Next Article in Journal
Gathering Pipeline Methane Emissions in Utica Shale Using an Unmanned Aerial Vehicle and Ground-Based Mobile Sampling
Next Article in Special Issue
Evaluation of the SOA Formation in the Reaction of Furfural with Atmospheric Oxidants
Previous Article in Journal
Investigation of Aerosol Climatology, Optical Characteristics and Variability over Egypt Based on Satellite Observations and In-Situ Measurements
Previous Article in Special Issue
Kinetic Measurements of Cl Atom Reactions with C5–C8 Unsaturated Alcohols
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:

Gas-Phase Reaction of trans-2-Methyl-2-butenal with Cl: Kinetics, Gaseous Products, and SOA Formation

Instituto de Investigación en Combustión y Contaminación Atmosférica, Universidad de Castilla-La Mancha, Camino de Moledores s/n, 13071 Ciudad Real, Spain
Departamento de Química Física, Universidad de Castilla-La Mancha, Avda, Camilo José Cela 1B, 13071 Ciudad Real, Spain
Author to whom correspondence should be addressed.
Atmosphere 2020, 11(7), 715;
Received: 25 May 2020 / Revised: 1 July 2020 / Accepted: 2 July 2020 / Published: 5 July 2020


The gas-phase reaction between trans-2-methyl-2-butenal and chlorine (Cl) atoms has been studied in a simulation chamber at 298 ± 2 K and 760 ± 5 Torr of air under free-NOx conditions. The rate coefficient of this reaction was determined as k = (2.45 ± 0.32) × 10−10 cm3 molecule−1 s−1 by using a relative method and Fourier transform infrared spectroscopy. In addition to this technique, gas chromatography coupled to mass spectrometry and proton transfer time-of-flight mass spectrometry were used to detect and monitor the time evolution of the gas-phase reaction products. The major primary reaction product from the addition of Cl to the C-3 of trans-2-methyl-2-butenal was 3-chloro-2-butanone, with a molar yield (YProd) of (52.5 ± 7.3)%. Acetaldehyde (Y = (40.8 ± 0.6)%) and HCl were also identified, indicating that the H-abstraction by Cl from the aldehyde group is a reaction pathway as well. Secondary organic aerosol (SOA) formation was investigated by using a fast mobility particle sizer spectrometer. The SOA yield in the Cl + trans-2-methyl-2-butenal reaction is reported to be lower than 2.4%, thus its impact can be considered negligible. The atmospheric importance of the titled reaction is similar to the corresponding OH reaction in areas with high Cl concentration.

1. Introduction

Carbonyl compounds are volatile organic compounds (VOCs) emitted into the troposphere by several natural sources and by on-road traffic [1,2,3]. In addition, they can be generated through the oxidation of other VOCs present in the troposphere [4]. For example, unsaturated carbonyls, such as trans-2-methyl-2-butenal (E-CH3CH=C(CH3)C(O)H), are emitted into the lower atmosphere from vegetation and human activities such as road vehicles and industries, and methylbutenals have been proposed as oxidation products of isoprene initiated by hydroxyl (OH) radicals in the presence of NO [5,6]. Trans-2-methyl-2-butenal can also be found in food items such as herbs and spices, tomatoes, animal foods, and spearmint, and it is a building block in organic synthesis [7].
Recently, there have been multiple studies on the gas-phase reactivity of unsaturated oxygenated compounds with tropospheric oxidants such as OH radicals, nitrate (NO3) radicals, or ozone (O3), but kinetic data on the reaction initiated by chlorine (Cl) atoms are scarce [8]. Some examples are the results previously published on the Cl reactivity of linear unsaturated aldehydes [9,10], methacrolein [11], or 3-methyl-2-butenal [12]. The gas-phase kinetics of trans-2-methyl-2-butenal was experimentally studied with OH radicals and O3 [13,14] and an estimation was reported for the NO3 and OH reactions by using Structure–Reactivity and Linear Free-Energy Relationships [15]. In contrast, there is no investigation or estimation of the rate coefficient for the reaction of trans-2-methyl-2-butenal with Cl or the products that are generated in reaction (R1).
E-CH3CH = C(CH3)C(O)H + Cl → Products.
As aldehydes are known to be important contributors to the formation of secondary organic aerosols (SOA) [16,17], it is expected that SOA could be produced during the tropospheric oxidation of trans-2-methyl-2-butenal by Cl atoms. For the OH reaction, a SOA yield of 39.1% was determined by Chan et al. [18].
The aim of this research is, firstly, to determine the rate coefficient, k, of the gas-phase reaction (R1) at 298 ± 2 K and 760 ± 5 Torr under free-NOx conditions by using two atmospheric simulation chambers. In the kinetic study, a relative method has been employed, using Fourier transform infrared spectroscopy (FTIR) as quantification technique. Secondly, in a separate set of experiments, the gaseous products of reaction (R1) have been detected by three different techniques: FTIR, gas chromatography coupled to mass spectrometry (GC-MS), and proton transfer time-of-flight mass spectrometry (PTR-ToF-MS). The formation of SOA has been monitored as a function of the reaction time by a Fast Mobility Particle Sizer (FMPS) spectrometer. A reaction mechanism is proposed based on all the identified products. Finally, a discussion on the impact of reaction (R1) in coastal clean environments, where there are high Cl and low NOx concentrations is presented.

2. Experiments

The kinetic and product studies were performed in two atmospheric simulation chambers that were already described in previous studies [19,20]: a 16-L gas cell and a 264-L chamber. The 16-L gas cell is made of Pyrex and is a White-type cell with three mirrors inside and an optical path length of 96 m. The 264-L chamber is a cylindrical chamber made of Pyrex with stainless steel covers at the flat parts. Both chambers are surrounded by actinic lamps (Philips Actinic BL TL 40W/10 1SL/25, λ = 340–400 nm): four for the 16-L gas cell and eight for the 264-L chamber. These lamps were used to generate Cl atoms in situ by photolysis of Cl2. Gas-phase species were introduced from a gas-line with two capacitor pressure transducers (Leybold, model Ceravac, 10 and 1000 Torr full scale). Coupled to the chambers and depending on the experiment performed, specific instrumentation was used to monitor the time evolution of gaseous and particulate species. All the experiments were run by using synthetic air as bath gas at 760 ± 5 Torr and 298 ± 2 K.

2.1. Kinetic Study

For the kinetic experiments, mixtures of trans-2-methyl-2-butenal (T2M2B, henceforth), a reference compound (Ref, cyclohexane or isoprene), and Cl2 were introduced in the 16-L cell. Ranges of the initial concentrations in the cell were [T2M2B]0 = (3.4–7.1) × 1014 molecule cm−3, [cyclohexane]0 = (2.9–5.5) × 1014 molecule cm−3 or [isoprene]0 = (4.6–6.4) × 1014 molecule cm−3, and [Cl2]0 = (4.7–10.4) × 1014 molecule cm−3. In the performed experiments, T2M2B and the reference compound mainly react with Cl with rate coefficients k and kRef, respectively, although they can also be lost by heterogeneous reaction onto the walls, photoinduced processes, and/or reaction with the oxidant precursor. The additional loss is described by the first-order rate coefficients kloss and kRef,loss that were evaluated in preliminary experiments in which the decay of the compound was monitored without Cl precursor in dark conditions and with the lamps switched on, and in the presence of Cl2 in the dark, as described in previous studies [19,20]. Considering the overall losses for T2M2B and Ref, the integrated rate equation is described by the following equation:
l n ( [ T 2 M 2 B ] 0 [ T 2 M 2 B ] t ) - k loss t = k k Ref   [ l n ( [ Ref ] 0 [ Ref ] t ) - k Ref , loss t ] ,
where the subscript 0 indicates the initial concentrations of T2M2B and the reference compound and the subscript t indicates those concentrations at a reaction time t. These concentrations were monitored by a FTIR spectrometer (Thermo Fisher Scientific, model Nicolet Nexus 870, Madison, WI, USA) coupled to the 16-L cell that has a liquid N2-cooled MCT (Mercury Cadmium Telluride) detector. IR spectra were recorded between 650 and 4000 cm−1 at a resolution of 2 cm−1, after the accumulation of 32 interferograms, every 2 min. The IR bands selected for monitoring the loss of T2M2B and the reference compounds were 1710–2710 cm−1 for T2M2B, 2880 cm−1 for cyclohexane, and 860–950 cm−1 for isoprene.

2.2. Gaseous Products Study

For the determination of the gaseous products of reaction (R1), the two simulation chambers were used depending on the employed detection technique: FTIR spectroscopy, CG-MS, or PTR-ToF-MS.
When products were detected by FTIR spectroscopy, the 16-L cell and the same instrumentation used in the kinetic experiments described above were used again [19,20]. Experiments were run by irradiating the air mixture with T2M2B ((2.3–5.3) × 1014 molecule cm−3) and Cl2 ((6.0–7.7) × 1014 molecule cm−3) in the cell.
A GC-MS system (Thermo Electron, models Trace GC Ultra and DSQ II, Milan, Italy) and a PTR-ToF-MS (IONICON, model PTR-TOF 4000, Innsbruck, Austria) were coupled to the 264-L chamber, but in independent experiments. The GC-MS was equipped with a BPX35 column (30 m × 0.25 mm ID × 0.25 μm, SGE Analytical Science, Milton Keynes, UK) [19] working at a temperature ramp that ranged between 40 and 250 °C. The Solid-Phase Microextraction (SPME) was used as sampling technique with a 50/30 μm divinylbenzene/carboxen/polydimethylsiloxane (DVB/CAR/PDMS) fiber (Supelco) that was exposed to the gas mixture in the chamber during 5 min. In this case, the initial concentrations of T2M2B and Cl2 ranged between 5.4 and 8.6 × 1014 molecule cm−3 and between 5.1 and 8.4 × 1014 molecule cm−3, respectively.
The PTR-ToF-MS employs H3O+ as the primary ion in the proton transfer procedure. The mass spectra of the reactive gas mixture were recorded with a time resolution of 20 s and the detected mass range was set between 29 and 390.86 amu. The E/N factor of the instrument was set at 137 Td and products were quantified by using the transmission calibration of the instrument. Since this instrument is more sensitive than the FTIR spectrometer and the SPME/GC-MS system, to avoid saturation of the intensity, the initial concentration of T2M2B and Cl2 in the chamber was reduced with respect to that employed in the FTIR and GC-MS experiments: (1.9–2.1) × 1013 molecule cm−3 for T2M2B and (2.3–2.4) × 1013 molecule cm−3 for Cl2. In addition, to get intensity signals below the saturation limit, the gas sample had to be diluted with an air flow at the inlet of the PTR-ToF-MS by means of a dynamic inlet dilution system. A dilution factor of 1/5 was enough to not saturate the intensity signal. This dilution factor was achieved taking into account that the fixed flow going into the reaction chamber of the PTR-ToF-MS is 80 sccm (standard cubic centimeter per minute), and setting the additional inlet flow at 70 sccm, so the total flow going through the inlet was 150 sccm. Since the dilution flow was set at 120 sccm, only 30 sccm of the total 150 sccm going through the inlet were sampled from the 264-L chamber.
In all the experiments, the products of the reaction of T2M2B with Cl were monitored during 60 min, and tests were done to establish the products generated during the UV light exposure of T2M2B and by its reaction with Cl2 in the dark. The product yield of a product (YProd) was determined as the ratio of its concentration, [Prod], and the loss of reactant, Δ[T2M2B]:
Y Prod = [ Prod ] Δ [ T 2 M 2 B ] .

2.3. SOA Formation Study

As the quantification of SOAs formed in reaction (R1) requires the knowledge of the loss of T2M2B by reaction with Cl atoms, the experiments were performed simultaneously in the 16-L and 264-L chambers, which were connected by a Teflon tube. Thus, the FMPS spectrometer (TSI Incorporated, model 3091, Shoreview (MN), USA) sampled from the 264-L chamber and its outlet flow was brought to the 16-L cell. With this configuration, the gas mixture was continuously flowing through the two chambers, and data of the particles in the 5.6–560 nm range inside the chambers could be recorded by the FMPS every 1 s (although they were averaged for 1 min), and gaseous T2M2B could be monitored at the same time with the FTIR spectrometer every 2 min. The total timescale of the experiment was 80 min. In the first 10 min, the Cl2/T2M2B/air mixture was not irradiated (i.e., no Cl reaction was taking place) to monitor the dark losses of gaseous T2M2B or its reaction with Cl2. After that, the lamps were turned on and the Cl reaction started, monitoring T2M2B loss and particles during 60 min. To evaluate the loss of the formed SOAs by wall loss or through the filters of the FMPS, the lamps were switched off for 20 min more. At each reaction time, the concentration of T2M2B and the SOA mass were corrected by accounting for their loss as described in a previous research. [20] The SOA yield was determined as the ratio between the aerosol mass formed, MSOA, and the loss of reactant due to the Cl reaction, Δ[T2M2B]:
Y SOA = M SOA Δ [ T 2 M 2 B ] .

2.4. Chemicals

Gases: Synthetic air (Air Liquide, 99.999%) and Cl2 (Sigma Aldrich, 99.8%) were used as supplied. Liquids from Sigma Aldrich, with purities in brackets, were used after freeze-pump-thaw cycles: trans-2-methyl-2-butenal (96%), cyclohexane (99.9%), and isoprene (99%).

3. Results

This section includes the experimental results for the kinetic and product studies for reaction (R1), presenting the measurement of the Cl-rate coefficient, the identification of products both in the gas and particle phases, and the determination of the SOA yield.

3.1. Determination of the Rate Coefficient

In the preliminary experiments performed in the absence of UV light and/or in the absence of Cl2, different loss processes for T2M2B (kloss) and the two reference compounds (kref,loss) were investigated and considered in the kinetic data analysis. The pseudo-first order rate coefficient in this case is given by
kloss = kw + k + kCl2[Cl2].
Wall losses (kw) for T2M2B and the two reference compounds were observed, whereas UV photoinduced processes (k) were perceptible only for T2M2B, and the dark reaction with Cl2 (kCl2) was detected only for isoprene. kw, k, and kCl2 were quantified in each case and are summarized for the three compounds in Table 1. These losses contributed around 1–10% to the total decay of T2M2B and the reference compounds.
In Figure 1, the loss of T2M2B with respect to that for the reference compound is plotted for all the experiment series carried out with each reference compound. Plots of ln([T2M2B]0/[T2M2B]t)-klosst versus ln([Ref]0/[Ref]t)-kRef,losst show a good linearity, indicating that there were no kinetic complications. According to Equation (1), k/kRef was obtained from the slope of these plots. Then, the rate coefficient of reaction (R1), k, was determined at room temperature considering the rate coefficients of the reference compounds previously reported for the Cl reaction of cyclohexane and isoprene [21,22]. The individual rate coefficients k are summarized in Table 2 for the two reference compounds. The averaged value of k was determined to be (2.45 ± 0.32) × 10−10 cm3 molecule−1 s−1. The ±2σ uncertainty in k includes the propagation of the reported errors in kRef, the statistical errors from the slope of the plots shown in Figure 1, and the uncertainties in kloss.

3.2. Identification of the Reaction Products in the Gas-Phase

As mentioned in the previous section, complementary detection techniques were used to identify and/or quantify the products generated in reaction (R1): SPME/GC-MS, FTIR spectroscopy, and PTR-ToF-MS. Prior to that, tests were done to check if products were generated during the UV light exposure of T2M2B and its dark reaction with Cl2 In the experiments performed with SPME/GC-MS, no products were observed in these tests, whereas when PTR-ToF-MS and FTIR spectroscopy were used, it was possible to detect the formation of some products during the UV light exposure of T2M2B.

3.2.1. Detection by SPME/GC-MS

Figure 2a shows the chromatogram obtained after 60 min of irradiation. The peak corresponding to T2M2B was observed at a retention time (RT) of 4.62 min. The new peaks that appeared in the chromatogram can be assigned to a product according to the mass spectrum of each RT (in min), as shown in Figure 2b. The detected products were acetaldehyde (RT = 2.13), methylglyoxal (RT = 2.57), acetic acid (RT = 3.11), 2,3-butanedione (RT = 3.15), 3-chloro-2-butanone (RT = 4.38, most intense), and 2-methyl-2-butenoic acid (RT = 6.08). Other small peaks in the chromatogram were due to the degradation of the SPME fiber and the column.

3.2.2. Detection by PTR-ToF-MS

The PTR-ToF-MS detects protonated molecular ions for non-chlorinated organic compounds. All the reaction products observed by SPME/GC-MS, except 3-chloro-2-butanone, were also observed by PTR-ToF-MS: acetaldehyde (C2H4OH+, m/z = 45.03), acetic acid (C2H4O2H+, m/z = 61.02), methylglyoxal (C3H4O2H+, m/z = 73.02), 2,3-butanedione (C4H6O2H+, m/z = 87.05), and 2-methyl-2-butenoic acid (C5H8O2H+, m/z = 101.6). In addition, other products were observed such as formaldehyde (CH2OH+, m/z = 31.01), methanol (CH4OH+, m/z = 33.03), ketene (C2H2OH+, m/z = 43.01), propene (C3H6H+, m/z = 43.05), formic acid (CH2O2H+, m/z = 47.01), propanal (C3H6OH+, m/z = 59.08), butyric acid (C4H8O2H+, m/z = 89.05), and 2-butenal (C4H6OH+, m/z = 71.03). Given that molecular ions are detected, it is possible that an isomer of the mentioned products would be present. In Figure 3, it is observed that the major products detected by PTR-ToF-MS are acetaldehyde, ketene, and formaldehyde, with product yields of (40.8 ± 0.6)%, (23.5 ± 0.4)%, and (11.0 ± 0.2)%, respectively. For the minor reaction products, the yields were determined to be less than 5%. The three major products, acetaldehyde, ketene, and formaldehyde, were also formed during the exposure of T2M2B to the UV light in the test experiments performed prior the Cl reaction, but their amount was negligible compared with the observed concentration after the Cl reaction.

3.2.3. Detection by FTIR Spectroscopy

The FTIR spectra recorded during reaction (R1) showed features that agree with the products observed by SPME/GC-MS and PTR-ToF-MS as can be seen in Figure 4. By comparison with the reference spectra (shown in central panels of Figure 4), the most abundant products observed were HCl, CO, 3-chloro-2-butanone, and acetaldehyde. The obtained product yields were YHCl = (92.8 ± 12.9)%, YCO = (97.3 ± 10.0)%, and Y3-chloro-2-butanone = (52.5 ± 7.3)%. The quantification of acetaldehyde by FTIR spectroscopy was very imprecise due to the presence of other minor products that have similar features in the IR spectrum. The minor products that were identified are formaldehyde, acetyl chloride, methanol, methyl glyoxal, acetic acid, 2,3-butanedione, and butanone. After subtracting all these products and by comparison with the IR features described by Wallington et al. [23], ketene (CH2C(O)) was also identified in the 2100–2200 cm−1 range of the residual spectrum. No reference spectrum was available for ketene given its instability. Despite this identification, there are still some IR features that could be due to an unknown carbonyl compound or 2-methyl-2-butenoic acid. This acid was observed by SPME/GC-MS and PTR-ToF-MS, but no IR reference spectrum could be obtained due to experimental limitations. Nevertheless, given the amount detected by the two other techniques, it is expected that the concentration detected by FTIR will be very low too. During the exposure to UV light test of T2M2B, small amounts of CO, formaldehyde, and acetaldehyde were detected, but, similarly, as observed by PTR-ToF-MS, in a lesser extent than the observed during the Cl reaction.

3.3. SOA Formation Study

In Figure 5, the size distribution of particles is shown in terms of the normalized particle number, dN/dlogDp, and mass, dM/dlogDp. As depicted in Figure 5a, shortly after the beginning of the Cl reaction (at t = 2 min), the appearance of a high concentration (in terms of number) of ca. 20-nm particles was observed. At subsequent times, the diameter of the particles increased, being centered at ca. 100 nm at t = 60 min, while the number of particles decreased. Figure 5b shows that the maximum mass of the first formed particles was centered at a ca. 30 nm diameter, reaching a value of around 10 μg m−3. As Cl reaction continued, the maximum of the mass increased up to 200 μg m−3 and was centered at 130 nm. Both graphs indicate that the formation of a big number of small particles took place 2 min after Cl reaction started and this formation was due to a nucleation process. It was followed by the growth of the particles due to coagulation, which caused that the number of particles was reduced at longer times even though the mass kept increasing.
The SOA yield, YSOA, was determined under different conditions from the slope of the plot of MSOA versus Δ[T2M2B] (Figure 6). The correction of MSOA was done considering the rate coefficient for the loss of particles determined in each experiment (average value: kloss particle = 4.2 × 10−2 s−1). The rate coefficient for the dark loss of T2M2B was also determined at the beginning of each experiment and was used for correcting its concentration at each reaction time. This rate coefficient averaged kloss = 3.4 × 10−3 s−1. The results of YSOA are listed in Table 3 together with the conditions used in this research.
The gas/particle absorption model proposed by Pankow [26,27] can describe the mechanism of SOA formation accordingly to the relationship between YSOA and the maximum value of MSOA reached in every experiment [28]:
Y SOA = M SOA i n α i K p , i 1 + K p , i M SOA ,
where αi is the mass-based stoichiometric coefficient and Kp,i is the gas/particle partitioning coefficient of the i semi-volatile species formed. In this research, data could be fitted to a one-product model (i = 1), as can be seen in Figure 7, yielding α = (2.4 ± 0.2)%, and Kp = (2.7 ± 0.5) × 10−3 m3 μg−1. These parameters indicate, respectively, that YSOA tends towards 2.4% at very high MSOA values and that the semi-volatile product that causes the SOA formation is mostly in the vapor phase rather than in the condensed phase.

4. Discussion

4.1. Comparison of the Cl Reactivity with Unsaturated Aldehydes

As far as we know, the present research is the first kinetic study of the reaction Cl + T2M2B. The rate coefficient that has been determined in this study is within the same order of magnitude of the reported for other aldehydes as summarized in Table 4. The rate coefficients for the other aldehydes were determined by using a relative method in all cases, similarly to this research, with the techniques shown in Table 4.
Considering the available kinetic data for the Cl reaction with other unsaturated aldehydes, a structure–activity trend of the Cl reactivity can be derived. As shown in Table 4 and also reported by Rodríguez et al. [9], the rate coefficient seems to slightly increase with the hydrocarbon chain for the linear unsaturated aldehydes, E-CH3(CH2)xCH=CHC(O)H, when x = 5–7. This would indicate that the H-abstraction from the hydrocarbon chain is playing a role. However, the rate coefficient determined for a shorter unsaturated aldehyde, E-CH3CH=CHC(O)H, reported by Thévenet et al. [10], indicates that this trend may not be as clear and further studies would be needed. For branched unsaturated aldehydes with a central double bond, such as E-CH3CH=C(CH3)C(O)H and (CH3)2C=CHC(O)H, the Cl reactivity seems to increase, according to what has been reported by Rodríguez et al. [10], with respect to that of the linear unsaturated aldehyde E-CH3CH2CH=CHC(O)H, that has the same number of C and H atoms. This trend could indicate that the branching of the main chain by the electron donor methyl groups accelerates the reaction. However, the rate coefficient for E-CH3CH=CHC(O)H, reported by Thévenet et al. [10], is similar to the reported in this research for E-CH3CH=C(CH3)C(O)H, which would indicate that the presence of the methyl group has no effect on the reactivity. As stated above, further studies on the reactivity of the linear unsaturated aldehydes are needed to better establish the reactivity trend as a function of the structure. When looking at the length of the chain of branched unsaturated aldehydes, it seems to slightly reduce the Cl reactivity as observed when comparing the rate coefficients for T2M2B and methacrolein (CH2=C(CH3)C(O)H) [11]. It is also possible to compare the effect of the position of the methyl group in the reactivity by looking at the rate coefficients of 3-methyl-2-butenal, (CH3)2C=CHC(O)H, [12], and T2M2B. Both compounds have almost the same rate coefficient (considering the errors), indicating that the position of the methyl group does not affect the Cl reactivity in this case. Finally, the Cl-reactivity of saturated aldehydes was reported to be faster than that for unsaturated aldehydes [9]. There are no available data for the reaction of 2-methylbutanal with Cl to compare with trans-2-methyl-2-butenal, and thus the comparison can be done with pentanal, CH3(CH2)3C(O)H, which has the same amount of C atoms, showing a very similar rate coefficient ((2.56 ± 0.27) × 10−10 cm3 molecule−1 s−1, [9]).

4.2. Reaction Mechanism to Form Gaseous Products

The great variety of products detected by three complementary techniques allows to propose a reaction mechanism. What seems clear is that HCl, CO, 3-chloro-2-butanone, and acetaldehyde are the products for which the yields are higher. There are two reaction pathways, depicted in Figure 8 and Figure 9, that can explain the presence of these reaction products: the addition of Cl to the double bond in the C-3 position (Figure 8) and the H-abstraction from the aldehyde group (Figure 9). In both figures, the species in bold are the ones identified in this study.
The addition of Cl to C-3 of T2M2B can explain the formation of the observed products: 3-chloro-butanone, methylglyoxal, acetaldehyde, acetyl chloride, methanol, and formaldehyde. The initial step of this pathway leads to the formation of a chlorinated alkyl radical (CH3CH(Cl)C(CH3)C(O)H) that, following the general reactivity trend, reacts with O2 and a peroxy radical to generate the alkoxy radical CH3CH(Cl)CO(CH3)C(O)H. This alkoxy radical can react with O2, as described by Hasson et al. [29] for carbonyl containing peroxy radicals, to form 3-chloro-2-butanone, CH3CH(Cl)C(O)CH3, or it can decompose to generate methylglyoxal (CH3C(O)C(O)H)) and the CH2CHCl radical that continues to react with O2, RO2, and decompose to generate acetaldehyde (CH3C(O)H) and acetyl chloride (HC(O)Cl), and, through further reactions of the methyl radical, methanol (CH3OH) and formaldehyde (HC(O)H). However, the decomposition route of the CH3CH2Cl radical seems to be almost negligible, given the low yield of methyl glyoxal, (1.17 ± 0.08)%. The C-3 addition mechanism was expected, according to previous studies for unsaturated aldehydes [9], to be inhibited because of the conjugation between the double bond and the carbonyl group that reduces the partial negative charge on that carbon atom. However, the presence of the methyl group in this molecule seems to activate this channel, since one of the most abundant products observed, 3-chloro-2-butanone (CH3CH(Cl)C(O)CH3) can only be explained by this reaction pathway. The observed yield for this product indicates that this pathway represents around 53% of the overall reaction.
The H-abstraction from the -C(O)H group can explain the presence of acetaldehyde, HCl, CO, 2-methyl-2-butenoic acid, butanone, butadiene, and ketene. The first step leads to the formation of HCl, a major product, and a carbonyl radical that can decompose or react with O2 followed by the reaction with RO2 or HO2 radicals. The reaction with HO2 can generate the 2-methyl-2-butenoic acid, CH3CH=C(CH3)C(O)OH, one of the minor products of this reaction, the decomposition generates the CH3CH=CCH3 radical, and the RO2 reaction leads to the formation of the CH3CH=C(CH3)C(O)O radical that can decompose to generate CO2 and the unsaturated alkyl radical CH3CH=CCH3, as described in various previous studies for unsaturated aldehydes [30,31,32]. The CH3CH=CCH3 radical reacts with O2 to form acetaldehyde, CH3C(O)H, and the acetyl radical, CH3C(O), or the CH3CH=C(CH3)OO radical. The acetyl radical can react with Cl atoms and can generate HCl and ketene [33], another product observed at high concentration. The CH3CH=C(CH3)OO radical can react either with HO2 or RO2 radicals. The reaction with HO2 radicals explains the generation of butanone (CH3CH2C(O)CH3) through its corresponding enol. The RO2 reaction followed by the reaction with O2 generates an intermediate similar to what has been previously suggested by Magneron et al. [30] and which can decompose to form CO and acetaldehyde, or can isomerize to 2,3-butanedione (CH3C(O)C(O)CH3).
The addition of the Cl atom to C-2 was also considered as possible, since acetaldehyde, formaldehyde, and CO could also be generated through this pathway. However, the presence of other chlorinated products such as CH3CH(Cl)C(O)H or ClC(O)CH3, that would be generated if this mechanism was occurring, could not be confirmed with the analytical techniques used in this research, so this pathway seems to be negligible. Given that acetaldehyde is generated mostly by the H-abstraction pathway, its molar yield shows that around 40% of the overall reaction proceeds through this pathway, as depicted in Figure 9. Theoretical calculations on the relative importance of the reaction pathways of the first step of the mechanism could be useful to confirm the reaction pathways reported in this study.

4.3. SOA Formation Study

The SOA yields determined in this research for the Cl reaction of T2M2B range between 0.26% and 1.65% under NOx-free conditions. Under high NOx conditions and using ammonium sulfate as seed, Chan et al. reported a much higher SOA yield (39.1%) for the corresponding OH reaction [18]. The difference between the two studies may be due to the formation of less volatile products in the OH reaction than those obtained in the Cl reaction that contribute to the SOA formation. However, there are studies that show that SOA yields in the Cl reactions are comparable to the formed in other oxidation scenarios (OH or O3 reaction, photolysis, etc.), such as a study reported for some monoterpenes [34]. Therefore, the low values determined in this research compared to the OH reaction [18] can be attributed to the different conditions that were used and that may change the mechanism of SOA formation and affecting the SOA yield. First, the effect of NOx in YSOA seems to be very complex as there are multiple studies that show contradictory results, as summarized by Chan et al. [18], so it is hard to state clearly if the observed difference can be due to this factor. Secondly, the presence of ammonium sulfate seeds enhances YSOA [35] and would explain the difference observed between the OH reaction studied by Chan et al. [18] and the results presented in this study. Moreover, there are other factors that can affect the SOA yields, such as the temperature and the relative humidity. Temperature in this research was slightly higher than the temperature set by Chan et al. [18] (the difference is less than 10 K), and at higher temperatures the semi-volatile species are more present in the gas phase, but it is hard to know if this can explain the lower SOA yields observed in this study. Finally, the relative humidity in both studies is similar, since no additional H2O was added in any of them, so this factor should not be the source of the difference observed.

4.4. Atmospheric Implications

The tropospheric lifetime due to the Cl reaction of trans-2-methyl-2-butenal, τCl, was estimated as in previous studies [19,20] using the rate coefficient determined in this research and two different Cl atoms concentrations: a 24 h average (1 × 103 atom cm−3, [36]) and a peak concentration (1.3 × 105 atom cm−3, [37]). The reason for this is to evaluate the influence of this reaction in areas with low levels of Cl and other zones with high Cl concentration, such as coastal or industrial areas. In the first scenario, τCl,24h was estimated to be 46 days, while considering the peak concentration, τCl,peak was 8.7 h. The individual tropospheric lifetimes for the OH reaction and the O3 reaction of T2M2B were previously estimated as 6.8 h [13] and 3 days [14], respectively. Therefore, if the peak Cl scenario is considered, the tropospheric lifetime due to the three homogeneous reactions is 3.6 h. In this case the contribution of the Cl reaction to the T2M2B homogeneous loss is 42%, very similar to the OH radical contribution (53%). This indicates that, although the Cl reaction is faster than the OH reaction by one order of magnitude, the importance of this degradation route in the troposphere can be approximately the same. The upper limit of the tropospheric lifetime due to UV photolysis was estimated in a previous study as 0.7 h [38], thus, in the most favorable conditions for photolysis this would be the most important degradation route.
In terms of the contribution of the Cl + T2M2B reaction to the formation of secondary pollutants, 3-chloro-2-butanone and acetaldehyde can be formed with 52.5% and 40.8% yields, respectively, contributing to smog episodes in clean atmospheres where low NOX levels are present. Further photooxidation of these carbonyl compounds can also yield to other pollutants. The concentration levels of these species and, therefore, their atmospheric impact will depend on the emitted quantity of T2M2B. As far as we know, this compound has not been detected at high concentrations in the troposphere, so the impact of the generated products is expected not to be very important. The contribution of the SOA formed in the Cl + T2M2B reaction can be considered as negligible taking into account that the yield is YSOA < 2.4%, so its impact on the air quality is expected to be low. Finally, as HCl and CO are also formed with 92.8% and 97.3% yields, respectively, they can impact at a local or regional scale contributing to the acidity of the atmosphere [39] and the formation of the tropospheric ozone in a polluted environment, respectively.

5. Conclusions

In this research, we have reported for the first time the room temperature rate coefficient of the reaction between Cl and trans-2-methyl-2-butenal at 760 ± 5 Torr. Although this rate coefficient is quite high, with a similar value as the previously reported rate coefficients for other saturated and unsaturated aldehydes, the contribution of the Cl reaction to the homogeneous loss of T2M2B in the troposphere is less than 42%. This research also presents the first detailed product study for the titled reaction, using three complementary detection techniques. In summary, the main gaseous products identified were
  • Acetaldehyde, methylglyoxal, acetic acid, and 2,3-butanedione, detected by the three techniques;
  • 3-chloro-2-butanone, detected by SPME/GC-MS and FTIR;
  • Formaldehyde, methanol, and ketene, detected by PTR-ToF-MS and FTIR;
  • HCl, CO, and ClC(O)H, detected only by FTIR.
The major reaction products are HCl ((92.8 ± 12.9)%), CO ((97.3 ± 10.0)%), 3-chloro-2-butanone ((52.5 ± 7.3)%), and acetaldehyde ((40.8 ± 0.6)%), indicating that the Cl-addition to C-3 and the H-abstraction from the aldehyde group of T2M2B are the major reaction pathways with around 53% and 40% contribution, respectively. Formation of ultrafine particles (5.6–560 nm) was investigated for the first time and we concluded that the SOA yield is very low. In conclusion, the impact of the observed degradation products, especially secondary pollutants (HCl, CO, carbonyl compounds, and aerosols) on air quality or acid rain episodes is expected to be low at the expected mission levels of T2M2B.

Author Contributions

Conceptualization, M.A. (María Antiñolo) and E.J.; formal analysis, M.A. (María Asensio); funding acquisition, J.A. and E.J.; investigation, M.A. (María Antiñolo) and M.A. (María Asensio); methodology, M.A. (María Antiñolo) and E.J.; project administration, J.A. and E.J.; supervision, J.A. and E.J.; writing—original draft, M.A. (María Antiñolo); writing—review & editing, J.A. and E.J. All authors have read and agreed to the published version of the manuscript.


This research was funded by the University of Castilla-La Mancha (UCLM) through the project 2019-GRIN-27175 (Ayudas para la financiación de actividades de investigación dirigidas a grupos). Authors would like to thank the Spanish Ministry of Science, Innovation and Universities and the European Union for funding through the European Regional Development Fund project (FEDER, Ref. EQC2018-004157-P). M.A. (María Asensio) also acknowledges the NANOCOSMOS Synergy grant (SyG-610256) awarded by the European Research Council and M.A. (María Antiñolo) acknowledges UCLM Plan Propio de Investigación for funding their research contracts.

Conflicts of Interest

The authors declare no conflict of interest.


  1. Kawamura, K.; Steinberg, S.; Kaplan, I.R. Homologous series of C1–C10 monocarboxylic acids and C1–C6 carbonyls in Los Angeles air and motor vehicle exhausts. Atmos. Environ. 2000, 34, 4175–4191. [Google Scholar] [CrossRef]
  2. Grosjean, D.; Grosjean, E.; Gertler, A.W. On-Road Emissions of Carbonyls from Light-Duty and Heavy-Duty Vehicles. Environ. Sci. Technol. 2001, 35, 45–53. [Google Scholar] [CrossRef] [PubMed]
  3. Wildt, J.; Kobel, K.; Schuh-Thomas, G.; Heiden, A.C. Emissions of Oxygenated Volatile Organic Compounds from Plants Part II: Emissions of Saturated Aldehydes. J. Atmos. Chem. 2003, 45, 173–196. [Google Scholar] [CrossRef]
  4. Atkinson, R.; Arey, J. Atmospheric Degradation of Volatile Organic Compounds. Chem. Rev. 2003, 103, 4605–4638. [Google Scholar] [CrossRef]
  5. Yu, J.; Jeffries, H.E.; Le Lacheur, R.M. Identifying Airborne Carbonyl Compounds in Isoprene Atmospheric Photooxidation Products by Their PFBHA Oximes Using Gas Chromatography/Ion Trap Mass Spectrometry. Environ. Sci. Technol. 1995, 29, 1923–1932. [Google Scholar] [CrossRef]
  6. Park, J.; Jongsma, C.G.; Zhang, R.; North, S.W. Cyclization reactions in isoprene derived β-hydroxy radicals: Implications for the atmospheric oxidation mechanism. Phys. Chem. Chem. Phys. 2003, 5, 3638–3642. [Google Scholar] [CrossRef]
  7. Wishart, D.S.; Feunang, Y.D.; Marcu, A.; Guo, A.C.; Liang, K.; Vázquez-Fresno, R.; Sajed, T.; Johnson, D.; Li, C.; Karu, N.; et al. HMDB 4.0: The human metabolome database for 2018. Nucleic Acids Res. 2017, 46, D608–D617. [Google Scholar] [CrossRef]
  8. Jiménez, E.; Barnes, I. Daytime Atmospheric Chemistry of C4–C7 Saturated and Unsaturated Carbonyl Compounds. In Environment, Energy and Climate Change I: Environmental Chemistry of Pollutants and Wastes; Jiménez, E., Cabañas, B., Lefebvre, G., Eds.; Springer International Publishing: Berlin/Heidelberg, Germany, 2015; pp. 53–103. [Google Scholar]
  9. Rodríguez, D.; Rodríguez, A.; Notario, A.; Aranda, A.; Díaz-de-Mera, Y.; Martínez, E. Kinetic study of the gas-phase reaction of atomic chlorine with a series of aldehydes. Atmos. Chem. Phys. 2005, 5, 3433–3440. [Google Scholar] [CrossRef][Green Version]
  10. Thévenet, R.; Mellouki, A.; Le Bras, G. Kinetics of OH and Cl reactions with a series of aldehydes. Int. J. Chem. Kinet. 2000, 32, 676–685. [Google Scholar] [CrossRef]
  11. Wang, W.; Ezell, M.J.; Ezell, A.A.; Soskin, G.; Finlayson-Pitts, B.J. Rate constants for the reactions of chlorine atoms with a series of unsaturated aldehydes and ketones at 298 K: Structure and reactivity. Phys. Chem. Chem. Phys. 2002, 4, 1824–1831. [Google Scholar] [CrossRef][Green Version]
  12. Blanco, M.B.; Barnes, I.; Teruel, M.A. FTIR gas-phase kinetic study of the reactions of Cl atoms with (CH3)2CCHC(O)H and CH3CHCHC(O)OCH3. Chem. Phys. Lett. 2010, 488, 135–139. [Google Scholar] [CrossRef]
  13. Jiménez, E.; Lanza, B.; Antiñolo, M.; Albaladejo, J. Influence of temperature on the chemical removal of 3-methylbutanal, trans-2-methyl-2-butenal, and 3-methyl-2-butenal by OH radicals in the troposphere. Atmos. Environ. 2009, 43, 4043–4049. [Google Scholar] [CrossRef]
  14. Sato, K.; Klotz, B.; Taketsugu, T.; Takayanagi, T. Kinetic measurements for the reactions of ozone with crotonaldehyde and its methyl derivatives and calculations of transition-state theory. Phys. Chem. Chem. Phys. 2004, 6, 3969–3976. [Google Scholar] [CrossRef]
  15. Grosjean, D.; Williams, E.L. Environmental persistence of organic compounds estimated from structure-reactivity and linear free-energy relationships. Unsaturated aliphatics. Atmos. Environ. Part A Gen. Top. 1992, 26, 1395–1405. [Google Scholar] [CrossRef]
  16. Jang, M.; Czoschke, N.M.; Lee, S.; Kamens, R.M. Heterogeneous Atmospheric Aerosol Production by Acid-Catalyzed Particle-Phase Reactions. Science 2002, 298, 814. [Google Scholar] [CrossRef] [PubMed]
  17. Kroll, J.H.; Seinfeld, J.H. Chemistry of secondary organic aerosol: Formation and evolution of low-volatility organics in the atmosphere. Atmos. Environ. 2008, 42, 3593–3624. [Google Scholar] [CrossRef]
  18. Chan, A.W.H.; Chan, M.N.; Surratt, J.D.; Chhabra, P.S.; Loza, C.L.; Crounse, J.D.; Yee, L.D.; Flagan, R.C.; Wennberg, P.O.; Seinfeld, J.H. Role of aldehyde chemistry and NOx concentrations in secondary organic aerosol formation. Atmos. Chem. Phys. 2010, 10, 7169–7188. [Google Scholar] [CrossRef][Green Version]
  19. Ballesteros, B.; Jimenez, E.; Moreno, A.; Soto, A.; Antinolo, M.; Albaladejo, J. Atmospheric fate of hydrofluoroolefins, CxF2x+1CH=CH2 (x = 1,2,3,4 and 6): Kinetics with Cl atoms and products. Chemosphere 2017, 167, 330–343. [Google Scholar] [CrossRef]
  20. Antiñolo, M.; Olmo, R.D.; Bravo, I.; Albaladejo, J.; Jiménez, E. Tropospheric fate of allyl cyanide (CH2CHCH2CN): Kinetics, reaction products and secondary organic aerosol formation. Atmos. Environ. 2019, 219, 117041. [Google Scholar] [CrossRef]
  21. Aschmann, S.M.; Atkinson, R. Rate constants for the gas-phase reactions of alkanes with Cl atoms at 296 ± 2 K. Int. J. Chem. Kinet. 1995, 27, 613–622. [Google Scholar] [CrossRef]
  22. Orlando, J.J.; Tyndall, G.S.; Apel, E.C.; Riemer, D.D.; Paulson, S.E. Rate coefficients and mechanisms of the reaction of cl-atoms with a series of unsaturated hydrocarbons under atmospheric conditions. Int. J. Chem. Kinet. 2003, 35, 334–353. [Google Scholar] [CrossRef]
  23. Wallington, T.J.; Ball, J.C.; Straccia, A.M.; Hurley, M.D.; Kaiser, E.W.; Dill, M.; Schneider, W.F.; Bilde, M. Kinetics and mechanism of the reaction of Cl atoms with CH2 CO (Ketene). Int. J. Chem. Kinet. 1996, 28, 627–635. [Google Scholar] [CrossRef]
  24. Nielsen, O.J.; University of Copenhangen, København, Denmark. Personal communication, 2019.
  25. Eurochamp Data Center. 2017. Available online: (accessed on 1 June 2020).
  26. Pankow, J.F. An absorption model of gas/particle partitioning of organic compounds in the atmosphere. Atmos. Environ. 1994, 28, 185–188. [Google Scholar] [CrossRef]
  27. Pankow, J.F. An absorption model of the gas/aerosol partitioning involved in the formation of secondary organic aerosol. Atmos. Environ. 1994, 28, 189–193. [Google Scholar] [CrossRef]
  28. Odum, J.R.; Hoffmann, T.; Bowman, F.; Collins, D.; Flagan, R.C.; Seinfeld, J.H. Gas/particle partitioning and secondary organic aerosol yields. Environ. Sci. Technol. 1996, 30, 2580–2585. [Google Scholar] [CrossRef]
  29. Hasson, A.S.; Tyndall, G.S.; Orlando, J.J.; Singh, S.; Hernandez, S.Q.; Campbell, S.; Ibarra, Y. Branching Ratios for the Reaction of Selected Carbonyl-Containing Peroxy Radicals with Hydroperoxy Radicals. J. Phys. Chem. A 2012, 116, 6264–6281. [Google Scholar] [CrossRef]
  30. Magneron, I.; Thévenet, R.; Mellouki, A.; Le Bras, G.; Moortgat, G.K.; Wirtz, K. A Study of the Photolysis and OH-initiated Oxidation of Acrolein and trans-Crotonaldehyde. J. Phys. Chem. A 2002, 106, 2526–2537. [Google Scholar] [CrossRef]
  31. Orlando, J.J.; Tyndall, G.S. Mechanisms for the Reactions of OH with Two Unsaturated Aldehydes:  Crotonaldehyde and Acrolein. J. Phys. Chem. A 2002, 106, 12252–12259. [Google Scholar] [CrossRef]
  32. Tuazon, E.C.; Aschmann, S.M.; Nishino, N.; Arey, J.; Atkinson, R. Kinetics and products of the OH radical-initiated reaction of 3-methyl-2-butenal. Phys. Chem. Chem. Phys. 2005, 7, 2298–2304. [Google Scholar] [CrossRef]
  33. Maricq, M.M.; Ball, J.C.; Straccia, A.M.; Szente, J.J. A diode laser study of the Cl + CH3CO reaction. Int. J. Chem. Kinet. 1997, 29, 421–429. [Google Scholar] [CrossRef]
  34. Cai, X.; Griffin, R.J. Secondary aerosol formation from the oxidation of biogenic hydrocarbons by chlorine atoms. J. Geophys. Res. Atmos. 2006, 111. [Google Scholar] [CrossRef][Green Version]
  35. Chu, B.; Jiang, J.; Lu, Z.; Wang, K.; Li, J.; Hao, J. Effects of Inorganic Seeds on Secondary Organic Aerosol (SOA) Formation. In Atmospheric Aerosols—Regional Characteristics—Chemistry and Physics; Abdul-Razzak, H., Ed.; IntechOpen: London, UK, 2012. [Google Scholar]
  36. Singh, H.B.; Thakur, A.N.; Chen, Y.E.; Kanakidou, M. Tetrachloroethylene as an indicator of low Cl atom concentrations in the troposphere. Geophys. Res. Lett. 1996, 23, 1529–1532. [Google Scholar] [CrossRef]
  37. Spicer, C.W.; Chapman, E.G.; Finlayson-Pitts, B.J.; Plastridge, R.A.; Hubbe, J.M.; Fast, J.D.; Berkowitz, C.M. Unexpectedly high concentrations of molecular chlorine in coastal air. Nature 1998, 394, 353–356. [Google Scholar] [CrossRef]
  38. Lanza, B.; Jiménez, E.; Ballesteros, B.; Albaladejo, J. Absorption cross section determination of biogenic C5-aldehydes in the actinic region. Chem. Phys. Lett. 2008, 454, 184–189. [Google Scholar] [CrossRef]
  39. Sanhueza, E. Hydrochloric acid from chlorocarbons: A significant global source of background rain acidity. Tellus B Chem. Phys. Meteorol. 2001, 53, 122–132. [Google Scholar] [CrossRef]
Figure 1. Plot of Equation (1) for the two references used in this research.
Figure 1. Plot of Equation (1) for the two references used in this research.
Atmosphere 11 00715 g001
Figure 2. (a) Chromatogram obtained after 60 min of the chlorine (Cl) reaction of trans-2-methyl-2-butenal (T2M2B). (b) Mass spectra of the most intense peaks of the chromatogram that were attributed to products.
Figure 2. (a) Chromatogram obtained after 60 min of the chlorine (Cl) reaction of trans-2-methyl-2-butenal (T2M2B). (b) Mass spectra of the most intense peaks of the chromatogram that were attributed to products.
Atmosphere 11 00715 g002
Figure 3. Time evolution of the concentration of T2M2B (C5H8OH+, on the right axis) and the products measured by proton transfer time-of-flight mass spectrometry (PTR-ToF-MS) during the trans-2-methyl-2-butenal + Cl reaction. t = 0 min, depicted with a yellow dashed line, was set as the moment in which the reaction started when the lamps were turned on.
Figure 3. Time evolution of the concentration of T2M2B (C5H8OH+, on the right axis) and the products measured by proton transfer time-of-flight mass spectrometry (PTR-ToF-MS) during the trans-2-methyl-2-butenal + Cl reaction. t = 0 min, depicted with a yellow dashed line, was set as the moment in which the reaction started when the lamps were turned on.
Atmosphere 11 00715 g003
Figure 4. FTIR spectra. Top panel shows the spectrum obtained after 40 min of Cl reaction of trans-2-methyl-2-butenal with the features of this compound subtracted. The bottom panel shows the residual spectrum after the subtraction of the IR features corresponding to the detected products. HC(O)Cl spectrum was provided by Nielsen [24] and the CH3C(O)C(O)H spectrum was taken from the FTIR database of the EUROCHAMP project [25].
Figure 4. FTIR spectra. Top panel shows the spectrum obtained after 40 min of Cl reaction of trans-2-methyl-2-butenal with the features of this compound subtracted. The bottom panel shows the residual spectrum after the subtraction of the IR features corresponding to the detected products. HC(O)Cl spectrum was provided by Nielsen [24] and the CH3C(O)C(O)H spectrum was taken from the FTIR database of the EUROCHAMP project [25].
Atmosphere 11 00715 g004
Figure 5. Evolution of the size of the secondary organic aerosol (SOA) generated in the Cl reaction of T2M2B in terms of the normalized particle number (a) and mass (b). Reaction starts at t = 0 min and ends at t = 60 min.
Figure 5. Evolution of the size of the secondary organic aerosol (SOA) generated in the Cl reaction of T2M2B in terms of the normalized particle number (a) and mass (b). Reaction starts at t = 0 min and ends at t = 60 min.
Atmosphere 11 00715 g005
Figure 6. Some examples of the plots of SOA mass (MSOA) versus Δ[T2M2B] used to determine the SOA yield (YSOA).
Figure 6. Some examples of the plots of SOA mass (MSOA) versus Δ[T2M2B] used to determine the SOA yield (YSOA).
Atmosphere 11 00715 g006
Figure 7. SOA yield curve determined in this research for the trans-2-methyl-2-butenal reaction with Cl.
Figure 7. SOA yield curve determined in this research for the trans-2-methyl-2-butenal reaction with Cl.
Atmosphere 11 00715 g007
Figure 8. Proposed mechanism for the Cl reaction of trans-2-methyl-2-butenal through for the Cl-addition to C-3.
Figure 8. Proposed mechanism for the Cl reaction of trans-2-methyl-2-butenal through for the Cl-addition to C-3.
Atmosphere 11 00715 g008
Figure 9. Proposed mechanism for the Cl reaction of trans-2-methyl-2-butenal through the initial H-abstraction from the aldehyde group.
Figure 9. Proposed mechanism for the Cl reaction of trans-2-methyl-2-butenal through the initial H-abstraction from the aldehyde group.
Atmosphere 11 00715 g009
Table 1. Rate coefficients for the different loss processes observed for the compounds used in the kinetic study. Errors are ±2σ.
Table 1. Rate coefficients for the different loss processes observed for the compounds used in the kinetic study. Errors are ±2σ.
Compoundkw/10−6 s−1k/10−4 s−1kCl2/10−20 cm3 molecule−1 s−1
Trans-2-methyl-2-butenal8.40 ± 5.338.33 ± 5.60-
Cyclohexane0.400 ± 0.417--
Isoprene3.78 ± 1.65-2.70 ± 0.15
Table 2. Results obtained in the kinetic experiments for reaction (R1). Errors are ±2σ.
Table 2. Results obtained in the kinetic experiments for reaction (R1). Errors are ±2σ.
Referencek/kRefkRef/10−10 cm3 molecule−1 s−1k/10−10 cm3 molecule−1 s−1
Cyclohexane0.894 ± 0.0303.08 ± 0.12 12.75 ± 0.14
Isoprene0.491 ± 0.0144.35 ± 0.58 22.14 ± 0.29
Average 2.45 ± 0.32
1 Aschmann and Atkinson [21]. 2 Orlando et al. [22].
Table 3. Results of YSOA under different conditions. Errors are ±2σ.
Table 3. Results of YSOA under different conditions. Errors are ±2σ.
[T2M2B]0/1014 molecule cm−3[Cl2]0/1014 molecule cm−3MSOA/μg m−3YSOA (%)
5.624.4627.40.26 ± 0.01
6.792.5452.90.27 ± 0.01
5.992.6760.90.33 ± 0.01
7.175.961910.68 ± 0.01
6.316.932440.96 ± 0.01
7.799.534411.42 ± 0.03
7.5812.64911.49 ± 0.04
7.3915.05801.44 ± 0.02
6.7417.07641.56 ± 0.03
7.1019.98631.65 ± 0.03
Table 4. Summary of the Cl-rate coefficients of selected unsaturated aldehydes at 298 K.
Table 4. Summary of the Cl-rate coefficients of selected unsaturated aldehydes at 298 K.
Unsaturated Aldehydek/10−10 cm3 molecule−1 s−1TechniqueReference
LinearE-CH3CH=CHC(O)H2.60 ± 0.04GC-FID[10]
E-CH3CH2CH=CHC(O)H1.31 ± 0.19GC-MS[9]
E-CH3(CH2)2CH=CHC(O)H1.92 ± 0.22GC-MS[9]
E-CH3(CH2)3CH=CHC(O)H2.40 ± 0.29GC-MS[9]
BranchedE-CH3CH=C(CH3)C(O)H2.45 ± 0.32FTIRThis research
(CH3)2C=CHC(O)H2.48 ± 0.71FTIR[12]
CH2=C(CH3)C(O)H2.9 ± 0.8FTIR and GC-FID[11]

Share and Cite

MDPI and ACS Style

Antiñolo, M.; Asensio, M.; Albaladejo, J.; Jiménez, E. Gas-Phase Reaction of trans-2-Methyl-2-butenal with Cl: Kinetics, Gaseous Products, and SOA Formation. Atmosphere 2020, 11, 715.

AMA Style

Antiñolo M, Asensio M, Albaladejo J, Jiménez E. Gas-Phase Reaction of trans-2-Methyl-2-butenal with Cl: Kinetics, Gaseous Products, and SOA Formation. Atmosphere. 2020; 11(7):715.

Chicago/Turabian Style

Antiñolo, María, María Asensio, José Albaladejo, and Elena Jiménez. 2020. "Gas-Phase Reaction of trans-2-Methyl-2-butenal with Cl: Kinetics, Gaseous Products, and SOA Formation" Atmosphere 11, no. 7: 715.

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop