Daniel
Kinzel
a,
Shmuel
Zilberg
b and
Leticia
González
*a
aInstitute of Theoretical Chemistry, University of Vienna, Währinger Straße 17, 1090 Vienna, Austria. E-mail: leticia.gonzalez@univie.ac.at
bInstitute of Chemistry and the Lise-Meitner-Minerva Center for Computational Quantum Chemistry, The Hebrew University of Jerusalem, Jerusalem, Israel
First published on 25th July 2014
Ab initio non-adiabatic dynamics is used to monitor the attack of CH3+ to benzene. The results show that in the gas phase the reaction is ultrafast and is governed by a single electron transfer producing a radical pair.
The purpose of this paper is to find out which of these reaction mechanisms is operative in the gas phase. As a case study, we present for the first time the detailed direct molecular dynamics of the strong electrophile CH3+ for its facial, or broadside, attack on a benzene molecule incorporating all necessary electronically excited states. We employ ab initio non-adiabatic surface hopping molecular dynamics to study the attack of non-rotating CH3+ to benzene, PhH. This reaction has been previously studied using quantum chemistry10 and molecular dynamics11 in the ground state. Both studies concluded that a face-centered π-complex is not formed in the gas phase. However, excited states and the possibility of ET were not considered. Using a static analysis of potential energy surfaces based on complete active space self-consistent field (CASSCF)12 calculations, Xu et al. showed8 that the PhH + CH3+ reaction does start on an electronically excited state (see Fig. 2). Furthermore, they suggested that a conical intersection is a critical point en route to the final σ-complex discriminating the polar path via a π-complex (1) and the ET path (2) (see Fig. 1). But which path is really preferred is not elucidated in that paper. While previous studies are enlightening, a comprehensive mechanism can only be obtained by a dynamical study including excited states. The aim of this paper is to discern among all proposed mechanisms and, additionally, give important insights into the time-resolved evolution of the methyl cation – benzene intermediates and products.
The dynamic simulations have been done including the lowest four electronic singlet states. Potential energies, gradients and wavefunction overlaps for the full system (cation plus benzene) are computed on-the-fly at the CASSCF level of theory (see ESI† for more details). A total of 246 trajectories were simulated, each describing a direct facial attack of a non-rotating methyl cation towards the center of mass of the benzene molecule, CMB (for more details see ESI†). While this scenario is rather idealistic in terms of a real bimolecular collision, we believe that, based on the proposed [PhH–CH3]+-complex structures (see Fig. 2), the chosen collision vector is the most effective when studying the ET process, while leaving out the effect of rotational modes of either benzene or the methyl cation and intentionally neglecting other collision vectors such as a side attack. The initial conditions for both the methyl cation and benzene were represented by a Wigner distribution around their respective vibrational normal modes in the electronic ground state, so that each trajectory started with the vibrational energy equivalent to the quantum-mechanical zero-point energy, which amounts to ca. 2 eV.
To understand the nature of the potential energy surfaces, it is informative to calculate one-dimensional potential curves along the reaction coordinate (r in Fig. 2), while keeping the rest of the degrees of freedom frozen. As it can be seen in Fig. 3(a), the ground state, S0, and the first excited state, S1, are asymptotically degenerated due to the symmetry of the benzene π orbitals. The entry channel, i.e. where the reaction starts, corresponds to the second excited state, S2. These potentials can also be plotted such that the character of the associated wavefunction is preserved (Fig. 3(b)). Then the entry channel corresponds to the [PhH CH3+] state (blue) and this potential crosses with that of the degenerated [PhH˙+ ˙CH3]deg state (yellow) where one electron has been taken from the benzene, PhH, by the electrophile, CH3. The pair of E states is only degenerate asymptotically but the degeneracy will be lifted during the dynamics due to e.g. vibrations. The crossing point between the entry channel and the ground state correlates with a conical intersection between three states that connects the ET and π-complex paths, leading to the radical pair and the π-complex, respectively. Note that the local minimum of the π-complex in this one-dimensional potential is actually a transition state of second order in full dimensions.8,11
![]() | ||
Fig. 3 MS-CASPT2 potential energy curves (see ESI†) for the three lowest electronic singlet states ordered according to energy (a) and according to the character of the wavefunction (b). CI and πTS stand for conical intersection and π-complex transition state, respectively. |
Dynamical simulations are required to unravel the path followed by the reaction. All simulated trajectories show a fast ET and are thereby considered reactive. However, only 63% are successful and lead to the stable formation of a σ-complex while 37% are reflected from the benzene plane and are labelled unsuccessful. In general, excess kinetic energy can either be redistributed in the internal degrees of freedom or can lead to re-dissociation of the [PhH–CH3]+ complex, determining the branching ratio. We believe that in this case the branching ratio is of purely statistical nature and can be associated to the energy flux in the internal degrees of freedom of the system,13 depending on the initial condition of each trajectory.
Snapshots of a representative trajectory for each case are shown in Fig. 4. At each time step, ET is visualized by plotting the density of the hole (compared to the neutral species), thereby localizing the positive charge of the system (see ESI† for details). Additionally, the Mulliken charge of the methyl carbon, QC7, is given for each snapshot. Note that a number of methods exist to describe the electronic distributions in terms of atomic charges and therefore, different definitions of ET can be defined, see e.g.ref. 14.
In both trajectories the methyl cation is approaching the benzene with the positive charge located in the p orbital of the methyl cation carbon – as expected from the entry channel (t = 330 fs). Between 330 and 345 fs the system passes through the three-state conical intersection and hops to one of the [PhH˙+ ˙CH3] states while charge transfer takes place. This process is found in all the trajectories, unambiguously indicating that the path for the electrophilic aromatic substitution in PhH + CH3+ is mediated by a very fast single ET. Up to t = 363 fs the methyl radical follows its momentum towards the benzene ring, but from here, the two trajectories differ. While in (a) the methyl group keeps approaching, in (b) it recoils. In (a), at t = 404 fs the methyl gains back some positive charge while redirecting its momentum to eventually form a σ-bond (t = 433 fs). After complete formation of the σ-bond, isomerization of an arenium ion occurs by shifting a hydrogen (denoted as H1) to another position in the aromatic ring (t = 955 fs and t = 983 fs). H-shifts in arenium ions have been reported to have very low barriers.10,11 In (b), the methyl radical is reflected from the benzene plane, leaving a benzene radical cation behind (t = 404 fs and t = 480 fs). Also in this case, ET has occurred although no stable σ-complex is formed.
Fig. 2 shows the most relevant structures observed in the dynamics. 1 is the reactant, i.e. the methyl cation carbon is not bonded to any other carbon atom. In the σ-complex, 2, the methyl cation carbon is bonded to one carbon of the benzene ring. When the methyl cation carbon is bonded to two carbons a bridged side-π structure, 3, is formed. 4 depicts the situation where one benzene carbon binds to two hydrogens in the σ-complex, on the way to H-shift. Monitoring these structures in time allows identifying the reaction paths. The corresponding connectivities are defined with bond distance thresholds of C–C less than 2.10 Å and C–H less than 1.55 Å. Unsuccessful trajectories can proceed from 1 to 1 directly, or via2 or 3, that is, reflecting but forming a “hot” σ-complex on the way. A stable σ-complex implies the transition from 1 to 2, either directly, or via3, i.e. forming a σ-complex via a side-π-structure. A CH3-shift is described as a transition from 2 to 3 to 2′, and a H-shift is a transition from 2 to 4.
The details of the dynamics involved in the successful and unsuccessful trajectories are presented in Fig. 5. Panels (a) and (g) show the time-dependent spectrum of the distance r, correlating with the number of trajectories at certain r values. It is interesting that both sets of trajectories go through the conical intersection before forming a stable σ-complex or reflecting. Panel (b) shows that the formation of the bond between the methyl and the benzene is not selective. An average C7–C1 of ca. 1.4 Å indicates bond formation at C1, ca. 2.8 Å represents bonding to C2 or C3, and ca. 4.0 Å represents bonding to C4, C5 or C6. Panels (c) and (i) show the relative number of trajectories encountering the structures 1–4 in time. Note that the relative populations of Fig. 5(c) do not add up to 1 because combined 1/2/3 + 4 structures are also possible. Initially, all trajectories start with 1. At t = 375 fs (panel c) there is a rapid increase of the number of trajectories forming a σ-complex (2), although ca. 22% form a side-π structure (3) before forming the single bonded σ-complex. Once the σ-complex is established (after t = 420 fs) rapid H-shifts occur (4). This process stops between t = 550 fs and t = 700 fs, while CH3-shifts happen, as seen by the increasing number of non-bonded (1) and doubly bonded (3) methyl structures while single bonded (2) methyl trajectories decrease. The CH3-shifts are also nicely illustrated in the same time range in panel (b), where the methyl carbon changes positions on the benzene ring. Within the unsuccessful trajectories (panel i), 37% form a “hot” σ-bond (2) or side-π-structure (3), while the remaining 63% is reflected without forming any bond.
![]() | ||
Fig. 5 Time-dependent (td) properties of successful (a–f) and unsuccessful (g–l) trajectories. (a) and (g) td-spectrum of r. (b) and (h) td-spectrum of the distance between the methyl carbon and C1 of benzene. (c) and (i) Accumulated relative amounts of geometries 1–4. (d) and (j) td adiabatic state population in the S0, S1 and S2 states depicted in Fig. 3(a). (e) and (k) td-spectrum and average of the Mulliken charge at the methyl carbon C7, QC7. The inset shows the average in the trajectories reflecting and those forming a “hot” σ-bond. (f) and (l) Expected value of the potential energy of a trajectory. |
The ET process from the benzene to the methyl group is best monitored by the population analysis of the involved states sketched in Fig. 3(a), see Fig. 5 panels (d) and (j). The ET takes place sharply around t = 340 fs, before any bond is formed. Note that 90% of the population transfer takes place through two areas of two-state intersections (S2/S1 and S1/S0), instead of directly from S2 to S0, which accounts for the remaining 10%. The predominance of the former mechanism can also be inferred from the number of hops plotted in Fig. 6. At the S1/S0 and S2/S1 hopping geometries the energy difference between the involved states accounts for ca. 0.3 eV, indicating that the hopping event takes place very close to the conical intersections, while the energy difference from S2 to S0 is larger. The increase in the Mulliken charge at the methyl carbon, both in the successful (e) and unsuccessful (k) trajectories, nicely correlates with the occurrence of an ultrafast ET. As the methyl cation is capturing an electron from the benzene the charge of the methyl carbon is increased by 1e. Subsequently, the methyl carbon forms a σ-bond (Fig. 5e) with the benzene cation. In that case, the positive charge is delocalized over the whole aromat + CH3 and the Mulliken charge at the C7 decreases by 0.2–0.3e (averaged over all trajectories). A similar process takes place in the reflected trajectories (Fig. 5(k)).
![]() | ||
Fig. 6 Number of S2/S1, S1/S0 and S2/S0 hops for the trajectories forming a σ-complex (a) and reflecting (b). |
Fig. 5(f) and (l) show the expectation value of the potential energy of a trajectories relative to the ground state energy at far r distances. The initial zero-point energy amounts to ca. 2 eV, hence, in the beginning, the trajectories possess a potential energy of 3.3 eV. As the methyl cation is approaching the center of mass of benzene, the potential energy decreases as expected from the topology of the potential energy profiles (recall Fig. 3). Accordingly, during the approach, the system gains kinetic energy until t = 400 fs. According to panel (f), the formation of the σ-complex requires to overcome a potential barrier of about 1 eV (t = 470 fs). In view of the large amount of internal kinetic energy, this barrier can be easily surmounted and for practical purposes, it does not represent an obstacle – in agreement with previous studies10,11 that claimed that the formation of the σ-complex occurs barrierless. It can also be argued that the barrier observed here is a result of the momentum gained after the approach of the methyl group, which leads to structures where the r distance is much smaller than the one for the corresponding πTS structure, and hence, creating a pseudo barrier as the methyl is moving back to a benzene carbon. The oscillations in the potential energy after 400 fs reflect the excess kinetic energy of the system, which is responsible for the rapid H- and CH3-shifts observed during the formation of the σ-complex. Barriers of 0.4 eV for the H-shift process were calculated by Ishikawa and coworkers11 in the ground state. Furthermore, from Fig. 5(f), we can retrieve a binding energy of about 2.9 eV for the formation of a stable σ-complex. This value is in good agreement with those obtained from optimized ground state structures and energies reported in ref. 10 and 11. In the unsuccessful trajectories (panel l) most of the kinetic energy leads to re-dissociation and the rest gets internally redistributed after the collision.
Footnote |
† Electronic supplementary information (ESI) available: Computational details. See DOI: 10.1039/c4cp01456a |
This journal is © the Owner Societies 2014 |