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Article

Quantum-Chemical Study of the Benzene Reaction with Fluorine

by
Sergey O. Adamson
1,
Daria D. Kharlampidi
2,3,
Anastasia S. Shtyrkova
2,
Stanislav Y. Umanskii
1,
Yuri A. Dyakov
1,4,
Igor I. Morozov
1 and
Maxim G. Golubkov
1,*
1
Semenov Federal Research Center for Chemical Physics, Russian Academy of Sciences, 119334 Moscow, Russia
2
Department of Biology and Chemistry, Moscow State Pedagogical University, 119435 Moscow, Russia
3
Department of Gravitation and Cosmology, RUDN University, 117198 Moscow, Russia
4
Research Center for Environmental Changes, Academia Sinica, Taipei 115, Taiwan
*
Author to whom correspondence should be addressed.
Atoms 2023, 11(10), 132; https://doi.org/10.3390/atoms11100132
Submission received: 1 September 2023 / Revised: 10 October 2023 / Accepted: 14 October 2023 / Published: 17 October 2023
(This article belongs to the Section Quantum Chemistry, Computational Chemistry and Molecular Physics)
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Abstract

:
The reaction of benzene with fluorine atoms may be of interest as a source of phenyl and ipso-fluorocyclohexadienyl radicals or as a method for fluorobenzene gas phase synthesis. The structures and electronic energies of the equilibrium configurations and transition complexes of the C6H6F system are calculated in the density functional approximation. It was found that the interaction of benzene with atomic fluorine can proceed via two channels: hydrogen abstraction with the phenyl radical formation, and hydrogen substitution with the ipso-fluorocyclohexadienyl radical as primary product. Then the dissociation of the ipso-fluorocyclohexadienyl radical leads to creation of fluorobenzene and atomic hydrogen. The initiation of this reaction requires the activation energy near 27 kcal/mol, which indicates the low probability of this process, occurring at temperatures close to the standard (298 K). The calculations of the fluorocyclohexadienyl isomers and their cations also indicate that the formation of fluorobenzene as a product of secondary reactions is unlikely. The conclusions are confirmed by experimental data.

Graphical Abstract

1. Introduction

Chemical reactions between benzene and fluorine atoms began to attract the close attention of investigators more than fifty years ago [1]. Initially, the interest was due to the possibility of using hydrogen abstraction in studies of the structure and properties of free radicals as a source of phenyl and fluorocyclohexadienyl radicals [1,2]. Later, it was found that the interaction of benzene with fluorine atoms also results in the formation of fluorine-substituted derivatives of benzene in high yield, which made it possible to consider this reaction as a method for their synthesis [2,3].
Analysis of the electron paramagnetic resonance (EPR) spectra showed that the mixture of benzene and molecular fluorine during photolysis in an argon matrix presumably contains fluorocyclohexadienyl and phenyl radicals [1]. Based on this observation, a mechanism for benzene fluorination was proposed, which includes the reactions of hydrogen atom detachment followed by fluorine attachment:
C6H6 + F → C6H5 + HF,
C6H6 + F → C6H6F.
The formation of the fluorocyclohexadienyl radical has been confirmed later in molecular crossed beams experiments [4,5,6,7,8,9] and argon matrix [10].
At pressures of 0.4–4.0 atmosphere, the only stable product of gas-phase benzene fluorination is fluorobenzene. The reaction yield weakly depends on the pressure in the reaction vessel and varies in the range of 6–10% [11]. In order to explain this result, reaction (2) has been supplemented by stages of vibrationally excited fluorocyclohexadienyl radical C6H6F* formation, followed by collisional relaxation and dissociation, i.e.,
C6H6 + F → C6H6F* → C6H6F → C6H5F + H.
The presence of fluorobenzene in benzene fluorination products has been also confirmed by reactions in crossed molecular beams [7,8,12,13] and in a low-pressure flow reactor [2]. Experimental measurement of the ratio between rate constants of reactions (1) and (3) revealed that substitution (3) is the main channel of benzene fluorination [2,13,14]. In particular, the yield of fluorobenzene in the low-pressure flow reactor was estimated at 80 ± 20% [2], which significantly differs from another assessment [11].
The aim of this study is the calculation of structures and electronic energies of both equilibrium configurations and transition state complexes of the system C6H6 + F, which will make it possible to formulate a conclusion about the reaction mechanisms of hydrogen abstraction and substitution in benzene. The only known theoretical work related to this topic is devoted to complexes of benzene with halogens, including isomers of the fluorocyclohexadienyl radical [15]. The next sections of the article contain a thorough description of the calculation method, the main results, and a summary discussion.

2. Calculation Method

In order to isolate the reaction channels, we used the reaction path Hamiltonian approach. Taking into account the number of electrons in the system C6H6F, the density functional method (DFT) has been used to calculate the potential energy surface (PES) of the ground electronic state in the stationary points. The type of the functional, as far as the basis set of atomic orbitals (AO) has been calibrated during the calculations in order to reach sufficient agreement with reference data. It was shown previously that hybrid meta-functionals of the M06–M08 families make it possible to estimate the thermodynamic effects in the reactions of organic compounds with good accuracy [16,17,18], so as candidates we used M06, M06-2X, and M08-HX functionals. In the calculations we used basis sets A: 6-31++G** [19,20,21], B: aug-cc-pVDZ [22,23], and C: cc-pVTZ [22]. Diatomic molecules HF and CF were used as model systems for comparing functionals and AO bases. All calculations have been performed by the ab initio program package GAMESS US [24,25].
Comparison of the obtained results revealed that for HF and CF molecules the best agreement with the experimental data [26,27,28] for Re (equilibrium internuclear distance), we (vibrational constant), and De (dissociation energy) observed in basis C (functional M08-HX). Deviation for Re is not more than 0.002 Å, for we is about 10 cm−1, and for De is less than 0.15 eV (3.5 kcal/mol). In other combinations of the basis and functional, it is not possible to achieve simultaneous reproduction of the target parameters both for HF and CF (see Table 1). Subsequently, the functional M08-HX (basis C) has been chosen as a method for the further search of the PES stationary points.
To check the accuracy of the chosen method, we have performed energy calculations of transition state complexes and equilibrium configurations of the reaction participants, i.e.,
CH4 + F → CH4F → CH3 + HF.
This reaction has been selected due to the fact that the rate constants of hydrogen abstraction reactions (1) and (4) have similar values [29,30].
Table 1. The values of parameters Re (Å), we (cm−1), and De (eV) for HF and CF molecules.
Table 1. The values of parameters Re (Å), we (cm−1), and De (eV) for HF and CF molecules.
MethodAO BasisHF (X1Σ+)CF(X2Π)
ReweDeReweDe
B3LYPA0.927740755.961.290112705.65
B0.925940665.971.290612445.62
C0.922540945.941.276113055.80
M06A0.919642256.111.278613315.73
B0.918242386.091.278513055.67
C0.915342306.041.262213715.91
M06-2XA0.922741805.931.278113375.67
B0.921241675.941.278813115.66
C0.918341935.941.268113585.78
M06-HXA0.923441286.101.284212945.65
B0.921341136.101.284812615.64
C0.918341356.051.272613165.73
CCSD(T)A0.925041235.771.301212535.26
B0.923940805.841.305612065.20
C0.916341935.971.273513325.61
Experiment–0.9168 a,b4138 a6.14 b
6.11 c		1.2718 a1308 a,d5.50 e
5.75 f
(a) Ref. [26]; (b) Ref. [27]; (c) Ref. [31]; (d) Ref. [28]; (e) Ref. [32]; (f) Ref. [33].
For reaction (4) the relative energy of reaction products is E(4) = E(CH3 + HF) = −29.6 kcal/mol. The zero here is the energy of the initial reactants with zero point energy (ZPE) correction. Theoretical estimation of the enthalpy of reaction under standard conditions (here and below we use values p = 101,325 Pa and the temperature T = 298.15 K for pressure and temperature) is ΔH0R(4) = −28.9 kcal/mol, that is 2.6 kcal/mol more than the experimental values [34,35]. The experimental value of the activation energy is estimated in the range of 0.4–1.9 kcal/mol [36,37], and the best theoretical result is about −0.1 kcal/mol whereas other estimations lie in the range from −2.66 to 1.70 kcal/mol [38]. The calculated value of relative energy of the transition complex is E(CH4F) = −1.5 kcal/mol, which is in good agreement with the theoretical estimations given in [38].
The reaction (4) and its analogs have two channels, i.e., CH4 + F(2P3/2) and CH4 + F(2P1/2), differing in energy by 400 cm−1 (1.14 kcal/mol), with various transition complexes and the states of the products. To date, the employed experimental methods do not imply separate measurements of the rate constants of reaction (4) for the 2P3/2 and 2P1/2 components of the ground state of the fluorine atom [34,38]. As a consequence, both components must be present in the reaction mixture in a ratio depending on the method of atomic fluorine obtaining. Since the experimental activation energy of the reaction (4) (0.4–1.9 kcal/mol [36,37]) is close to the energy difference between the components of the fluorine electronic ground state, the corresponding rate constant measuring results are impossible to explain without dividing into 2P3/2 and 2P1/2 components of the fluorine atom ground state. Nevertheless, the close values of the experimental and theoretical values of the rate constants [34,38] indicate the possibility of using nonrelativistic semi-empirical PESs to interpret the experiments.
The theoretical estimates of the reaction enthalpy ΔH0R (4) under standard conditions (hereinafter, pressure is p = 101,325 Pa, and temperature is T = 298.15 K) are −28.9 kcal/mol (cc-pVTZ basis)), −29.9 kcal/mol (cc-pVQZ), −30.6 kcal/mol (aug-cc-pVTZ) and −30.8 kcal/mol (aug-cc-pVQZ) and converge to experimental values of −31.3 … −31.5 kcal/mol [34,35]. On the contrary, the relative energies (zero is taken to be the energy of the initial reactants with corrections for the energies of the main vibrational states) of the transition complex for the same AO basis range from −1.5 kcal/mol up to −1.0 kcal/mol, differing significantly from the experimental values of the activation energy [36,37].
The discrepancy between the experimental and theoretical values of the reaction (4) activation energies is not the result of the AO basis incompleteness or an unbalanced description of the CH4F transition complex and its dissociation products. However, it can be considered a method error when interpreting the results of nonrelativistic calculations.

3. Results and Discussion

On the base of the selected version of density functional (M08-HX, basis C), the equilibrium geometry configurations of ipso-, ortho-, meta-, para-fluorocyclohexadienyl radicals (C6H6F), van der Waals complex (C6H5F·H), and transition state complexes corresponding to the reactions (1) and (2) have been found (Table 2). Structures of equilibrium configurations and transition state complexes of fluorocyclohexadienyl radicals are presented in Figure 1. The obtained internuclear distances and bond angles for ipso-fluorocyclohexadienyl radical agree with the values calculated by B3LYP and BH&HLYP [15].
To identify the reaction channels with the found transition states, the minimum energy pathways were calculated for all transition states. Based on the analysis of stationary points and reaction pathways of the ground electronic state PES of C6H6F the next reactions can be expected (see Figure 2).
C6H6 + F → TS1 → C6H5 + HF,
C6H6 + F → C6H6F → TS2 → C6H5F·H → C6H5F + H.
Experimental estimates of the activation energy (5) were not carried out, but it was found that the vibrational-rotational levels with quantum numbers v = 1 (0.42–0.60) and v = 2 (0.30–0.40) are maximally populated in the HF molecule. Based on this fact, an assumption that the activation barrier is close to the reaction threshold (energy of the initial reagents) has been made. Moreover, the method of competing reactions shows that the ratio of the rate constants of hydrogen detachment in methane and benzene is close to unity, that is, the activation energies of these reactions should also have close values [13,29]. The theoretical value of the relative energy of the transition state E(TS1) = −2.9 kcal/mol falls below the reaction threshold, and 4.4 kcal/mol below the sum of the energies of phenyl radical and vibrationally excited hydrogen fluoride (v = 2) (Figure 2), which indicates an error in the calculation method, like in the case of reaction (4), arising due to the using of non-relativistic approach.
The transition state for the initial stage C6H6 + F → C6H6F of the reaction (6) could not be localized. ipso-C6H6F turned out to be the closest stationary point of the PES when the initial conditions (i.e., orientation and distance between the F atom and the benzene center of mass) were varied. That is why this stage of the reaction (6) was further considered barrierless. The relative energy of the intermediate is E(ipso-C6H6F) = −33.3 kcal/mol (Figure 2). This value of the relative energy agrees well with the values calculated using the functionals BH&HLYP (−28.9 kcal/mol) and B3LYP (−34.0 kcal/mol) [15]. The substitution reaction is finalized by the dissociation of the ipso-fluorocyclohexadienyl radical with the formation of fluorobenzene and hydrogen atoms. This stage is an endothermic process with activation energy ΔE = E(TS2) − E(ipso-C6H6F) = 26.9 kcal/mol, and relative products yield E(6) = E(C6H5F+H) = −14.6 kcal/mol.
Comparison of experimental and theoretical values of enthalpies of reaction products (5) and (6) shows that, as in the case of the reaction (4), the PES of C6H6F has systematic errors (Table 3). Information about the reagents and transition state complexes of reactions (5) and (6), obtained from quantum chemical calculations, can be used to estimate the rate constants in the framework of the statistical theory of chemical reactions. In order to compensate for the error of the method, it is necessary to introduce a correction (shift) for the relative energies (enthalpies) of the initial reagents (C6H6 + F) and products (C6H5 + HF). Taking into account that the activation energy of the reaction (5) should differ little from the activation energy (4), equal to 1 kcal/mol, the correction value can be estimated as approximately −4.5 kcal/mol (Table 3).
The comparison of absorption bands in the IR spectrum [10] with the frequencies of the ipso-fluorocyclohexadienyl radical fundamental vibrations, calculated in the “rigid rotator—harmonic oscillator” approximation, allows us to conclude that the frequencies and intensities of the experimental and calculated oscillations in most cases are close (Figure 3). Absorption bands at 1000 and 1094 cm−1 differ many times in intensities, and the band at 912 cm−1 does not coincide with any of the calculated frequencies of fundamental vibrations. Compared with the ones of other isomers of the composition C6H6F (see Figure 1), coincidence with the experimental bands is not observed, which indicates about the absence of isomerization of the ipso-fluorocyclohexadienyl radical.
The calculations also do not reveal any transition complexes corresponding to the isomerization of fluorocyclohexadienyl radicals. This can be explained by the fact that the deformation of the carbon skeleton of fluorocyclohexadienyl radicals is a relatively slow process, and requires a significant amount of energy. Hence, it follows that the transition complexes corresponding to rearrangements of isomers into each other should be metastable complexes of fluorobenzene and the hydrogen atom: C6H5F·H, with energies, close to the energy of the dissociation products of the ipso-fluorocyclohexadienyl radical (C6H5F + H), and having significant (2–3 Å) the length of one of the C-H bonds. Complexes of such structure can be formed as a result of collisions of fluorobenzene with hydrogen atoms, i.e., due to the interaction between the reaction products (6). Thus, the ipso-fluorocyclohexadienyl radical isomerization can be considered a negligible process.
A special consideration requires the question about the reasons for the appearance of fluorobenzene in the reaction mixture. Considering that the minimum output of 6–10% was found during the fluorination of benzene in a closed volume with radiochromatographic control of the reaction products [11], and the maximum of 80% in a low-pressure flow reactor with mass spectrometric control [2], it can be assumed that in addition to the dissociation of the ipso-fluorocyclohexadienyl radical (6), there may be other channels leading to its formation. The most probable can be a recombination of the fluorocyclohexadienyl radical with phenyl radical, as far as decomposition of the molecular ion C6H6F+ directly in the chamber of the mass spectrometer.
Formally, fluorobenzene can be a product of C6H6F and C6H5 radical recombination, i.e.,
C6H5 + C6H6F → C6H5F + C6H6.
This reaction is exothermic, the theoretical estimate of the reaction enthalpy is ΔH0R (298 K) = −94.10 kcal/mol, which indicates that the reaction is possible. The mass spectrum of benzene fluorination products contains fluorobenzene molecular ions (m/z = 96) and, in a much smaller amount, ions of phenyl radical (m/z = 77), but there are no molecular benzene ions (m/z = 78) [2]. Because there is no significant amount of benzene molecules in the mixture, the reaction (7) is unlikely.
Analysis of the experimental results shows that the molecular ion C6H6F+ has two main dissociation channels, i.e.,
C6H6F+ → C6H5+ + HF,
C6H6F+ → C6H4F+ + H2.
Channel (8) is the lowest in energy, and the channel threshold (9) is 20.3 kcal/mol lower than the threshold (8). The main stable dissociation product is HF, which corresponds to the decay through the channel (8), whereas contribution to the dissociation from (9) does not exceed 4% [40,41,42].
Theoretical reaction mechanism (8) predicts the possibility of rearrangement of ortho- and ipso-isomers C6H6F+ into the ion-dipole complex C6H5+·HF (F-isomer) followed by barrier-free dissociation into C6H5+ and HF [40]. This result is partially confirmed by experiment: in the IR region of the absorption spectrum of the reaction mixture, there are individual lines of ortho- and para-isomers of ions C6H6F+ [41] and ion-dipole complex C6H5+·HF (F-isomer) [42,43,44]. In addition, the possibility of dissociation of ortho- and ipso-isomers C6H6F+ was shown through metastable vibrational states, bypassing the stage of formation of F-isomer [42]. Our calculations confirm the mechanism [40], deviations in the relative energies of stable isomers and transition states do not exceed 2 kcal/mol (Figure 4). Structural parameters for the charged isomers C6H6F+ and transition complexes are consistent with the previously calculated ones [40,41,42,43]. Summing up the intermediate result, we note that the formation of fluorobenzene as a result of the decay of isomeric ions C6H6F+ should be assumed unlikely since the main stable products of their decay are HF and H2.
It remains to be assumed that fluorobenzene is formed as a result of a two-channel reaction of F and C6H6 (see (5), (6), and Figure 2), passing by pathway (6) through an intermediate complex C6H6F* (TS2). As mentioned above, the stage of dissociation of ipso-fluorocyclohexadienyl radical has a rather high activation threshold (near 26.9 kcal/mol), which indicates about low probability of this reaction occurring under standard conditions. However, in most studies, the source of fluorine atoms was the dissociation reaction F2 → 2F, activated thermally [4,5,6,7,8,9,12,13] or by high-frequency discharge [2,30,39]. The oven temperature ranged from 1023 K [4,5,6,7,8,9] up to 1100 K [12,13] whereas the fluorine thermal atomization threshold is about 650 K [12]. Temperature measurements in the reaction zone were not carried out, but in one of the works it was estimated as the arithmetic mean of the temperatures of benzene and atomic fluorine, and was rated at 660–700 K [12,13]. This estimate, despite its approximate nature, confirms the possibility of the formation of fluorobenzene in the reaction (6). Note, that the dissociation of F2 under the influence of a microwave discharge is a typical method for fluorine atomization in the method of competing reactions [30,39,45]. In this case, the degree of F2 dissociation was estimated at approximately 97%, which indicates a higher temperature of the reaction mixture compared to previous results [12,13].
It should be noted that the formation of fluorobenzene in the presence of methane [30] may pass through a more complex mechanism, with the formation of ions CH5+ and their subsequent interaction with fluorobenzene molecules, including the formation of an intermediate CH5+C6H5F [44] and its dissociation in the chamber of the mass spectrometer
CH5+ + C6H5F → CH5+C6H5F → CH4 + C6H6F+.
The degree of influence of these processes on the yield of fluorobenzene has not been studied to date.

4. Conclusions

Thus, the calculations predict two channels for the interaction of benzene with atomic fluorine: the elimination of hydrogen to form the phenyl radical and the addition of fluorine to form the ipso-fluorocyclohexadienyl radical, in full agreement with the experimental results. Calculated values of the enthalpies of intermediates and reaction product formation are in good agreement both with their experimental values and with the values found in independent calculations. Calculations predict that dissociation of the ipso-fluorocyclohexadienyl radical into fluorobenzene and atomic hydrogen is unlikely at standard temperature since this stage of the reaction has a rather high activation barrier. The experimentally observed dissociation of the ipso-fluorocyclohexadienyl radical with the formation of fluorobenzene can be explained by the fact that the temperature of fluorine atoms (near 1000 K) is sufficient to initiate this reaction. The formation of fluorobenzene due to the occurrence of secondary reactions is unlikely.

Author Contributions

Conceptualization, S.O.A., D.D.K., S.Y.U., I.I.M. and M.G.G.; methodology, S.O.A., D.D.K., S.Y.U., Y.A.D. and M.G.G.; software, S.O.A., D.D.K., A.S.S. and Y.A.D.; validation, S.O.A., D.D.K. and S.Y.U.; formal analysis, S.O.A., A.S.S. and S.Y.U.; investigation, S.O.A., D.D.K., A.S.S., S.Y.U., Y.A.D., I.I.M. and M.G.G.; resources, S.O.A., D.D.K. and Y.A.D.; data curation, S.O.A., D.D.K., A.S.S., S.Y.U., Y.A.D. and M.G.G.; writing—original draft preparation, S.O.A., D.D.K., A.S.S., S.Y.U., Y.A.D. and M.G.G.; writing—review and editing, S.O.A., S.Y.U., I.I.M. and M.G.G.; visualization, S.O.A. and D.D.K.; supervision, S.Y.U., I.I.M. and M.G.G.; project administration, M.G.G.; funding acquisition, M.G.G. All authors have read and agreed to the published version of the manuscript.

Funding

This study was carried out in the framework of State Assignment of the Ministry of Science and Higher Education of the Russian Federation (project No. 122040500060-4). Y.A.D. was funded by Taiwan National Science and Technology Council (NSTC) grant NSTC 111-2111-M-001-008.

Data Availability Statement

Not applicable.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Cochrain, E.L.; Adrian, F.J.; Bowers, V.A. Electron Spin Resonance Study of Elementary Reactions of Fluorine Atoms. J. Phys. Chem. 1970, 74, 2083–2090. [Google Scholar] [CrossRef]
  2. Ebrecht, J.; Hack, W.; Wagner, H.G. Elementary Reactions of Fluorine Atoms with Benzene, Toluene, p-Xylene and Etylbenzene. Bericht. Bunseng. Phys. Chem. 1989, 93, 619–626. [Google Scholar] [CrossRef]
  3. Vasek, A.H.; Sams, L.C. The Reaction of Atomic Fluorine with Fluorobenzene. J. Fluor. Chem. 1974, 3, 397–401. [Google Scholar] [CrossRef]
  4. Parson, J.M.; Lee, Y.T. Crossed Molecular Beam Study of F + C2H4, C2D4. J. Chem. Phys. 1972, 56, 4658–4666. [Google Scholar] [CrossRef]
  5. Parson, J.M.; Shobatake, K.; Lee, Y.T.; Rice, S.A. Unimolecular Decomposition of the Long-lived Complex Formed in the Reaction F + C4H8. J. Chem. Phys. 1973, 59, 1402–1415. [Google Scholar] [CrossRef]
  6. Parson, J.M.; Shobatake, K.; Lee, Y.T.; Rice, S.A. Substitution Reactions of Fluorine Atoms with Unsaturated Hydrocarbons. Crossed Molecular Beam Studies of Unimolecular Decomposition. Farad. Disc. Chem. Soc. 1973, 55, 344–356. [Google Scholar] [CrossRef]
  7. Shobatake, K.; Parson, J.M.; Lee, Y.T.; Rice, S.A. Laboratory Angular Dependence and the Recoil-Energy Spectrum of the Products of the Reaction F + C6D6 → D + C6D5F. J. Chem. Phys. 1973, 59, 1427–1434. [Google Scholar] [CrossRef]
  8. Shobatake, K.; Lee, Y.T.; Rice, S.A. Reactions of F atoms and Aromatic and Heterocyclic Molecules: Energy Distribution in the Reaction Complex. J. Chem. Phys. 1973, 59, 1435–1448. [Google Scholar] [CrossRef]
  9. Grover, J.R.; Wen, Y.; Lee, Y.T.; Shobatake, K. Crossed-Beam Reactive Scattering of F2 Plus C6H6: Heat of Formation of Ipso-Fluorocyclohexadienyl Radical. J. Chem. Phys. 1988, 89, 938–946. [Google Scholar] [CrossRef]
  10. Jacox, M.E. Reaction of F Atoms with C6H6 Vibrational Spectrum of the C6H6F Intermediate Trapped in Solid Argon. J. Phys. Chem. 1982, 86, 670–675. [Google Scholar] [CrossRef]
  11. Cramer, J.A.; Rowland, F.S. Gas Phase Fluorination of Benzene, Fluorobenzene, m-difluorobenzene, and Trifluoromethylbenzene by Reactions of Thermal Fluorine-18 Atoms. J. Am. Chem. Soc. 1974, 96, 6579–6584. [Google Scholar] [CrossRef]
  12. Moehlmann, J.G.; Gleaves, J.T.; Hudgens, J.W.; McDonald, J.D. Infrared Chemiluminescence Studies of the Reaction of Fluorine Atoms with Monosubstituted Ethylene Compounds. J. Chem. Phys. 1974, 60, 4790–4799. [Google Scholar] [CrossRef]
  13. Moehlmann, J.G.; McDonald, J.D. Infrared Chemiluminescence Investigation of the Abstraction Reactions between Fluorine Atoms and Unsaturated Compounds. J. Chem. Phys. 1975, 62, 3061–3065. [Google Scholar] [CrossRef]
  14. Obara, M.; Fujioka, T. Pulsed HF Chemical Lasers from Reactions of Fluorine Atoms with Benzene, Toluene, Xylene, Methanol, and Acetone. Jpn. J. Appl. Phys. 1975, 14, 1183–1187. [Google Scholar] [CrossRef]
  15. Tsao, M.L.; Hadad, C.M.; Platz, M.S. Computational Study of the Halogen Atom-Benzene Complexes. J. Am. Chem. Soc. 2003, 125, 8390–8399. [Google Scholar] [CrossRef]
  16. Zhao, Y.; Truhlar, D.G. Density Functionals with Broad Applicability in Chemistry. Acc. Chem. Res. 2008, 41, 157–167. [Google Scholar] [CrossRef]
  17. Zhao, Y.; Truhlar, D.G. Exploring the Limit of Accuracy of the Global Hybrid Meta Density Functional for Main-Group Thermochemistry, Kinetics, and Noncovalent Interactions. J. Chem. Theory Comp. 2008, 4, 1849–1868. [Google Scholar] [CrossRef]
  18. Adamson, S.O. Reactions C2H2 + OH and C2 + H2O: Ab Initio Study of the Potential Energy Surfaces. Russ. J. Phys. Chem. B 2016, 10, 143–152. [Google Scholar] [CrossRef]
  19. Hehre, W.J.; Ditchfield, R.; Pople, J.A. Self-Consistent Molecular Orbital Methods. XII. Further Extensions of Gaussian-Type Basis Sets for Use in Molecular Orbital Studies of Organic Molecules. J. Chem. Phys. 1972, 56, 2257–2261. [Google Scholar] [CrossRef]
  20. Hariharan, P.C.; Pople, J.A. The Influence of Polarization Functions on Molecular Orbital Hydrogenation Energies. Theor. Chim. Acta 1973, 28, 213–222. [Google Scholar] [CrossRef]
  21. Clark, T.; Chandrasekhar, J.; Spitznagel, G.W.; Schleyer, P.V.R. Efficient Diffuse Function-Augmented Basis Sets for Anion Calculations. III. The 3-21 + G Basis Set for First-Row Elements, Li-F. J. Comp. Chem. 1983, 4, 294–301. [Google Scholar] [CrossRef]
  22. Dunning, T.H., Jr. Gaussian Basis Sets for Use in Correlated Molecular Calculations. I. The Atoms Boron through Neon and Hydrogen. J. Chem. Phys. 1989, 90, 1007–1023. [Google Scholar] [CrossRef]
  23. Kendall, R.A.; Dunning, T.H., Jr.; Harrison, R.J. Electron Affinities of the First-Row Atoms Revisited. Systematic Basis Sets and Wave Functions. J. Chem. Phys. 1992, 96, 6796–6806. [Google Scholar] [CrossRef]
  24. Schmidt, M.W.; Baldridge, K.K.; Boatz, J.A.; Elbert, S.T.; Gordon, M.S.; Jensen, J.H.; Koseki, S.; Matsunaga, N.; Nguyen, K.A.; Su, S.; et al. General Atomic and Molecular Electronic Structure System. J. Comp. Chem. 1993, 14, 1347–1363. [Google Scholar] [CrossRef]
  25. Gordon, M.S.; Schmidt, M.W. Advances in electronic structure theory: GAMESS a decade later. In Theory and Applications of Computational Chemistry: The First Forty Years; Dykstra, C.E., Frenking, G., Kim, K.S., Scuseria, G.E., Eds.; Elsevier: Amsterdam, The Netherlands, 2005; pp. 1167–1189. [Google Scholar] [CrossRef]
  26. Huber, K.P.; Herzberg, G. Molecular Spectra and Molecular Structure. IV. Constants of Diatomic Molecules, 1st ed.; Springer: New York, NY, USA, 1979; 716p. [Google Scholar] [CrossRef]
  27. Feller, D.; Peterson, K.A. Hydrogen Fluoride: A Critical Comparison of Theoretical and Experimental Results. J. Mol. Struct. Theochem. 1997, 400, 69–92. [Google Scholar] [CrossRef]
  28. Gondal, M.A.; Rohrbeck, W.; Urban, W. Vibration-Rotation Transitions in the CF Radical, Studied by Laser Magnetic Resonance Spectroscopy at 7.8 p.m. J. Mol. Spectr. 1983, 100, 290–302. [Google Scholar] [CrossRef]
  29. Smith, D.J.; Setser, D.W.; Kim, K.C.; Bogan, D.J. HF Infrared Chemiluminescence. Relative Rate Constants for Hydrogen Abstraction from Hydrocarbons, Substituted Methanes, and Inorganic Hydrides. J. Phys. Chem. 1977, 81, 898–905. [Google Scholar] [CrossRef]
  30. Vasiliev, E.S.; Volkov, N.D.; Karpov, G.V.; Savilov, S.V.; Morozov, I.I.; Lunin, V.V. Mass Spectrometry Study of the Reaction of Fluorine Atoms with Benzene. Russ. J. Phys. Chem. A 2020, 94, 2004–2009. [Google Scholar] [CrossRef]
  31. Darwent, B. Bond Dissociation Energies in Simple Molecules; National Bureau of Standarts: Washington, DC, USA, 1970; 48p. [Google Scholar]
  32. Porter, T.L.; Mann, D.E.; Acquista, N. Emission Spectrum of CF. J. Mol. Spectr. 1965, 16, 228–263. [Google Scholar] [CrossRef]
  33. Hildenbrand, D.L. Dissociation Energy and Ionization Potentlal of the Molecule CF. Chem. Phys. Lett. 1975, 32, 523–526. [Google Scholar] [CrossRef]
  34. Burgess, D.R., Jr.; Manion, J.A. Rate Constants for Abstraction of H from the Fluoromethanes by H, O, F, and OH. J. Phys. Chem. Ref. Data 2021, 50, 023102:1–023102:47. [Google Scholar] [CrossRef]
  35. Atkinson, R.; Baulch, D.L.; Cox, R.A.; Hampson, R.F.; Kerr, J.A.; Rossi, M.J.; Troe, J. Evaluated Kinetic, Photochemical and Heterogeneous Data for Atmospheric Chemistry: Supplement V. IUPAC Subcommittee on Gas Kinetic Data Evaluation for Atmospheric Chemistry. J. Phys. Chem. Ref. Data 1997, 26, 521–1011. [Google Scholar] [CrossRef]
  36. Foon, R.; Reid, G.P. Kinetics of the Gas Phase Fluorination of Hydrogen and Alkanes. Trans. Faraday Soc. 1971, 67, 3513–3520. [Google Scholar] [CrossRef]
  37. Persky, A. Kinetics of the Reactions F + H2S and F + D2S at 298 K. Chem. Phys. Lett. 1998, 298, 390–394. [Google Scholar] [CrossRef]
  38. Espinosa-Garcia, J.; Bravo, J.L.; Rangel, C. New Analytical Potential Energy Surface for the F(2P) + CH4 Hydrogen Abstraction Reaction: Kinetics and Dynamics. J. Phys. Chem. A 2007, 111, 2761–2771. [Google Scholar] [CrossRef]
  39. Vasiliev, E.S.; Volkov, N.D.; Karpov, G.V.; Morozov, I.I.; Nigmatullin, D.R.; Saigina, E.A.; Savilov, S.V.; Umanskii, S.Y.; Butkovskaya, N.I. Determination of the Rate Constant of the Reaction of Benzene with Atomic Fluorine by the Method of Competing Reactions. Russ. J. Phys. Chem. B 2021, 15, 789–794. [Google Scholar] [CrossRef]
  40. Hrusak, J.; Schroder, D.; Weiske, T.; Schwarz, H. Combined ab Initio MO and Experimental Studies on the Unimolecular HF Loss from Protonated Fluorobenzene in the Gas Phase. J. Am. Chem. Soc. 1993, 115, 2015–2020. [Google Scholar] [CrossRef]
  41. Dopfer, O.; Solca, N.; Lemaire, J.; Maitre, P.; Crestoni, M.-E.; Fornarini, S. Protonation Sites of Isolated Fluorobenzene Revealed by IR Spectroscopy in the Fingerprint Range. J. Phys. Chem. A 2005, 109, 7881–7887. [Google Scholar] [CrossRef]
  42. Dopfer, O. IR Spectroscopic Strategies for the Structural Characterization of Isolated and Microsolvated Arenium Ions. J. Phys. Organ. Chem. 2006, 19, 540–551. [Google Scholar] [CrossRef]
  43. Solca, N.; Dopfer, O. Protonation of Gas-Phase Aromatic Molecules: IR Spectrum of the Fluoronium Isomer of Protonated Fluorobenzene. J. Am. Chem. Soc. 2003, 125, 1421–1430. [Google Scholar] [CrossRef]
  44. Mason, R.S.; Parry, A.J.; Milton, D.M.P. Proton Transfer to the Fluorine Atom in Fluorobenzene. Temperature and Pressure Dependence. J. Chem. Soc. Faraday Transact. 1994, 90, 1373–1380. [Google Scholar] [CrossRef]
  45. Vasiliev, E.S.; Karpov, G.V.; Shartava, D.K.; Morozov, I.I.; Savilov, S.V.; Morozova, O.S.; Khomyakova, P.S. Mass Spectrometric Study of the Reaction of a Fluorine Atom and Monocloroacetic Acid. Russ. J. Phys. Chem. B 2022, 16, 388–394. [Google Scholar] [CrossRef]
Atoms 11 00132 g001
Figure 1. Structural models of (1i) ipso-, (1o) ortho-, (1m) meta-, (1p) para-fluorocyclohexadienyl radicals, (2) C6H5F⋅H complex, and transition complexes (TS1), (TS2). Internuclear distances and angles are given in angstroms (Å) and degrees. The relative energies (ΔE) of C6H6F-isomers are given in kcal/mol.
Figure 1. Structural models of (1i) ipso-, (1o) ortho-, (1m) meta-, (1p) para-fluorocyclohexadienyl radicals, (2) C6H5F⋅H complex, and transition complexes (TS1), (TS2). Internuclear distances and angles are given in angstroms (Å) and degrees. The relative energies (ΔE) of C6H6F-isomers are given in kcal/mol.
Atoms 11 00132 g001
Atoms 11 00132 g002
Figure 2. Reactions of detachment and substitution of hydrogen in benzene. The ipso-fluorocyclohexadienyl radical and complex C6H5F·H are denoted as 1i and 2 subsequently. Calculated values of the relative energies are presented without parentheses. Relative energies taking into account the error of the method are presented in parentheses. All the values of relative energies are given in kcal/mol.
Figure 2. Reactions of detachment and substitution of hydrogen in benzene. The ipso-fluorocyclohexadienyl radical and complex C6H5F·H are denoted as 1i and 2 subsequently. Calculated values of the relative energies are presented without parentheses. Relative energies taking into account the error of the method are presented in parentheses. All the values of relative energies are given in kcal/mol.
Atoms 11 00132 g002
Atoms 11 00132 g003
Figure 3. Absorption of the C6H6F radical in the IR region of the spectrum. The black bars correspond to the experimental absorption lines [10]. The empty ones correspond to the scaled values of the calculated frequencies of the ipso-C6H6F isomer fundamental oscillations with scaling factor of 0.98. Absorption intensity I is given in relative units, frequency ω is in cm−1.
Figure 3. Absorption of the C6H6F radical in the IR region of the spectrum. The black bars correspond to the experimental absorption lines [10]. The empty ones correspond to the scaled values of the calculated frequencies of the ipso-C6H6F isomer fundamental oscillations with scaling factor of 0.98. Absorption intensity I is given in relative units, frequency ω is in cm−1.
Atoms 11 00132 g003
Atoms 11 00132 g004
Figure 4. Isomerization and decay of the C6H6F+ ion. The ipso-, ortho-, meta-, para-fluorocyclohexadienyl cations numbered as 1, 2, 3, and 4 correspondingly, and F–isomer C6H5+·HF denoted as 5. Calculated values of the relative energies are presented without parentheses. The relative energies in round and square parentheses were obtained in refs. [40,41]. The relative energies are given in kcal/mol.
Figure 4. Isomerization and decay of the C6H6F+ ion. The ipso-, ortho-, meta-, para-fluorocyclohexadienyl cations numbered as 1, 2, 3, and 4 correspondingly, and F–isomer C6H5+·HF denoted as 5. Calculated values of the relative energies are presented without parentheses. The relative energies in round and square parentheses were obtained in refs. [40,41]. The relative energies are given in kcal/mol.
Atoms 11 00132 g004
Table 2. The main properties of stable participants and transitional complexes of hydrogen abstraction and substitution reactions. The values of the electron energies Eel and the ground vibrational state energies EZPE are given in Hartree units. The rotational constants A, B, C are given in cm−1.
Table 2. The main properties of stable participants and transitional complexes of hydrogen abstraction and substitution reactions. The values of the electron energies Eel and the ground vibrational state energies EZPE are given in Hartree units. The rotational constants A, B, C are given in cm−1.
IntermediatesSymmetryEelEZPERotational Constants
ABC
C6H6(benzene)D6h−232.2727280.1009430.1916270.1915680.095799
ipso-C6H6FCs−332.0521500.1020670.1645040.0869380.061077
ortho-C6H6FCs−332.0578410.1015820.1761250.0835020.057234
meta-C6H6FCs−332.0555400.1011940.1765680.0824520.056778
para-C6H6FCs−332.0542490.1012240.1781960.081805 0.056636
C6H5F·HCs−332.0167140.0942090.1754580.0827740.059285
C6H5(phenyl)C2v−231.5804030.0878490.2116080.1885920.099719
C6H5FC2v−331.5123980.0928070.1908050.0861910.059372
TS1Cs−331.9993920.0978210.1785900.0614720.047088
TS2Cs−332.0021180.0948820.1816640.0840460.058891
HFC∞v−100.4474560.0094190.00000020.86952520.869525
F—−99.725232————
H—−0.499810————
ipso-C6H6F+Cs−331.7746570.1022660.1745150.0856690.058663
ortho-C6H6F+Cs−331.8031160.1031790.1793980.0847880.058169
F-C6H6F+Cs−331.7527150.1011840.1832840.0783640.055143
C6H5+C2v−231.2746210.0856220.2295560.1816450.101405
TS12C1−331.7702140.1007310.1802770.0852175.851448
TS15Cs−331.7052360.0975870.1809560.0823770.057044
TS25C1−331.7051700.0971990.1809740.0846880.058268
Table 3. The enthalpies of intermediates and products of benzene fluorination in kcal/mol.
Table 3. The enthalpies of intermediates and products of benzene fluorination in kcal/mol.
Intermediate (Product)ΔH0R (298.15 K)
ipso-C6H6FC6H5 + HFC6H5F + H
Calculation−33.9
−31.0 a		−20.5−14.4
Experiment−24.8 b−25.0 c
−25.9 d		−15.0 c
−12.7 d
(a) Ref. [15]; (b) Ref. [9]; (c) Ref. [2]; (d) Refs. [30,39].
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Adamson, S.O.; Kharlampidi, D.D.; Shtyrkova, A.S.; Umanskii, S.Y.; Dyakov, Y.A.; Morozov, I.I.; Golubkov, M.G. Quantum-Chemical Study of the Benzene Reaction with Fluorine. Atoms 2023, 11, 132. https://doi.org/10.3390/atoms11100132

AMA Style

Adamson SO, Kharlampidi DD, Shtyrkova AS, Umanskii SY, Dyakov YA, Morozov II, Golubkov MG. Quantum-Chemical Study of the Benzene Reaction with Fluorine. Atoms. 2023; 11(10):132. https://doi.org/10.3390/atoms11100132

Chicago/Turabian Style

Adamson, Sergey O., Daria D. Kharlampidi, Anastasia S. Shtyrkova, Stanislav Y. Umanskii, Yuri A. Dyakov, Igor I. Morozov, and Maxim G. Golubkov. 2023. "Quantum-Chemical Study of the Benzene Reaction with Fluorine" Atoms 11, no. 10: 132. https://doi.org/10.3390/atoms11100132

APA Style

Adamson, S. O., Kharlampidi, D. D., Shtyrkova, A. S., Umanskii, S. Y., Dyakov, Y. A., Morozov, I. I., & Golubkov, M. G. (2023). Quantum-Chemical Study of the Benzene Reaction with Fluorine. Atoms, 11(10), 132. https://doi.org/10.3390/atoms11100132

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