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Understanding the oxidation mechanism of methanesulfinic acid by ozone in the atmosphere

Scientific Reportsvolume 9, Article number: 322 (2019) | Download Citation

Abstract

Methanesulfinic acid (MSIA) is an important intermediate in the oxidation of dimethyl sulfide (DMS) in the marine boundary layer. The oxidation of MSIA by ozone in the gas phase to form methanesulfonic acid (MSA) was investigated using theoretical calculations in this paper. Three pathways can be found for the reaction of MSIA with ozone. The highest energy barrier is 13.02 kcal mol−1 in the most favorable pathway. By comparing the reaction rate of MSIA + O3 with that of MSIA + OH, it can be concluded that the oxidation of MSIA by O3 to form MSA is of minor significance relative to its oxidation by OH radical in the gas phase. This study can provide some information for the theoretical and experimental studies in the significantly heterogeneous and aqueous-phase oxidation of MSIA by O3.

Introduction

Dimethyl sulfide (CH3SCH3, DMS) emitted by oceans is the main natural source of S-containing compound1,2,3. The oxidation of dimethyl sulfide is considered of great importance in the marine boundary layer, because the main oxidation products, methanesulfonic acid (MSA) and sulfuric acid, can contribute to the formation of non-sea salt sulfate (nss-SO42−) aerosol, which can act as the cloud condensation nuclei and can promote the formation of marine stratus clouds4,5,6. The reactions with OH radical during the day time5,7 and with NO3 radical5,8,9 in the night initiate the DMS oxidation, and these reactions can be classified as adduct reactions and abstraction reactions. Numerous intermediates such as dimethyl sulfoxide (CH3SOCH3: DMSO), methanesulfinic acid (CH3S(O)OH: MSIA), dimethyl sulfone (CH3SO2CH3: DMSO2) and CH3SOx(x = 0−3) radicals can be formed through the subsequent reaction5,10. The branching and many intermediates indicate that the DMS oxidation mechanism is complicated. Therefore, although a number of studies have worked on this area5,6,10,11,12,13,14,15,16,17,18,19, the oxidation mechanism still cannot be understood completely.

MSIA, an important intermediate in the process of DMS oxidation, is formed through the OH radical addition to DMSO with the elimination of CH3 radical. Using LFP-TDLAS technique, Urbanski et al.20 have proved that the reaction of DMSO with OH radical can form MSIA and CH3 radical in high yield. The same conclusion also is obtained in subsequent researches including laboratory studies and quantum chemistry calculations21,22,23,24,25,26,27. Barnes et al.5 also concluded that the MSIA is an important DMS secondary oxidation product through OH radical oxidation of DMSO in their review paper.

In addition to the formation of MSIA, their further oxidation also needs to be focused on. The MSIA is soluble in water, and its Henry’s law coefficient is higher than that of DMSO and lower than that of MSA5. Thus, the reaction involving MSIA can occur in gas phase, in aqueous phase and on the surface of aqueous atmospheric media. The OH radical and O3 are thought as the main oxidants in oxidizing the MSIA5,6,18,28,29. The ab initio and density functional theory (DFT) calculations are useful tools for mechanism research. Tian et al.28 have used DFT method to study the reaction of OH radical with methanesulfinic acid (MSIA). They found that the association-decomposition reaction (MSIA + OH → adduct → CH3SO2 + H2O → CH3 + SO2 + H2O) is more favorable than direct CH3 radical-abstraction reaction (MSIA + OH → adduct → CH3 + H2SO3 → CH3 + SO2 + H2O). In another theoretical study29, the author also found the two kinds of reaction mechanism, and concluded that the formation channel of CH3 radical and H2SO3 should not be negligible because more than 30% of MSIA react with OH via this channel within the range of 298–600 K.

For the oxidation of MSIA by O3, some studies have considered it. Enami et al.18 have performed the experiment to investigate the OH radical-initiated oxidation of DMSO on the air-water interface. In their work, they have concluded that the MSIA (or dissociated methanesulfinic acid) formed by the reaction OH + DMSO can further be oxidized by O3 or OH + O2, producing the MSA. In the modeling study of Hoffmann et al.6, the reaction of MSIA and dissociated methanesulfinic acid with O3 leading to MSA in the aqueous phase contribute in total 42% to MSIA degradation. However, to our knowledge, the mechanism of the reaction MSIA + O3 has not been considered by the theoretical study.

In this paper, we will investigate the reaction of MSIA with ozone using DFT method and ab initio method. To find the most favorable pathway, the reaction energy barrier in different pathways is calculated and compared. We also compared rate constants of the MSIA + O3 reaction with that of the MSIA + OH reaction, so as to evaluate their atmospheric importance.

Results and Discussion

The reaction of MSIA with O3

Figure 1 shows the potential energy profile for MSIA + O3 reaction. The corresponding structures of reactants, intermediates, transition states and products are drawn in Fig. 2. The thermodynamic data for the reaction MSIA with O3 are summarized in Supplementary Information (Table S1). For MSIA, as shown in Fig. 1 and Fig. 2, two conformers, called as MSIA-I and MSIA-II, can be found. The MSIA-I can transform into MSIA-II with a transition state (energy barrier of 1.00 kcal mol−1), which is depicted in Supplementary Fig. S1. Two pathways are identified in the reaction of MSIA-I and O3 (path 1: starting from C1-1, path 2: from C2-1 to MSA + 1O2). In path 1, as MSIA-I approaches the O3 molecule, the complex C1-1 can be formed. The C1-1 is stabilized by 4.60 kcal mol−1 with respect to MAIA-I + O3. The complex C1-1 is held together by two hydrogen bonds and one van der Waals interaction. As shown in Fig. 2, the hydrogen atom of MSIA-I interacts with the two oxygen atoms of ozone to form the two hydrogen bonds, whereas sulfur atom is involved in the formation of van der Waals interaction with an oxygen atom of ozone. After the formation of the complex C1-1, the reaction proceeds via a transition state (TS1-1) with the energy barrier of 13.02 kcal mol−1 related to C1-1 to form the C1-2. In the complex C1-2, one oxygen atom has bonded with sulfur atom. The subsequent transformation from C1-2 to C1-3 corresponds to the hydrogen atom transfer process. The energy barrier with the transition state TS1-2 is 3.43 kcal mol−1. For C1-3, it is obviously more stable than C1-2 because its energy is lower 44.97 kcal mol−1 than that of C1-2. The result indicates that the effect of hydrogen atom transfer process is to adjust the structure so as to increase the stability of complex. The C1-3 passes through a transition state TS1-3 with energy barrier of 11.87 kcal mol−1 to form the complex consisting of MSA with 1O2 (C1-4), which is lie 3.74 kcal mol−1 below the final product (MSA + 1O2).

Figure 1
Figure 1

The calculated potential energy profile for the reaction of MSIA with ozone at the CCSD(T)/aug-cc-pV(T + d)Z//M06-2X/aug-cc-pV(T + d)Z level.

Figure 2
Figure 2

Optimized structures of reactants, complexes, transition states and products for the reaction of MSIA with ozone at the M06-2X/aug-cc-pV(T + d)Z level.

In path 2, the reaction begins with the formation of complex C2-1 with the binding energy of 2.98 kcal mol−1. The C2-1 involves one van der Waals interaction between an oxygen atom of MSIA-I and an oxygen atom of ozone. The complex C2-2 can be formed through a transition state TS2-1 with the energy barrier of 36.89 kcal mol−1. Then, the C2-2 transform to the complex (C2-3) via a transition state TS2-2 with the energy barrier of 5.53 kcal mol−1. The TS2-2 involves the breaking of O-O bond and simultaneously the formation of O-S bond. The C2-3 is held together by one van der Waals interaction between an oxygen atom of methanesulfonic acid (MSA) and an oxygen atom of 1O2, and is expected to be stable toward break up to MSA + 1O2.

In the reaction between MSIA-II and O3, only one pathway (named as path 3) can be found. As the similar structure between MSIA-I and MSIA-II, its sequence of steps C3-1 → TS3-1 → C3-2, has the same feature as the sequence C2-1 → TS2-1 → C2-2. The binding energy of C3-1 relative to MSIA-II and ozone is 3.01 kcal mol−1. The barrier height in the process for path 3 is 38.44 kcal mol−1. After the complex (C3-2) formation, the reaction proceeds through transforming the dihedral angle O1SO2Ha to C2-2. The transformation process needs to go through a transition state TS3-2, and overcome the energy barrier of 0.95 kcal mol−1. Then the reaction goes on along the sequence of steps C2-2 → TS2-2 → C2-3.

To sum up, there are three pathways in the reaction of methanesulfinic acid (MSIA) with ozone. For path 2 and path 3, the initial step needs to overcome the energy barrier of around 40 kcal mol−1, and the energy for most of complexes and transition states is 30 kcal mol−1 higher than that of reactants. All barrier heights in path 1 do not exceed 14 kcal mol−1, and only the energy of TS1-1 is 8.42 kcal mol−1 higher than that of reactants. Thus, the path 1 is the most favorable reaction pathway.

Atmospheric implications

To evaluate the importance of the methanesulfonic acid (MSA) formation by the reaction MSIA + O3, we will compare the rate between the reaction of MSIA with ozone and the reaction of MSIA with OH radical. Considering that the channel in which the CH3 radical and H2SO3 are formed accounts for about 1/3 for the reaction of MSIA with OH radical, we will compare this slower reaction channel with the favorable channel (path 1) in the reaction of MSIA with ozone.

Although the channel mentioned above in the reaction MSIA + OH has been reported, we also recalculate it at the CCSD(T)/aug-cc-pV(T + d)Z//M06-2X/aug-cc-pV(T + d)Z level to perform a fully legitimate comparison at the same level of theory. Figure 3 shows the potential energy and the structure of all stationary points for MSIA + OH reaction. The thermodynamic data are tabulated in Supplementary Information (Table S2). For this channel, we found that only MSIA-I can react with OH radical to form CH3 radical and H2SO3, which is called as path 4 in this paper. The complex (C4-1) consisting of MSIA-I and OH radical is firstly formed with the binding energy of 7.49 kcal mol−1 in this channel, which agrees with the value (8.14 kcal mol−1) calculated by González-García et al.29. Then, the C4-1 can evolve via TS4-1 with the energy barrier of 3.06 kcal mol−1, into the complex C4-2 whose energy is 10.61 kcal mol−1 lower than that of reactants. Once the C4-2 is formed, it can be easily transformed with a transition state TS4-2 into CH3 radical and H2SO3. The barrier height in the transformation from C4-2 to products is only 0.87 kcal mol−1. The barrier for the transformation from C4-1 to C4-2 is also in agreement with 3.39 kcal mol−1 in the literature29. The binding energy of C4-2 in our calculation is slightly higher than the value (12.40 kcal mol−1) obtained by González-García et al.29. As for the energy barrier connecting C4-2 and products, our calculated result may be more accurate than that in the mentioned literature because the value in this literature is −0.01 kcal mol−1. These results obtained from comparison about the reaction MSIA + OH help us to conclude that the difference between our calculation and the literature is slight.

Figure 3
Figure 3

The calculated potential energy profile for the reaction of MSIA with OH radical at the CCSD(T)/aug-cc-pV(T + d)Z//M06-2X/aug-cc-pV(T + d)Z level.

As for path 1 (considering C1-4 as the end in kinetics analysis) and path 4, the main reaction step can be expressed as equation (1) and equation (2) in the follows:

$$\mathrm{MSIA} \mbox{-} {\rm{I}}+{{\rm{O}}}_{{\rm{3}}}\to \mathrm{C1} \mbox{-} 1\mathop{\longrightarrow }\limits^{TS1-1}\mathrm{C1} \mbox{-} 2\mathop{\longrightarrow }\limits^{TS1-2}\mathrm{C1} \mbox{-} 3\mathop{\longrightarrow }\limits^{TS1-3}\mathrm{C1} \mbox{-} 4$$
(1)
$$\mathrm{MSIA} \mbox{-} {\rm{I}}+{\rm{OH}}\to \mathrm{C4} \mbox{-} 1\mathop{\longrightarrow }\limits^{TS4-1}\mathrm{C4} \mbox{-} 2\mathop{\longrightarrow }\limits^{TS4-2}{{\rm{CH}}}_{{\rm{3}}}+{{\rm{H}}}_{{\rm{2}}}{{\rm{SO}}}_{{\rm{3}}}$$
(2)

Assuming the complex C1-1 and C4-1 is in equilibrium with their corresponding reactants, and the steady state approximation is applied, the reaction rates can be formulated as:

$${v}_{1}={K}_{eq1}{k}_{uni1}[\mathrm{MSIA} \mbox{-} {\rm{I}}][{{\rm{O}}}_{{\rm{3}}}]={k}_{1}[\mathrm{MSIA} \mbox{-} {\rm{I}}][{{\rm{O}}}_{{\rm{3}}}]$$
(3)
$${v}_{4}={K}_{eq4}{k}_{uni4}[\mathrm{MSIA} \mbox{-} {\rm{I}}][{\rm{OH}}]={k}_{4}[\mathrm{MSIA} \mbox{-} {\rm{I}}][{\rm{OH}}]$$
(4)

Where ν represents the reaction rate, Keq is the equilibrium constant for the formation of C1-1 (or C4-1) from the corresponding reactants; kuni is the rate constant of unimolecular rearrangement, and the subscript 1 or 4 represents path 1 or path 4.

As the multiple transition states occur in path 1 and path 4, the unified statistical model30 is applied to calculate kuni.

$$\frac{1}{{k}_{uni1}}=\frac{1}{{k}_{TS1-1}}+\frac{1}{{k}_{TS1-2}}+\frac{1}{{k}_{TS1-3}}$$
(5)
$$\frac{1}{{k}_{uni4}}=\frac{1}{{k}_{TS4-1}}+\frac{1}{{k}_{TS4-2}}$$
(6)

The relative rate for path 1 and path 4 can be obtained as follows:

$$\frac{{v}_{1}}{{v}_{4}}=\frac{{K}_{eq1}{k}_{uni1}[\mathrm{MSIA} \mbox{-} {\rm{I}}][{{\rm{O}}}_{{\rm{3}}}]}{{K}_{eq4}{k}_{uni4}[\mathrm{MSIA} \mbox{-} {\rm{I}}][{\rm{OH}}]}=\frac{{K}_{eq1}{k}_{uni1}[{{\rm{O}}}_{{\rm{3}}}]}{{K}_{eq4}{k}_{uni4}[{\rm{OH}}]}=\frac{{k}_{1}[{{\rm{O}}}_{{\rm{3}}}]}{{k}_{4}[{\rm{OH}}]}$$
(7)

The rate constant k1, k4 and the ratio between k1 and k4 within the range of 220 K to 298 K are shown in Table 1. The corresponding Keq, kTS and kuni are put into Supplementary Information (Table S3). As shown in Table 1, the rate constant of path 1 changes from 1.22 × 10−24 to 1.79 × 10−22 cm3 molecule−1 s−1 within the range of 220 to 298 K, whereas that of path 4 is transformed from 3.87 × 10−9 cm3 molecule−1 s−1 at 220 K to 2.84 × 10−10 cm3 molecule−1 s−1 at 298 K. It is obvious from the ratio between k1 and k4 that the rate constant for the reaction MSIA + O3 is about 1013–1016 times lower than that for the reaction MSIA + OH within the range of 220 K to 298 K. The concentration of ozone in the troposphere is a few tens of parts per billion by volume (ppbv) in mix ratio31. After converting the mix ratio to concentration in molecules cm−3 (10 ppbv = 2.50 × 1011 molecules cm−3 at 1 atm and 298 K), the concentration of ozone is ~1011 molecules cm−3. The concentration of OH radical is ~106 molecules cm−3 in the troposphere32. The concentration ratio between ozone and OH radical is about 105. Thus, considering the rate constants and concentration, the reaction rate of MSIA with ozone is 108–1011 times slower than that of MSIA with OH within the range of 220–298 K. The conclusion can be drawn that the gas-phase oxidation of MSIA by ozone to form MSA is of minor importance relative to the reaction of MSIA with OH radical. The result also indicates that the oxidation of DMSO through MSIA intermediate in the gas phase mainly produce SO2 (subsequently converting to H2SO4).

Table 1 The rate constant (cm3 molecule−1 s−1) and rate constant ratio for the reaction of MSIA with ozone and with OH radical.

Conclusion

The oxidation of methanesulfinic acid (CH3S(O)OH: MSIA) by ozone in the atmosphere has been investigated in this paper using the quantum chemical calculations. Two conformers of MSIA and the three reaction pathways can be found. The pathway (MSIA-I + O3 → C1-1 → TS1-1 → C1-2 → TS1-2 → C1-3 → TS1-3 → C1-4 → MSA + 1O2) is the most favorable because its highest energy barrier is 13.02 kcal mol−1, which is evidently lower than those of another two pathways. By kinetics analysis, the oxidation of MSIA by ozone is 8–11 orders of magnitude slower than that by OH radical in the range of 220–298 K. The result indicates that the oxidation of MSIA by ozone is minor important in most cases relative to its oxidation by OH radical in the gas phase. Although it has shown the unimportance of the reaction in the gas phase, the study about the gas-phase oxidation of MSIA by ozone is meaningful because it can provide some information for the theoretical and experimental studies in the significantly heterogeneous and aqueous-phase oxidation of MSIA by ozone.

Methods

All geometric structures were optimized using M06-2X method33 with the aug-cc-pVTZ basis set34 for the H, C, O atoms and aug-cc-pV(T + d)Z basis set35 for the S atom (for simplification, the group of basis set was called as aug-cc-pV(T + d)Z). For aug-cc-pV(T + d)Z basis set, it is to add one additional high-exponent d function to aug-cc-pVTZ so as to obtain satisfactory convergence behavior35. The revised basis set has been used in many sulfur-containing systems, and it has been proved that the aug-cc-pV(T + d)Z basis set can obtain more accurate results36,37,38. After optimization, the frequency calculation was performed in order to confirm the energy minimum points and transition states, and to obtain the zero point energy correction and thermal correction. The intrinsic reaction coordinate (IRC) calculation39,40,41 also was carried out to ensure that the transition states connected with the corresponding reactants and products. For M06-2X method, the ultrafine integration grid was chosen to enhance calculation accuracy at reasonable additional cost. Single-point energies were refined using the CCSD(T) method42,43 with aug-cc-pV(T + d)Z basis set. To estimate the extent of nondynamic correlation, the T1 diagnostic (computed using CCSD(T)/aug-cc-pV(T + d)Z) was used44. If the value of T1 is more than 0.04, the single reference wave function is considered to be unreliable45. The value of T1 calculated for all species in this paper (see Supplementary Table S4) is below 0.04, indicating that the CCSD(T) method is suitable. All quantum chemistry calculations were carried out with Gaussian 09 suit of software46. The geometries were drawn using the CYLview software package47.

For the reaction of MSIA with O3, it involves in the O3 of biradical character and produced 1O2, which makes the optimization process more complex. It is because for biradical stationary points the unrestricted formalism needs to be considered so as to obtain the stable broken-symmetry solution. Our strategy is firstly to use the restricted M06-2X method to gain all stationary points in these pathways, then to verify the stability of the wave function using the keyword stable in Gaussian. It can be found that there are two kinds of stationary points related to the unstable wave function: one is from the beginning of pathway, which consists of O3-MSIA complex and the first transition state in the pathway; another is from the end of pathway, which composes of the last transition state and produced 1O2-MSA complex. For the former, the reason of wave function instability is biradical character of O3. We re-optimize these points by specifying the keyword stable = opt to generate a stable initial guess. After the geometries were optimized, the stability of wave function is tested again using the keyword stable. If the instability is found, it needs to repeat the optimized process until the wave function is stable. For the letter, the wave function instability is understandable because the ground state of O2 is a triple state. Since the MSIA with O3 react in the singlet potential energy surface, the produced O2 is singlet state. Thus, in this case, the stationary points related to wave function instability do not need to re-optimize.

For the kinetics analysis, the electronic energies based on the CCSD(T)/aug-cc-pV(T + d)Z level of theory, while the partition functions obtained from the M06-2X/aug-cc-pV(T + d)Z level of theory. The conventional transition-state theory (TST)48 with Wigner tunneling correction was used to calculate the rate constants. All rate constants were calculated by using the KiSThelP program49.

Data Availability

The data generated or analyzed during the current study are available from the corresponding author on reasonable request.

Additional information

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Acknowledgements

This work is supported by National Natural Science Foundation of China (21337001 and 21607011), Natural Science Foundation of Shandong Province (ZR2018MB043), and The Fundamental Research Funds of Shandong University (2018JC027).

Author information

Affiliations

  1. Environment Research Institute, Shandong University, Jinan, 250100, China

    • Guochun Lv
    •  & Xiaomin Sun
  2. College of Biological and Environmental Engineering, Binzhou University, Binzhou, 256600, China

    • Chenxi Zhang

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Contributions

G.C.L., C.X.Z. and X.M.S. conceived and designed the research. G.C.L. performed the calculation and analyzed the data, and wrote the main manuscript text. C.X.Z. and X.M.S. revised the initial manuscript. All of the authors discussed the results, and contribute to the final manuscript.

Competing Interests

The authors declare no competing interests.

Corresponding author

Correspondence to Xiaomin Sun.

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https://doi.org/10.1038/s41598-018-36405-0

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