Detecting Intermediates and Products of Fast Heterogeneous Reactions on Liquid Surfaces via Online Mass Spectrometry

One of the research priorities in atmospheric chemistry is to advance our understanding of heterogeneous reactions and their effect on the composition of the troposphere. Chemistry on aqueous surfaces is particularly important because of their ubiquity and expanse. They range from the surfaces of oceans (360 million km2), cloud and aerosol drops (estimated at ~10 trillion km2) to the fluid lining the human lung (~150 m2). Typically, ambient air contains reactive gases that may affect human health, influence climate and participate in biogeochemical cycles. Despite their importance, atmospheric reactions between gases and solutes on aqueous surfaces are not well understood and, as a result, generally overlooked. New, surface-specific techniques are required that detect and identify the intermediates and products of such reactions as they happen on liquids. This is a tall order because genuine interfacial reactions are faster than mass diffusion into bulk liquids, and may produce novel species in low concentrations. Herein, we review evidence that validates online pneumatic ionization mass spectrometry of liquid microjets exposed to reactive gases as a technique that meets such requirements. Next, we call attention to results obtained by this approach on reactions of gas-phase ozone, nitrogen dioxide and hydroxyl radicals with various solutes on aqueous surfaces. The overarching conclusion is that the outermost layers of aqueous solutions are unique media, where most equilibria shift and reactions usually proceed along new pathways, and generally faster than in bulk water. That the rates and mechanisms of reactions at air-aqueous interfaces may be different from those in bulk water opens new conceptual frameworks and lines of research, and adds a missing dimension to atmospheric chemistry.


Introduction
A recent expert report delineated the research priorities in atmospheric chemistry [1].It called for "developing a stronger understanding of the influences that heterogeneous chemistry exerts on tropospheric composition", "developing the next generation of accurate, sensitive and specific measurement capabilities for atmospheric constituents . . . on surfaces", and "identifying and quantifying the individual oxidants in the condensed phase that contribute to toxicity".Together, these issues point to surfaces as significant media in atmospheric chemistry.
"God made the bulk.Surfaces were invented by the devil", Wolfgang Pauli famously said.The definition of a surface itself raises thorny questions: how thick is the layer of atoms or molecules that can be considered the surface of an object, i.e., where does a surface end and the bulk begins?Or, on the topic at hand, how air-liquid interfaces behave when probed from the liquid or the airside?These are fundamental questions, to which experimental and theoretical studies have provided answers as varied and conflicting as those of the six blind men about the elephant [2].
The surface of water is prominent because it is everywhere.The interfacial layers of water represent a distinct phase where the density of water drops five orders of magnitude (from 1 g cm −3 to 1.7 × 10 −5 g cm −3 at 300 K) in ~1 nm [3].This precipitous density gradient at the molecular scale represents a steep slide on which species nevertheless find equilibrium positions according to their properties.Hydrophobic gases, such as hydrocarbons, tend to accumulate at the relatively dry surface rather than immerse in bulk water [4,5], while ions do the opposite.Reactive gases could be depleted so fast by aqueous solutes in interfacial layers that they never reach bulk water.These are key issues that call for educated guesses.One might ask whether the vast information available on the structure of interfacial water, obtained by surface-specific spectroscopic techniques and molecular dynamics calculations, provides useful hints about interfacial chemistry.The caveat is that the temporal and spatial scales of the interfacial structures revealed by spectroscopic techniques may not match those of interfacial reactions.Furthermore, it is fair to say that the relative sparsity of dynamic/kinetic versus structural studies [6,7] is not on par with the importance of interfacial processes [8].For this reason, we wanted to call attention to our experiments on the kinetics and mechanisms of interfacial reactions, and to some of the results we obtained on some outstanding issues of atmospheric importance.
The objectives of this paper are to validate online pneumatic ionization mass spectrometry (o-PI-MS, a variant of electrospray ionization mass spectrometry, see below) of liquid microjets dosed by reactive gases as a versatile technique to investigate interfacial processes, and to review some significant results obtained by this approach.Validation was considered necessary because it might not be readily apparent that the o-PI-MS technique could be applied to investigate interfacial reactions [6,9].The main reason is that transferring ions from liquids to the gas-phase is a complex phenomenon.In contrast with the monochromatic signals and selection rules of surface-specific spectroscopic techniques, one is confronted with a sequence of events that begins with the nebulization of liquids into microscopic droplets carrying net charges, followed by rapid solvent evaporation, a series of Coulomb explosions, and ends with ion desolvation and their release to the gas-phase [10].
Questions arise about whether it is valid to assign o-PI mass spectra to the products of gas-liquid reactions occurring in the outermost interfacial layers of liquid microjets.For example: (1) are the detected species drawn from the interfacial layers or the bulk of the liquid microjets?and (2) is the chemistry affected by the electric fields required for ion detection?Below, we analyze experiments specifically designed to address these questions.Our approach to studying interfacial processes via o-PI-MS neither is a new idea nor is as farfetched as it might seem.Yamashita and Fenn had already suggested that electrospray ionization mass spectrometry could be used to investigate liquid interfaces in their seminal 1984 paper [11].

Online Mass Spectrometry of Chemical Reactions on Liquid Microjets
Because our experimental setup and experiments have been described in several publications from our laboratories [12][13][14][15][16], here we focused on their essential features.At the outset, we wish to emphasize that electrospray ionization mass spectrometers are not all alike.Therefore, it is crucial to report the particular configuration of the mass spectrometer used in each case, and the specific experimental conditions under which results were obtained.Key differences are whether the nebulizer is grounded or not, and whether the liquid microjets are directly ejected (along the X-axis) (see Figure 1) towards the inlet orifice in the metal plate (MP) that separates the spraying chamber from the low pressure section of the mass spectrometer, along a perpendicular (Y-axis) direction, or in a Z-configuration [17].Comparisons of results obtained using different instruments should always bear in mind these issues.for additional details).The spraying chamber is at atmospheric pressure and ambient temperature.MP is a metal plate polarized at ≤ 3.5 kV (relative to the grounded nebulizer) which has a pinhole inlet to the mass analyzer section of the mass spectrometer (not shown).
In our experiments, solutions of diverse solutes in water or its mixtures with fully miscible organic solvents such as acetonitrile, tetrahydrofuran or 1,4-dioxane, were pumped through a grounded stainless-steel syringe injector (100 μm bore).The linear speed of the liquid microjets flowing into the spraying chamber of the mass spectrometer is ∼10 cm s −1 (chamber at 1 atmosphere and room temperature).Liquid microjets were nebulized by a codirectional N2(g) flow (at >100 m s −1 , through a sheath coaxial with the syringe injector).The large difference between the speeds of the liquid microjet and the nebulizer gas forced the liquid to fragment into fine, electrically charged, primary ∼10 micrometer diameter droplets [18,19] within τ ≤ 10 microseconds, as revealed by high-speed photography of the shearing of cylindrical water jets by fast annular gas flows [20][21][22][23].Primary droplets were rapidly blown by the nebulizer gas into liquid "bags", which broke up into secondary, sub-micron size droplets carrying net charges [20].Experiments have shown that: (1) the thin bag films are enriched in anions, whereas cations accumulate in the thick bag rims, as expected from the higher affinity of the former for the air-water interface [20,24], and (2) the extent of ion segregation (between anions in the films from cations in the rims, and from different anions within the films) increases with nebulizer gas flow rate [15].Aerodynamic considerations indicate that the smaller (less than ∼10 micrometer) secondary and later generation progeny microdroplets cannot be further deformed by the nebulizer gas.The fate of later generation microdroplets is in fact controlled by the balance of surface tension versus electrostatic repulsion among excess charges (see below).During nebulization, the kinetic energy of the nebulizing gas provides energy for creating the droplets surfaces, and for charging droplets by separating the anions and cations already present in the liquid microjets.The net result is that the gas-liquid sprays issuing from a grounded nozzle injector consist of normal distributions of weakly charged droplets centered at charge zero, as expected from statistical charge separation during the fragmentation of a neutral liquid [25].It is apparent that the aerodynamic charging process naturally discriminates against the production of highly charged droplets, simply because they would require more energy.Solvent evaporation in the spraying chamber (continuously flushed with dry N2(g)) could lead to droplet shrinkage and concomitant surface charge crowding.Consequently, droplets become mechanically unstable at the point where electric repulsion of interfacial charges overtakes liquid cohesion, thereby triggering Coulomb explosions into smaller droplets.Charged microdroplets are deflected towards the mass analyzer sector by applying an electric bias to the inlet port MP.In this sector, charged microdroplets  [12][13][14][15][16] for additional details).The spraying chamber is at atmospheric pressure and ambient temperature.MP is a metal plate polarized at ≤ 3.5 kV (relative to the grounded nebulizer) which has a pinhole inlet to the mass analyzer section of the mass spectrometer (not shown).
In our experiments, solutions of diverse solutes in water or its mixtures with fully miscible organic solvents such as acetonitrile, tetrahydrofuran or 1,4-dioxane, were pumped through a grounded stainless-steel syringe injector (100 µm bore).The linear speed of the liquid microjets flowing into the spraying chamber of the mass spectrometer is ~10 cm s −1 (chamber at 1 atmosphere and room temperature).Liquid microjets were nebulized by a codirectional N 2 (g) flow (at >100 m s −1 , through a sheath coaxial with the syringe injector).The large difference between the speeds of the liquid microjet and the nebulizer gas forced the liquid to fragment into fine, electrically charged, primary ~10 micrometer diameter droplets [18,19] within τ ≤ 10 microseconds, as revealed by high-speed photography of the shearing of cylindrical water jets by fast annular gas flows [20][21][22][23].Primary droplets were rapidly blown by the nebulizer gas into liquid "bags", which broke up into secondary, sub-micron size droplets carrying net charges [20].Experiments have shown that: (1) the thin bag films are enriched in anions, whereas cations accumulate in the thick bag rims, as expected from the higher affinity of the former for the air-water interface [20,24], and (2) the extent of ion segregation (between anions in the films from cations in the rims, and from different anions within the films) increases with nebulizer gas flow rate [15].Aerodynamic considerations indicate that the smaller (less than ~10 micrometer) secondary and later generation progeny microdroplets cannot be further deformed by the nebulizer gas.The fate of later generation microdroplets is in fact controlled by the balance of surface tension versus electrostatic repulsion among excess charges (see below).During nebulization, the kinetic energy of the nebulizing gas provides energy for creating the droplets surfaces, and for charging droplets by separating the anions and cations already present in the liquid microjets.The net result is that the gas-liquid sprays issuing from a grounded nozzle injector consist of normal distributions of weakly charged droplets centered at charge zero, as expected from statistical charge separation during the fragmentation of a neutral liquid [25].It is apparent that the aerodynamic charging process naturally discriminates against the production of highly charged droplets, simply because they would require more energy.Solvent evaporation in the spraying chamber (continuously flushed with dry N 2 (g)) could lead to droplet shrinkage and concomitant surface charge crowding.Consequently, droplets become mechanically unstable at the point where electric repulsion of interfacial charges overtakes liquid cohesion, thereby triggering Coulomb explosions into smaller droplets.Charged microdroplets are deflected towards the mass analyzer sector by applying an electric bias to the inlet port MP.In this sector, charged microdroplets are electrically driven through a heated capillary, where ions are desolvated and released bare to the gas-phase [26].The preceding description shows that the ions detected by the mass spectrometer are produced from the shearing of the interfacial layers of the liquid microjets, followed by the breakup of primary microdroplets.
That the droplets produced by nebulizing liquids are charged has been known for more than a century [20,21], and has important applications [27].It is important to realize that droplet charging does not require [28,29], although may be enhanced by the presence of electric fields.Below, we show that in our setup the creation of net charge was mainly due to pneumatic nebulization rather than to the applied electric field.This is the reason why we referred to our technique as online pneumatic ionization mass spectrometry, o-PI-MS.It should be emphasized that, electric fields could participate in droplet charging in other electrospray ion source configurations, and at higher applied voltages.
Because the surface of liquid microjets containing mobile ions is equipotential with the grounded injector, the electric field inside the microjets is null.Applied electric fields, however, induce surface charges of densities determined by the MP voltage and the local curvature of the liquid surface.The sign of surface charges is determined by the voltage polarization, i.e., a MP at positive voltage relative to ground induces negative charges on the surface of microjets, and vice versa.Below, we show that the surface charges induced by the applied electric field played a minimal role, if any, in our experiments.
In a typical experiment, streams of reactive gases, such as O 3 (g) or NO 2 (g), are directed to the liquid microjets as they emerge from the tip of the nebulizer.Some reactions between gases and solutes do occur at the gas-liquid interfaces of the microjets during their τ ≤ 10 µs lifetimes [22].Note that only fast heterogeneous reactions meet such a constraint.This constraint, however, is not as restrictive as it may seem because, remarkably, interfacial reactions have been found to be much faster (up to several orders of magnitude) than estimated from kinetic parameters determined in bulk liquids [14, [30][31][32].

Mass Spectra Reflect the Composition of the Outermost Interfacial Layers of the Liquid Microjets
The first indication that we sampled the interfacial layers rather than the bulk of the microjets was provided by the mass spectra of equimolar solutions of the sodium salts of a series of anions [33,34].We found that the mass signal intensities of the various anions were not identical, as would be expected if mass spectra reflected the composition of the bulk equimolar solutions, but rather scaled exponentially with anion radii.This outcome suggested that our experiments probed interfacial layers where anions had fractionated following a Hofmeister series [35].We obtained more direct, semi-quantitative evidence from other experiments.We will illustrate this with the following examples.
In one set of experiments, liquid microjets of n-hexanoic acid (PCOOH, pK a = 4.8; P = n-pentyl) solutions in 1:1 (vol:vol) H 2 O/D 2 O at pH 7 (reported pH is always of the injected bulk solutions, as measured with a calibrated pH-meter.pD = pH + 0.4) were dosed with HNO 3 (g) or DNO 3 (g) streams [36].Mass spectra in the negative ion mode revealed that n-hexanoate PCOO The key observation was that the relative intensities of the hydronated PCOOH signals significantly changed upon switching from HNO 3 (g) to DNO 3 (g).From the measured flow rates of the liquid microjets and the HNO 3 (g)/DNO 3 (g) streams, we estimated that the inflows of H/D atoms (atoms s −1 ) carried by the liquid microjets into the spraying chamber was >1000 times larger than those carried by HNO 3 (g) or DNO 3 (g).Therefore, the fact that the isotopic composition of hydronated PCOOH changed upon switching from HNO 3 (g) to DNO 3 (g) implied that PCOOH hydronation must have taken place in relatively thin interfacial layers rather than in the bulk liquid.We calculated the thickness δ of the interfacial layers probed in our experiments from the proton concentrations required to half PCOO − m/z = 115 signals.Such proton concentrations were generated from the flux of protons n H+ (in protons cm −2 s −1 ) deposited by HNO 3 (g) in interfacial layers of thickness δ during τ ≤ 10 µs contact times.n H+ was evaluated by means of the kinetic theory of gases (see below) by assuming a unitary uptake coefficient, γ ~1, for HNO 3 (g) on the surface of aqueous electrolytes [36].In this manner, we estimated: δ ~2 ± 1 nm, values.Note that τ, γ and δ were directly correlated, i.e., γ < 1, τ ≤ 10 µs values would lead to δ < 2 ± 1 nm interfacial layers.
A second piece of evidence was obtained in the competitive protonation versus lithiation of gas-phase trimethylamine TMA(g) on the surface of aqueous microjets containing 100 mM LiCl at various pH values [38].Plots of the intensities of TMAH + (m/z = 60) and TMALi + (m/z = 66) signals as functions of TMA(g) concentration showed that TMAH + signals plateaued above a few parts per million by volume (ppmv) TMA(g) both at pH 2.0 and 3.5, while TMALi + kept increasing up to 150 ppmv TMA(g).These observations signal the presence of a finite pool of protons available to TMA(g) at the gas-liquid interface.This could happen if the available protons were those already present in interfacial layers (rather than in the much larger pool provided by the bulk liquid), and the self-ionization of water were too slow to replenish the interfacial layers with protons within ~10 µs.In another set of experiments, acidified D 2 O microjets were simultaneously exposed to TMA(g) and H 2 O(g).The detection of TMAD + and TMAH + signals of comparable intensities, despite the fact that the inflow of H 2 O(g) was <D 2 O(l)/1000, provided further evidence that TMA(g) was hydronated in nanoscopic interfacial layers.
Additional evidence was the fact that in most of our heterogeneous ozonation experiments, the mass spectral signals of the reactive solutes X never vanished, even at the highest O 3 (g) concentrations (~100 ppm, ~2 × 10 15 molecules cm −3 ), but bottomed out at about half of their initial values [14, 16,31,39].This observation implies that our experiments sampled interfacial layers where solutes X are both consumed by O 3 , via Equation (1): and replenished by diffusion from underlying layers.The thickness of the interfacial layers can be estimated from simple considerations.By assuming that gas-diffusion resistance can be neglected for O 3 (g) approaching microjets of 100 µm diameter, the concentrations N (in molecules cm −3 ) of O 3 injected into interfacial layers of thickness δ during contact times τ ≤ 10 µs can be evaluated from the kinetic theory of gases, Equation (2): In Equation ( 2), γ ≤ 1 × 10 −2 is the uptake coefficient of O 3 (g) on water [40], c = 3.6 × 10 4 cm s −1 is the mean thermal speed of O 3 molecules and n the concentration of O 3 (g) in molecules cm −3 .In typical experiments, solute concentrations dropped by 50% and bottomed out upon exposure to n ≥ 1 × 10 14 O 3 molecules cm −3 (≥5 ppm).Under such conditions: N ~9 × 10 10 (1/δ).The fact that these O 3 concentrations could only deplete half of the 1 mM (6 × 10 17 molecules cm −3 ) solutes present in interfacial layers, is expressed by Equation (3): which leads to δ ~3 × 10 −7 cm, i.e., interfacial layers of thickness of a few nanometers.

Products of Gas-Liquid Reactions are Mainly Formed on Liquid Microjets Rather Than on Daughter Microdroplets
This was demonstrated by the well-defined RCOO − (R = n-alkyl) mass signals versus pH titration curves (inflection points at pK a (RCOOH) = 4.8) obtained from aqueous RCOOH solutions [14,37,38,[41][42][43][44][45].Well-defined pK a (RCOOH) = 4.8 titration curves imply that the sampled layers have well-defined proton activities [46].given by the pH values of the injected RCOOH solutions.Therefore, the sampled layers must be those of the intact microjets or the primary microdroplets, i.e., those from where RCOO − ions are separated from protons H + , before significant solvent evaporation has taken place.In other words, well-defined titration curves exclude later generation microdroplets, which have a broad distribution of (higher) acidities from extensive evaporation, as the source of mass signals.
Further evidence came from experiments involving the ozonolysis of β-caryophyllene (a very reactive sesquiterpene that adds O 3 (g) within ~10 µs) in two different configurations.In the first one, microjets of 1 mM β-caryophyllene solutions in acetonitrile/water mixtures containing 1 mM NaCl (to bind the neutral α-hydroxyhydroperoxide products into detectable chloride adducts) [47] were injected at 100 µL min −1 (injection of 1 × 10 9 β-caryophyllene molecules s −1 into the spraying chamber) and dosed on and off by O 3 (g) streams.Intense mass spectral signals of functional carboxylates (FC, m/z = 251) and chloride adducts of the α-hydroxyhydroperoxides (HH, m/z = 305 and 307), the products of reactions of the Criegee intermediates generated in the ozonolysis of β-caryophyllene, appeared upon dosing with O 3 (g).In the second set of experiments, microjets of 1 mM NaCl in acetonitrile/water solutions (i.e., without β-caryophyllene) were injected into the spraying chamber simultaneously with O 3 (g) and β-caryophyllene vapor (at 4 × 10 15 β-caryophyllene molecules s −1 ).Although the flow of β-caryophyllene molecules injected into the spraying chamber in this case was much larger than in the first set of experiments, product signals remained within background noise (Figure S2, Reference 48) [48].Therefore, in our experiments, products were generated on the surface of intact liquid microjets, rather than on daughter microdroplets or in the gas-phase.
In experiments on the protonation of gas-phase isoprene on acidic pH ≤ 4 water microjets, we found that varying the distance from the injector of gas-phase isoprene to the tip of the nebulizer decreased the intensities of product signals.This is again consistent with the protonation of isoprene on intact microjets of well-defined acidities, rather than on superacidic microdroplets [49].We want to point out that the reactive uptake coefficient of gas-phase isoprene estimated from our experiments on pH ≤ 3 water: 5× 10 −7 ≤ γ ISO ≤ 2 × 10 −6 , is in good accordance with the values reported from independent experiments on acidic NH 4 HSO 4 /H 2 SO 4 aerosols: γ ISO = 4 × 10 −6 [50], and on 70% H 2 SO 4 films: γ ISO = 1 × 10 −6 [51].

Applied Electric Fields Deflected Charged Microdroplets but Did Not Affect Interfacial Chemistry
Initial evidence that our observations could not be ascribed to electric field effects came from experiments involving the protonation of gas-phase trimethylamine TMA(g) [38] and the deprotonation of gas-phase alkyl-carboxylic acids CA(g) (acetic and hexanoic acids) [52] on the surface of water as a function of bulk pH.In the CA experiments [52], we detected carboxylate anions by polarizing the metal plate MP at positive voltages.In this case, electrostatics dictates that the electric field induces negative surface charge density on the microjets, i.e., an overpopulation of interfacial hydroxide ions [53,54].Therefore, CA(g) should be deprotonated on the surface of water at pH values lower than in bulk water.This was indeed the case: half of CA(g) were deprotonated on the surface of pH = 2.8 water, i.e., two pH units lower than their pK a = 4.8 in bulk water [52].The same logic predicts that gas-phase TMA should be protonated on the surface of water of pH values higher than its pK a = 9.8 in bulk water.However, at variance with this prediction, we found that TMA(g) was protonated only on the surface of pH < 4 water, i.e., about 10 6 times more acidic than pH = 9.8 water [38].It is apparent that the shifts of the titration curves of both gas-phase acids and bases on the surface of water towards pH values lower than in bulk water cannot be ascribed to the surface charges induced by the applied electric fields, but correspond to an unrelated phenomenon.In fact, both gas-phase bases and acids being protonated and deprotonated on the surface of water of pH ~3 ± 1 suggests that the underlying mechanism is associated with the properties of interfacial water itself, as we and others have proposed elsewhere [55,56].
More direct evidence was obtained from the dependence of the FC (m/z = 251) and HH-Cl − (m/z = 305 and 307) product signal intensities in the ozonolysis of β-caryophyllene (see Section 4, above) as functions of the applied polarizing voltage [48].It was found that signal intensities strictly increased (with a correlation coefficient ρ 2 = 0.99) with the square root of the polarizing voltage V 1/2 (see Figure S3 of Reference 48) [48].This is the dependence of a purely kinematic effect on the trajectories of charged microdroplets in the spraying chamber towards the inlet of the MP (Figure 1), rather than from electric field effects on chemistry.
This follows from simple considerations.In our setup, microdroplets were carried forward (along the Y-axis, Figure 1) by the nebulizer gas at >100 m/s linear speeds.At these speeds, the microdroplets covered the 2 cm separating the tip of the nebulizer from the x-axis through the inlet in τ < 0.250 milliseconds.In order to capture charged microdroplets and detect the ions they carry, an electric field must be applied to deflect them along to the X-axis towards the MP.The instantaneous acceleration a x imposed on the microdroplets by the electric field along the X-axis is given by Equation (4): where ne − is the charge and m the mass of microdroplets, V is the potential difference and d the distance between the tip of the grounded nebulizer and MP.As noted above, the mass of microdroplets may not be constant due to continuous solvent evaporation.The net charge of microdroplets, in contrast, only changes in Coulomb explosions upon reaching Rayleigh's thresholds [57].Therefore, applied voltages V must be such that the ∆x = 1 cm distance between the Y-axis and the MP is covered by the accelerated microdroplets in t ≤ τ times, Equation ( 5): i.e., t ∝ V −1/2 .Thus, the shorter the flight times t, the larger the number of microdroplets deflected towards the polarized MP, i.e., mass spectral signal intensities should increase as (1/t) ∝ V 1/2 , as observed.We ascribed the stronger V 1/2 dependence of the HH signals relative to FC signals (see Figure S3 in Reference 48) to the fact that the neutral α-hydroxyhydroperoxides will only bind to Cl − after microdroplets are desolvated in the mass analyzer section and, therefore, will partially evaporate in the spraying chamber.Hence, evaporation losses of neutral α-hydroxyhydroperoxides will be minimized at shorter flight times t.The net result is that larger amounts of α-hydroxyhydroperoxides will be detected (as Cl − adducts) at shorter t times, an effect that follows the same V 1/2 dependence and combines with that of the kinematics of microdroplets deflection.Additionally, this analysis shows that mass spectra preferentially reflect the composition of the lighter, more easily deflected microdroplets sheared from the outermost interfacial layers of the microdroplets.The larger inertia of the heavier microdroplets generated from the core of the microjets carries them forward to the bottom of the spraying chamber, and escape detection.In summary, in the configuration of our setup, an electric field must be applied to deflect the charged microdroplets towards the MP.The surface charges induced by these electric fields have a negligible effect on chemistry under the experimental conditions employed.Below, we summarize some experimental results on gas-liquid reactions involved in key environmental processes.Our studies deal with processes taking place in the outermost interfacial layers of aqueous solutions.Heterogeneous reactions on viscous liquids that cannot be nebulized [58][59][60], such as those of aged secondary organic aerosols, fall outside the scope of our technique.

Iodide Catalyzes Ozone Oxidations in Marine Aerosols
A few bromine atoms per trillion have been shown to trigger the fast destruction of ozone in the polar boundary layer in early spring [61].This phenomenon requires the pre-existence of a significant pool (≥10 pptv) of Br-containing gas-phase species (photo-Br) that can be rapidly photolyzed into Br-atoms at sunrise.Photo-Br must be produced from seawater Br − , the sole source of bromine in remote regions, by a dark process during polar winters.Our goal was to elucidate the mechanism of the thermal oxidation of marine Br − into photo-Br.The standing hypothesis at the time of our study was that photo-Br was the end-product of the short wavelength photolysis (above the stratospheric ozone layer) of long-lived Br-containing gases, such as biogenic methyl bromide of marine origin and anthropogenic halons.Models based on such an assumption, however, significantly underpredicted field measurements of the proxy BrO radicals [62].
Fine marine aerosol drops, which are highly enriched in Br − and I − ions relative to seawater [63], and remain suspended long enough to undergo significant chemical processing, are likely vehicles for producing photo-Br.We reasoned that the thermal, dark oxidizer had to be O 3 (g).However, the direct oxidation of Br − (aq) by O 3 (g) into Br 0 is a slow reaction: k(Br − +O 3 ) = 248 M −1 s −1 , in bulk water [64], A significant clue to the puzzle was the report that more Br 2 (g) is emitted from sea salt than from pure NaBr upon exposure to O 3 (g).It seemed that the oxidation of Br − ions by O 3 (g) was catalyzed by unidentified components of sea salt [65].
We performed experiments in which we exposed microjets of micromolar NaI, NaBr or NaI + NaBr solutions to O 3 (g).In the case of NaI, we detected the formation of iodate IO 3 − (m/z = 175) and triiodide I 3 − (m/z = 381) ions, in proportions that depended on solute and gas reactants concentrations.
NaBr solutions under the same conditions did not produce new mass spectral signals, as expected from the low reactivity of Br − (aq) ions towards O 3 (g).The ozonation of mixed (NaI + NaBr) solutions, in contrast, led to mass spectra displaying strong signals at m/z = 285 (I 79 Br 79 Br − ), 287 (I 79 Br 81 Br − ) and 289 (I 81 Br 81 Br − ).The presence of two bromines in these trihalide anions meant that at least one of them had to be Br 0 .In other words, in the presence of I − ions, Br − ions are rapidly oxidized by O 3 (g) at the air-water interface.We inferred that the (I − + O 3 ) reaction generates intermediates that oxidize Br − ions faster than molecular O 3 itself.We hypothesized that the intermediate could be hypoiodous acid HOI, from O-atom transfer to I − ions, or the trioxide I-OOO − , from O 3 addition.Unpublished results from experiments in our laboratory revealed that the latter was the case.A recent X-ray photoelectron spectroscopy study reported the formation of a related Br-OOO − intermediate [66].
Another key observation was that the depletion of I − (aq) on the surface of liquid microjets within τ ≤ 10 µs was faster than expected from the rate constant k(I − + O 3 ) = 1.2 × 10 9 M −1 s −1 in bulk water [64], and the (maximum) [O 3 (aq)] in equilibrium with the O 3 (g) partial pressures P O3(g) used in our experiments: [O 3 (aq)] = H P O3(g) (H = 1.2 × 10 −2 M atm −1 , is Henry's law constant for O 3 (g) in water at 298K) [67].The acceleration of reactions at the air-water interface, relative to similar reactions in bulk water, has proven to be a general phenomenon [68].This is the reason why it is questionable to interpret and "quantify" interfacial processes based on models parametrized with rate constants determined in bulk water.This is also the reason why, at this stage, our approach to interfacial chemistry is empirical, meaning that we focus on the physical implications of the experiments, and rely on semi-quantitative estimates.
A final consideration is that I − ions will outcompete Br − ions for O 3 (g) in marine aerosols, because even though I − ion concentrations are ~10 −3 times smaller than Br − ions [69], I − ions react with O 3 (g) 10 7 times faster [64].In summary, our experiments revealed that I − ions are the "unidentified component of sea salt" that catalyzes the oxidation of Br − ions by O 3 (g) on sea salt and marine aerosol drops.The iodide-catalyzed oxidation of Br − ions by O 3 (g) on the surface of marine aerosols naturally enriched in Br − and I − ions should be a major source of photo-Br in the Arctic boundary layer during the polar night.

The Disproportionation of Nitrogen Dioxide Catalyzed by Anions on Aqueous Aerosols Is the "Unknown Source of Atmospheric Nitrous Acid"
Modeling the production of the secondary organic aerosol (SOA) has become a major endeavor in tropospheric chemistry.This goal is approached via three-dimensional (3D) transport models that include gas/vapor emission strengths, gas-phase chemistry and aerosol microphysics.An implicit assumption common to most studies is that aerosols are a chemical dead end, i.e., once formed they cease to participate in tropospheric chemical cycles.Since "the key to understanding tropospheric chemistry begins with the OH radical" [70], a critical test for any model is how well it reproduces OH-radical concentrations under diverse conditions.Suggestively, one of the most important shortcomings of current atmospheric chemistry models is their failure to simulate how OH-radical concentrations respond to actinic flux and NOx level variations, and to systematically under-predict atmospheric nitrous acid (HONO) concentrations.Since the rapid λ ≤ 395 nm photolysis of gas-phase HONO produces OH-radicals with unitary quantum efficiency, Equation ( 6): HONO + hν(λ ≤ 395 nm) = NO + •OH (6) the noted shortcomings point to a mechanistic feature that couples OH-radical and HONO chemistries.
What is missing is a strong, yet unidentified, heterogeneous reaction that produces HONO from primary NO 2 (g) emissions at significant rates.This is the problem generally described as the "unknown source of HONO" [71,72].The consensus is that the mechanism of the "unknown source of HONO" will be revealed by more field measurements with improved instrumentation [72].
The implicit assumption is that the "unknown source of HONO" cannot be the reaction that could produce HONO from NO 2 (g) on aqueous surfaces, such as SOA surfaces in humid air, Equation ( 7): because NO 2 (g) is barely soluble in water (Henry's law constant = 0.01 M atm −1 ) [73], and its uptake coefficient on pure water, γ(NO 2 ) w < 1 × 10 −7 [74], is very small.This argument overlooks the fact that aqueous aerosols are not pure water, but contain significant concentrations of organic and inorganic electrolytes.Defying expectations and prevailing assumptions, we found that the uptake coefficient of NO 2 (g) on the surface of aqueous electrolytes: γ(NO 2 ) e = 10 −3 -10 −4 , is orders of magnitude larger than γ(NO 2 ) w .The underlying process is genuinely interfacial, because γ(NO 2 ) e is significantly enhanced by cationic surfactants, weakly depressed by anionic surfactants, and unaffected by hydrophobic 1-octanol [41,[75][76][77][78]. Significantly, the range of our estimated γ(NO 2 ) e values bracket the γ(NO 2 ) e ~10 −4 value measured on ∼3 mM NaCl droplets within a cloud chamber in the absence of electric fields [79,80].Our experiments in fact validate the larger γ(NO 2 ) e ~10 −4 value on electrolyte solutions vis-à-vis γ(NO 2 ) w < 1 × 10 −7 on pure water, a finding that remained unexplained and consequently ignored by the atmospheric chemistry community.In short, in the presence of dense SOA, such as those developing in midday urban smog, the hydrolytic disproportionation of NO 2 , Equation ( 7), may become competitive with the photolysis of NO 2 (g), Equation (8): thereby switching the source of OH-radicals from the photolysis of O 3 (produced from the ground-state O( 3 P) atoms generated the photolysis of NO 2 , Equation ( 8)) to the more direct and faster photolysis of HONO.We have shown that our findings may account for the dependences of NO 2 (g), HONO(g) and OH-radical concentrations as functions the J(NO 2 ) and J(HONO) actinic fluxes found in a comprehensive field study [81].An important corollary is that the existence of alternative photochemical sources of OH-radicals, i.e., HONO and O 3 photolyses, at rates controlled by the competition between NO 2 hydrolysis, Equation (7), and NO 2 photolysis, Equation (8), as a function of aerosol surface density, should buffer OH-radical concentrations [82].The buffering of OH-radical concentrations explains the similar values (τ D = 4 ± 1 h) of the decay lifetimes of NO 2 (g) in urban plumes retrieved from satellite sightings of megacities ranging from Singapore to Moscow at all seasons [82,83].This is an astonishing finding, because it is at odds with the textbook mechanism for the decay of NO 2 (g) into photochemically inert HNO 3 (g) via Equation (9).
The reason for this is that, since OH-radical concentrations "follow the sun" [84], i.e., they roughly scale with solar irradiance, τ D = (k 5 [OH]) −1 .Therefore, they should significantly increase in winter and at high latitudes.From the perspective gained by our results, a relatively constant τ D value is consistent with a combination of alternative NO 2 (g) decay processes.NO 2 (g) will decay in part via hydrolysis into NO 3 − , at rates that depend on aerosol surface area density, or into HNO 3 (g) at rates that scale with buffered OH-radical concentrations.In summary: our experiments showed that the surfaces of aqueous aerosols could be the substrates of key processes in tropospheric chemistry.Additionally, in all probability, the hydrolysis of NO 2 , Equation ( 7), is the "unknown source of HONO".It is unlikely that the "unknown source of HONO" could have been inferred from field campaigns, model parametrizations or theoretical calculations.

Chemistry on the Surface of the Human Lung Is Unusually Selective
The causality of the adverse effects of air pollution on human health is yet to be established.Numerous epidemiological studies have consistently found positive correlations of cardiovascular (CV) and all-cause (AC) premature mortalities with O 3 and PM 2.5 (particulates of <2.5 micrometer diameter) levels in ambient air [85].A recent statistical analysis of the most extensive air pollution data and age-specific CV and AC premature mortality rates for 483 counties in 15 US states from 2000 to 2010 confirmed such associations [86].However, in a key test of causality, the same study showed that the ∼30% decreases of PM 2.5 and O 3 levels achieved in that period due to the implementation of more stringent emission controls, did not translate into statistically significant changes in premature mortality rates.This is asignificant finding that begets the question of how stringent future regulations on air quality should be in order to achieve tangible improvements.It is apparent that socially optimal levels of control, i.e., those which balance marginal benefits versus the marginal costs of abatement, cannot be designed solely based on epidemiological data alone, but will require information on the detailed chemical and biological mechanisms of the adverse health effects induced by specific air pollutants.
Inhaled oxidants, such as O 3 (g) and NO 2 (g), do not reach the lung tissue, as is generally assumed, because they are scavenged by antioxidants contained in the epithelial fluids (ELFs) lining the respiratory tract.Evidence that adverse health effects do not simply involve local injury to the lung tissue is that inhalation of oxidants pollutants impairs the functions of both heart and lungs within hours.Mortality from acute cardiovascular syndromes markedly increases during episodes of high O 3 and PM 2.5 levels.This phenomenon strongly suggests a systemic response of the innate immune system to oxidative insult.
The major antioxidant in ELFs is reduced glutathione (GSH, 100−500 µM), an endogenous tripeptide (γ-L-glutamyl-L-cysteinyl-glycine) possessing a -SH thiol group.The conventional assumption was that the main function of GSH is to scavenge exogenous oxidants into innocuous "ox-GSH" species.The current notion, in contrast, is that GSH do deactivate oxidants; however, the [GSH]/["ox-GSH"] ratios generated in ELFs relay the intensity of oxidative stress to the immune system, thereby unleashing systemic responses [87][88][89].A nonspecific systemic immune response would be expected if all inhaled oxidants converted GSH to a common "ox-GSH" species.Given the exquisite selectivity of the immune system the issue is, of course, the identity of "ox-GSH" species.It has been long assumed without positive evidence that "ox-GSH" was the disulfide GSSG that would be produced from the recombination of the thiyl GS-radicals ensuing H-abstraction from S−H by OH-radicals.
Reduced glutathione GSH is a diacid that can exist as a mono-or di-anion, depending on the pH.We found that at physiological pH ~7.5, O 3 (g) rapidly oxidizes the dianion GS 2− (aq) (but not the monoanion GS − ) to a sulfonate GSO 3 − rather than to GSSG [90].Under the same conditions, the oxidation of cysteine (Cys), the S-containing residue in GSH, by O 3 (g) at the air−water interface yields Cys-sulfenic, Cys-sulfinic and Cys-sulfonic acids rather than CySSCy [91].In more recent experiments, we found that, in contrast with O 3 , OH-radicals can oxidize the monoanion GS − (aq).
The products are the sulfenic acid GSOH (a weak acid), sulfinate GSO 2 − and sulfonate GSO 3 − , from successive •OH additions to S-atoms, rather than to GSSG from GS-H abstraction [43].Additionally, we have shown that in the presence of pervasive transition metal ions such as Fe 2+ , O 3 (g) can oxidize the monoanion GS − to the same products, via the reactive intermediates generated in fast Fenton-type chemistry at the air−water interface [92].The relevance of our findings is highlighted by the increasing recognition of the biochemical role of sulfenic and sulfinic acids in regulating the activity of the immune system, such as the promotion of B-and T-cells [93][94][95].In hindsight, the reason for the belated awareness of the importance of sulfenic acids was the lack of suitable analytical techniques for their identification and quantitation at the low concentrations they reach in vivo.This fact underscores the power of our technique for identifying novel species down to submicromolar concentrations in complex mixtures.
From a purely chemical point of view, our experiments reveal the extraordinary specificity of •OH for attacking the S-atom of GSH on the surface of water versus its lack of selectivity in bulk water.Such specificity implies an unprecedented steering mechanism during [•OH-GSH] interfacial encounters at the air-water interface, which bypasses the fast, unselective H-abstractions (in bulk water) by •OH from S−H and the multiple C−H and N−H bonds of GSH.Significantly, our observations are in line with a previous theoretical study on radical recognition and steering mechanism, in which •OH is captured by GSH carboxylic groups and directed toward the reactive −SH group by a concerted process involving multiple H-bonded interactions within a flexible GSH framework [96].

Summary
The novelty and atmospheric relevance of the results obtained by online mass spectrometry underscore its unique advantages over spectroscopic techniques for studying chemistry on liquid surfaces in real time.Online mass spectrometry probes the surfaces of fresh, uncontaminated, fast flowing liquids.It is very sensitive, being able to routinely detect < 1 µM ionic species, i.e., at concentrations that are orders of magnitude lower those required by most spectroscopic techniques.Most importantly, mass spectrometry can unambiguously characterize species via their mass-to-charge ratios, thereby dispensing with spectroscopic fingerprints and spectral deconvolution analyses.At this stage of development, it provides semi-quantitative estimates of reactive uptake coefficients and rate constants for interfacial reactions.For all these reasons, online mass spectrometry seems ideally suited for investigating processes at gas-liquid interfaces.

Figure 1 .
Figure 1.A schematic representation of the electrospray source used in our experiments (See [12-16]

Figure 1 .
Figure1.A schematic representation of the electrospray source used in our experiments (See[12][13][14][15][16] for additional details).The spraying chamber is at atmospheric pressure and ambient temperature.MP is a metal plate polarized at ≤ 3.5 kV (relative to the grounded nebulizer) which has a pinhole inlet to the mass analyzer section of the mass spectrometer (not shown).