Correction to “Experimental study on synchrotron radiation photoionization of secondary organic aerosol derived from styrene ozonolysis”

Abstract

M. -Q. Huang, H. -H. Wang, X. -B. Shan, L.-S. Sheng, C.-J. Hu, X. -J. Gu, W. -J. Zhang

J. Chin. Chem. Soc. 2023, 70, 938

https://doi.org/10.1002/jccs.202200557

In fact, photoionization mass spectra of styrene particles are obtained at under synchrotron radiation of 15.0, 12.5, and 10.0 eV. Due to our carelessness, the synchrotron radiation energy was mistakenly written as 15.0, 12.5, and 10.5 eV.

In this correction, we present the photoionization mass spectra of styrene particles with synchrotron radiation photon energies of 10.0, 12.5, and 15.0 eV, respectively. Meanwhile, the photon energy of synchrotron radiation in the text is modified. The main conclusions of the original work remain unaffected by the corrections. The corrections are as follows.

The VUV-PIMS in U14-A of the Hefei National Synchrotron Radiation Laboratory is used to detect styrene particles in real-time.

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The synchrotron photon energy provided by U14-A is ranged from 8 to 16 eV. While photon energy at 10.5 eV is generally used to measure the photoionization mass spectrum of organic compounds in our previous studies.

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photon energies of 10.5, 13.0, and 15.5 eV are selected successively in an increment of 2.5 eV for the measurement of styrene particles.

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During the detection, the energy of the synchrotron radiation photon is 10.5 eV.

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Figure 3 shows the photoionization mass spectra of styrene particles with synchrotron radiation photon energies of 10.5, 13.0, and 15.5 eV, respectively. The molecular ion (C₈H₈⁺, m/z = 104) and protonated molecular ion peak (C₈H₉⁺, m/z = 105) of styrene are detected when the photon energy is 10.5 eV.

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When the photon energy is 13.0 eV, fragment peaks with m/z = 103 and m/z = 77 are detected. When the photon energy is 15.5 eV, the intensity of the peaks with m/z = 103 and m/z = 77 increases significantly. According to the structure of the styrene molecule, the peaks of m/z = 103 and m/z = 77 may be the fragmentation peaks generated by photodissociation of the hydrogen atom and vinyl group from the molecular ion peak.

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However, photoionization efficiency curve (PIE) of styrene molecular ion (C₈H₈⁺) shown in Figure 4 is the same as the PIE figure obtained by Kobayashi et al.(Kobayashi T., Phys. Lett. A 1978, 69, 105.)

Figure 4 displays the photoionization efficiency curve of the styrene molecular ion (C₈H₈⁺). There is an obvious threshold at 8.46 eV, and the ionization potential of the styrene molecule (IP(C₈H₈⁺)) is (8.46 ± 0.03) eV.

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Also, the error bar is drawn with the average value as the midpoint and the standard deviation of the three repeated measurements as half of the line segment length, as shown in Figure 5.

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Figure 5 The average corrected mass concentration of

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Figure 6 Size distribution of stabilized styrene SOA particles

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Figure 7 Photoionization mass spectra of styrene SOA particles at 10.5 eV photon energy.

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Figure 6. The size of SOA particles formed from styrene.

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Figure 7 is the photoionization mass spectra of styrene SOA particles measured at the photon energy of synchrotron radiation of 10.5 eV.

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While the obtained photoionization efficiency curves in the range of 7.5–11.5 eV for m/z = 78, 94, 106, and 122 are shown in Figure 8.

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As shown in Figure 8 and Table 1,

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Figure 8 The photoionization efficiency curves

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As shown in Figure 9

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as illustrated in Figure 9

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Figure 9 The suggested mechanism of ozone reaction with styrene to produce carbonyl and phenolic compounds.

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as shown in Figure 7.

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As shown in Figure 10

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Figure 10 The UV–Vis spectra of extraction solution for

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Figure 11 The infrared spectra of extraction solution for

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Figure 11 is relatively strong

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In the originally published version of the article, the importance of styrene is described in Introduction Section (Left column Line 2–6, Right column Line 1–7 on page 938, Left column Line 1–9 on page 939):

Styrene is an organic compound formed from substituting one hydrogen atom of benzene with vinyl group. As vinyl double bond can be polymerized, styrene as one of the most important monomers is widely used in the production of polystyrene, styrene butadiene rubber, styrene butadiene latex, and so forth [1, 2]. Styrene is discharged into atmosphere via natural sources such as plants and microorganisms, and solvent use, fuel combustion, industrial processes, and other anthropogenic sources [3–5]. Similar to other aromatic hydrocarbons, styrene is a harmful environmental pollutant in atmosphere. It is inherently toxic and can damage the central nervous and reproductive systems of the human body. It is also classified as a potential carcinogen by the International Cancer Research Institute of World Health Organization [6, 7]. In addition, styrene mainly undergoes reaction with ozone and other oxidant in atmosphere to form secondary organic aerosol (SOA) [8–12]. SOA particles can absorb and scatter sunlight, reduce atmospheric visibility [13, 14]. penetrate deep into the lungs and bronchus, and endanger human health [15].

However, there are some ambiguous sentences in these descriptions. In this correction, we revise these sentences. The main conclusions of the original work remain unaffected by the corrections. The corrections are as follows.

Styrene is the substance generated from substituting benzene's hydrogen atom by vinyl group. As vinyl double bond can be polymerized, styrene as the vital monomer is extensively utilized while manufacturing styrene butadiene rubber, polystyrene, and so forth [1, 2]. Apart from natural sources of microorganisms, plants, etc., industrial processes, fuel combustion, and other anthropogenic sources also discharge styrene into atmosphere [3–5]. Like other aromatics, styrene is a harmful environmental pollutant. It is inherently toxic and can vandalize the reproductive and central nervous systems of the human body. It is also classified as a potential carcinogen by the International Cancer Research Institute of World Health Organization [6, 7]. In addition, styrene mainly reacts with ozone and other oxidant in atmosphere to form secondary organic aerosol (SOA) [8–12]. SOA can scatter and absorb sunlight, reduce visibility [13, 14], and penetrate deep into the lungs and bronchus, endangering human health [15].