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Article

Theoretical Investigation of the NO3 Radical Addition to Double Bonds of Limonene

by
Lei Jiang
1,2,
Wei Wang
2,* and
Yi-Sheng Xu
2
1
College of Water Sciences, Beijing Normal University, Beijing 100875, China
2
Atmospheric Chemistry and Aerosol Research Division, Chinese Research Academy of Environmental Science, Beijing 100012, China
*
Author to whom correspondence should be addressed.
Int. J. Mol. Sci. 2009, 10(9), 3743-3754; https://doi.org/10.3390/ijms10093743
Submission received: 7 August 2009 / Revised: 18 August 2009 / Accepted: 19 August 2009 / Published: 27 August 2009
(This article belongs to the Section Physical Chemistry, Theoretical and Computational Chemistry)
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Abstract

:
The addition reactions of NO3 to limonene have been investigated using ab initio methods. Six different possibilities for NO3 addition to the double bonds, which correspond to the two C–C double bonds (endocyclic or exocyclic) have been considered. The negative activation energies for the addition of NO3 to limonene are calculated and the energies of NO3-limonene radical adducts are found to be 14.55 to 20.17 kcal mol-1 more stable than the separated NO3 and limonene at the CCSD(T)/6–31G(d) + CF level. The results also indicate that the endocyclic addition reaction is more energetically favorable than the exocyclic one.

Graphical Abstract

1. Introduction

Total emissions of volatile organic compounds (VOCs) from vegetation have been estimated to be about 1,150 Tg carbon year−1 [1]. More than half (54%) of the emissions are related to isoprene and monoterpenes (~11%), such as α- and β-pinene and limonene [2]. Atmospheric oxidation of VOCs, which is initiated by reactions with a variety of oxidants including OH radical, NO3 radical and ozone is a common atmospheric chemistry reaction of the lower troposphere layer. During the day the major sinks for VOCs are their reactions with OH radical and O3, while with nitrate radical (NO3) can be a very important, and often dominant, loss process at nighttime [3–6]. The reactions of NO3 species, formed by the reaction of NO2 and O3 [7], with atmospheric VOCs can lead to formation of HNO3 [8], peroxyacyl nitrate (PAN) [9], RO2 [9,10], and toxic compounds such as dinitrates [10].
Limonene or 4-isopropenyl-1-methyl-cyclohexene is the most abundant monoterpene, and has both highly active endocyclic and exocyclic double bonds [11]. Plants non-native to Europe, e.g., Australian eucalyptus, have limonene emissions of more than 30% of monoterpene [12] and limonene represents one of the four highest terpenes emitted in North America. Many reactions of monoterpenes with OH radical and O3 have received considerable attention with regard to their initiated oxidations, reaction kinetics, reaction products and secondary organic aerosol (SOA) formation whereas those with NO3 have received relatively little consideration, especially the reaction of limonene with NO3. The initial reaction of limonene and NO3 proceeds mainly by NO3 addition to the C–C double bond, forming the NO3-limonene radical adduct. Under atmospheric conditions, the NO3-limonene radical adduct is expected to react primarily with oxygen molecules to form the nitrooxyalkyl peroxy radicals, which further react with NO, engage in a self-reaction or crossreaction with other peroxy radicals, or react with HO2. The products and aerosol formation from the NO3 radical initiated oxidation of limonene have been investigated in the EUPHORE photoreactor facility [13]. In EUPHORE study, the results indicated that endolim had been identified as the major reaction products of the NO3 radical initiated oxidation of limonene and the total SOA mass formed occurs mainly through the secondary chemistry of its major product endolim. Hence, the nighttime reaction between limonene and NO3 contributes significantly to the degradation of limonene and SOA formed. However, such important processes and quantities as the formation of the NO3-limonene radical adduct and the isomer-specific reactions have yet to be clarified.
To examine the reaction mechanism of NO3 with limonene, a theoretical exploration of the NO3-initiated limonene oxidation mechanism with different possibilities for the initial step of the NO3 addition to the limonene was carried out and is reported here, as the isomeric branching of the initial NO3 addition to limonene is crucial in determining the final product distribution. The present study is mainly focused on comparison of different reaction pathways and determination energetically favorable bonds needed for the further elaboration of the oxidation mechanisms and assessment of the products identified in experiments. Moreover, the quantum chemical study can supply some insight on the reactions between NO3 and monoterpenes, especially important to understand the night-time atmospheric chemistry in the troposphere.

2. Theoretical Methods

The theoretical computations have been carried out on the SGI ALTIX 4700 supercomputer using the GAUSSIAN 03 suite of programs [14]. The geometry optimization of all reactants, transition states, and radical adducts was performed at UB3LYP/6–31G(d,p) with harmonic vibrational frequencies analyses. The stationary points were classified as minima in the case, when no imaginary frequencies were found, and as a transition state if only one imaginary frequency was obtained. The DFT optimized structures were then used in the single-point energy ab initio calculations using frozen core second-order Møller-Plesset perturbation theory (MP2) and coupled-cluster theory with single and double excitations including perturbative corrections for the triple excitations (CCSD(T) with various basis sets to obtain accurate energy information.
Density functional theory (DFT) has been widely employed for atmospheric oxidation reactions of VOCs with NO3 radical, OH radical and ozone [15–21]. These studies implied that deviations of the B3LYP geometries from the CASSCF ones are small enough to consider that the former level is a good compromise between quality and computational cost in the nitrate radical addition reaction and provides reasonable reaction energies and barriers for most of the ozonolysis steps insofar as the calculated B3LYP values are more accurate than those obtained with MP2 theory. So, to some degree, DFT was identified a reliable and economical method that provides a reasonable description of the VOCs-radical reactions.
In addition, for more accurate single-point energy, the basis set effects on calculated energies for NO3-limonene reactions were corrected at MP2 level according to the recently developed method by Zhang et al. in his investigation of the complex reaction mechanisms and pathways of various volatile organic compounds (VOCs) in the atmosphere [22]. A correction factor (CF) was determined from the energy difference between the MP2/6–31G(d) and MP2/6–311++G(d,p) levels. The values of calculated energies were then evaluated by CCSD(T)/6–31G(d) + CF method. The applied method has been validated for several isoprene reactions initiated by NO3, OH and O3 [16,22,23], and of limonene initiated by O3 [24].

3. Results and Discussion

The computational results show that there are six possibilities for the NO3 upon addition to the double bond of the limonene, namely, four possibilities involving the endocyclic C–C double bond (see Figure 1) and two possibilities for the exocyclic C–C double bond (see Figure 2). Transition states are not found in the evaluated pathways of the NO3 addition to limonene, which proceed in the direction of the terminal carbon atom (C9) of the exocyclic C–C double bond. This can be explained by the stronger selectivity of the NO3 and the initial step proceeds predominantly via electrophilic addition mechanism for the reactions of NO3 with alkenes [13,25,26].

3.1. Reaction Mechanism

T1 diagnostic values, spin eigenvalues of the unrestricted wavefunction (<S2>) and its projection (<S2>A) for all stationary points in the NO3 addition to the limonene are provided in Table 1. All calculations of T1 diagnostic values were run at CCSD(T)/6–31G(d)//UB3LYP/6–31G(d,p) level of theory. T1 diagnostic values give a qualitative assessment of the nondynamical correlation significance and ensure the reliability of this treatment. For closed-shell systems, T1 values should be under 0.02 and for open-shell systems under 0.045 [27,28].
As seen from Table 1, the closed-shell T1 diagnostic value is 0.0100 for limonene, and the the largest open-shell T1 diagnostic value is 0.0289 for TS2. Hence, T1 values calculated for all the stationary points are clearly under these thresholds. At the UB3LYP/6–31G(d,p) level of theory, the calculated spin eigenvalues, <S2>, are 0.754 and 0.768 for radicals NO3, TS1–TS6 and Adduct1–Adduct6, respectively. After proper projection, the spin eigenvalues are reduced to 0.750 for all the open-shell stationary points, indicating that contamination of the unrestricted Hartree-Fock wave function from higher spin states is negligible.
Figure 1 presents the optimized geometries of the stationary points for the NO3 addition to the endocyclic C–C double bond obtained at the UB3LYP/6–31G(d,p) level of theory and values of the most important geometrical properties.
As seen from this Figure, the NO3 addition reaction can proceed either on the H-substituted carbon atom (C1), or on the methyl-substituted carbon atom (C2). On each carbon atom of relevant double bond, there are two possible attacking directions. Four transition states (TS1, TS2, TS3 and TS4) associated with the addition of NO3 to the endocyclic C–C double bond leading to the formation of the NO3-limonene radical adducts (Adduct1–Adduct4) have been identified. Each transition state has only one imaginary harmonic vibrational frequency and can be classified as the first-order saddle point. The values of imaginary frequencies for TS1, TS2, TS3, and TS4 transition states are 157.10i, 67.07i, 157.82i, and 228.95i, respectively.
In the 1-endo pathway, the C–C double bond distance (1.339 Å), increases by 0.058 Å and 0.149 Å in the transition states (TS1) and NO3-limonene radical adduct (Adduct1), respectively, which clearly demonstrates that a single bond property on the formation of the NO3-limonene radical adducts presented during the reaction procedure. The disappearance of the double bond is also shown in the reaction channel. The NO3-limonene distance in the TS1 is 2.045 Å, while in the Adduct1 is 1.507 Å. In NO3 radical, the three N–O bond lengths are the same values (1.239 Å). While in the TS1, the length of the N–O bond oriented towards the C–C double bond, increases a length of 0.096 Å and becomes to 1.400 Å for the Adduct1. Meanwhile it shows decreasing tendency to the other two bonds. Compared with those in the NO3 radical, the bond lengths have less variation and decrease 0.007–0.029 Å in the TS1 and Adduct1. Other three pathways of transition states (TS2, TS3 and TS4) and NO3-limonene radical adducts (Adduct2, Adduct 3 and Adduct 4) exhibit a similar pattern.
The optimized geometries for the NO3 addition to the exocyclic C–C double bond are illustrated in Figure 2. In this case, the NO3 addition could proceed on the methyl-substituted carbon atom (C8). Two transition states (TS5 and TS6) associated with the addition of NO3 to the exocyclic C–C double bond leading to the formation of the NO3-limonene radical adducts (Adduct5 and Adduct6) have been identified too. The values of imaginary frequencies for TS5 and TS6 transition states are 191.62i and 231.50i, respectively.
In comparison of the 1-endo pathway, the 1-exo and 2-exo pathways exhibited a similar addition mode are shown in Figure 2. The C–C double bond distance (1.338 Å), increases by a length of 0.06 Å in the transition states (TS), and to 1.450–1.487 Å in the NO3-limonene radical adducts, and clearly becomes a single bond. The NO3-limonene radical distance in the two TS is in the range of 2.056–2.068 Å, and in the two adduct isomers is between 1.496 and 1.521 Å. In the TS, the length of the N–O bond oriented towards the C–C double bond, increases lengths in the range of 0.1–0.102 Å and increases to 1.400–1.406 Å in the adduct isomers. While the other two N–O bonds lengths vary less and decrease 0.011–0.029 Å in the TS and adduct isomers.

3.2. Thermochemical Analysis

The NO3-limonene reaction energies computed at different levels of theory with different basis sets with the zero-point correction included are presented in Table 2. As seen from this data, the reaction energies of the NO3 addition to limonene calculated at different levels of theory are quite different. The values predicted by MP2/6–31G(d) and B3LYP/6–311 + G(3df,2pd) are comparable and differ by −2.7–2.28 kcal mol−1. The values obtained at CCSD(T)/6–31G(d) level theory are 5.32–13.52 kcal mol−1 more stable than those calculated with MP2 and B3LYP. Another important detail is that the values determined by using MP2 and B3LYP and with two different basis sets differ by 1.71–2.73 kcal mol−1 and 3.22–4.06 kcal mol−1, respectively. At the CCSD(T)/6–31G(d) + CF level of theory, the NO3-limonene radical adducts are 14.55–20.17 kcal mol−1 more stable than the separate NO3 and limonene. Adduct2 is more stable than others, The difference in the relative stability of the six NO3-limonene radical adducts does not exceed 5.62 kcal mol−1.
The NO3-limonene activation energies with the zero-point correction (ZPE) included computed at different levels of theory with different basis sets, are given in Table 3. As seen from this Table, the activation energies for the formation of the NO3-limonene reactions with the zero-point correction included are very sensitive to the effects of electron correlation and basis set. The activation energies of the NO3-limonene reaction are positive activation energies and significantly overestimate with MP2 method. B3LYP/6–311 + G(d,p), B3LYP/6–311 + G(3df,2pd) (except for ΔE2-exo), CCSD(T)/6–31G(d) and CCSD(T)/6–31G(d) + CF (except for ΔE2-exo) levels are negative activation energies, which corresponds to the NO3 + propene reaction, ozonolysis of isoprene and the OH + ethane reaction reported in the previous theoretical studies [15,22,29,30]. The negative activation energies given by B3LYP/6–311 + G(3df,2pd) and CCSD(T)/6–31G(d) are comparable, with a largest difference of 4.04 kcal mol−1 for ΔE2-exo. Compared with CCSD(T)/6–31G(d) + CF, there are noticeable differences in the calculated activation energies for the NO3-limonene reaction with the UB3LYP/6–31G(d,p) methods of and results differ by 1.12–5.98 kcal mol−1, while there are little differences with B3LYP/6–311 + G(3df,2pd), and they differ by −0.6–3.32 kcal mol−1. The activation energies obtained at the CCSD(T)/6–31G(d) + CF level of theory are −3.47 kcal mol−1 for 1-endo, −2.03 kcal mol−1 for 2-endo, −4.36 kcal mol−1 for 3-endo, −3.60 kcal mol−1 for 4-endo, −1.43 kcal mol−1 for 1-exo and 1.67 kcal mol−1 for 2-exo. This indicates that 3-endo is the most favorable pathway. It also implies that the endocyclic addition is more energetically favorable than the exocyclic one and that the NO3 attack predominantly takes place at the endo-double bonded carbons.
As seen from Table 3, relatively low activation or slightly negative energies obtained for the reaction of NO3 with limonene in our work, which agree with the values obtained for the reaction of NO3 with alkenes and other terpenes. Hence, the reaction of the NO3 addition to limonene is entirely consistent with a radical addition process [25]. Figure 3 illustrates the relative energies of the stationary points located on the singlet ground-state separate NO3 and limonene potential energy surface at the CCSD(T)/6–31G(d) + CF level of theory.
The NO3-limonene reaction enthalpies, Gibbs free energies and entropies computed at B3LYP/6–31G(d,p) level of theory with the thermal Correction included, are shown in Table 4. The NO3-limonene addition reaction is exothermic for the six pathways. The six radical adducts (Adduct1–Adduct6) are 9.32–17.42 kcal mol−1 more stable than the reactants. The endocyclic addition reactions are more stabilized than the exocyclic addition reaction, except for the 4-endo pathway. In the endocyclic addition reactions, the Adduct2, corresponding to the 2-endo pathway, is the most stabilized, with value of −17.42 kcal mol−1. Adduct5 is more stabilized, with a value of −11.73 kcal mol−1, corresponding to the 1-exo pathway in the exocyclic addition reactions. The NO3-limonene reaction Gibbs free energies range from −4.69 to 3.61 kcal mol−1 for the six pathways. The values of Gibbs free energies are negative for 1-endo, 2-endo and 3-endo pathways, implying that the reaction of NO3 with limonene can take place spontaneously.
Additionally, the formation of a prereactive van der Waals complex has been used to explain the negative values found for the experimental activation energies [31]. A van der Waals complex was formed prior to addition have been reported in quantum chemical studies on the OH addition reaction to alkenes [30,32,33]. A transition state connecting the van der Waals complex with the adduct has also been found. But, as for the case of the propene + NO3 reaction, no van der Waals complexes in the limonene + NO3 reaction have been found at the UB3LYP/6–31G(d,p) level of calculation, since the DFT method fails in case of Van der Waals and loose transition states and actually represent only small irregularities on the potential energy hypersurface [15]. The van der Waals complexes do not have a profound effect on the kinetics [30] and are not chemically relevant in the reaction mechanisms [34], although they will probably exist.

4. Conclusions

Our theoretical investigation reveals several important aspects regarding the gas phase reaction of the initial NO3 addition to the limonene using computational quantum, which has importance in nighttime atmospheric chemistry.
(1) The activation energies for the formation of the NO3-limonene reaction have been determined first. At CCSD(T)/6–31G(d) + CF//UB3LYP/6–311 + G(d,p), our results indicate that relatively low activation or slightly negative energies were obtained, and 3-endo pathway is the most favorable branching for the initial step of the NO3-limonene reactions. From the obtained activation energies, we concluded that the reaction of the NO3 addition to limonene is entirely consistent with a radical addition process.
(2) The calculated activation energies of the NO3-limonene reactions are very sensitive to electron correlation and basis set effects. The activation energies of the NO3-limonene reaction were significantly overestimated with the MP2 method. Compared with CCSD(T)/6–31G(d) + CF, there are noticeable differences in the calculated activation energies for the NO3-limonene reaction with the methods of UB3LYP/6–31G(d,p), while there was little difference with B3LYP/6–311 + G(3df,2pd).
(3) Six possibilities for the NO3 addition to double bond on the limonene were found; the two possibilities for the NO3 addition proceeding on the terminal carbon atom (C9) of the exocyclic C–C double bond are not found. The endocyclic addition is more energetically favorable than the exocyclic one. Those are consistent with the EUPHORE study by Spittler et al., who could not detect the products formaldehyde or 4-acetyl-1-methylcyclohex-1-ene, an indication of an attack of NO3 on the exocyclic double bond in limonene. Hence, the computation results verified that the high selectivity of NO3 towards different C–C double bonds and the initial step proceeds predominantly via electrophilic addition for the reactions of NO3 with limonene.

Acknowledgments

This work was supported by National Natural Science Foundation of China (Grant 40705043), Social Public Welfare Projects (Grant no. 200809152) and the Science Foundation of Chinese Research Academy of Environmental Science (Grant 2007KYYW36). Additional support was provided by the CRAES Supercomputing Facilities (SGI 4700 supercomputers).

References

  1. Gill, KJ; Hites, RA. Rate constants for the gas-phase reactions of the hydroxyl radical with isoprene, α-and β-pinene, and limonene as a function of temperature. J. Phys. Chem. A 2002, 106, 2538–2544. [Google Scholar]
  2. Guenther, A; Hewitt, CN; Erickson, D; Fall, R; Geron, C; Graedel, T; Harley, P; Klinger, L; Lerdau, M; McKay, WA; Pierce, T; Scholes, B; Steinbrecher, R; Tallamraju, R; Taylor, J; Zimmerman, PJ. A global model of natural volatile organic compound emissions. J. Geophys. Res 1995, 100, 8873–8892. [Google Scholar]
  3. Grosjean, D; Williams, EL; Grosjean, E; Andino, JM; Seinfeld, JH. Atmospheric oxidation of biogenic hydrocarbons, reactions of ozone with β-pinene, d-limonene and transcaryophylene. Environ. Sci. Technol 1993, 27, 2754–2758. [Google Scholar]
  4. Kleindienst, TE; Harris, GH; Pitts, JN, Jr. Rates and temperature dependence of the reaction of OH with isoprene, its oxidation products, and selected terpenes. Environ. Sci. Technol 1982, 16, 844–846. [Google Scholar]
  5. Shu, Y; Atkinson, R. Rate constants for the gas-phase reactions of O3 with a series of terpenes and OH radical formation from the O3 reactions with sesquiterpenes at 296 ± 2 K. Int. J. Chem. Kinet 1994, 26, 1193–1205. [Google Scholar]
  6. Atkinson, R. Gas-phase tropospheric chemistry of organic compounds. J. Phys. Chem. Ref. Data, Monogr 1994, 2, 1–216. [Google Scholar]
  7. Wayne, RP. The nitrate radical: Physics, chemistry and the atmosphere. Atmos. Environ 1991, 25A, 1–206. [Google Scholar]
  8. Atkinson, R; Plum, CN; Carter, WPL; Winer, AM; Pitts, JN, Jr. Kinetics of the gas-phase reactions of NO3 radicals with a series of alkanes at 296 ± 2K. J. Phys. Chem 1984, 88, 2361–2364. [Google Scholar]
  9. Cantrell, CA; Davidson, JA; Busarow, KL; Calvert, JG. The CH3CHO-NO3 reaction and possible night-time PAN generation. J. Geophys. Res 1986, 91, 5347–5353. [Google Scholar]
  10. Bandow, H; Okuda, M; Akimoto, H. Mechanism of the gas-phase reactions of propylene and nitroxy radicals. J. Phys. Chem 1980, 84, 3604–3608. [Google Scholar]
  11. Guenther, A; Geron, C; Pierce, T; Lamb, B; Harley, P; Fall, R. Natural emissions of non-methane volatile organic compounds, carbon monoxide, and oxides of nitrogen from North America. Atmos. Environ 2000, 34, 2205–2230. [Google Scholar]
  12. He, C; Murray, F; Lyons, T. Monoterpene and isoprene emissions from 15 eucalyptus species in Australia. Atmos. Environ 2000, 34, 645–655. [Google Scholar]
  13. Spittler, M; Barnes, I; Bejan, I; Brockmann, KJ; Benter, Th; Wirtz, K. Reactions of NO3 radicals with limonene and α-pinene: Product and SOA formation. Atmos. Environ 2006, 40, S116–S127. [Google Scholar]
  14. Frisch, MJ; Trucks, GW; Schlegel, HB; Scuseria, GE; Robb, MA; Cheeseman, JR; Montgomery, JA, Jr; Vreven, T; Kudin, KN; Burant, JC; Millam, JM; Iyengar, SS; Tomasi, J; Barone, V; Mennucci, B; Cossi, M; Scalmani, G; Rega, N; Petersson, GA; Nakatsuji, H; Hada, M; Ehara, M; Toyota, K; Fukuda, R; Hasegawa, J; Ishida, M; Nakajima, T; Honda, Y; Kitao, O; Nakai, H; Klene, M; Li, X; Knox, JE; Hratchian, HP; Cross, JB; Bakken, V; Adamo, C; Jaramillo, J; Gomperts, R; Stratmann, RE; Yazyev, O; Austin, AJ; Cammi, R; Pomelli, C; Ochterski, JW; Ayala, PY; Morokuma, K; Voth, GA; Salvador, P; Dannenberg, JJ; Zakrzewski, VG; Dapprich, S; Daniels, AD; Strain, MC; Farkas, O; Malick, DK; Rabuck, AD; Raghavachari, K; Foresman, JB; Ortiz, JV; Cui, Q; Baboul, AG; Clifford, S; Cioslowski, J; Stefanov, BB; Liu, G; Liashenko, A; Piskorz, P; Komaromi, I; Martin, RL; Fox, DJ; Keith, T; Al-Laham, MA; Peng, CY; Nanayakkara, A; Challacombe, M; Gill, PMW; Johnson, B; Chen, W; Wong, MW; Gonzalez, C; Pople, JA. Gaussian 03; Revision E01; Gaussian, Inc: Wallingford, CT, USA, 2004. [Google Scholar]
  15. Pérez-Casany, MP; Nebot-Gil, I; Sánchez-Marín, J. Ab initio study on the mechanism of tropospheric reactions of the nitrate radical with alkenes: Propene. J. Phys. Chem. A 2000, 104, 6277–6286. [Google Scholar]
  16. Suh, I; Lei, W; Zhang, R. Experimental and theoretical studies of isoprene reaction with NO3. J. Phys. Chem. A 2001, 105, 6471–6478. [Google Scholar]
  17. Lei, W; Zhang, R; McGivern, WS; Derecskei-Kovacs, A; North, SW. Theoretical study of isomeric branching in the isoprene-OH reaction: Implications to final product yields in isoprene oxidation. Chem. Phys. Lett 2000, 326, 109–114. [Google Scholar]
  18. Vereecken, L; Peeters, J. Theoretical study of the formation of acetone in the OH-initiated atmospheric oxidation of α-pinene. J. Phys. Chem. A 2000, 104, 11140–11146. [Google Scholar]
  19. Gutbrod, R; Kraka, E; Schindler, RN; Cremer, D. Kinetic and theoretical investigation of the gas-phase ozonolysis of isoprene: Carbonyl oxides as an important source for OH radicals in the atmosphere. J. Am. Chem. Soc 1997, 119, 7330–7342. [Google Scholar]
  20. Olzmann, M; Kraka, E; Cremer, D; Gutbrod, R; Andersson, S. Energetics, kinetics, and product distributions of the reactions of ozone with ethene and 2,3-dimethyl-2-butene. J. Phys. Chem. A 1997, 101, 9421–9429. [Google Scholar]
  21. Aplincourt, P; Ruiz-López, MF. Theoretical study of formic acid anhydride formation from carbonyl oxide in the atmosphere. J. Phys. Chem. A 2000, 104, 380–388. [Google Scholar]
  22. Lei, W; Derecskei-Kovacs, A; Zhang, R. Ab initio study of OH addition reaction to isoprene. J. Chem. Phys 2000, 113, 5354–5360. [Google Scholar]
  23. Zhang, D; Zhang, R. Mechanism of OH formation from ozonolysis of isoprene: A quantum-chemical study. J. Am. Chem. Soc 2002, 124, 2692–2703. [Google Scholar]
  24. Jiang, L; Wang, W; Xu, Y. Ab initio investigation of O3 addition to double bonds of limonene submitted for publication.
  25. Martínez, E; Cabañas, B; Aranda, A; Martín, P; Salgado, S. Absolute rate coefficients for the gas-phase reactions of NO3 radical with a series of monoterpenes at T=298 to 433 K. J. Atmos. Chem 1999, 33, 265–282. [Google Scholar]
  26. Shu, Y; Kwok, ESC; Tuazon, EC; Atkinson, R; Arey, J. Products of the gas-phase reactions of linalool with OH radicals, NO3 radicals, and O3. Environ. Sci. Technol 1997, 31, 896–904. [Google Scholar]
  27. Lee, TJ; Taylor, PR. A diagnostic for determining the quality of single-reference electron correlation methods. Int. J. Quantum Chem. Symp 1989, 23, 199–207. [Google Scholar]
  28. Rienstra-Kiracofe, JC; Allen, WD; Schaefer, HF, III. The C2H5 + O2 reaction mechanism: High-level ab initio characterizations. J. Phys. Chem. A 2000, 104, 9823–9840. [Google Scholar]
  29. Pérez-Casany, MP; Nebot-Gil, I; Sánchez-Marín, J. DFT theoretical study on the reaction mechanism of the nitrate radical with alkenes: 2-Butene, isobutene, 2-methyl-2-butene, and 2,3-dimethyl-2-butene. J. Phys. Chem. A 2000, 104, 10721–10730. [Google Scholar]
  30. Alvarez-Idaboy, JR; Mora-Díez, N; Vivier-Bunge, A. A quantum chemical and classical transition state theory explanation of negative activation energies in OH addition to substituted ethenes. J. Am.Chem. Soc 2000, 122, 3715–3720. [Google Scholar]
  31. Mozurkewich, M; Lamb, JJ; Benson, SW. Negative activation energies and curved Arrhenius plots. 2. Hydroxyl + carbon monoxide. J. Phys. Chem 1984, 88, 6435–6441. [Google Scholar]
  32. Ramírez-Ramírez, VM; Nebot-Gil, I. Theoretical study of the OH addition to the endocyclic and exocyclic double bonds of the d-limonene. Chem. Phys. Lett 2005, 409, 23–28. [Google Scholar]
  33. Díaz-Acosta, I; Alvarez-Idaboy, JR; Vivier-Bunge, A. Mechanism of the OH-propene-O2 reaction: An ab initio study. Int. J. Chem. Kinet 1999, 31, 29–36. [Google Scholar]
  34. García-Cruz, I; Ruiz-Santoyo, ME; Alvarez-Idaboy, JR; Vivier-Bunge, A. Ab-initio study of initial atmospheric oxidation reactions of C3 and C4 alkanes. J. Comput. Chem 1999, 20, 845–856. [Google Scholar]
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Figure 1. Geometries of stationary points involved in the NO3 addition to limonene endocyclic double bond obtained at UB3LYP/6-31G(d,p) level of theory. Bond distances are given in Å. TS1, TS2, TS3, and TS4 are abbreviations for 1-endo, 2-endo, 3-endo and 4-endo transition states, respectively.
Figure 1. Geometries of stationary points involved in the NO3 addition to limonene endocyclic double bond obtained at UB3LYP/6-31G(d,p) level of theory. Bond distances are given in Å. TS1, TS2, TS3, and TS4 are abbreviations for 1-endo, 2-endo, 3-endo and 4-endo transition states, respectively.
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Figure 2. Geometries of stationary points involved in the NO3 addition to limonene exocyclic double bond obtained at UB3LYP/6–31G(d,p) level of theory. Bond distances are given in Å. TS5 and TS6 are abbreviations for 1-exo and 2-exo transition states, respectively.
Figure 2. Geometries of stationary points involved in the NO3 addition to limonene exocyclic double bond obtained at UB3LYP/6–31G(d,p) level of theory. Bond distances are given in Å. TS5 and TS6 are abbreviations for 1-exo and 2-exo transition states, respectively.
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Figure 3. NO3-limonene reaction coordinates: relative energies of the stationary points located on the separate NO3 and limonene ground-state potential energy surface. The energy values are given in kcal mol−1 and are calculated using CCSD(T)/6–31G(d) + CF//UB3LYP/6–31G(d,p).
Figure 3. NO3-limonene reaction coordinates: relative energies of the stationary points located on the separate NO3 and limonene ground-state potential energy surface. The energy values are given in kcal mol−1 and are calculated using CCSD(T)/6–31G(d) + CF//UB3LYP/6–31G(d,p).
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Table
Table 1. T1 diagnostic values, spin eigenvalues of the unrestricted wavefunction and its projection for all stationary points in the NO3 addition to the limonene.a
Table 1. T1 diagnostic values, spin eigenvalues of the unrestricted wavefunction and its projection for all stationary points in the NO3 addition to the limonene.a
SpeciesCCSD(T)/6–31G(d)UB3LYP/6–31G(d,p)UB3LYP/6–31G(d,p)
T1<S2><S2>A
limonene0.01000.0000.000
  NO30.02280.7550.750
  TS10.02110.7610.750
Adduct 10.01480.7540.750
  TS20.02890.7600.750
Adduct 20.01490.7540.750
  TS30.02300.7640.750
Adduct 30.01490.7540.750
  TS40.02020.7640.750
Adduct 40.01560.7540.750
  TS50.02200.7680.750
Adduct 50.01460.7540.750
  TS60.02150.7680.750
Adduct 60.01450.7540.750
aAll optimized geometries calculated at the UB3LYP/6–31G(d,p) level.
Table
Table 2. NO3-limonene Reaction Energies (RE) with Zero-Point Correction Included (kcal mol−1) computed at different levels of theory for the six pathways a.
Table 2. NO3-limonene Reaction Energies (RE) with Zero-Point Correction Included (kcal mol−1) computed at different levels of theory for the six pathways a.
MethodRE1-endoRE2-endoRE3-endoRE4-endoRE1-exoRE2-exo
PMP2/6–31G(d)−9.76−12.19−11.41−5.68−9.15−8.72
PMP2/6–311++G(d,p)−7.06−9.46−8.99−3.97−6.45−6.18
B3LYP/6–31G(d,p)−15.26−16.90−14.00−8.73−11.26−10.08
B3LYP/6–311 + G(3df,2pd)−12.04−13.15−10.43−4.91−7.25−6.02
CCSD(T)/6–31G(d)−20.58−22.90−21.90−16.26−19.12−18.55
CCSD(T)/6–31G(d) + CF−17.88−20.17−19.49−14.55−16.42−16.02
aoptimized geometries, vibrational frequencies and ZPE obtained at the UB3LYP/6–31G(d,p) level.
Table
Table 3. NO3-limonene Activation Energies (ΔE) with Zero-Point Correction Included (kcal mol−1) computed at different levels of theory for the six pathways a.
Table 3. NO3-limonene Activation Energies (ΔE) with Zero-Point Correction Included (kcal mol−1) computed at different levels of theory for the six pathways a.
MethodΔE1-endoΔE2-endoΔE3-endoΔE4-endoΔE1-exoΔE2-exo
PMP2/6–31G(d)7.2013.687.687.158.6211.06
PMP2/6–311++G(d,p)10.0616.0610.559.4111.9414.50
B3LYP/6–31G(d,p)−8.17−8.01−7.72−4.72−4.34−0.92
B3LYP/6–311 + G(3df,2pd)−6.47−5.35−5.46−2.02−1.302.27
CCSD(T)/6–31G(d)−6.34−4.41−7.23−5.86−4.78−1.77
CCSD(T)/6–31G(d) + CF−3.47−2.03−4.36−3.60−1.461.67
aoptimized geometries, vibrational frequencies and ZPE obtained at the UB3LYP/6–31G(d,p) level.
Table
Table 4. NO3-limonene Reaction Enthalpies, Gibbs Free Energies and Entropies (ΔH and ΔG in kcal mol−1, ΔS in cal mole−1K−1) with Thermal Correction Included computed at B3LYP/6–31G(d,p) level of theory for the six pathways a.
Table 4. NO3-limonene Reaction Enthalpies, Gibbs Free Energies and Entropies (ΔH and ΔG in kcal mol−1, ΔS in cal mole−1K−1) with Thermal Correction Included computed at B3LYP/6–31G(d,p) level of theory for the six pathways a.
Method1-endo2-endo3-endo4-endo1-exo1-exo
ΔH−15.59−17.42−14.70−9.32−11.73−10.55
ΔG−3.64−4.69−0.973.611.802.83
ΔS−40.08−42.70−46.05−43.37−45.38−44.88
aoptimized geometries, vibrational frequencies and Thermal Correction to Enthalpy and Gibbs Free Energy obtained at the UB3LYP/6–31G(d,p) level.

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Jiang, L.; Wang, W.; Xu, Y.-S. Theoretical Investigation of the NO3 Radical Addition to Double Bonds of Limonene. Int. J. Mol. Sci. 2009, 10, 3743-3754. https://doi.org/10.3390/ijms10093743

AMA Style

Jiang L, Wang W, Xu Y-S. Theoretical Investigation of the NO3 Radical Addition to Double Bonds of Limonene. International Journal of Molecular Sciences. 2009; 10(9):3743-3754. https://doi.org/10.3390/ijms10093743

Chicago/Turabian Style

Jiang, Lei, Wei Wang, and Yi-Sheng Xu. 2009. "Theoretical Investigation of the NO3 Radical Addition to Double Bonds of Limonene" International Journal of Molecular Sciences 10, no. 9: 3743-3754. https://doi.org/10.3390/ijms10093743

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