Front. Environ. Chem. Frontiers in Environmental Chemistry Front. Environ. Chem. 2673-4486 Frontiers Media S.A. 732219 10.3389/fenvc.2021.732219 Environmental Chemistry Original Research In-Situ FTIR Study of Heterogeneous Oxidation of SOA Tracers by Ozone Wang et al. Heterogeneous Oxidation of Tracer Wang Runhua Huang Yajuan Hu Qian Cao Gang * Zhu Rongshu Shenzhen Key Laboratory of Organic Pollution Prevention and Control, Harbin Institute of Technology (Shenzhen), Shenzhen, China

Edited by: Fudong Liu, University of Central Florida, United States

Reviewed by: Giovanni Cagnetta, Tsinghua University, China

Biwu Chu, Research Center for Eco-Environmental Sciences (CAS), China

Tu Binh Minh, VNU University of Science, Vietnam

 *Correspondence: Gang Cao, caogang@hit.edu.cn

This article was submitted to Organic Pollutants, a section of the journal Frontiers in Environmental Chemistry

 29 10 2021 2021 2 732219 28 06 2021 14 10 2021 Copyright © 2021 Wang, Huang, Hu, Cao and Zhu. 2021 Wang, Huang, Hu, Cao and Zhu

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Secondary organic aerosols (SOA) play an important role in global climate change and air quality, and SOA tracers can directly characterize the source and reaction mechanism of SOA. However, it is not well known that whether the tracers can be oxidized or how the instability of the tracers in the atmosphere. In this paper, in-situ FTIR was used to analyze the chemical structure changes of erythritol, analogue of 2-methyl erythritol (AME) that is, a tracer of isoprene SOA, and 2, 3-dihydroxy-4-oxopentanoic acid (DHOPA), a tracer of toluene SOA, when exposed to high concentration of ozone for short periods. Under the condition of 20 ppm ozone exposure for 30 min, the change rate of absorption area of AME at 3,480 and 1700 cm−1 was −0.0134 and 0.00117 int.abs/s, respectively, and the change rate of the absorption area of DHOPA at 1,640 and 3340cm−1 was −0.00191 and 0.00218 int.abs/s, respectively. The pseudo-first-order reaction rate constant k app were 1.89 × 10−8 and 2.12 × 10−7 s−1, and the uptake coefficients of ozone on the surface of AME and DHOPA were (1.3 ± 0.8) × 10−8 and (4.5 ± 2.7) × 10−8, respectively. These results showed the oxidation processes of AME and DHOPA were slow in the presence of high concentrations of ozone, which implied that AME and DHOPA could be considered to be stable in the atmospheric environment with ozone as the main oxidant.

 SOA tracers in-situ FTIR ozone uptake coefficient pseudo-first-order reaction 2 Foundation for Innovative Research Groups of the National Natural Science Foundation of China10.13039/501100012659 Introduction

Organic tracers have been used widely for source apportionment of organic aerosols under the assumption that they are not reactive in the atmosphere (Katrib et al., 2005; Kleindienst et al., 2007; Ding et al., 2012; Lai et al., 2014). However, previous studies have indicated that some of those tracers may not remain stable, which leads to the inaccurate estimation of source contributions (And and Smith, 2004; Weitkamp et al., 2008a; Hoffmann et al., 2010; Lambe et al., 2012; Wang et al., 2020). Weitkamp et al. studied the ozone oxidation of primary organic tracers of cooking oil emission (oleic acid, palmitoleic acid, and cholesterol etc.) through a series of chamber experiments. The results showed that the rate constant of ozone heterogeneous oxidation of oleic acid was 1.5 × 10−11 cm3 molec−1 sec−1, which was ten times of cholesterol and four times of palmitoleic acid (Weitkamp et al., 2008b). Lambe et al. studied the effective reaction rate of oxidation reaction of norhopane, an organic tracer of motor oil by hydroxyl radical, and the rate constant of norhopane was 8.4 × 10−12 cm3 molec−1 s−1 (Lambe et al., 2009). The study of Hennigan et al. indicated that rate constant of levoglucosan was 1.1 × 10−11 cm3 molecule−1s−1 when biomass burning particles were exposed to 1 × 106 molecules cm−3 of OH (Hennigan et al., 2010).

The above studies were focused on the heterogeneous oxidation of primary organic tracers, while such investigations on the secondary organic tracers have seldom been reported. And there is no clear conclusion about the complexity of heterogeneous oxidation of secondary tracers. Kessler et al. used the erythritol as a surrogate for 2-methyltetrols and studied heterogeneous oxidation of pure erythritol particles by gas-phase OH radicals with an effective OH uptake coefficient, γ eff, of 0.77 ± 0.1 and a corresponding chemical lifetime of ∼13.8 ± 1.4 days at a relative humidity (RH) of 30 % (Kessler et al., 2010). However, Xu et al. investigated the heterogeneous OH oxidation of pure erythritol aerosols that contained erythritol and ammonium sulfate (AS) at different dry inorganic-to-organic mass ratios (IOR) in an aerosol flow tube reactor at a high relative humidity of 85 %. Their kinetic data would suggest that 2-methyltetrols in atmospheric particles were likely chemically stable against heterogeneous OH oxidation under humid conditions (Xu et al., 2020).

The laboratory studies on atmospheric heterogeneous oxidation reactions, using Knudsen cell (Seisel et al., 2006; Zhou and Wang, 2014), flow tube reactor (Lelièvre et al., 2004; Kessler et al., 2010), FTIR (Zeng et al., 2013; He et al., 2016), smog chamber (Lee et al., 2004; Hartz et al., 2007; Weitkamp et al., 2007; Ge et al., 2016), have developed rapidly in the determination of kinetic constants of trace gases and adsorption reactions on particle surfaces (Lee and Harris, 2006; Goldstein et al., 2008; Nieto et al., 2008; He and Zhang, 2019). In recent years, in-situ FTIR technology has been widely used in heterogeneous oxidation studies of various compounds by monitoring functional group transformation as reactions progressed (Zeng et al., 2013; He et al., 2016; Gao et al., 2019). The evolution of the FTIR absorption peak with time is generally used to estimate the uptake coefficient, which refers to the fraction of gaseous oxidants irreversibly reacted in the surface of compounds after collision (Hudson et al., 2001; Smith et al., 2002; Hung et al., 2005). It is an important physicochemical parameter to characterize the heterogeneous reaction in the atmosphere, and an important quantitative index for the surface uptake ability of atmospheric particles (Moise and Rudich, 2002; Thornberry and Abbatt, 2004; Ziemann, 2005; Hung and Tang, 2010). The heterogeneous reaction rate between gaseous oxides and the condensed compounds can be calculated based on a pseudo-first-order rate equation with the corresponding uptake coefficient (Worsnop et al., 2002). Gao et al. studied the heterogeneous reactions of ozone with oleic acid via a flow system combined with ATR-FTIR, and reported the uptake coefficient γ of ozone on oleic acid was (4.6 ± 1.0) × 10−4 (Gao et al., 2019). The uptake coefficients of ozone on oleic acid in previous studies ranged from (7.8 ± 2) × 10−3 to (1.9 ± 0.6) × 10−5 (Hartz et al., 2007; Hearn and Smith, 2004; Nash et al., 2006; Smith et al., 2002; Rosen et al., 2008).

In this paper, in order to study the ozone heterogeneous oxidations of Erythritol, Analogue of 2-Methyl Erythritol (AME) and 2, 3-Dihydroxy-4-oxopentanoic Acid (DHOPA) which are secondary organic tracers of the largest natural source of non-methane hydrocarbons (isoprene) and the representative precursor of anthropogenic SOA (toluene) respectively, an in-situ FTIR was used to analyze the chemical structure changes of AME and DHOPA, when exposed to high concentrations of ozone for short periods. The uptake coefficients of ozone on the surface of AME and DHOPA were measured and the pseudo-first-order reaction rate constant of AME and DHOPA were estimated.

 Materials and Methods Materials and Instruments

All chemicals used for this study had purity levels greater than 99%. -AME was supplied by Aladdin, and DHOPA was supplied by TRC. Ozone was generated photolytically using a Xonics ozone generator (Jelight Model 600, Irvine, CA) and the ozone concentration was measured with a photometric ozone detector (2BTechnologies Model 106L). The experiment was carried out at room temperature, in that low constant temperature water baths (DHC-0505-A, qiwei), which controlled the temperature of ambient chamber at 25°C. Analyses of heterogeneous oxidation of the AME and DHOPA were carried out in an in-situ FTIR (Is-50FT-IR, Thermo). The in-situ FTIR was composed of a reaction chamber and a Harrick Praying Mantis. The reaction chamber consisted of an ambient chamber and a dome which equipped with two round KBr observation windows. The external facilities of the Harrick Praying Mantis included observation windows, purge door and purge line fitting, as well as two tilted mirrors and four horizontal mirrors in the Praying Mantis.

Figure 1 showed the experimental setup for measuring the uptake coefficients of ozone on the surface of AME or DHOPA solid powder using in-situ FTIR. The general procedures of the experiments were briefly outlined below: Firstly, a transmittance spectrum with the Praying Mantis in the sample compartment was collected when the wavenumber at 2,500 cm−1 reached the maximum value. Then, dry air was blown for 5 min, and the background was collected. Finally, 1 mg AME/DHOPA solid powders were spread out evenly at the bottom of the sample cup of the ambient chamber, and 20 ppm ozone was injected for 30 min continuously. The characteristic infrared absorption peaks of surface of solid powder during the process of the ozone oxidation of AME or DHOPA were monitored online under the FTIR operational conditions of the infrared resolution of 4 cm−1, the background scanning of 64 times, the series sample scanning of 32 times, the sample interval of 41.27 s, and the scanning range of 4,000–400 cm−1. After each experiment completed, the residual ozone in the ambient chamber was removed by blowing dry air through the outlet.

in-situ FTIR experimental setup.

 Calculation of Uptake Coefficient

The method used to measure the uptake coefficients in this work was similar to that used in previous studies on ozone oxidations of oleic acid and linoleic acid (Jaoui et al., 2004; Hung et al., 2005; Engelke et al., 2010). Zeng et al. studied the heterogeneous reaction of linoleic acid with ozone. It was confirmed that the rate constant of linoleic acid oxidation was in accordance with the pseudo-first-order reaction rate constant. When the sample was exposed to 250 ppb ozone concentration at 30% RH, k app was 5.98 × 10−4 s−1 and the uptake coefficient was 5.79 × 10−4 (Zeng et al., 2013).

In our experiments, the molar ratio of ozone to AME or DHOPA remained at more than three orders of magnitude. Under such pseudo-first order reaction, the second-order reaction of ozone (as A in Eq. 1) and AME or DHOPA (as B in Eq. 1) can be considered as the pseudo-first-order reaction, the rate constant for which can be calculated by Eq. 2 (Gao et al., 2019). A+B → P d [ B ] d t = k app [ B ]  when  k a p p [ B ] = k [ A ] [ B ]

k a p p ——Pseudo-first-order rate constant (s−1);

k——Second order rate constant (cm3·molecule−1·s−1);

 The uptake coefficient γ was calculated using the change rate of the integral area of characteristic absorption peaks at specific wavelengths of AME or DHOPA based on Eq. 3 (Worsnop et al., 2002; Gao et al., 2019). d [ C i a ] d t = - γ ( N A P O 3 c ¯ 4 R T ) S A V

[ C i a ]—— the initial concentration of i (molecules·cm−3);

d [ C i a ] dt —— the rate of molecular change of i (molecules·cm−3·s−1);

c ¯ —— average rate of ozone in the gas phase (cm·s−1);

NA—— Avogadro’s number (6.02 × 1023 molecules·mol−1);

P O 3 —— atmospheric pressure of ozone (Pa = kg·m−1·s−2);

R—— gas constant or proportionality constant (8.314 J mol−1 K−1);

T—— temperature (K);

S A V —— the specific surface area of i (cm−1).

In this study, the surface area of the reaction chamber (20 cm−1) was assumed as the specific surface area for collision. However, the collision area corresponds to the sample preparation methods and affects the uptake coefficient. In order to distinguish the changes of FTIR absorption peaks during the process of the oxidation reactions, enough amounts of samples was used, resulting in the formation of pores within the solid powder for ozone to permeate. As a result, our experiments measured the upper bounds of the uptake coefficients of AME and DHOPA.

 Results and Discussion Ozone Oxidation of AME

Figure 2 showed the infrared spectrum of AME at a room temperature of 25°C and 30% RH.

Infrared spectrum of AME at room temperature.

To resolve the broad O–H stretching band of carboxyl groups that was superimposed on the peaks of interest between 3,700 and 2,500 cm−1, the six superimposed peaks were separated by 8.5 origin Gaussian fitting, including the stretching bands of -OH at 3,180 cm−1 and 3,480 cm−1, -CH2 antisymmetric stretching at 2,910 cm−1, -CH stretching at 2,823 cm−1, -CH2 symmetric stretching at 2,718 cm−1, and -CH stretching at 2,663 cm−1, as shown in Figure 3 (Injae et al., 1998; Luo et al., 2003; Branca et al., 2016). The detailed assignment of spectral bands for AME was summarized in Table 1.

Gaussian fitting results of AME in the 3,700–2500cm−1 region.

IR frequencies and assignments for functional groups in AME.

Wavenumber (cm−1) Band assignment
3259 -OH stretching
2910 -CH2 antisymmetric stretching
2823 -CH stretching
2718 -CH2 symmetric stretching
2663 -CH Stretching
2348 Carbonyl (C=O)
2122 Carbonyl (C=O)
1970 Carbonyl (C=O)
1414 Deformation of C-O-H
1366 Deformation of C-O-H
1305 -OH in-plane
1255 -OH in-plane
1217 C-C Stretching
1055 C-O Stretching
968 Deformation of C-H
884 Deformation of C-H

The heterogeneous oxidation of ozone on AME was carried out in a reaction chamber of FTIR under the same ambient conditions. The FTIR spectra of the AME were recorded as a function of time. Figure 4A showed that the area of the absorption peak at wavenumber 3480 cm−1 (-OH stretching) decreased with time when exposed to ozone. In addition, a small absorption peak at 1700 cm−1 appeared and the area of this peak increased with time, as shown in Figure 4B. It was likely the infrared absorption caused by the C=O stretching of the reaction product. Changes in AME absorption peaks at 3,480 cm−1 and at 1700 cm−1 during the experiments indicated that–OH at the end chain of AME was oxidized to C=O bond by ozone. Based on the changes in the absorption peak area at 3,480 and 1700 cm−1, the change rates of peak areas were calculated as −0.00134 int. abs/s and 0.00117 int. abs/s, respectively.

Changes of the AME absorption peak at 3,480 and 1700 cm−1 in the course of reactions. (A) 3,480 cm−1 (B) 1700 cm−1.

 Ozone Oxidation of DHOPA

The infrared spectrum of DHOPA at a room temperature of 25°C and 30% relative humidity was presented in Figure 5. To resolve the broad O–H stretching band of alcohol OH and carboxylic acid -OH that were superimposed on the peaks of interest between 4,000 and 3,000 cm−1, as well as the peaks between 1800 and 1,600 cm−1, 8.5 origin Gaussian fitting was used for peak separation. The resolved peaks, included the stretching bands of -OH at 3,540 and 3,340 cm−1, C=O of carboxylic acid (COOH) and of ketone at 1730 and 1,640 cm−1 respectively as shown in Figure 6. A comprehensive interpretation of FTIR spectra was tabulated in Table 2, which summarized the detailed assignment of spectral bands for DHOPA.

Infrared absorption spectrum of DHOPA at room temperature.

Gaussian fitting results of DHOPA in the 4,000–3,000 and 1800–1,600 cm−1 region.

IR frequencies and assignments for functional groups in DHOPA.

Wavenumber (cm−1) Band assignment
3430 -OH Stretching
2930 -CH3 antisymmetric stretching
2342 Carbonyl (C=O)
1730 Carboxylic acid (COOH)
1640 Carbonyl (C=O)
1371 -CH3 symmetric stretching
1255 -OH in-plane
1133 C-C Stretching
1090 C-O Stretching
973 Deformation of C-H
884 C-H Deformation

The heterogeneous oxidations of DHOPA and ozone were carried out in a reaction chamber of FTIR. The FTIR spectra of the DHOPA were monitored with time as the reactions processed. The results showed that the area of the absorption peak at wavenumber 1640 cm−1 (C=O stretching) decreased with time when exposed to ozone, as shown in Figure 7A. Furthermore, the appearance of a small absorption peak at 3,340 cm−1 and the increase of this peak area with time were observed, as shown in Figure 7B. It was likely the infrared absorption caused by the O–H stretching of the reaction products. Changes in DHOPA absorption peaks at 1,640 cm−1 and at 3,340 cm−1 during the experiments indicated that C=O of DHOPA was oxidized to CO–OH by ozone. Because COOH is more stable than C=O, the most reasonable product is 2, 3, 4-trihydroxyvaleric acid. Based on the evolution in the absorption peak area at 1,640 and 3,340 cm−1 with time, the change rates of peak areas were calculated as −0.00191 int.abs/s and 0.00218 int.abs/s, respectively.

Changes of the DHOPA absorption peak at 1,640 and 3,340 cm−1 in the course of reactions. (A) 1,640 cm−1 (B) 3,340 cm−1.

 Determination of Uptake Coefficient and Reaction Rate

Figure 8 showed the standard curve of the number of AME molecules vs. the characteristic absorption peak area of AME at 3,480 cm−1. The equation was y = 6.95 × 1016 x = 2.57 × 1019 with the correlation coefficient of 0.9805. Figure 9 showed the standard curve of the number of DHOPA molecules vs. the characteristic absorption peak area of DHOPA at 1,640 cm−1. The equation was y = 4.51 × 1016 x = 5.33 × 1018, and the correlation coefficient was 0.9783.

Standard curve of number of AME molecules vs. absorption peak area at 3,480 cm−1.

Standard curve of number of DHOPA molecules vs. absorption peak area at 1,640 cm−1.

Based on the change rate of the absorption peak area (−0.00134 int.abs/s at 3,480 cm−1) obtained in Ozone Oxidation of AME, the calculated change rate of number of AME molecules was −9.313 × 1013 molecules·s−1 according to the standard curve shown in Figure 8. In the same way, with the change rate of DHOPA peak area at 1,640 cm−1 (−0.00191 int.abs/s), the calculated change rate of number of DHOPA molecules was −8.614 × 1013 molecules·s−1. Under the pseudo-first order reaction of this study, the uptake coefficients γ and the pseudo-first-order reaction rate constants k app could be calculated using the change rates of the absorption peak areas at 3,480 cm−1 of AME and 1,640 cm−1 of DHOPA based on Eqs 2, 3, using the surface area of the reaction chamber of 20 cm−1 as the specific surface area for collision, the concentration of ozone of 20 ppm and the average rate of ozone of 115 ml/min. The pseudo-first-order reaction rate constant k app were 1.89 × 10−8 s−1 and 2.12 × 10−7 s−1, and the uptake coefficients of ozone on the surface of AME and DHOPA were (1.3 ± 0.8) × 10−8 and (4.5 ± 2.7) × 10−8, respectively.

This experiment is the first time to study the uptake coefficient of AME and DHOPA, so we find the data of ozone heterogeneous oxidation of some other organic substances for comparison. Table 3 summarized the uptake coefficients of ozone on the surface of organic compounds reported in the literature and obtained in this study. It clearly showed that the uptake coefficients of ozone on AME and DHOPA were quite different from other organic compounds, which were 2-5 orders of magnitude lower than those of oleic acid, linoleic acid, and cholesterol, as well as no significant correlation with ozone concentration.

Uptake coefficients of ozone on surface of organic matters.

Reactants concentration (O3) Uptake coefficient (γ) Reference
AME 20 ppm (1.3 ± 0.8) × 10−8 This work
DHOPA 20 ppm (4.5 ± 2.7) × 10−8 This work
Oleic acid 200 ppb (5 ± 3) × 10−4 Hartz et al. (2007)
Oleic acid 90 ppm (7.5 ± 1.2) × 10−4 Hearn and Smith (2004)
Linoleic acid 90 ppm (1.1 ± 0.2) × 10−3 Hearn and Smith (2004)
Cholesterol 200 ppb 5 × 10−4 Hartz et al. (2007)
Cholesterol 2 ppm (2.8 ± 0.4) × 10−6 Dreyfus et al. (2005)
Fatty acid 200 ppb (2.08 ± 0.04) × 10−5 Hartz et al. (2007)
Adipic acid 200 ppb (1.67 ± 0.08) × 10−5 Hartz et al. (2007)
Oleyl alcohol 90 ppm 7.5 × 10−4 Hearn and Smith (2004)
Caprylic acid 200 ppb (1.08 ± 0.07) × 10−5 Hartz et al. (2007)
Conclusion

In this study, in-situ FTIR was utilized to study the heterogeneous oxidations of two secondary organic tracers (AME and DHOPA) by ozone. Under the condition of 20 ppm ozone exposure for 30 min, the heterogeneous oxidations of AME and DHOPA by ozone were carried out in a reaction chamber of FTIR at a room temperature of 25°C and 30% relative humidity. The results showed that the AME absorption peak area at 3,480 cm−1 (-OH stretching) decreased while a small absorption peak area increased at 1700 cm−1 during ozone passing over the AME solid powder. Such changes indicated that–OH, at the end chain of AME, was oxidized to C=O bond by ozone. For DHOPA, the absorption peak area at 1,640 cm−1 (Carbonyl C=O stretching) decreased while a small absorption peak area increased at 3,340 cm−1 during the ozone oxidation. It was likely the infrared absorption caused by the O–H stretching of the reaction products. Based on the changes in the absorption peak area at 3,480 and 1700 cm−1 of AME, as well as the changes at 1,640 and 3,340 cm−1 of DHOPA, the change rates of peak areas were calculated as -0.00134 and 0.00117 int.abs/s for AME, as well as −0.00191 and 0.00218 int.abs/s for DHOPA, respectively. The pseudo-first-order reaction rate constant k app were 1.89 × 10−8 s−1 and 2.12 × 10−7 s−1, and the uptake coefficients of ozone on the surface of AME and DHOPA were (1.3 ± 0.8) × 10−8 and (4.5 ± 2.7) × 10−8, respectively.

The oxidation rates of AME and DHOPA were found to be relatively slow compared with those of the primary organic tracers reported in previous literature, even exposed to relative high ozone concentrations. It indicates that AME and DHOPA could be reactive, but the oxidation processes would be so slow that the changes of AME and DHOPA due to ozone oxidation are negligible. Therefore, under the atmospheric conditions with ozone as the main oxidant, AME and DHOPA, the secondary organic tracers of isoprene and toluene respectively, can be considered the source contribution estimated on the basis of the tracer methods are reliable. In this paper, the heterogeneous oxidation of secondary organic tracers in ozone environment was discussed. The heterogeneous oxidation of organic tracers by different oxidants needs to be studied more comprehensively in the future.

 Data Availability Statement

The original contributions presented in the study are included in the article/Supplementary Material, further inquiries can be directed to the corresponding author.

 Author Contributions

RW Participate in experiments and write this paper YH Participate in experiments QH Participate in experiments GC Support and guide experiments RZ Guide experiments.

 Funding

This study was financially supported by the National Natural Science Foundation of China (21876036) and the Fund for the Research and Development of Science and Technology in Shenzhen (JCYJ20150625142543472, ZDSYS201603301417588).

 Conflict of Interest

The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.

 Publisher’s Note

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