The 11 selected high-purity (≥96 %) sulfur-VOCs liquid standards (Sigma-Aldrich and Macklin) are listed in Table S1. These liquid standards were then used to generate individual sulfur-VOC standard gases with our laboratory partial-pressure gas mixing system (Li et al., 2025; Wang et al., 2020). The experimental setup is shown in Fig. S1 in the Supplement. A 0.53 m³ polytetrafluoroethylene (PTFE) chamber was employed to conduct atmospheric oxidation experiments of sulfur-VOCs with ⚫OH. The experimental conditions including the initial mixing ratios of sulfur-VOCs, O₃ concentration, and relative humidity (RH), are summarized in Table 1. These experiments were used for product identification and yield estimates for multi-sulfur products. OH radicals were generated by photolysis of O₃ under humid conditions using a 253 nm ultraviolet lamp (Philips TUV 16 W).

During these experiments, the evolution of 11 sulfur-VOCs was monitored by a Vocus-PTR-LToF-MS, and their oxidation intermediates and products (e.g., sulfur-containing peroxy radicals, gaseous H₂SO₄ and multi-sulfur products) were detected using a nitrate-CI-LToF-MS (Ehn et al., 2014; Krechmer et al., 2018). The Vocus-PTR-LToF-MS detects sulfur-VOCs mainly through proton-transfer reactions between reagent ions (i.e., hydronium ions (H₃O⁺) and their water-cluster ions (H₂O)₂₋₃⚫H⁺) and sulfur-VOCs with proton affinities higher than that of water. The nitrate-CI-LToF-MS employs nitrate reagent ions, including NO3-, HNO₃⚫NO3-, and (HNO₃)₂⚫NO3-, to detect sulfuric acid and highly oxygenated organic oxidation products mainly through nitrate-adduct cluster formation. Additionally, a more detailed description of instrument operation, mass calibration, and calibration procedures is provided in Sect. S1. The estimation of wall and dilution loss of sulfur-VOCs in our chamber was described in Sect. S3. The procedure used to quantify sulfur-containing oxygenated organic molecules (sulfur-OOMs) was described in Sect. S5. In addition, an ozone monitor (Thermo, 49i) and a temperature and humidity sensor (Vaisala HMP110) were used to record O₃ concentration and monitor environmental conditions in the chamber. Because the chamber is not collapsible, a make-up flow of high-purity zero air at 15 L min⁻¹ generated from a zero air generator (AADCO 737 series) was continuously introduced to the chamber and an RH of 20 %–25 % was maintained.

Relative-rate experiments were conducted for selected representative sulfur-VOCs to obtain their ⚫OH reaction rate constants. Isoprene was used as the reference compound because its ⚫OH reaction rate constant at room temperature is well established and k (isoprene + ⚫OH) was taken as 10.00×10-11 cm³ molec.⁻¹ s⁻¹ at 298 K (Iida et al., 2002; Medeiros et al., 2018). In these experiments, each selected sulfur-VOC was introduced simultaneously with isoprene into the chamber at 298±2 K and 1 atm and their temporal decays were monitored by Vocus-PTR-LToF-MS. The concentrations of sulfur-VOCs and isoprene were corrected for dilution and wall loss before relative-rate analysis. Each relative-rate experiment was conducted in triplicate. Details of the relative-rate calculation, wall/dilution loss correction, and uncertainty estimation are provided in Sect. S2.

Freshwater samples with algae were collected from Taihu Lake (approximately 2338.1 km²), China, which is the third-largest freshwater lake in China (Qin et al., 2019; Wang et al., 2023c), at the Taihu Lake Ecosystem Research Station (Fig. S2a). In recent years, frequent large-scale algal blooms have occurred in Taihu Lake due to anthropogenic nutrient inputs and endogenous pollutant releases in summer (Wang et al., 2019; Xu et al., 2021). Therefore, the water samples with algae taken from Taihu Lake were treated as representative samples of freshwater algae. Approximately 10 L of algae-containing lake water was collected using a clean 12 L polyethylene terephthalate (PET) drinking-water bottle. The sample was promptly transported to the laboratory and kept in the laboratory at approximately 21 °C for approximately 2 d before the chamber experiment. No filtration or other turbidity-removal treatment was applied before use.

During the emission characterization process, water samples were divided into 12 petri dishes (with a total exposed liquid surface area of 0.213 m²) and placed in the chamber. The chamber containing the water samples was then flushed with zero air at a flow rate of 15 L min⁻¹ for 2 h. After the flushing was completed, no additional gas was introduced, and the water samples were kept under static conditions in the chamber for 18 h at approximately 21 °C to allow the release of VOCs (Fig. S2b). After this static period, the VOCs released from the water samples were measured by Vocus-PTR-LToF-MS for approximately 30 min before O₃ was introduced into the chamber. After that, approximately 90 ppb of O₃ was injected into the chamber and two 253 nm UV lamps were turned on to generate ⚫OH by photolysis of O₃ under humid conditions (Fig. S3). A Vocus-PTR-LToF-MS, which was calibrated using selected sulfur-VOC standards (Sect. S4), was employed to measure and identify sulfur-VOCs and other VOC species released from freshwater algae, as well as their low-oxygenated oxidation products, while a nitrate-CI-LToF-MS was used to identify the mono-sulfur and multi-sulfur products derived from the reactions of sulfur-VOCs from the algal source with ⚫OH. A filtration control experiment was also performed to examine whether the detected sulfur-VOCs were associated with algae. The sample was filtered using three stacked layers of ordinary qualitative laboratory filter paper, and the filtration procedure was repeated three times to enhance the removal of visible algal particles. Further details of the filtration control experiment are provided in Sect. S7.

The ⚫OH reaction rate constants were reported in Table 2 and determined from relative-rate experiments. The selected sulfur-VOCs covered representative functional groups, including monothiol, dithiol, acyclic sulfide, cyclic sulfide, and disulfide. Representative relative-rate plots are shown in Fig. 1. The linear relationships between the loss-corrected logarithmic depletion of sulfur-VOCs and that of isoprene indicate that the relative-rate method provides stable constraints on the ⚫OH reaction rate constants under the present experimental conditions. The rate constants obtained in this work span more than one order of magnitude, ranging from (0.83±0.08) ×10-11 cm³ molec.⁻¹ s⁻¹ for DMS to (26.99±1.04) ×10-11 cm³ molec.⁻¹ s⁻¹ for trimethylene sulfide at 298±2 K.

For species with available literature data, the relative-rate-derived values agree well with previous values. For ethanethiol, the rate constant obtained in this work is 4.51±0.32×10-11 cm³ molec.⁻¹ s⁻¹, which is consistent with previously reported values of 3.89±0.57 to 4.50±0.50×10-11 cm³ molec.⁻¹ s⁻¹ near room temperature (Barnes et al., 1986; Wang et al., 2008; Wine et al., 1984). For DMS, the rate constant obtained in this work is 0.83±0.08×10-11 cm³ molec.⁻¹ s⁻¹, also consistent with that from previous studies. For DMDS (CH₃S₂CH₃), the relative-rate-derived value obtained in this work is 20.18±1.53×10-11 cm³ molec.⁻¹ s⁻¹, which agrees well with previously reported values of 19.80±1.80 to 23.90±3.00×10-11 cm³ molec.⁻¹ s⁻¹ at 297–298 K (Abbatt et al., 1992; Cox and Sheppard, 1980; Wine et al., 1981). These agreements support the reliability of our relative-rate method and the obtained kinetic dataset.

The relative-rate results further show that ⚫OH reactivity depends strongly on molecular structures of sulfur-VOCs (Fig. 2), but not in a simple monotonic way with either sulfur atom number or cyclic structure. The dithiol 1,2-ethanedithiol (HS(CH₂)₂SH) exhibits a relatively high rate constant of 14.36±0.26×10-11 cm³ molec.⁻¹ s⁻¹, consistent with the high reactivity of S-H functional groups toward ⚫OH. For thiols, previous kinetic and theoretical studies have shown that H-abstraction from the S-H group is an important and efficient initiation reaction pathway with ⚫OH, leading to the formation of sulfur-centered radicals (Atkinson and Arey, 2003; Cruz-Torres and Galano, 2007; Douroudgari et al., 2020; Mai et al., 2020). The presence of S-H groups therefore provides reactive H-abstraction sites and can enhance overall ⚫OH reactivity, which is also consistent with previous experimental rate-constant measurements for aliphatic thiols (Barnes et al., 1986; Wang et al., 2008; Wine et al., 1984). However, the comparison among sulfur-VOCs also indicates that the number of sulfur atoms alone does not determine the rate constants. For example, bis(methylthio)methane (CH₃SCH₂SCH₃) contains two sulfur atoms but shows a moderate rate constant of 3.50±0.09×10-11 cm³ molec.⁻¹ s⁻¹, behaving kinetically more like an acyclic sulfide than a highly reactive dithiol or disulfide.

The two cyclic sulfides investigated show contrasting reactivities. Trimethylene sulfide (C₃H₆S) exhibits the highest rate constant (26.99±1.04×10-11 cm³ molec.⁻¹ s⁻¹) among the selected sulfur-VOCs. This high reactivity is likely associated with its strained three-membered ring structure, which may facilitate ⚫OH-initiated reaction pathways. In contrast, 1,3-dithiolane (C₃H₆S₂) shows a lower rate constant of 0.95±0.05×10-11 cm³ molec.⁻¹ s⁻¹. This contrast indicates that cyclic structure alone does not necessarily lead to enhanced ⚫OH reactivity, and ring strain, sulfur functionality, and specific molecular configuration need to be considered together.

Acyclic and cyclic sulfides can react with ⚫OH through both H-abstraction from α-C-H bonds and ⚫OH-addition to the sulfur atom. Previous studies have shown that the ⚫OH-addition pathway can become more competitive under lower-temperature conditions (Barnes et al., 2006; Ye et al., 2022). Because the rate constants reported here are derived from overall precursor decay, the observed values represent the combined contribution of possible initiation pathways, and the relative branching between H-abstraction and ⚫OH-addition cannot be directly separated in the present experiments. Overall, the kinetic results demonstrate that the ⚫OH reaction rate constants of sulfur-VOCs depend on molecular features, such as reactive S-H groups, sulfur functionality, α-C-H sites and ring strain.

During our chamber experiments, many multi-sulfur products which contain 2 sulfur atoms in their chemical formulas were detected by nitrate-CI-LToF-MS (Table S3). The formation pathways of multi-sulfur products from ⚫OH-initiated oxidation of 11 selected sulfur-VOCs under NO_x-free conditions were investigated. The 11 sulfur-VOCs examined here comprise 5 thiols (CH₃CH₂SH, CH₃(CH₂)₂SH, (CH₃)₂CHSH, HS(CH₂)₂SH, HS(CH₂)₃SH), 3 acyclic sulfides (CH₃SCH₃, CH₃CH₂SCH₃, CH₃SCH₂SCH₃), 2 cyclic sulfides (C₃H₆S, C₃H₆S₂) and 1 disulfide (CH₃S₂CH₃). Among them, to exhibit the formation pathways of multi-sulfur products, DMS and HS(CH₂)₃SH are adopted as representative compounds for acyclic sulfides and thiols, respectively, whereas DMDS is treated as a representative compound for disulfide.

The reactions between DMS and ⚫OH primarily proceed via two competing pathways (Scheme 1). One is that ⚫OH adds to sulfur atom to form CH₃S⚫(OH)CH₃. Another is that ⚫OH abstracts H-atom from the methyl group to generate the CH₃SCH₂⚫. These primary radicals subsequently react with O₂ to form a series of sulfur-containing RO₂⚫, including the initially formed DMS-derived RO₂⚫ (e.g., CH₃SCH₂OO⚫), as well as other sulfur-containing RO₂⚫ intermediates (Berndt et al., 2023; Goss and Kroll, 2024; Shen et al., 2022). Notably, under NO_x-free conditions, sulfur-containing RO₂⚫ are not efficiently removed by NO, and their subsequent fate is expected to involve competition among unimolecular isomerization via H-migration, and bimolecular reactions of RO₂⚫ + HO₂⚫ and RO₂⚫ + R'O₂⚫ (Jenkin et al., 2003; Orlando and Tyndall, 2012). Recent studies of DMS oxidation have shown that H-shift isomerization of CH₃SCH₂OO⚫ can be an important pathway associated with hydroperoxymethyl thioformate (HPMTF) formation (Berndt et al., 2019; Jernigan et al., 2022; Ye et al., 2022). In the box-model analysis of DMS oxidation by ⚫OH, this H-shift process was included to evaluate its competition with bimolecular reactions of RO₂⚫ (Sect. S6; Fig. S7). The model results indicate that H-shift dominates the initial fate of CH₃SCH₂OO⚫ under the present chamber conditions. However, based on the detection by nitrate-CI-LToF-MS, various multi-sulfur bimolecular products (e.g., C₂H₆O₄S₂ and C₂H₆O₅S₂) resulting from RO₂⚫-R'O₂⚫ reactions were still identified (Fig. S5). Among these, C₂H₆O₄S₂ may originate from the bimolecular reaction of CH₃SOO⚫ with CH₃S(O)₂OO⚫ or the self-polymerization of CH₃S(O)OO⚫, while C₂H₆O₅S₂ may be formed by the bimolecular reaction between CH₃S(O)₂OO⚫ and CH₃S(O)OO⚫ (Scheme 1).

Previous studies on the ⚫OH-initiated oxidation of DMS have extensively investigated the formation and fate of sulfur-RO₂⚫, and have highlighted the potential importance of RO₂⚫-R'O₂⚫ reactions, particularly under low-NO_x or NO_x-free conditions (Barnes et al., 2006; Ye et al., 2022). However, direct molecular-level identification of multi-sulfur products has been very limited in earlier studies. Most previous investigations mainly focused on major oxidation products such as C₂H₆OS (dimethyl sulfoxide), C₂H₆O₂S (dimethyl sulfone), CH₄SO₃, and SO₂, rather than explicit characterization of individual bimolecular products from RO₂⚫-R'O₂⚫ chemistry (Chen et al., 2023; Hatakeyama et al., 1982). Self- and cross-reactions of RO₂⚫ are known to produce organic peroxides (ROOR') and multimeric products, and such pathways have been experimentally confirmed for a variety of alkyl peroxy radicals (Cho et al., 2023; Nozière, 2025; Orlando and Tyndall, 2012). In addition, studies on highly oxygenated organic molecules (HOMs) formation from biogenic VOC oxidation have demonstrated that RO₂⚫-R'O₂⚫ reactions can lead to complex, multifunctional products that are efficiently detected using nitrate-CIMS (Bianchi et al., 2019; Ehn et al., 2014; Gao et al., 2023). Nevertheless, there have been no previous reports explicitly identifying molecular formulas such as C₂H₆O₄S₂ and C₂H₆O₅S₂ as products of RO₂⚫-R'O₂⚫ reactions in the atmospheric oxidation of sulfur-VOCs. The formation of these multi-sulfur products can likely be favored by low-NO_x and NO_x-free experimental conditions, which can prolong the lifetime of sulfur-containing RO₂⚫ and favor their bimolecular reactions.

As shown in Scheme S1, the ⚫OH-initiated oxidation of DMDS follows a reaction framework similar to that of sulfides. Cleavage of the S-S bond leads to the formation of sulfur-centered radical intermediates which are analogous to those generated from acyclic sulfides. Among the multi-sulfur products detected from the ⚫OH-initiated oxidation of DMDS, C₂H₆O₄S₂ was identified under the present experimental conditions, and its formation is also derived from RO₂⚫-R'O₂⚫ bimolecular reactions inferred for the DMS oxidation system.

For thiols, the reactions between HS(CH₂)₃SH and ⚫OH are initiated predominantly by H- abstraction from the S-H group (Scheme 2), forming the sulfur-centered radical (HS(CH₂)₃S⚫) (Berndt et al., 2023; Douroudgari et al., 2020; Mai et al., 2020). Subsequent reactions lead to the formation of a few sulfur-containing RO₂⚫ intermediates, including HS(CH₂)₃OO⚫, HOO(CH₂)₃SOO⚫, and HOO(CH₂)₃S(O)₂OO⚫. Compared to RO₂⚫ derived from acyclic sulfides and disulfides, thiol-derived RO₂⚫ are more structurally diverse, enabling more bimolecular reaction pathways. As a result, more multi-sulfur products were identified (Fig. S9), including C₆H₁₄O₈S₂, C₆H₁₄O₉S₂, C₆H₁₄O₁₀S₂, etc. Plausible formation pathways for these multi-sulfur products are illustrated in Scheme 2. Specifically, C₆H₁₄O₉S₂ can originate from the bimolecular reaction of HOO(CH₂)₃S(O)₂OO⚫ with HOO(CH₂)₃S(O)OO⚫. The formation pathways of C₆H₁₄O₈S₂ and C₆H₁₄O₁₀S₂ are similar with C₆H₁₄O₉S₂. In addition, multi-sulfur products were also detected for other investigated sulfur-VOCs (Figs. S8 and S10–S12). Although acyclic sulfides and disulfides are structurally distinct, the reaction pathways presented above indicate that their ⚫OH-initiated oxidation proceeds through similar sulfur-centered radical intermediates and subsequent reactions of sulfur-RO₂⚫.

To evaluate the yields and volatility distributions of these multi-sulfur products, Fig. 3 summarizes the estimated volatility distributions and formation yields from the ⚫OH-initiated oxidation of 10 sulfur-VOCs except for ethanethiol. No multi-sulfur products were detected for ethanethiol, suggesting that their formation was either negligible or that the resulting concentrations were below the detection limit of the nitrate-CI-LToF-MS. The volatilities were estimated using the parameterization proposed by Li et al. (2016). Overall, the total yields of multi-sulfur products varied substantially among the 10 sulfur-VOCs, ranging from 0.001 % to 11.73 % (Table S3), indicating a strong dependence on precursor structure and sulfur functionality.

Among all investigated compounds, trimethylene sulfide (C₃H₆S) exhibited the highest total yield (11.73 %), suggesting its highly efficient formation of multi-sulfur products. In contrast, several thiol systems and certain acyclic sulfides produced only trace amounts of multi-sulfur products, with total yields below 0.1 %. Acyclic sulfides and disulfide systems predominantly generated semi-volatile organic compounds (SVOCs), with total multi-sulfur yields generally below 4 %. In comparison, cyclic sulfides displayed more diverse volatility distributions. For C₃H₆S, multi-sulfur products extended into the low-volatility organic compounds (LVOCs) and extremely low-volatility organic compounds (ELVOCs) regimes, with a significant fraction of the total yield residing in these low-volatility classes. By contrast, 1,3-dithiolane (C₃H₆S₂) mainly produced SVOCs-range multi-sulfur products, and individual species yields remained below 0.4 %, despite a moderate summed yield. Thiols (e.g., HS(CH₂)₃SH) exhibited a distinct pattern: although their oxidation generated products extending into the LVOCs and ELVOCs regimes, the overall formation efficiency was low, with total yields ranging from 0.001 % to 0.40 %. This suggests that structural factors, such as the position and number of -SH groups, may influence both RO₂⚫ reactivity and multi-sulfur product formation efficiency. The presence of LVOCs and ELVOCs multi-sulfur products, particularly for cyclic sulfides, implies a potential role in secondary organic aerosol formation and particle growth.

It should be noted that the semi-quantification of these multi-sulfur products is based on the calibration factor of gaseous sulfuric acid (H₂SO₄) (Sect. S5), a common approach in nitrate-CIMS measurements due to the lack of authentic standards for highly oxygenated organic compounds (Ehn et al., 2014; Jokinen et al., 2012). It was assumed that the ionization efficiency of H₂SO₄ towards the reagent ions ((HNO₃)_n ⚫NO3-, n= 0, 1 and 2) is the same as that of multi-sulfur products. As a result, the reported yields may have an additional uncertainty because of differences in ionization efficiency between H₂SO₄ and multi-sulfur products towards the reagent ions, as discussed in previous studies (Ehn et al., 2014; Hyttinen et al., 2015).

Although the formation yields of many detected multi-sulfur products are relatively low, their low volatility indicates SOA forming potential. The reported yields represent only the gas-phase multi-sulfur products detected by nitrate-CI-LToF-MS and should not be interpreted as total oxidation product yields. A substantial fraction of sulfur may be converted to inorganic sulfur products and mono-sulfur oxidation products, such as SO₂, H₂SO₄, sulfoxides, sulfones, methanesulfonic acid, and other mono-sulfur oxygenated compounds, which are not included in the reported multi-sulfur product yields. In addition, nitrate-CI-LToF-MS preferentially detects highly oxygenated and low-volatility compounds, while more volatile or less oxygenated sulfur-containing products may be underrepresented. Product wall loss and possible particle-phase transfer may further reduce the observed gas-phase concentrations of multi-sulfur products. Therefore, the reported yields should be treated as lower-limit gas-phase yields of multi-sulfur products.

As shown in Fig. 4a, the emitted VOCs from freshwater algae were measured by Vocus-PTR-LToF-MS and 240 compounds in total were identified, including 143 CHO species, 43 CH species, 20 sulfur-VOCs, and 34 other VOCs. High-resolution peak fittings for the assigned sulfur-VOCs were shown in Fig. S15. The molecular formulas and mixing ratios of 20 sulfur-VOCs are summarized in Table S5 and Fig. 4b.

Under the specific treatment conditions (see Sect. 2.2), mixing ratios of emitted VOCs spanned over three orders of magnitude, ranging from 0.01 to 11.77 ppbv. Among the 20 identified sulfur-VOCs, 6 monosulfur species were detected and they are dominated ones. Specifically, CH₄S reached the highest level (11.77 ppbv), followed by C₂H₆S (8.60 ppbv), CH₂S (4.09 ppbv), and C₂H₄S (3.57 ppbv), while the remaining monosulfur species were present at sub-ppbv levels. 9 disulfur species were identified with generally lower abundances, spanning from 0.04 to 0.78 ppbv, with C₆H₁₄S₂ (0.78 ppbv) and C₃H₆S₂ (0.69 ppbv) representing the most abundant disulfur species. 3 trisulfur species were detected at similarly low levels, ranging from 0.06 to 0.50 ppbv, with C₄H₁₀S₃ showing the highest mixing ratio within this group. In contrast, 2 tetrasulfur species were the least abundant, with mixing ratios decreasing to about 0.01 ppbv for C₂H₆S₄ and C₃H₆S₄. Overall, a clear and systematic decrease in mixing ratios was observed with increasing sulfur number. Because Vocus-PTR-LToF-MS measurements constrain molecular formulas rather than isomer-specific structures, isomeric species (e.g., DMS and ethanethiol, C₂H₆S) cannot be distinguished solely by their exact mass and may have different sensitivities. Therefore, the reported mixing ratios should be interpreted as semi-quantitative apparent ones rather than definitive isomer-specific concentrations.

In addition, photographs taken before and after repeated filtrations show that the green algal suspension became nearly clear, indicating effective removal of most visible algal biomass (Fig. S16). Consistently, removal of algal biomass by repeated filtrations through stacked qualitative filter papers led to a remarkable decrease in the abundance of sulfur-VOCs (Fig. S17), suggesting that the emissions of sulfur-VOCs were closely associated with the algal biological processes. Although only molecular formulas rather than structures could be assigned, the results still provide a comprehensive inventory of freshwater algae-emitted sulfur-VOCs. However, because the freshwater lake samples contained natural microbial communities and the filtration procedure was not designed to sterilize the samples or fully remove bacteria, this experiment cannot distinguish direct algal emissions or other biological processing. Notably, the molecular formulas of sulfur-VOCs targeted in our chamber study were also present in the list of sulfur-VOCs emitted from freshwater algae. Although Vocus-PTR-LToF-MS measurements constrain molecular formulas rather than isomer-specific structures, the co-occurrence of these formula families in algal emissions supports the atmospheric relevance of the structure-resolved kinetics and oxidation mechanisms derived from our chamber experiments.

In subsequent atmospheric oxidation experiments of these emitted VOCs including sulfur-VOCs, our chamber was maintained under NO_x-free conditions, hence the termination of RO₂⚫ by NO_x was suppressed and bimolecular reactions of RO₂⚫ were favored. Approximately 110 oxidation products were identified using nitrate-CI-LToF-MS, including dozens of mono-sulfur organic compounds, a few inorganic sulfur-containing species (e.g., H₂SO₄ and its clusters), and 11 multi-sulfur products (Fig. 5 and Table S6). Among 11 multi-sulfur products, 7 of them could be inferred from our selected sulfur-VOCs chamber simulation experiments and their high-resolution peak fitting plots were also shown in Fig. S18. Additionally, 4 multi-sulfur products could not be reproduced from our chamber simulation experiments (Fig. S19). These experimental results not only provide evidence that multi-sulfur products can be formed from bimolecular reactions of sulfur-containing RO₂⚫ under low-NOx conditions, but also improve our understanding of the atmospheric oxidation chemistry of algae-emitted sulfur-VOCs in ambient air (especially in low-NO_x environments). Notably, the detection of H₂SO₄ and its clusters, which are well-established precursors for atmospheric new particle formation, suggests that the oxidation of algae-emitted sulfur-VOCs may contribute to secondary particle formation (Jokinen et al., 2012; Lee et al., 2019; Yao et al., 2018). These findings expand the current understanding of the atmospheric processing of biogenic sulfur-VOCs released from freshwater algae and suggest that their chemical complexity may have broader implications for sulfur transformation and secondary aerosol formation. However, due to the complex composition of algae-derived sulfur-VOCs, specific formation pathways of these multi-sulfur products need to be further elucidated.

Although the oxidation experiments were conducted under NO_x-free conditions, such chemical regimes are still representative of atmospherically relevant environments characterized by low-NO_x conditions and strong biogenic sulfur-VOC emissions (e.g., inland eutrophic lakes, remote marine boundary layer and polar regions). In these environments, NO_x concentrations are typically very low and RO₂⚫ termination by NO_x is strongly suppressed, while RO₂⚫ + HO₂⚫ and RO₂⚫ + R'O₂⚫ pathways may become more important (Berresheim et al., 1998; Novak et al., 2022; Read et al., 2008; Steinke et al., 2018). Field observations in these environments have reported sulfur-VOCs such as DMS and methanethiol at dozens to hundreds of pptv levels (Berresheim et al., 1998; Novak et al., 2022; Read et al., 2008). Therefore, multi-sulfur products derived from RO₂⚫-R'O₂⚫ bimolecular reactions during atmospheric oxidation of sulfur-VOCs may have SOA forming potential in these environments. While the quantitative contribution of sulfur-VOCs-derived multi-sulfur products to SOA formation remains uncertain, the present results only highlight the detection and formation pathways of multi-sulfur products from atmospheric oxidation of sulfur-VOCs.