Methyl peroxy, a key radical in tropospheric chemistry, was recently shown to react with the hydroxyl radical at an unexpectedly high rate. Here, the molecular reaction mechanisms are elucidated using high-level quantum chemical methodologies and statistical rate theory. Formation of activated methylhydrotrioxide, followed by dissociation into methoxy and hydroperoxy radicals, is found to be the main reaction pathway, whereas methylhydrotrioxide stabilization and methanol formation (from activated and stabilized methylhydrotrioxide) are viable minor channels. Criegee intermediate formation is found to be negligible. Given the theoretical uncertainties, useful constraints on the yields are provided by atmospheric methanol measurements. Using a global chemistry-transport model, we show that the only explanation for the high observed methanol abundances over remote oceans is the title reaction with an overall methanol yield of ∼30%, consistent with the theoretical estimates given their uncertainties. This makes the title reaction a major methanol source (115 Tg per year), comparable to global terrestrial emissions.
Methyl peroxy radical (CH3O2) is the most important organic peroxy radical in the atmosphere, with a global production (∼50 Tmoles or 2,500 Tg per year) primarily due to the oxidation of ubiquitous methane by hydroxyl (OH) radicals1. Its reaction with nitric oxide (NO) accounts for ∼25% of the global production of tropospheric ozone2,3, second in importance only to HO2+NO. Under pristine conditions, CH3O2 reacts chiefly with hydroperoxy radicals HO2 to form methyl hydroperoxide CH3OOH, depleting odd hydrogen radicals (HOx≡OH+HO2) directly and through the further reaction of CH3OOH with OH. The reaction of CH3O2 with organic peroxy radicals (RO2) is only a minor sink4, but it is also the only well-documented photochemical source of atmospheric methanol, amounting to 18–38 Tg per year globally according to model estimates5. Note that a much larger total photochemical source (50–100 Tg per year) was invoked by Jacob et al.4 to rationalize serious model underestimations of methanol observations during an aircraft campaign over the Pacific6.
Although the possibility of a reaction of CH3O2 with OH was previously considered7,8, it is only recently that a direct, absolute determination of its rate has been reported. Coupling Laser Induced Fluorescence and cw-Cavity Ring-Down Spectroscopy to laser photolysis, Bossolasco et al.9 measured a rate of (2.8±1.4) × 10−10 cm3 molecule−1 s−1. This unexpectedly high value makes this reaction a major sink of CH3O2 in pristine conditions. Using campaign data in Cape Verde, Fittschen et al.10 estimated that it accounts for ∼25% of the overall CH3O2 sink at that remote site, rivalling the reaction with HO2. Its impact on atmospheric chemistry is however critically dependent on the nature and yields of the products. Three exothermic overall reaction channels were envisaged8:
with CH2O2 the singlet Criegee intermediate, H2C=O(+)−O(−). The Criegee channel (1) has been invoked as the possible source of a missing oxidant of SO2 inferred from observations at a coastal site11. A large Criegee yield would also lead to a very large source of formic acid through reaction of stabilized CH2O2 with water12. The reaction was therefore speculated8,13 to explain part of the missing source of HCOOH required to sustain the high HCOOH levels observed in the atmosphere14,15, although it was found to degrade model/data correlation for measurement campaigns over the U.S.13 The methoxy channel (2) leads ultimately to two HO2 radicals and formaldehyde, which is the end product of both CH3O2+NO and (through CH3OOH) CH3O2+HO2. The methanol channel (2) was noted to be a potentially very significant source of methanol8,13, but no quantitative assessment has been made to this date.
A recent quantum chemical study of CH3O2+OH by Bian et al.16 could identify only one thermally accessible pathway commensurate with the high measured rate constant: combination of the reactants into an activated methylhydrotrioxide CH3OOOH (TRIOX), followed by direct dissociation into CH3O and HO2, which are about 4 kcal mol−1 more stable than the reactant radicals. Another recent theoretical study by Nguyen et al.17 briefly addressed the reaction, concluding that the dominant pathway in atmospheric conditions is collisional stabilization of CH3OOOH, whereas production of Criegee is negligible.
In view of the likely major importance of the title reaction for key oxygenated organic compounds and its potentially large impact on HOx radicals in the remote troposphere, this work proposes to: (i) elucidate the molecular mechanisms of the reaction by constructing detailed potential energy surfaces, using suitable high-level density functional theory (DFT) and ab initio methodologies for the singlet and triplet (biradical) intermediates; (ii) identify the kinetically viable reaction channels and distinguish between the major and minor product routes using appropriate statistical rate theories; (iii) use a global chemistry-transport model, the Intermediate Model for the Annual and Global Evolution of Species (IMAGES, see the ‘Methods section’), to assess the impact of the reaction and constrain the yields through comparisons with atmospheric measurements. For those readers most interested in the implications for atmospheric chemistry, the results relating to goals (i) and (ii) are succinctly summed up before the section on atmospheric modelling, and we invite such readers to move directly to this summary.
Potential energy surface and reaction kinetics
We characterized all three exothermic overall reaction channels (reactions (1), (2), (3)) and all other relevant pathways of the title reaction using quantum chemical methods. Structures and vibrational frequencies were computed with DFT, at the M06-2X-D3/6-311++G(3df,3pd) level of theory (Supplementary Fig. 1, Supplementary Fig. 2, and Supplementary Table 1). More accurate energies were computed using coupled-cluster theory, with explicit (‘F12’) treatment of electron–electron distances, as shown in Fig. 1. The DFT and coupled-cluster calculated properties of various complexes and transition states are summarized in Table 1.
The reaction of CH3OO with OH starts by the barrier-less formation of singlet reactant complex 1RC and triplet reactant complex 3RC, in which OH donates a hydrogen bond to CH3OO, and in which the singlet and triplet states are near degenerate. Hydrogen abstraction starting from 1RC and 3RC to form the Criegee intermediate 1CH2OO and the triplet biradical 3CH2OO via TS2 and TS3, respectively, involve significant barriers. In absence of intersystem crossing (ISC) 3RC→1RC, the reaction CH3O2+OH ↔ 3RC will be quasi-equilibrated such that the bimolecular rate constant for the overall triplet channel CH3O2+OH→3CH2O2+H2O can be found from transition state theory (TST)18,19,20, yielding 3kbi,3(298 K)=2.6 × 10−15 cm3 molecule−1 s−1. This channel is therefore entirely negligible, as are the other triplet entrance routes described by Bian et al.16, all proceeding through transition states that lie even much higher. Instead, rapid ISC of 3RC to the nearly-degenerate 1RC could channel much of the triplet entrance flux also towards the singlet surface and hence to TRIOX (see below), rationalizing the high measured overall rate constant9 of 2.8 × 10−10 cm3 molecule−1 s−1.
The favoured reaction channel of the chemically activated 1RC is the formation of the stable methylhydrotrioxide TRIOX over the very low-energy TS1. Direct dissociation of TRIOX into CH3O and HO2 is not a minimum energy pathway; instead, the energetically favoured decomposition route passes through the singlet product complex 1PC over TS4, which involves concerted CH3O–OOH bond-breaking and formation of a CH3O–HOO hydrogen bond. The relative energy and vibrational properties of saddle-point TS4 play an important role in determining selectivity, but this point is also very difficult to characterize accurately. As explained below, the best results are obtained by using a structure optimized with the M06-D3 DFT method, rather than M06-2X-D3 as used for the other stationary points. Like the reactant complex, the hydrogen-bonded PC has near-degenerate singlet and triplet states. From 1PC, CH2O+HOOH can be formed through TS5, or CH3OH+1O2 can be obtained through TS7. Equally, 1PC can convert to triplet product complex 3PC, and 3PC can form CH3OH+3O2 through the very low TS6.
Transition states TS2, TS3, TS5, TS6 and TS7 corresponding to the abstraction or transfer of a hydrogen atom are straightforward and their identity has been carefully confirmed using intrinsic reaction coordinate (IRC) calculations. The coupled-cluster relative energies agree well with those from DFT, supporting the use of the M06-2X-D3 functional for geometry optimization. However, TS1 and TS4 are more problematic and need further discussion, in particular as these crucial transition states (TSs) largely determine the dominant reactant pathways. Both TSs can be considered to correspond to breaking of one of the O–O bonds in TRIOX. However, this step does not proceed with monotonously increasing energy towards the fragments, due to the existence of the hydrogen-bonded RC and PC. As the relative orientation of the fragments in the complexes differs from that in TRIOX, the TSs have combined O–O bond breaking and fragment reorientation character. Also, TRIOX has a closed-shell singlet electronic structure, with the transition to the open-shell radical pair nature of PC or RC occurring in the region near the TSs. For open-shell singlets with completely uncoupled electrons, singlet and triplet states are near-degenerate (as in RC and PC). Unrestricted DFT calculations and coupled-cluster calculations based on unrestricted Hartree-Fock reference wavefunctions are reasonably accurate in this case. However, for partially uncoupled electrons, the triplet is significantly higher in energy, and unrestricted approaches are less accurate, introducing artefacts in the shape of the energy curve. For TS1, we are able to locate two saddle points, TS1 and TS1′, with the M06-2X-D3 functional. The first one corresponds mostly to reorientation of the OH fragment, while TS1′ has essentially only O–O bond stretching character. Large-active-space CASSCF (complete active space self-consistent field) and CASPT2 (complete active space perturbation theory 2) calculations (Supplementary Fig. 3 and Supplementary Note 1), which can treat systems with partially uncoupled electrons in a balanced way, strongly suggest TS1′ to be purely an artefact based on inaccurate description of the developing low-spin open-shell electronic structure, whereas the TS1 is more reliable.
For TS4, only one TS structure, TS4′, is obtained with M06-2X-D3, but CASSCF and CASPT2 calculations show it is an artefact, similar to TS1′. In contrast, the M06-D3 functional yields a TS structure, denoted TS4, which is closer to the correct TS according to CASSCF and CASPT2. The difference in structure is quite large: the M06-2X-D3 TS4′ structure is very ‘early’ (O–O distance of 1.967 Å) whereas the M06-D3 TS4 has an O–O distance of 2.447 Å. Accordingly, we have used the TS4 structure in this study. For the other stationary points, the CCSD(T)-F12 (coupled cluster—single, double and triple excitation theory) total energies at the M06-D3 and M06-2X-D3 structures differ by <0.2 kcal mol−1, and the vibrational frequencies are very similar also.
The chemically activated singlet reactant complex 1RC, with average vibrational energy <Ev>=4.8 kcal mol−1, including an average 2.1 kcal mol−1 thermal energy at 298 K inherited from the reactants (see the ‘Methods section’), reacts nearly barrier-free (TS1) to form the closed-shell CH3OOOH molecule, TRIOX, much faster than forming Criegee 1CH2O2 and H2O over a barrier of 3.7 kcal mol−1 (TS2). The RRKM-based (Rice, Ramsperger, Kassel, Marcus)21,22 unimolecular rate coefficients averaged over the (narrow) distribution function of formation F(Eth,v) (see the ‘Methods section’) are <k1>=1.8 × 1013 s−1 and <k2>=3.4 × 1010 s−1, respectively. The k-subscripts refer to the TS numbering in Fig. 1. All F(Eth,v)-averaged rate coefficients of the activated reaction steps given in this subsection are for 298 K and 1,013 hPa (air). They are listed also in Table 2, together with the values for 285 K and 750 hPa, as well as these for 256 K and 400 hPa (see next subsection). Since the other pathways to 1CH2O2+H2O theoretically characterized by Bian et al.16 and Nguyen et al.17 contribute even less as they involve TSs lying ≥7 kcal mol−1 above the initial reactants, it is clear that Criegee formation contributes not more than ∼1% overall.
TRIOX, with average chemical activation energy <Ev> of 31.1 kcal mol−1 (at 298 K) converts rapidly to the product complex 1PC over the low-lying and very loose TS4, characterized above, far outrunning the other isomerization/decomposition reactions through high-lying transition states16. The rate coefficient integrated over the formation distribution function F(Eth,v) is evaluated at <k4>=2.4 × 1010 s−1, implying a TRIOX lifetime of ∼40 ps during which it should lose ∼0.45 kcal mol−1 by collisions at 298 K and 1,013 hPa (see below), shifting down also the energy distribution F(Eth,v) for 1PC. The CH3O·HO2 complex 1PC has a decisive role in our system; the ∼7 kcal mol−1 strong CH3O–HOO hydrogen bond explains why the minimum energy pathway of CH3OOOH to CH3O+HO2 passes through it. The fastest reaction of 1PC, with <Ev>(1PC)≈12.4 kcal mol−1, is dissociation into these radicals by breaking the H-bond without exit barrier. The F(Eth,v)- averaged <kdiss> was estimated by variational RRKM21,22. The energy, zero-point vibrational energy (ZPVE) and integrated density of states Gvar(Ev—Evar) were computed for a series of structures with increasing H-bond length, using the unprojected vibrational frequencies, as listed in Supplementary Table 2; the use of projected frequencies23,24,25 for the sum of states would have resulted in ∼12% higher <kdiss> and <3kdiss>, with a minor effect on the overall product yields (see Supplementary Note 3). The variational bottleneck that minimizes Gvar(Ev—Evar), shown in Fig. 2, was found for an H-bond length of 3.2 Å, and relative energy 1.7 kcal mol−1 below the separated CH3O+HO2, giving <kdiss>≈2.4 × 1012 s−1.
The decomposition of 1PC into CH2O+H2O2 over the fairly high TS5, with RRKM-calculated rate of only <k5>=9.7 × 109 s−1 is negligibly slow, whereas decomposition into CH3OH+O2(1Δ) over TS7, at averaged rate <k7>=1.2 × 1011 s−1, is a channel of atmospheric relevance. Importantly, conversion of the initially formed 1PC to 3PC will affect the relative yields of the different products. Spin–orbit coupling between the lowest singlet and triplet states in PC is very small, but the spin–orbit coupling between the lowest singlet state and the second-lowest triplet state (or between the second-lowest singlet and the lowest triplet) is much larger, as there is now an orbital angular momentum difference, and we calculate a root-mean-square coupling matrix element of 58 cm−1 in both cases. Simply assuming Rabi cycling between the two states, a ‘rate constant’ for singlet-triplet conversion of 1.7 × 1012 s−1 is estimated. Using a more rigorous statistical rate theory for reactions with spin-state change26,27 (see Supplementary Note 2), we obtain a remarkably similar estimate of <kISC>=3.5 × 1012 s−1, while the reverse <k−ISC>=1.9 × 1012 s−1. The reverse reaction 1PC→TRIOX occurs with an average rate <k−4> of 1.3 × 1011 s−1, which is ∼3% of the total 1PC removal rate, such that the net TRIOX→1PC conversion rate k4n(Ev)=0.97 × k4(Ev).
3PC decomposes into CH3OH and ground state 3O2 over a very low barrier (TS6), with RRKM-calculated average <3k6> of 4.1 × 1011 s−1, faster than the singlet 1PC reaction to CH3OH, above. It must compete with the reverse ISC, above and also with the fast dissociation of 3PC into CH3O+HO2 at variational-RRKM rate <3kdiss>≈3.4 × 1012 s−1 (see data in Supplementary Table 3), but still results in twice more CH3OH+3O2 production than the CH3OH+1O2 afforded by 1PC, above. Accounting for the rates of all reactions of 1PC and 3PC, the two latter routes together are found to result in a CH3OH yield through activated TRIOX of 7.8% at 298 K and 1,013 hPa. Given the possible error of ∼1.5 kcal mol−1 on the energies of the transition states to CH3OH relative to the (variational) transition states of the PC dissociations, and taking into account also a likely error of a factor of ∼2 on the ratio of kISC/kdiss, we estimate an uncertainty margin on the CH3OH yield of a factor of ∼3.5. Note that about 45% of the products of activated TRIOX arise via ISC of 1PC to 3PC. Of major importance is that TRIOX does not decompose directly but via the complex 1PC, which enables production of CH3OH, while direct methanol formation from CH3OOOH would face a quasi-unsurmountable barrier16.
A (minor) fraction of the activated TRIOX will suffer energy loss by successive collisions with air molecules to yield thermalized CH3OOOH, of which the subsequent fates are discussed in Supplementary Note 4. Using the bi-exponential energy transfer model of Troe28 with an assumed average energy transferred per collision <ΔE>all of −0.9 kcal mol−1—fairly high because TRIOX has several low-frequency vibration modes—and taking into account the distribution function F(Eth,v) of the activated TRIOX, the fraction of stabilization at a collision frequency of 1.2 × 1010 s−1 at 298 K and 1,013 hPa was evaluated (see the ‘Methods section’) to be fstab≈10.7%. However, this result is quite uncertain, first of all because it is very sensitive to the assumed value of <ΔE>all: doubling it increases fstab nearly threefold while halving it reduces fstab to <2%. Moreover, the calculated fstab depends also strongly on k4(Ev), which itself bears a possible error of a factor ∼1.5–2. We therefore estimate a stabilized CH3OOOH yield at 298 K and 1 atm in the range 0–35%. The much higher fstab of ∼90% predicted by Nguyen et al.17 can be ascribed to their TS for TRIOX→1PC conversion being our artefactual TS4′, which on account of its far higher rigidity than TS4 leads to a much lower calculated rate of TRIOX→1PC and hence much more TRIOX stabilization.
Reaction products and estimated yields in the troposphere
The theoretical investigation above predicts that the dominant product route of the title reaction is channel (2) yielding the radicals CH3O+HO2, whereas the suggested channel (1)8,9 producing the Criegee Intermediate CH2O2 is found to be entirely negligible. On the other hand, we find that the title reaction yields a sizable fraction of collisionally thermalized (but chemically labile) CH3OOOH, of order of 10% at 1 atm and 298 K, while we also uncovered two parallel pathways leading directly to CH3OH+O2 with overall yield around 7% in the same conditions. No evidence could be found for any other significant product routes. It must be stressed that the yield estimates of CH3OOOH and CH3OH given above and listed in Table 3 are subject to large uncertainty factors of ∼3.5 for each, as detailed in the previous subsection.
As detailed in the next subsection, the title reaction is most important above the tropical oceans, where NO levels are low but OH concentrations moderate to high. The rate of the reaction as a function of decreasing pressure (or of increasing altitude) and as a function of latitude is depicted in Supplementary Fig. 4. Near the Equator, accounting for the temperature profile, ∼50% of the reaction occurs below 750 hPa (altitude ∼2.4 km) where the average temperature is 285 K, and nearly ∼95% below 400 hPa (altitude ∼7.5 km) where temperature is 256 K. Given that the CH3OOOH stabilization fraction should show a considerable pressure and temperature dependence, and a minor temperature dependence is also expected for other pathways (see the ‘Methods section’) we have evaluated the CH3OOOH and CH3OH yields also for the ‘median’ conditions 750 hPa and 285 K, and for the ‘limit’ conditions 400 hPa and 256 K, above. The results, together with those for 1,013 hPa and 298 K, are listed in Table 3. The pronounced pressure- and temperature dependences of the CH3OOOH stabilization fraction can be expressed within a few per cent by the power function fstab(P,T)=0.107 × (P/1,013 hPa)2.0 × (298 K/T)5.0.
Modelled global impact
Adopting the measured rate9 of CH3O2+OH, the reaction accounts for 20% of the global CH3O2 sink according to IMAGES simulations. The global flux through that reaction is considerable: ∼11 Tmoles per year, comparable to, for example, the global source of isoprene29. Although it is only a minor sink (∼10%) of CH3O2 at high latitudes and over polluted continental regions (Fig. 3) where the reaction with NO is by far the largest sink (Supplementary Fig. 5), the reaction with OH represents 20–30% of the sink over tropical oceans and deserts, where CH3O2+HO2 is however still dominant (30–50% of total sink).
Table 4 summarizes the model simulations. The best theoretical estimates are used in run B, while runs C and D adopt yields approaching respectively the high end and low end of the estimated uncertainty range of both the direct CH3OH yield and the TRIOX stabilization fraction. Relative to a simulation neglecting the title reaction, the HO2 radical abundances are increased by 10–20% over tropical oceans (Supplementary Fig. 6). Unsurprisingly, the impact is highest when the HO2 yield is highest (run D). The changes are negligible or even negative in high-NOx areas.
The changes in OH are of opposite sign to those of HO2, reaching up to −7% over remote oceans. Loss of OH due to reaction with CH3O2 and the products CH3OOH and CH3OH is partially offset by OH recycled from enhanced HO2. The globally averaged OH concentration decreases by 1.5–3.2% depending on the simulation, increasing the methane lifetime by up to 0.3 years in run C. The largest OH changes are calculated in run C, due to its lower HO2 yield and higher OH loss through reaction with CH3OOOH and CH3OH. Surface ozone is decreased due to the CH3O2+OH reaction, by up to 6% over remote oceans, and by 1–2% (<1 ppbv) over Europe, North America and East Asia in July (Supplementary Fig. 7). Hydrogen peroxide (H2O2) is strongly impacted, owing to the quadratic dependence of its production on HO2 levels. Its concentrations increase by up to 30% in run C (Fig. 4) and ∼50% in runs B and D.
Methyl peroxy radical abundances are reduced by up to 40% over tropical oceans (Fig. 4), irrespective of the yield assumption. This strong drop in concentration reflects increased loss through reaction with OH and HO2, and slightly decreased production from CH4+OH. The decreases in CH3OOH are also substantial (up to −30%). Formaldehyde is almost unaffected, being an end product to all CH3O2 sink pathways. Methanol, however, shows drastic differences among the simulations: whereas its concentrations increase or decrease by ∼20% at most in runs B and D, the global methanol burden is increased by 60% in run C, with concentration increases reaching 30–100% over remote oceans (Fig. 4). Even over continents, methanol increases by 10–20% over most areas and by 80–200% over desert regions with very low methanol emissions. Methanol formation from CH3O2+OH is largely due to the direct pathway to CH3OH+O2 (56%), but indirect formation through stabilized TRIOX is significant (44%). Reaction on aerosols is calculated to be the largest TRIOX sink globally, followed by reaction with OH and reaction with (H2O)2 (Supplementary Fig. 8, Supplementary Note 4). The calculated average yield of methanol from stabilized TRIOX is 65%.
Model evaluation for peroxides and formaldehyde
We limit our evaluation to stable compounds over oceans, where strongest impacts are expected. Both the modelled vertical profile and latitudinal profile of H2O2 agree generally fairly well with the observations from aircraft and ship campaigns (Supplementary Fig. 9, Supplementary Fig. 10, and Supplementary Fig. 11), indicating that its sources and sinks are reasonably well described by the model. As seen in Supplementary Table 4, the average model bias across all campaigns is improved when including the title reaction, from −14% in run A to +3 and −2% in runs B and C, respectively. Although this improvement could be fortuitous, given the known uncertainties in HOx modelling30, the title reaction clearly does not lead to noticeable inconsistencies with the data. As expected, the reaction has negligible impact on modelled CH2O (Supplementary Fig. 12) which agrees very well with aircraft data over oceans.
For CH3OOH, the title reaction leads to model underestimations (>∼25%) of airborne measurements, but it improves significantly the model agreement with ship measurements (Supplementary Fig. 11, Supplementary Fig. 13, and Supplementary Table 5). The contradiction between the conclusions from either ship or aircraft data is difficult to explain given the wide geographical area covered by both platforms. As in a previous modelling study13, the largest biases are found for INTEX-B (ref. 31). Since even the run ignoring the title reaction largely underestimates the observations in several campaigns, measurement issues and/or model uncertainties likely cause the discrepancies. For example, the estimated uncertainty in the rate constant of the CH3OOH+OH reaction is a factor of 1.4 (ref. 32). Adopting a rate constant measurement33 about 25% lower than the current Jet Propulsion Laboratory recommendation32 used in the model increases the CH3OOH concentrations by 15–20% and goes already a long way to compensating the deterioration of model performance against aircraft campaigns (Supplementary Fig. 13 and Supplementary Table 5). Other relevant processes might be also uncertain. More work is needed to address those issues.
A large source of methanol
In agreement with previous studies4,5,34,35, our simulation omitting CH3O2+OH underestimates CH3OH observations by a factor of ∼2 over the remote Pacific (Fig. 5). When including the reaction, methanol production from CH3O2+RO2 is halved, from 33 to 15 Tg per year (Supplementary Table 6) due to its near-quadratic dependence on CH3O2 levels. The CH3O2+OH reaction would therefore worsen the model underestimations unless methanol is produced by the reaction with a sufficient yield. The model/data mismatch is barely reduced in run B, with its low overall methanol yield (∼12%), while it nearly vanishes in run C, with an overall yield of 32%. Both the average concentration and vertical profile shape are greatly improved in this case.
Similar conclusions hold for comparisons at the most remote sites Mauna Loa and Cape Verde, which was shown to be under mostly maritime and Saharan influences36 (Table 5, Supplementary Fig. 15). The other campaigns listed in Table 5 were probably more impacted by continental emissions, which are likely overestimated in the model since they were derived by inverse modelling34 while neglecting the contribution of CH3O2+OH. Nevertheless, including the reaction improves the model performance against airborne measurement at mid-latitudes (Supplementary Fig. 16). An overestimation of oceanic emissions likely contributes also to the strong model overestimation for the Atlantic Meridional Transect cruise AMT-22 (Supplementary Fig. 17), since flux measurements by eddy covariance during that campaign37 indicated no emission, only deposition with an average dry deposition velocity (0.68 cm s−1) close to the corresponding model value (0.63 cm s−1). Suppressing oceanic emissions in the model (run C_NO) leads to a much closer agreement with the latitudinal profile of AMT-22 data. That this setting leads however to large underestimations at other sites (Table 5) suggests that ocean/atmosphere exchanges are more variable than currently assumed.
The theoretical results presented above leave little doubt that the Criegee pathway (1) is negligible in atmospheric conditions, that is, CH2O2 is not formed in any significant amount from CH3O2+OH which therefore cannot be an important source of formic acid. Actually, any sizable contribution of the reaction to HCOOH formation would lead to huge overestimations of its modelled concentrations over the Southern Pacific (Supplementary Fig. 18) where median concentrations of only 19 pptv were measured in the boundary layer during spring38, almost an order of magnitude below modelled values assuming a 40% stabilized CH2O2 yield.
The theoretical calculations further inform us that the methoxy pathway (2) is expected to dominate, whereas both methanol formation (3) and stabilization of the trioxide are viable, but likely minor. Of fundamental interest is that significant direct methanol production can occur only because the activated CH3OOOH intermediate decomposes indirectly through the CH3O·HO2 complex. The share of each of the two minor channels likely does not exceed ∼20% of the total reaction rate. Theory alone cannot provide precise yield estimates, due to uncertainties in key parameters, that is, precise barrier heights, average energy losses per collision, and the singlet ↔ triplet ISC rate that impacts methanol production.
Fortunately, atmospheric measurements provide valuable constraints. The persistent model underestimation of CH3OH measurements over the remote Pacific4,5,34,35 cannot be explained by ocean/atmosphere exchanges, since higher emissions would cause strong decreasing vertical gradients not seen in campaign data; on the contrary, eddy covariance measurements37 indicate that oceanic emissions might be very low. Another remote source of methanol, the photochemical production due to CH3O2+RO2 reactions, could be underestimated. But since it is largely dominated by the CH3O2 self-reaction of which the methanol yield (∼0.63) cannot be much underestimated, and since CH3O2 production from CH4+OH is also well constrained, only a large production of organic peroxy radicals from non-methane organic precursors could boost this source of methanol. High observed acetaldehyde over oceans6,36,39 suggested indeed the existence of unknown sources of CH3CHO or of its precursors. However, besides the noted inconsistency39 of those observations with measured PAN:NOx ratios, the good agreement of modelled CH2O with observations over oceans (Supplementary Fig. 12) shows that those potential sources cannot weigh heavily on CH2O and CH3O2 production.
The only viable candidate for the missing remote source of methanol is therefore CH3O2+OH, with an overall methanol yield crudely estimated to be ∼30%, consistent with theoretical estimates given their uncertainties. Given the experimental uncertainty (50%) in the total rate constant of the reaction9, this inferred overall yield could be even higher, or possibly lower. The total photochemical source of methanol in run C (130 Tg per year) slightly exceeds the range (50–100 Tg per year) estimated by Jacob et al.4, because of a higher net ocean sink and lower continental emissions in our simulations. The contribution of CH3O2+OH (115 Tg per year globally) is comparable in magnitude to the total terrestrial emission source. Further work will be needed to evaluate how this source will impact our understanding of the methanol budget. Clearly, a better understanding of ocean-atmosphere exchanges is required to refine the top–down yield estimation presented above. It is not currently possible to determine which of the direct methanol formation channel or indirect pathway through the stabilised TRIOX is dominant. A more direct experimental determination is obviously needed. Hopefully TRIOX can be measured, although loss to walls might prove challenging, and atmospheric concentrations should be very low, a few pptv at most.
Reaction with OH might be also significant for other peroxy radicals, such as those formed from biogenic terpenoids. We expect that for the much larger activated ROOOH†, conversion to a complex RO—HO2 and eventual dissociation to RO+HO2 will be substantially slower than for CH3OOOH†, such that collisional stabilisation of ROOOH† should be a major if not dominant product route. However, the global relevance for large peroxys formed from biogenic terpenoids is expected to be lower compared with CH3O2+OH, because OH levels are generally lower in the boundary layer over forests than in the oceanic lower troposphere, and because the reaction of HO2 with large peroxys is considerably faster than the reaction of CH3O2 with HO2 (ref. 40). Assuming a rate constant similar to that of CH3O2+OH, the reaction of large biogenic peroxy radicals with OH is estimated here to account for ∼3% of their total sink over remote forests.
All the structures presented on the potential energy surface were fully optimized with DFT using the M06-2X-D3/6-311++G(3df,3pd) level of theory in Gaussian 09 version D.01 (ref. 41; see Supplementary Table 7), except where explicitly stated otherwise. The M06-2X-D3 method was benchmarked and recommended for the general main group elements including the evaluation of thermochemistry, kinetics and noncovalent interactions42. For the geometry optimization and the corresponding frequency calculations, a tight convergence criterion and a superfine integration grid (150,974) were adopted. Wherever appropriate, an unrestricted ansatz was used, and careful checks were made to ensure that low-spin open-shell solutions were found to the Kohn–Sham equations. The calculated vibrational frequencies have been used for evaluation of zero-point energies and RRKM rate calculations. All the transition states for the reactions involving the abstraction or transfer of a hydrogen atom were confirmed by IRC calculations, while for the reactions from the reactant complex 1RC via TRIOX to the product complex 1PC, attempts to generate IRC curves failed due to the low curvature of the potential energy surface, so instead, various scans were used to explore the behaviour of those two loose TSs (Supplementary Fig. 3 and Supplementary Note 1).
Various single-point calculations were carried out using CASSCF, CASPT2 and CCSD(T)-F12. The CASSCF and CASPT2 calculations were performed with Molpro 2012.1 (refs 43, 44) with an active space of 18 electrons in 13 active orbitals (which corresponds to a full-valence active space, but omitting the O–H and C–H bonding orbitals and the C–H anti-bonding orbitals), with the cc-pVTZ basis set45. We also calculated the spin–orbit coupling constant with Molpro at CASSCF(18,13)/cc-pVTZ level of theory.
Explicitly correlated CCSD(T)-F12 energies were obtained with the ORCA 3.03 package46, using an unrestricted HF-reference wavefunction for reactant and product radicals and the open-shell singlet intermediates, and a restricted reference otherwise. The cc-pVTZ-F12 basis set47 and appropriate auxiliary basis sets were used. Unless mentioned otherwise, all reported energies derive from CCSD(T)-F12/cc-pVTZ-F12 calculations with ZPVE corrections from M06-2X-D3/6-311++G(3df,3pd).
Theoretical reaction kinetics
The statistical-kinetics rates for thermal as well as chemically activated reactions were estimated using the energies obtained at our highest level and including the ZPVE (scaled by a factor 0.97 (ref. 48)) as stated above, while partition functions or integrated sums of vibration states and vibration state densities were based on the M06-2X-D3 harmonic vibration frequencies (scaled by a factor 0.983 (ref. 48)) and rigid-rotor rotation constants. For all structures and transition states involved we adopted the harmonic oscillator approximation, commensurate with our aim of identifying the relevant reaction pathways and distinguishing between major and minor routes based on an approximate, semi-quantitative assessment of end-product yields.
As detailed in the Results section, the only thermal bimolecular reaction that needs to be considered was found to be unimportant if not negligible. Its thermal rate coefficient at 298 K was computed using conventional transition state theory22, with tunnelling factor estimated assuming an asymmetric Eckart potential49,50.
The majority of the relevant reaction steps are chemically activated unimolecular reactions of (i) the initial singlet reactant complex 1RC, (ii) the closed-shell singlet intermediate TRIOX and (iii) the resulting product complexes 1PC and 3PC. We employed RRKM theory21,22 to estimate the micro-canonical rate coefficients for each of the steps:
in which α is the reaction path degeneracy, h Planck’s constant, E≠ the TS energy, Ev the vibration energy of the reacting activated intermediate, N(Ev) its density of vibration states and G≠(Ev−E≠) the sum of accessible vibration states of the TS; both the latter were evaluated by exact count22. The conservation of angular momentum was accounted for in reasonable approximation by correcting the potential energies (inclusive ZPVE) of the activated reactants and transition structures by their average rotation energy relative to that of the reactant complex 1RC, adopting the quasi-diatom approximation (see Supplementary Note 5). The changes in effective potential energy21,22 are at most ±0.3 kcal mol−1 and the rotational effects on the chemically activated rate coefficients remain minor for all reactions (1–20%). Tunnelling corrections for all relevant activated reactions were found negligible because of the relatively high excess vibration energies (Ev–E≠) and low imaginary frequencies (see Supplementary Table 1). The rate constants for the dissociation of the singlet and triplet product complexes 1PC and 3PC were calculated using variational RRKM21,22 by locating the structure ‘var’ that minimizes Gvar(Ev−Evar). The rate constant for ISC of 1PC to 3PC was calculated based on locating the minimum energy crossing point using the code developed by Harvey and Aschi51,52. (see Supplementary Note 2)
In the total distributable energy Ev, we duly include the thermal vibration energy Eth,v that the intermediates inherit from the thermal reactants CH3O2+OH, and for each step the rates k(Ev) were averaged over the thermal distribution function F(Eth,v) of formation. As the lifetime of the initial complex 1RC is <1 ps, the original thermal distribution F(Eth,v) remains conserved up to the TRIOX intermediate, but it shifts down for 1PC and 3PC by ∼0.45 kcal mol−1 at 298 K/1,013 hPa, ∼0.35 kcal mol−1 at 285 K/750 hPa and ∼0.25 kcal mol−1 at 256 K/400 hPa, respectively, due to the average of ∼0.5, 0.4 and 0.3 collisions, respectively, that TRIOX suffers in the atmosphere during its lifetime (see <k4> rate values in Table 2). The lifetime of <0.3 ps of 1PC and 3PC is too short for further collisional losses. The width of F(Eth,v), of ∼2 kcal mol−1, is much less than the average excess energy (Ev−E≠) for most reaction steps, and the k(Ev) are generally not far from their high-energy asymptotes, such that the F(Eth,v)-averaged <k(Ev)> differ only 1–20% from k(<Ev>). The only exception is the 1PC reaction through TS2, which anyway is negligibly slow compared with the competing reaction through TS1. As a result, the precise shape of F(Eth,v) is of little importance for the overall kinetics of the chemically activated unimolecular reactions of our system, though the average value of the thermal <Eth,v> is of some significance. As there is no entrance barrier and the entrance transition state TSin is variational (see Fig. 1), the formation distribution function F(Eth,v) cannot be evaluated in the usual way21. However, the average initial <Eth,v>, of ∼2.1, 2.0 and 1.75 kcal mol−1 at 298, 285 and 256 K, respectively, could be estimated with sufficient accuracy for our purpose and a reasonable F(Eth,v) could be derived accordingly as detailed in Supplementary Note 6.
Different from the effective rates of the unimolecular reactions, the (minor) fraction fstab of the activated TRIOX that becomes collisionally stabilized depends markedly on the vibration energy of the activated TRIOX and is therefore quite sensitive to F(Eth,v). The stabilization competes with the much faster rearrangement TRIOX→1PC through TS4 at net rate kn4(Ev) (≈0.97 × k4(Ev) due to the reverse reaction). The Lennard-Jones collision frequency of CH3OOOH with air molecules, kcoll=ZLJ[M], is estimated53 to be about 1.2, 0.92 and 0.55 × 1010 s−1 at 298 K/1,013 hPa, 285 K/750 hPa and 256 K/400 hPa, respectively. The bi-exponential energy transfer model of Troe28 was used and implemented in a quasi-stochastic approach; the average energy transferred per collision, a critical quantity for the overall fstab but highly uncertain, was assumed to be <ΔE>all=−0.9 kcal mol−1, amounting at 298 K to an average energy lost per down-collision α≈1.34 kcal mol−1 and average energy gained per up-collision β≈0.44 . For a given initial energy Ev,in of TRIOX, the stabilization fraction was found as the repetitive product of the successive, increasing probabilities of a (new) jth collision at constant rate kcoll in competition with TRIOX→1PC rearrangement at net rate kn4(Ej−1) that decreases on average after each collision:
Given the initial excess energy of TS4 of ∼7 kcal mol−1, this product converges rapidly after some 8–10 collisions for the adopted <ΔE>all. The overall fstab was finally found by integrating over the distribution function F(Eth,v). As the net TRIOX conversion rate kn4(Ev) at the initial energies is relatively high, fstab is small and depends strongly on <ΔE>all but also markedly on kn4(Ev) itself. Obviously, at higher altitudes in the troposphere, fstab decreases with decreasing pressures, but this is partially offset by the pronounced, multiple effect of the simultaneous temperature decrease: through the lower kn4(Ev), the lower average Eth,v to be lost for stabilization, the effect on the number density of N2/O2 and the higher Ω2,2 collision integral. Thus, the combined effects of the decreasing pressure P and temperature T in the troposphere above tropical oceans result in a dependence fstab∼P2 × T−5.
Overall and net reaction rates and end-product yields were obtained in a straightforward way by duly considering the fractional contribution of each competing reaction for each intermediate in the complete scheme.
IMAGES54,55 calculates the distribution of 172 compounds at 2° × 2.5° resolution, using meteorological fields from ERA-Interim analyses of the European Centre of Medium-Range Weather Forecasts (ECMWF). Simulations were made for the year 2010 with a spin-up time of 6 months starting in July 2009. Anthropogenic emissions are obtained from a global inventory (edgar.jrc.ec.europa.eu/overview.php?v=42) overwritten by regional inventories over Europe, Asia and the U.S. Biomass burning emissions are provided by the Global Fire Emissions Database GFEDv4s (www.globalfiredata.org). Isoprene fluxes are based on the Model of Emissions of Gases and Aerosols from Nature (MEGAN)55. Biogenic methanol emissions (100 Tg per year globally) are obtained from an inverse modelling study34 using IMAGES and methanol total columns from Infrared Atmospheric Sounding Interferometer. Parameterization of ocean-atmosphere methanol exchanges follows a two-layer model resulting in an oceanic source of 39 Tg (in 2010) and an oceanic uptake represented as dry deposition (between 46 and 66 Tg per year depending on the model simulation). The isoprene degradation mechanism has been updated to account for the revised peroxy radical kinetics of the Leuven Isoprene Mechanism LIM1 (ref. 56) as well as for the chemistry of isoprene epoxides57. Wet scavenging is parameterized based on ECMWF cloud and precipitation fields58. Dry deposition follows Wesely’s resistance-in-series scheme59, with aerodynamic resistances based on Monin-Obukhov similarity theory (ECMWF, IFS Documentation—Cy40r1, Operational implementation 22 November 2013, Part IV: Physical processes, European Centre for Medium-Range Weather Forecasts, Shinfield Park, Reading, England, 2014.) using sensible heat fluxes and friction velocities from ECMWF operational analyses and quasi-laminar layer resistances dependent on gas-phase diffusivity60. Surface resistances are calculated depending on mesophyll, cuticular, ground and in-canopy aerodynamic resistances59,61,62. The surface resistances are adjusted to provide a better match of modelled dry deposition velocities with eddy-covariance estimates over a forest by Nguyen et al.63; in particular, the H2O2 surface resistance becomes negligible after this adjustment.
As detailed in Supplementary Note 4, the reactions of the stabilized trioxide include the thermal conversion to the product complex 1PC; reaction with OH; reaction with the water dimer; and reactive uptake on aqueous aerosols. Aerosol uptake is calculated54 based on sulfate/ammonium/nitrate and carbonaceous aerosols calculated by IMAGES, and sea salt aerosols obtained from the MACC (Monitoring Atmospheric Composition & Climate) Reanalysis (apps.ecmwf.int/datasets/data/macc-reanalysis/levtype=sfc/). The water dimer concentrations are calculated using an equilibrium constant expression64 validated with available experimental data.
The authors declare that the data supporting the findings of this study are available within the article and its Supplementary Information file. Any further relevant code and data used in the paper are available from the authors upon request.
How to cite this article: Müller, J.-F. et al. The reaction of methyl peroxy and hydroxyl radicals as a major source of atmospheric methanol. Nat. Commun. 7, 13213 doi: 10.1038/ncomms13213 (2016).
This work received support from project PRODEX ACROSAT of the European Space Agency funded by the Belgian Science Policy Office (Belspo). It was also sponsored in part by Belspo under contract SD/CS/05A (project BIOSOA) in the frame of the Science for Sustainable Development programme, and by the Office of China Postdoctoral Council (No. 20140061) through the International Postdoctoral Exchange Fellowship Program. We acknowledge the free use of merged data sets from NASA tropospheric chemistry campaigns. We thank Maite Bauwens for her assistance with data management.
About this article
Rights and permissions
This work is licensed under a Creative Commons Attribution 4.0 International License. The images or other third party material in this article are included in the article’s Creative Commons license, unless indicated otherwise in the credit line; if the material is not included under the Creative Commons license, users will need to obtain permission from the license holder to reproduce the material. To view a copy of this license, visit http://creativecommons.org/licenses/by/4.0/