], and recently an aromatic polyester [89], are further examples of such an occurrence. [Pg.85]

Salem no.ni) as well as Bartlett and Schneller 15> have approached this point, and written of "retarded one-step and "thoroughly concerted two-barrier reactions. We find it meaningful to describe such processes as bondingly and orbitally concerted, yet energetically nonconcerted reactions, ormore terselyas concerted, two-step reactions. Thus every energetically concerted reaction must be concerted in the other senses, but not vice versa. [Pg.23]

This equilibrium hypothesis is, however, not necessarily valid for rapid chemical reactions. This brings us to the second way in which solvents can influence reaction rates, namely through dynamic or frictional effects. For broad-barrier reactions in strongly dipolar, slowly relaxing solvents, non-equilibrium solvation of the activated complex can occur and the solvent reorientation may also influence the reaction rate. In the case of slow solvent relaxation, significant dynamic contributions to the experimentally determined activation parameters, which are completely absent in conventional transition-state theory, can exist. In the extreme case, solvent reorientation becomes rate-limiting and the transition-state theory breaks down. In this situation, rate con-... [Pg.148]

Figure 2 Reaction potential barriers a — very low barrier, reaction occurs almost instantaneously b — medium barrier, measurable reaction rate c — very high barrier, reaction rate is too slow to be measured...

Quantum Tunneling versus Classical Over Barrier Reactions... [Pg.34]

In all these calculations it was found that although the activation energy seems to be rather low, which might support the occurrence of classical over barrier reactions, the actual process is, however, a pure quantum mechanical tunneling process. [Pg.39]

The derivation of expressions for the multiple kinetic isotope effects of the triple hydrogen transfer case is analogous to the HH-transfer but more tedious. Therefore, the reader is referrred to refs. [25] and [26]. The main results are included in Table 6.2. As in the case of the HH-transfer, the kinetic isotope effects derived for the stepwise transfers are valid in the presence of turmeling and are independent of the tunneling model used. By contrast, the kinetic isotope effects of the single barrier reaction are affected by tunneling. [Pg.160]

In Ref [26] three limiting cases were considered, i.e. a single barrier (Fig. 6.10), a double barrier (Fig. 6.17) and a quadruple-barrier reaction pathway (Fig. 6.18). The first process does not involve any intermediate. The second process consists essentially of consecutive double proton transfer steps, where each step involves a single barrier. There are two possibilities, either protons 1, 2 are transferred first, followed by protons 3, 4, or vice versa, proceeding via the zwitterionic intermediates 1100 or 0011. It is again assumed that the intermediates can be treated as separate species, i.e. that there are no delocalized states involving different potential wells. This assumption will be realized when the barriers are large. Each reaction step is then characterized by an individual rate constant. The process con-... [Pg.161]

The kinetic Fn-I/FID and FID/DD isotope effects are about 5 at room temperature and are similar, i.e. follow the rule of the geometric mean (RGM) as predicted by Fig. 6.14(a). The total HH/DD isotope effect is about 25. Concave Arrhenius curves indicate tunneling at low temperatures. This finding has been interpreted in terms of a single barrier reaction where all H loose zero-point energy in the transition state. [Pg.190]

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