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Transition State Theory. Atkins & Depaula: 7.6-7.7

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Transition State Theory. Atkins & Depaula: 7.6-7.7 University of Washington Department of Chemistry Chemistry 453 Winter Quarter 2015 Lecture 22: Transition State Theory. Atkins & DePaula: 7.6-7.7 A. Activated Kinetics Kinetic rate equations are governed by several principles. The first is the Law of Mass Action. It state that for a chemical reaction k f ABAB P (22.1) the rate of formation of product i.e. d[P]/dt is dependent of the reaction concentrations: dP AB kA B (22.2) dt f However, the explicit dependence of stoichiometric coefficients is not general and rigorously only applies to elementary reactions. Deviations may occur for multiple steps involving reaction intermediates. The Principle of Detailed Balance states the relationship of kinetic constants k at equilibrium. For a reversible reaction: ABf at equilibrium the kr forward and reverse reactions are equal: rateforward rate reverse kA kB (22.3) freq eq k B K feq kA r eq Equation 22.3 means the kinetic constants kf and kr are not independent. Their ratio is the equilibrium constant. In equilibrium thermodynamics the van’t Hoff equation gives the temperature dependence of the enthalpy: dKln H (22.4) dT RT 2 Arrhenius proposed an analogous relationship for the temperature dependence of the kinetic constant dkln E f a (22.5) dT RT 2 The assumption of the Arrhenius equation 22.5 is that the reaction rate is determined by the activation barrier Ea at which point on the reaction coordinate molecules are in a high energy ‘activated state” or “transition-state”. The diagram below schematizes the activation barrier Ea. A chemical or physical process whose rate follows equation 22.5 is called an activated process. B. Transition State Theory Transition State Theory (TST) or Activated Complex Theory (ACT) is a reaction mechanism originally developed to describe gas phase collision reactions. It has the general reaction scheme: K † † † A B ABk AB (22.6) where the reactants A and B collide to first form a transition state or activated complex which is designated (AB)†. The idea behind TST is that the transition state is an unstable, short-lived complex. In the case of a simple diatomic collision the transition state (AB)† consists of the AB pair joined by a very weak bond. The colliding molecules A and B are assumed in “equilibrium” with the transition state where Figure 22.1: Barrier of Activation of Height Ea. The Transition State Complex formed between reactants is at the top of the Barrier AB† K † (22.7) AB This equilibrium notation however involves the transition state which actually exists at a energy maximum and is thus transitory in nature, as its name implies. For the diatomic reaction mechanism the rate is given by †† †† rate k AB k K A B k2 A B (22.8) To evaluate the rate constant k2, we can apply statistical methods to K † † qAB qN† K † N AB (22.9) qq AB qqAB NN † † where the partition functions of A, B, and AB are qA, qB, q AB, respectively . † The treatment of qAB requires some explanation about the properties of the transition complex. It is assumed that when A and B form the transition complex the complex acquires translation, rotational, vibrational and electronic motions, which all must be reflected in the partition function, i.e. ††††† qqqqqAB trans rot vib elec 3/2 † † 2† hkT /2 B 2 mkTB 8 IkT e † B † DkTeB/ 32† ge1 hh 1 ehkT / B 3/2 † 2† 2 mkTB 81 IkT † B † D0 /kTB 32† ge1 hh 1 ehkT / B h † where in 22.5 we have used the relationship DD†† (22.10) e 0 2 In 22.5 the mass of the transition state in the translational partition † function is just mmmAB. In the rotational partition function mm 2 where the reduced mass AB , I †† R is the mmAB moment of inertia of the transition complex and R† is the length of the bond that is in the process of forming between A and B. The † term g1 is the degeneracy of the ground electronic state of the transition complex. The vibrational motion is treated in the following way. We assume as A and B come together to form the transition complex that translational motion along the reaction coordinate is eventually converted in part to a vibrational motion of the bond also directed along the reaction coordinate. We use the notation ††† qqq † † AB,,, trans AB rot AB vib D0 /kTB KNge 1 (22.11) qqAB † 1 where qAB, vib † is a reduced vibrational partition 1 ehkT / B function. Now the vibrational of the bond in the transition complex is assumed to occur at a very low frequency such that † 11kTB qAB, vib † † (22.12) hkT / B † 1 e 11hkT /B h In other words the bond vibration is calculated in the high temperature † limit where kTB h . Now we also assume that the transition complex is converted to product AB within a vibrational period so that k †† . Using this expression and equation 22.7 we obtain †† qqAB,, trans AB rot kT D† /kT kkK†† †B Nge †0 B 21qq h † AB (22.13) †† qq † AB,, trans AB rot kTB † DkT0 / B Ng1 e qqAB h This is called the Eyring equation. To equation 22.13 is added ad hoc a constant 1. This is called the transmission coefficient and expresses the fact that not all collisions result in the formation of the transition complex. Normally 0.5 1, but can be quite small for atomic collisions. The final form for the Eyring equation is kT kKN B † (22.14) 2 h †† qq † ††AB,, trans AB rot D0 /kTB where Kge 1 is absent the degree of qqAB vibrational freedom treated in the high temperature limit and giving rise to kT the factor of B . h Reaction rates are normally measured as per mole quantities so in equation 22.9 N=NA: kT RT kNB K†† K (22.15) 2,mAhh B. Examples of Diatomic Transition State Calculations For the collision of two atoms we have 3/2 2†2 VmmkT2 ABB 8R kTB qqg††† g † AB,,1 trans AB rot hh32 1 3/2 VmkT2 AB qg A (22.16) A h3 1 3/2 VmkT2 BB qg B B h3 1 Then we obtain for the rate constant 3/2 2†2 kT DkT† / 2 mmkTABB 8RkT B kNB e0 B 2 A hhh32 (22.17) 33†† 2 † hhgkTg118 B † D0 /kTB 3/2 3/2 AB NReA AB gg gg 22mkTAB mkT BB 11 11 † If D0 is reported in units of Joules per mole we must write: † 2 † 8 kTB † g1 D0 /RT kN2 A RAB e (22.18) gg11 C. More Complicated Reactions: Ternary Complexes The simplest example of a ternary transition complex is the isotope exchange HDHDH2 (22.19) The transition complex has linear form HHD where the bonds lie along the reaction coordinate. The rate constant has the form: † qkTDkT† / kT keKHHD B0 B B † (22.20) 2 qq h h DH2 ††H2 where DDD000 . The partition functions for qD and qH2 are obtained as usual † for atomic and diatomic species. The transition complex partition function qHHD is treated as follows. The transition complex is linear so it has a single moment of inertia and rotations are calculated by the same procedure used for a linear triatomic like CO2 except that =1 for HHD. The vibrational partition function is treated as follows. Note for a linear triatomic there are four vibrational modes in the partition function corresponding to symmetric and asymmetric stretches and two equivalent bending modes HHD HHD HHD asymmetric symmetric Doublydeg enerate stretch stretch bend The asymmetric stretch contributes to the reaction coordinate, is therefore treated in the high temperature limit and yields the kBT/h term in the Eyring equation. The other three vibrational modes remain in the transition complex partition function 3/2 3 22 mmkTHDB 2IkT 1 qg†† HHD B (22.21) HHD 321 hkT jB/ h j1 1 e .C. Gibbs Energy of Activation Returning to the general expression for the molar reaction rate RT kNk K† , we define formally the Gibbs energy of activation 2,mA 2 h GRTK††ln (22.22) Using equation 28.15 we now define the kinetic constant as: RT † ke GRT/ (22.23) 2,m h Using the corresponding relationship between the Gibbs energy, enthalpy and entropy... GHTS†† † we further obtain: RT††† RT keGRT/// ee SR HRT (22.24) 2,m hh Note equation 22.24 sets an upper limit for the activated reaction rate . For G† 0 and 1 at T=300K: 23 1 kT 1.38 10JK 300 K ksmax B 6.25 1012 1 (22.25) 2 hJs6.62 1034 .
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