Sulfur dioxide

SO₂ is a bent molecule with C_2v symmetry point group.

A valence bond theory approach considering just s and p orbitals would describe the bonding in terms of resonance between two resonance structures.

File:Sulfur-dioxide-resonance-2D.svg

The sulfur–oxygen bond has a bond order of 1.5. There is support for this simple approach that does not invoke d orbital participation.{{cite journal

| title = Chemical bonding in oxofluorides of hypercoordinatesulfur

|author1=Cunningham, Terence P. |author2=Cooper, David L. |author3=Gerratt, Joseph |author4=Karadakov, Peter B. |author5=Raimondi, Mario | journal = Journal of the Chemical Society, Faraday Transactions

| year = 1997

| volume = 93

| issue = 13

| pages = 2247–2254

| doi = 10.1039/A700708F

}}

In terms of electron-counting formalism, the sulfur atom has an oxidation state of +4 and a formal charge of +1.

File:Io Aurorae color.jpg

Sulfur dioxide is found on Earth and exists in very small concentrations in the atmosphere at about 15 ppb.{{Cite web |last=US EPA |first=OAR |date=May 4, 2016 |title=Sulfur Dioxide Trends |url=https://www.epa.gov/air-trends/sulfur-dioxide-trends |access-date=2023-02-16 |website=www.epa.gov |language=en}}

On other planets, sulfur dioxide can be found in various concentrations, the most significant being the atmosphere of Venus, where it is the third-most abundant atmospheric gas at 150 ppm. There, it reacts with water to form clouds of sulfurous acid ({{chem2|SO2}} + {{chem2|H2O}} ⇌ {{chem2|HSO3−}} + {{chem2|H+}}), and is a key component of the planet's global atmospheric sulfur cycle. It has been implicated as a key agent in the warming of early Mars, with estimates of concentrations in the lower atmosphere as high as 100 ppm,{{cite journal|last1=Halevy|first1=I.|last2=Zuber|first2=M. T.|last3=Schrag|first3=D. P.|title=A Sulfur Dioxide Climate Feedback on Early Mars|journal=Science|volume=318|issue=5858|year=2007|pages=1903–1907|issn=0036-8075|doi=10.1126/science.1147039|pmid=18096802|bibcode=2007Sci...318.1903H|s2cid=7246517}} though it only exists in trace amounts. On both Venus and Mars, as on Earth, its primary source is thought to be volcanic. The atmosphere of Io, a natural satellite of Jupiter, is 90% sulfur dioxide{{cite book |last=Lellouch |first=E. |editor=Lopes, R. M. C. |editor1-link=Rosaly Lopes |editor2=Spencer, J. R. |title=Io after Galileo |date=2007 |publisher=Springer-Praxis |isbn=978-3-540-34681-4 |pages=231–264 |chapter=Io's atmosphere }} and trace amounts are thought to also exist in the atmosphere of Jupiter. The James Webb Space Telescope has observed the presence of sulfur dioxide on the exoplanet WASP-39b, where it is formed through photochemistry in the planet's atmosphere.{{cite web | url=https://phys.org/news/2022-11-james-webb-space-telescope-reveals.html?adlt=strict&toWww=1&redig=BF6DD536430F43AF981737C5EEABD064 | title=James Webb Space Telescope reveals an exoplanet atmosphere as never seen before }}

As an ice, it is thought to exist in abundance on the Galilean moons—as subliming ice or frost on the trailing hemisphere of Io,{{cite book |doi=10.1007/978-94-009-5418-2_55 |chapter=Sulfur Dioxide Ice on IO |title=ICES in the Solar System |year=1985 |last1=Cruikshank |first1=D. P. |last2=Howell |first2=R. R. |last3=Geballe |first3=T. R. |last4=Fanale |first4=F. P. |pages=805–815 |isbn=978-94-010-8891-6 }} and in the crust and mantle of Europa, Ganymede, and Callisto, possibly also in liquid form and readily reacting with water.[http://www.jpl.nasa.gov/news/news.php?release=2010-319 Europa's Hidden Ice Chemistry – NASA Jet Propulsion Laboratory]. Jpl.nasa.gov (October 4, 2010). Retrieved on September 24, 2013.

Sulfur dioxide is primarily produced for sulfuric acid manufacture (see contact process, but other processes predated that at least since 16th century). In the United States in 1979, 23.6 million metric tons (26 million U.S. short tons) of sulfur dioxide were used in this way, compared with 150,000 metric tons (165,347 U.S. short tons) used for other purposes. Most sulfur dioxide is produced by the combustion of elemental sulfur. Some sulfur dioxide is also produced by roasting pyrite and other sulfide ores in air.{{Ullmann| author = Müller, Hermann | title = Sulfur Dioxide | doi = 10.1002/14356007.a25_569}}

File:03. Горење на сулфур во атмосфера од кислород.webm. A flow-chamber joined to a gas washing bottle (filled with a solution of methyl orange) is being used. The product is sulfur dioxide (SO₂) with some traces of sulfur trioxide (SO₃). The "smoke" that exits the gas washing bottle is, in fact, a sulfuric acid fog generated in the reaction.]]

Sulfur dioxide is the product of the burning of sulfur or of burning materials that contain sulfur:

:{{chem2|S8}} + 8 {{chem2|O2}} → 8 {{chem2|SO2}}, ΔH = −297 kJ/mol

To aid combustion, liquified sulfur ({{convert|140|–|150|C|F}} is sprayed through an atomizing nozzle to generate fine drops of sulfur with a large surface area. The reaction is exothermic, and the combustion produces temperatures of {{convert|1000|–|1600|C|F}}. The significant amount of heat produced is recovered by steam generation that can subsequently be converted to electricity.

The combustion of hydrogen sulfide and organosulfur compounds proceeds similarly. For example:

:2 {{chem2|H2S}} + 3 {{chem2|O2}} → 2 {{chem2|SO2}} + 2 {{chem2|H2O}}

The roasting of sulfide ores such as pyrite, sphalerite, and cinnabar (mercury sulfide) also releases SO₂:Shriver, Atkins. Inorganic Chemistry, Fifth Edition. W. H. Freeman and Company; New York, 2010; p. 414.

:4 {{chem2|FeS2}} + 11 {{chem2|O2}} → 2 {{chem2|Fe2O3}} + 8 {{chem2|SO2}}

:2 {{chem2|ZnS}} + 3 {{chem2|O2}} → 2 {{chem2|ZnO}} + 2 {{chem2|SO2}}

:{{chem2|HgS + O2 -> Hg + SO2}}

:4 FeS + 7 {{chem2|O2}} → 2 {{chem2|Fe2O3}} + 4 {{chem2|SO2}}

A combination of these reactions is responsible for the largest source of sulfur dioxide, volcanic eruptions. These events can release millions of tons of SO₂.

Sulfur dioxide can also be a byproduct in the manufacture of calcium silicate cement; CaSO₄ is heated with coke and sand in this process:

:2 {{chem2|CaSO4}} + 2 {{chem2|SiO2}} + C → 2 {{chem2|CaSiO3}} + 2 {{chem2|SO2}} + {{chem2|CO2}}

Until the 1970s commercial quantities of sulfuric acid and cement were produced by this process in Whitehaven, England. Upon being mixed with shale or marl, and roasted, the sulfate liberated sulfur dioxide gas, used in sulfuric acid production, the reaction also produced calcium silicate, a precursor in cement production.[http://www.lakestay.co.uk/whitehavenmininghistory.html WHITEHAVEN COAST ARCHAEOLOGICAL SURVEY]. lakestay.co.uk (2007)

On a laboratory scale, the action of hot concentrated sulfuric acid on copper turnings produces sulfur dioxide.

:Cu + 2 {{chem2|H2SO4}} → {{chem2|CuSO4 + SO2 + 2 H2O}}

Tin also reacts with concentrated sulfuric acid but it produces tin(II) sulfate which can later be pyrolyzed at 360 °C into tin dioxide and dry sulfur dioxide.

:Sn + {{chem2|H2SO4}} → {{chem2|SnSO4 + H2}}

:{{chem2|SnSO4}} → {{chem2|SnO2}} + {{chem2|SO2}}

The reverse reaction occurs upon acidification:

:{{chem2|H+ + HSO3- -> SO2 + H2O}}

Sulfites result by the action of aqueous base on sulfur dioxide:

:{{chem2|SO2 + 2 NaOH → Na2SO3 + H2O}}

Sulfur dioxide is a mild but useful reducing agent. It is oxidized by halogens to give the sulfuryl halides, such as sulfuryl chloride:

:{{chem2|SO2 + Cl2 → SO2Cl2}}

Sulfur dioxide is the oxidising agent in the Claus process, which is conducted on a large scale in oil refineries. Here, sulfur dioxide is reduced by hydrogen sulfide to give elemental sulfur:

:{{chem2|SO2 + 2 H2S → 3 S + 2 H2O}}

The sequential oxidation of sulfur dioxide followed by its hydration is used in the production of sulfuric acid.

:{{chem2|SO2}} + {{chem2|H2O}} + {{frac|1|2}} {{chem2|O2}} → {{chem2|H2SO4}}

Sulfur dioxide dissolves in water to give "sulfurous acid", which cannot be isolated and is instead an acidic solution of bisulfite, and possibly sulfite, ions.

:{{chem2|SO2 + H2O ⇌ HSO3− + H+}}{{spaces|10}}K_a = 1.54{{e|−2}}; pK_a = 1.81

Sulfur dioxide is one of the few common acidic yet reducing gases. It turns moist litmus pink (being acidic), then white (due to its bleaching effect). It may be identified by bubbling it through a dichromate solution, turning the solution from orange to green (Cr³⁺ (aq)). It can also reduce ferric ions to ferrous.{{Cite web|url=http://publications.gc.ca/collections/collection_2017/rncan-nrcan/M34-20/M34-20-107-eng.pdf|title = Information archivée dans le Web}}

Sulfur dioxide can react with certain 1,3-dienes in a cheletropic reaction to form cyclic sulfones. This reaction is exploited on an industrial scale for the synthesis of sulfolane, which is an important solvent in the petrochemical industry.

:File:Cheletropic reaction of butadiene with SO2.svg

Sulfur dioxide can bind to metal ions as a ligand to form metal sulfur dioxide complexes, typically where the transition metal is in oxidation state 0 or +1. Many different bonding modes (geometries) are recognized, but in most cases, the ligand is monodentate, attached to the metal through sulfur, which can be either planar and pyramidal η¹.{{Greenwood&Earnshaw2nd}} As a η¹-SO₂ (S-bonded planar) ligand sulfur dioxide functions as a Lewis base using the lone pair on S. SO₂ functions as a Lewis acids in its η¹-SO₂ (S-bonded pyramidal) bonding mode with metals and in its 1:1 adducts with Lewis bases such as dimethylacetamide and trimethyl amine. When bonding to Lewis bases the acid parameters of SO₂ are E_A = 0.51 and E_A = 1.56.

The overarching, dominant use of sulfur dioxide is in the production of sulfuric acid.

Sulfur dioxide is an intermediate in the production of sulfuric acid, being converted to sulfur trioxide, and then to oleum, which is made into sulfuric acid. Sulfur dioxide for this purpose is made when sulfur combines with oxygen. The method of converting sulfur dioxide to sulfuric acid is called the contact process. Several million tons are produced annually for this purpose.

{{See also|Food preservation}}

Sulfur dioxide is sometimes used as a preservative for dried apricots, dried figs, and other dried fruits, owing to its antimicrobial properties and ability to prevent oxidation,{{cite conference |last1=Zamboni |first1=Cibele B. |last2=Medeiros |first2=Ilca M. M. A. |last3=de Medeiros |first3=José A. G. |title=Analysis of Sulfur in Dried Fruits Using NAA |url=https://www.ipen.br/biblioteca/2011/inac/17204.pdf |conference=2011 International Nuclear Atlantic Conference – INAC 2011 |isbn=978-85-99141-03-8 |date=October 2011 |access-date=2020-06-04 |archive-date=2020-06-04 |archive-url=https://web.archive.org/web/20200604193519/https://www.ipen.br/biblioteca/2011/inac/17204.pdf |url-status=dead }} and is called E220[http://www.food.gov.uk/safereating/chemsafe/additivesbranch/enumberlist#h_3 Current EU approved additives and their E Numbers], The Food Standards Agency website. when used in this way in Europe. As a preservative, it maintains the colorful appearance of the fruit and prevents rotting. Historically, molasses was "sulfured" as a preservative and also to lighten its color. Treatment of dried fruit was usually done outdoors, by igniting sublimed sulfur and burning in an enclosed space with the fruits.{{Citation |title=Preserving foods: Drying fruits and Vegetable |url=https://nchfp.uga.edu/publications/uga/uga_dry_fruit.pdf |publisher=University of Georgia cooperative extension service |access-date=2022-06-06 |archive-date=2022-09-27 |archive-url=https://web.archive.org/web/20220927163031/https://nchfp.uga.edu/publications/uga/uga_dry_fruit.pdf |url-status=dead }} Fruits may be sulfured by dipping them into sodium bisulfite, sodium sulfite or sodium metabisulfite.

Sulfur dioxide was first used in winemaking by the Romans, when they discovered that burning sulfur candles inside empty wine vessels keeps them fresh and free from vinegar smell.{{cite web|url=http://www.practicalwinery.com/janfeb09/page1.htm|publisher=www.practicalwinery.com|date=February 1, 2009|title=Practical Winery & vineyard Journal Jan/Feb 2009|url-status=dead|archive-url=https://web.archive.org/web/20130928111625/http://www.practicalwinery.com/janfeb09/page1.htm|archive-date=2013-09-28}}

It is still an important compound in winemaking, and is measured in parts per million (ppm) in wine. It is present even in so-called unsulfurated wine at concentrations of up to 10 mg/L.[http://www.morethanorganic.com/sulphur-in-the-bottle Sulphites in wine], MoreThanOrganic.com. It serves as an antibiotic and antioxidant, protecting wine from spoilage by bacteria and oxidation – a phenomenon that leads to the browning of the wine and a loss of cultivar specific flavors.Jackson, R.S. (2008) Wine science: principles and applications, Amsterdam; Boston: Elsevier/Academic Press{{cite journal | doi = 10.1016/j.tifs.2014.11.004| title = Demonstrating the efficiency of sulphur dioxide replacements in wine: A parameter review| journal = Trends in Food Science & Technology| volume = 42| pages = 27–43| year = 2015| last1 = Guerrero| first1 = Raúl F| last2 = Cantos-Villar| first2 = Emma| issue = 1}} Its antimicrobial action also helps minimize volatile acidity. Wines containing sulfur dioxide are typically labeled with "containing sulfites".

Sulfur dioxide exists in wine in free and bound forms, and the combinations are referred to as total SO₂. Binding, for instance to the carbonyl group of acetaldehyde, varies with the wine in question. The free form exists in equilibrium between molecular SO₂ (as a dissolved gas) and bisulfite ion, which is in turn in equilibrium with sulfite ion. These equilibria depend on the pH of the wine. Lower pH shifts the equilibrium towards molecular (gaseous) SO₂, which is the active form, while at higher pH more SO₂ is found in the inactive sulfite and bisulfite forms. The molecular SO₂ is active as an antimicrobial and antioxidant, and this is also the form which may be perceived as a pungent odor at high levels. Wines with total SO₂ concentrations below 10 ppm do not require "contains sulfites" on the label by US and EU laws. The upper limit of total SO₂ allowed in wine in the US is 350 ppm; in the EU it is 160 ppm for red wines and 210 ppm for white and rosé wines. In low concentrations, SO₂ is mostly undetectable in wine, but at free SO₂ concentrations over 50 ppm, SO₂ becomes evident in the smell and taste of wine.{{Citation needed|date=May 2009}}

SO₂ is also a very important compound in winery sanitation. Wineries and equipment must be kept clean, and because bleach cannot be used in a winery due to the risk of cork taint,[http://www.extension.purdue.edu/extmedia/FS/FS-50-W.pdf Chlorine Use in the Winery]. Purdue University a mixture of SO₂, water, and citric acid is commonly used to clean and sanitize equipment. Ozone (O₃) is now used extensively for sanitizing in wineries due to its efficacy, and because it does not affect the wine or most equipment.[https://www.practicalwinery.com/janfeb00/ozone.htm Use of ozone for winery and environmental sanitation] {{Webarchive|url=https://web.archive.org/web/20170912102459/https://www.practicalwinery.com/janfeb00/ozone.htm |date=September 12, 2017 }}, Practical Winery & Vineyard Journal.

Sulfur dioxide is also a good reductant. In the presence of water, sulfur dioxide is able to decolorize substances. Specifically, it is a useful reducing bleach for papers and delicate materials such as clothes. This bleaching effect normally does not last very long. Oxygen in the atmosphere reoxidizes the reduced dyes, restoring the color. In municipal wastewater treatment, sulfur dioxide is used to treat chlorinated wastewater prior to release. Sulfur dioxide reduces free and combined chlorine to chloride.{{cite book |last=Tchobanoglous |first=George |title=Wastewater Engineering |edition=3rd |location=New York |publisher=McGraw Hill |year=1979 |isbn=0-07-041677-X }}

Sulfur dioxide is fairly soluble in water, and by both IR and Raman spectroscopy; the hypothetical sulfurous acid, H₂SO₃, is not present to any extent. However, such solutions do show spectra of the hydrogen sulfite ion, HSO₃⁻, by reaction with water, and it is in fact the actual reducing agent present:

:SO₂ + H₂O ⇌ HSO₃⁻ + H⁺

In the beginning of the 20th century sulfur dioxide was used in Buenos Aires as a fumigant to kill rats that carried the Yersinia pestis bacterium, which causes bubonic plague. The application was successful, and the application of this method was extended to other areas in South America. In Buenos Aires, where these apparatuses were known as Sulfurozador, but later also in Rio de Janeiro, New Orleans and San Francisco, the sulfur dioxide treatment machines were brought into the streets to enable extensive disinfection campaigns, with effective results.{{cite journal |last1=Engelmann |first1=Lukas |title=Fumigating the Hygienic Model City: Bubonic Plague and the Sulfurozador in Early-Twentieth-Century Buenos Aires |journal=Medical History |date=July 2018 |volume=62 |issue=3 |pages=360–382 |doi=10.1017/mdh.2018.37 |pmid=29886876 |pmc=6113751 }}

Sulfur dioxide or its conjugate base bisulfite is produced biologically as an intermediate in both sulfate-reducing organisms and in sulfur-oxidizing bacteria, as well. The role of sulfur dioxide in mammalian biology is not yet well understood.{{cite journal |last1=Liu |first1=D. |last2=Jin |first2=H. |last3=Tang |first3=C. |last4=Du |first4=J. |title=Sulfur Dioxide: a Novel Gaseous Signal in the Regulation of Cardiovascular Functions |journal=Mini-Reviews in Medicinal Chemistry |year=2010 |volume=10 |issue=11 |pages=1039–1045 |doi=10.2174/1389557511009011039 |pmid=20540708 }} Sulfur dioxide blocks nerve signals from the pulmonary stretch receptors and abolishes the Hering–Breuer inflation reflex.

It is considered that endogenous sulfur dioxide plays a significant physiological role in regulating cardiac and blood vessel function, and aberrant or deficient sulfur dioxide metabolism can contribute to several different cardiovascular diseases, such as arterial hypertension, atherosclerosis, pulmonary arterial hypertension, and stenocardia.{{cite journal |last1=Tian |first1=Hong |title=Advances in the study on endogenous sulfur dioxide in the cardiovascular system |journal=Chinese Medical Journal |date=November 5, 2014 |volume=127 |issue=21 |pages=3803–3807 |doi=10.3760/cma.j.issn.0366-6999.20133031 |pmid=25382339 |s2cid=11924999 |doi-access=free }}

It was shown that in children with pulmonary arterial hypertension due to congenital heart diseases the level of homocysteine is higher and the level of endogenous sulfur dioxide is lower than in normal control children. Moreover, these biochemical parameters strongly correlated to the severity of pulmonary arterial hypertension. Authors considered homocysteine to be one of useful biochemical markers of disease severity and sulfur dioxide metabolism to be one of potential therapeutic targets in those patients.{{cite journal|vauthors=Yang R, Yang Y, Dong X, Wu X, Wei Y |title=Correlation between endogenous sulfur dioxide and homocysteine in children with pulmonary arterial hypertension associated with congenital heart disease|language=zh|journal=Zhonghua Er Ke Za Zhi|date=Aug 2014|volume=52|issue=8|pages=625–629|pmid=25224243}}

Endogenous sulfur dioxide also has been shown to lower the proliferation rate of endothelial smooth muscle cells in blood vessels, via lowering the MAPK activity and activating adenylyl cyclase and protein kinase A.{{cite journal|vauthors=Liu D, Huang Y, Bu D, Liu AD, Holmberg L, Jia Y, Tang C, Du J, Jin H |title=Sulfur dioxide inhibits vascular smooth muscle cell proliferation via suppressing the Erk/MAP kinase pathway mediated by cAMP/PKA signaling|journal=Cell Death Dis.|date=May 2014|volume=5|issue=5|pages=e1251|doi=10.1038/cddis.2014.229|pmid=24853429|pmc=4047873}} Smooth muscle cell proliferation is one of important mechanisms of hypertensive remodeling of blood vessels and their stenosis, so it is an important pathogenetic mechanism in arterial hypertension and atherosclerosis.

Endogenous sulfur dioxide in low concentrations causes endothelium-dependent vasodilation. In higher concentrations it causes endothelium-independent vasodilation and has a negative inotropic effect on cardiac output function, thus effectively lowering blood pressure and myocardial oxygen consumption. The vasodilating and bronchodilating effects of sulfur dioxide are mediated via ATP-dependent calcium channels and L-type ("dihydropyridine") calcium channels. Endogenous sulfur dioxide is also a potent antiinflammatory, antioxidant and cytoprotective agent. It lowers blood pressure and slows hypertensive remodeling of blood vessels, especially thickening of their intima. It also regulates lipid metabolism.{{cite journal|vauthors=Wang XB, Jin HF, Tang CS, Du JB |title=The biological effect of endogenous sulfur dioxide in the cardiovascular system.|journal=Eur J Pharmacol|date=November 16, 2011|volume=670|issue=1|doi=10.1016/j.ejphar.2011.08.031|pmid=21925165|pages=1–6}}

Endogenous sulfur dioxide also diminishes myocardial damage, caused by isoproterenol adrenergic hyperstimulation, and strengthens the myocardial antioxidant defense reserve.{{cite journal|vauthors=Liang Y, Liu D, Ochs T, Tang C, Chen S, Zhang S, Geng B, Jin H, Du J |title=Endogenous sulfur dioxide protects against isoproterenol-induced myocardial injury and increases myocardial antioxidant capacity in rats.|journal=Lab. Invest.|date=Jan 2011|volume=91|issue=1|pages=12–23|doi=10.1038/labinvest.2010.156|pmid=20733562|doi-access=free}}

Sulfur dioxide is a versatile inert solvent widely used for dissolving highly oxidizing salts. It is also used occasionally as a source of the sulfonyl group in organic synthesis. Treatment of aryl diazonium salts with sulfur dioxide and cuprous chloride yields the corresponding aryl sulfonyl chloride, for example:{{OrgSynth | author = Hoffman, R. V. | title = m-Trifluoromethylbenzenesulfonyl Chloride | collvol = 7 | collvolpages = 508 | year = 1990| prep = CV7P0508}}

:File:Preparation of m-trifluoromethylbenzenesulfonyl chloride.svg

As a result of its very low Lewis basicity, it is often used as a low-temperature solvent/diluent for superacids like magic acid (FSO₃H/SbF₅), allowing for highly reactive species like tert-butyl cation to be observed spectroscopically at low temperature (though tertiary carbocations do react with SO₂ above about −30 °C, and even less reactive solvents like SO₂ClF must be used at these higher temperatures).{{Cite journal|last1=Olah|first1=George A.|last2=Lukas|first2=Joachim.|date=August 1, 1967|title=Stable carbonium ions. XLVII. Alkylcarbonium ion formation from alkanes via hydride (alkide) ion abstraction in fluorosulfonic acid-antimony pentafluoride-sulfuryl chlorofluoride solution|journal=Journal of the American Chemical Society|volume=89|issue=18|pages=4739–4744|doi=10.1021/ja00994a030|issn=0002-7863}}

Being easily condensed and possessing a high heat of evaporation, sulfur dioxide is a candidate material for refrigerants. Before the development of chlorofluorocarbons, sulfur dioxide was used as a refrigerant in home refrigerators.

Sulfur dioxide content in naturally-released geothermal gasses is measured by the Icelandic Meteorological Office as an indicator of possible volcanic activity.{{Cite web |date=n.d. |title=Volcanic gases |url=https://en.vedur.is/volcanoes/volcanic-hazards/volcanic-gases/ |website=Iceland Met Office}}

File:20180519 USGS Leilani Estates Hawaii Volcanic EruptionDSC 0411 medium.jpg volunteer tests for sulfur dioxide after the 2018 lower Puna eruption.]]

In the United States, the Center for Science in the Public Interest lists the two food preservatives, sulfur dioxide and sodium bisulfite, as being safe for human consumption except for certain asthmatic individuals who may be sensitive to them, especially in large amounts.{{cite web | title = Center for Science in the Public Interest – Chemical Cuisine | url = http://www.cspinet.org/reports/chemcuisine.htm | access-date = March 17, 2010}} Symptoms of sensitivity to sulfiting agents, including sulfur dioxide, manifest as potentially life-threatening trouble breathing within minutes of ingestion.{{cite web | title = California Department of Public Health: Food and Drug Branch: Sulfites | url = http://www.cdph.ca.gov/pubsforms/Guidelines/Documents/fdb%20Sulfites.pdf | access-date = September 27, 2013 | url-status = dead | archive-url = https://web.archive.org/web/20120723065412/http://www.cdph.ca.gov/pubsforms/Guidelines/Documents/fdb%20Sulfites.pdf | archive-date = July 23, 2012 }} Sulphites may also cause symptoms in non-asthmatic individuals, namely dermatitis, urticaria, flushing, hypotension, abdominal pain and diarrhea, and even life-threatening anaphylaxis.{{cite journal |vauthors=Vally H, Misso NL |title=Adverse reactions to the sulphite additives |journal=Gastroenterol Hepatol Bed Bench |volume=5 |issue=1 |pages=16–23 |date=2012 |pmid=24834193 |pmc=4017440 |doi= |url=}}

Incidental exposure to sulfur dioxide is routine, e.g. the smoke from matches, coal, and sulfur-containing fuels like bunker fuel. Relative to other chemicals, it is only mildly toxic and requires high concentrations to be actively hazardous.[https://www.epa.gov/so2-pollution/ Sulfur Dioxide Basics] U.S. Environmental Protection Agency However, its ubiquity makes it a major air pollutant with significant impacts on human health.[https://www.epa.gov/so2-pollution Sulfur Dioxide (SO2) Pollution]. United States Environmental Protection Agency

In 2008, the American Conference of Governmental Industrial Hygienists reduced the short-term exposure limit to 0.25 parts per million (ppm). In the US, the OSHA set the PEL at 5 ppm (13 mg/m³) time-weighted average. Also in the US, NIOSH set the IDLH at 100 ppm.{{cite web |url=https://www.cdc.gov/niosh/npg/npgd0575.html |title=NIOSH Pocket Guide to Chemical Hazards }} In 2010, the EPA "revised the primary SO₂ NAAQS by establishing a new one-hour standard at a level of 75 parts per billion (ppb). EPA revoked the two existing primary standards because they would not provide additional public health protection given a one-hour standard at 75 ppb."

File:Volcanic injection.svgs on sulfate aerosol concentrations and chemical reactions in the atmosphere]]

Major volcanic eruptions have an overwhelming effect on sulfate aerosol concentrations in the years when they occur: eruptions ranking 4 or greater on the Volcanic Explosivity Index inject {{chem2|SO2}} and water vapor directly into the stratosphere, where they react to create sulfate aerosol plumes.{{cite web |url=http://volcanoes.usgs.gov/hazards/gas/s02aerosols.php |title=Volcanic Sulfur Aerosols Affect Climate and the Earth's Ozone Layer |access-date=February 17, 2009 |publisher=United States Geological Survey |archive-date=November 14, 2015 |archive-url=https://web.archive.org/web/20151114184944/https://volcanoes.usgs.gov/hazards/gas/s02aerosols.php |url-status=dead }} Volcanic emissions vary significantly in composition, and have complex chemistry due to the presence of ash particulates and a wide variety of other elements in the plume. Only stratovolcanoes containing primarily felsic magmas are responsible for these fluxes, as mafic magma erupted in shield volcanoes doesn't result in plumes which reach the stratosphere.{{cite journal |doi=10.1016/j.atmosenv.2004.06.017 |journal=Atmospheric Environment |volume=38 |issue=33 |year=2004 |pages=5637–5649 |title=Aerosol chemistry of emissions from three contrasting volcanoes in Italy |vauthors=Mathera TA, Oppenheimer AG, McGonigle A|bibcode=2004AtmEn..38.5637M }} However, before the Industrial Revolution, dimethyl sulfide pathway was the largest contributor to sulfate aerosol concentrations in a more average year with no major volcanic activity. According to the IPCC First Assessment Report, published in 1990, volcanic emissions usually amounted to around 10 million tons in 1980s, while dimethyl sulfide amounted to 40 million tons. Yet, by that point, the global human-caused emissions of sulfur into the atmosphere became "at least as large" as all natural emissions of sulfur-containing compounds combined: they were at less than 3 million tons per year in 1860, and then they increased to 15 million tons in 1900, 40 million tons in 1940 and about 80 millions in 1980. The same report noted that "in the industrialized regions of Europe and North America, anthropogenic emissions dominate over natural emissions by about a factor of ten or even more".IPCC, 1990: [https://www.ipcc.ch/site/assets/uploads/2018/03/ipcc_far_wg_I_chapter_01.pdf Chapter 1: Greenhouse Gases and Aerosols] [R.T. Watson, H. Rodhe, H. Oeschger and U. Siegenthaler]. In: [https://www.ipcc.ch/site/assets/uploads/2018/03/ipcc_far_wg_I_full_report.pdf Climate Change: The IPCC Scientific Assessment] [J.T.Houghton, G.J.Jenkins and J.J.Ephraums (eds.)]. Cambridge University Press, Cambridge, United Kingdom and New York, NY, USA, pp. 31–34, In the eastern United States in the early 2000s, sulfate particles were estimated to account for 25% or more of all air pollution. Exposure to sulfur dioxide emissions by coal power plants (coal PM_2.5) in the US was associated with 2.1 times greater mortality risk than exposure to PM_2.5 from all sources.{{cite journal |last1=Henneman |first1=Lucas |last2=Choirat |first2=Christine |last3=Dedoussi |first3=Irene |last4=Dominici |first4=Francesca |last5=Roberts |first5=Jessica|last6=Zigler |first6=Corwin |title=Mortality risk from United States coal electricity generation |journal=Science |date=November 24, 2023 |volume=382 |issue=6673 |pages=941–946|doi=10.1126/science.adf4915 |pmid=37995235 |pmc=10870829 |bibcode=2023Sci...382..941H |language=en}}

Meanwhile, the Southern Hemisphere had much lower concentrations due to being much less densely populated, with an estimated 90% of the human population in the north. In the early 1990s, anthropogenic sulfur dominated in the Northern Hemisphere, where only 16% of annual sulfur emissions were natural, yet amounted for less than half of the emissions in the Southern Hemisphere.{{Cite journal|last1=Bates|first1=T. S.|last2=Lamb|first2=B. K.|last3=Guenther|first3=A.|last4=Dignon|first4=J.|last5=Stoiber|first5=R. E.|date=April 1992|title=Sulfur emissions to the atmosphere from natural sources|url=http://link.springer.com/10.1007/BF00115242|journal=Journal of Atmospheric Chemistry|language=en|volume=14|issue=1–4|pages=315–337|doi=10.1007/BF00115242 |bibcode=1992JAtC...14..315B |s2cid=55497518|issn=0167-7764}}

File:Acid rain woods1.JPG]]

Such an increase in sulfate aerosol emissions had a variety of effects. At the time, the most visible one was acid rain, caused by precipitation from clouds carrying high concentrations of sulfate aerosols in the troposphere.{{Cite journal|last1=Burns|first1= Douglas A.|last2=Aherne|first2=Julian|last3=Gay|first3=David A.|last4=Lehmann|first4=Christopher M.~B.|title =Acid rain and its environmental effects: Recent scientific advances|journal = Atmospheric Environment|language=en|year = 2016|volume=146|pages = 1–4|doi = 10.1016/j.atmosenv.2016.10.019|bibcode= 2016AtmEn.146....1B|doi-access=free}}

At its peak, acid rain has eliminated brook trout and some other fish species and insect life from lakes and streams in geographically sensitive areas, such as Adirondack Mountains in the United States.{{Cite web|title=Effects of Acid Rain – Surface Waters and Aquatic Animals|url=http://www.epa.gov/acidrain/effects/surface_water.html|url-status=dead|archive-url=https://web.archive.org/web/20090514121649/http://www.epa.gov/acidrain/effects/surface_water.html|archive-date=May 14, 2009|website=US EPA}} Acid rain worsens soil function as some of its microbiota is lost and heavy metals like aluminium are mobilized (spread more easily) while essential nutrients and minerals such as magnesium can leach away because of the same. Ultimately, plants unable to tolerate lowered pH are killed, with montane forests being some of the worst-affected ecosystems due to their regular exposure to sulfate-carrying fog at high altitudes.{{Cite journal|last1=Rodhe|first1=Henning|last2=Dentener|first2=Frank|last3=Schulz|first3=Michael|date=October 1, 2002|title=The Global Distribution of Acidifying Wet Deposition|url=https://doi.org/10.1021/es020057g|journal=Environmental Science & Technology|volume=36|issue=20|pages=4382–4388|doi=10.1021/es020057g|pmid=12387412|bibcode=2002EnST...36.4382R|issn=0013-936X|url-access=subscription}}US EPA: [http://www.epa.gov/acidrain/effects/forests.html Effects of Acid Rain – Forests] {{webarchive |url=https://web.archive.org/web/20080726034352/http://www.epa.gov/acidrain/effects/forests.html |date=July 26, 2008 }}{{cite journal|doi=10.1126/science.272.5259.244|url=http://www.esf.edu/efb/mitchell/Class%20Readings/Sci.272.244.246.pdf|title=Long-Term Effects of Acid Rain: Response and Recovery of a Forest Ecosystem|year=1996|last1=Likens|first1=G. E.|last2=Driscoll|first2=C. T.|last3=Buso|first3=D. C.|journal=Science|volume=272|issue=5259|page=244|bibcode=1996Sci...272..244L|s2cid=178546205|access-date=February 9, 2013|archive-date=December 24, 2012|archive-url=https://web.archive.org/web/20121224203613/http://www.esf.edu/efb/mitchell/Class%20Readings/Sci.272.244.246.pdf|url-status=live}}{{Cite journal|last1=Larssen|first1=T.|last2=Carmichael|first2=G. R.|date=October 1, 2000|title=Acid rain and acidification in China: the importance of base cation deposition|url=http://www.sciencedirect.com/science/article/pii/S0269749199002791|journal=Environmental Pollution|language=en|volume=110|issue=1|pages=89–102|doi=10.1016/S0269-7491(99)00279-1|pmid=15092859|issn=0269-7491|access-date=April 22, 2020|archive-date=March 30, 2015|archive-url=https://web.archive.org/web/20150330041614/http://www.sciencedirect.com/science/article/pii/S0269749199002791|url-status=live|url-access=subscription}}{{Cite journal|last1=Johnson|first1=Dale W.|last2=Turner|first2=John|last3=Kelly|first3=J. M.|date=1982|title=The effects of acid rain on forest nutrient status|journal=Water Resources Research|language=en|volume=18|issue=3|pages=449–461|doi=10.1029/WR018i003p00449|bibcode=1982WRR....18..449J|issn=1944-7973}} While acid rain was too dilute to affect human health directly, breathing smog or even any air with elevated sulfate concentrations is known to contribute to heart and lung conditions, including asthma and bronchitis.[http://www.epa.gov/acidrain/effects/health.html Effects of Acid Rain – Human Health] {{Webarchive|url=https://web.archive.org/web/20080118120242/http://www.epa.gov/acidrain/effects/health.html |date=January 18, 2008 }}. Epa.gov (June 2, 2006). Retrieved on February 9, 2013. Further, this form of pollution is linked to preterm birth and low birth weight, with a study of 74,671 pregnant women in Beijing finding that every additional 100 μg/m³ of {{SO2}} in the air reduced infants' weight by 7.3 g, making it and other forms of air pollution the largest attributable risk factor for low birth weight ever observed.{{Cite journal |last1=Wang |first1=X. |last2=Ding |first2=H. |last3=Ryan |first3=L. |last4=Xu |first4=X. |s2cid=2707126 |date=May 1, 1997 |title=Association between air pollution and low birth weight: a community-based study |journal=Environmental Health Perspectives |volume=105 |issue=5 |pages=514–20 |issn=0091-6765 |pmc=1469882 |pmid=9222137 |doi=10.1289/ehp.97105514}}

File:Estimates of past and future SO2 global anthropogenic emissions.pngs. While no climate change scenario may reach Maximum Feasible Reductions (MFRs), all assume steep declines from today's levels. By 2019, sulfate emission reductions were confirmed to proceed at a very fast rate.{{Cite journal|last1=Xu|first1=Yangyang|last2=Ramanathan|first2=Veerabhadran|last3=Victor|first3=David G.|date=December 5, 2018|title=Global warming will happen faster than we think|journal=Nature|language=en|volume=564|issue=7734|pages=30–32 |url=https://www.researchgate.net/publication/329411074 |doi=10.1038/d41586-018-07586-5|pmid=30518902|bibcode=2018Natur.564...30X|doi-access=free}}]]

Due largely to the US EPA's Acid Rain Program, the U.S. has had a 33% decrease in emissions between 1983 and 2002 (see table). This improvement resulted in part from flue-gas desulfurization, a technology that enables SO₂ to be chemically bound in power plants burning sulfur-containing coal or petroleum.

In particular, calcium oxide (lime) reacts with sulfur dioxide to form calcium sulfite:

: CaO + SO₂ → CaSO₃

Aerobic oxidation of the CaSO₃ gives CaSO₄, anhydrite. Most gypsum sold in Europe comes from flue-gas desulfurization.

To control sulfur emissions, dozens of methods with relatively high efficiencies have been developed for fitting of coal-fired power plants.{{Cite journal|last1=Lin|first1=Cheng-Kuan|last2=Lin|first2=Ro-Ting|last3=Chen|first3=Pi-Cheng|last4=Wang|first4=Pu|last5=De Marcellis-Warin|first5=Nathalie|last6=Zigler|first6=Corwin|last7=Christiani|first7=David C.|date=February 8, 2018|title=A Global Perspective on Sulfur Oxide Controls in Coal-Fired Power Plants and Cardiovascular Disease|journal=Scientific Reports|language=en|volume=8|issue=1|pages=2611 |doi=10.1038/s41598-018-20404-2|pmid=29422539|issn=2045-2322|pmc=5805744|bibcode=2018NatSR...8.2611L}} Sulfur can be removed from coal during burning by using limestone as a bed material in fluidized bed combustion.{{cite book |last=Lindeburg |first=Michael R. |title=Mechanical Engineering Reference Manual for the PE Exam |location=Belmont, C.A. |publisher=Professional Publications, Inc |year=2006 |pages=27–3 |isbn=978-1-59126-049-3}}

Sulfur can also be removed from fuels before burning, preventing formation of SO₂ when the fuel is burnt. The Claus process is used in refineries to produce sulfur as a byproduct. The Stretford process has also been used to remove sulfur from fuel. Redox processes using iron oxides can also be used, for example, Lo-Cat[https://web.archive.org/web/20100304170107/http://www.gtp-merichem.com/support/index.php FAQ's About Sulfur Removal and Recovery using the LO-CAT® Hydrogen Sulfide Removal System]. gtp-merichem.com or Sulferox.[http://www.netl.doe.gov/technologies/coalpower/gasification/pubs/pdf/SFA%20Pacific_Process%20Screening%20Analysis_Dec%202002.pdf Process screening analysis of alternative gas treating and sulfur removal for gasification]. (December 2002) Report by SFA Pacific, Inc. prepared for U.S. Department of Energy (PDF) Retrieved on October 31, 2011.

Fuel additives such as calcium additives and magnesium carboxylate may be used in marine engines to lower the emission of sulfur dioxide gases into the atmosphere.May, Walter R. [http://www.fuelspec.com/library/Marine%20Emissions%20Abatement.pdf Marine Emissions Abatement] {{Webarchive|url=https://web.archive.org/web/20150402130001/http://www.fuelspec.com/library/Marine%20Emissions%20Abatement.pdf |date=April 2, 2015 }}. SFA International, Inc., p. 6.

Sulfur dioxide aerosols in the stratosphere can contribute to ozone depletion in the presence of chlorofluorocarbons and other halogenated ozone-depleting substances.{{cite journal|last1=Klobas|first1=J.E.|last2=Wilmouth|first2=D.M.|last3=Weisenstein|first3=D.K.|last4=Anderson|first4=J.G.|last5=Salawitch|first5=R.J.|title=Ozone depletion following future volcanic eruptions|journal=Geophysical Research Letters|volume=44|issue=14|pages=7490–7499|year=2017|doi=10.1002/2017GL073972|doi-access=free}} The effects of volcanic eruptions containing sulfur dioxide aerosols on the ozone layer are complex, however. In the absence of anthropogenic or biogenic halogenated compounds in the lower stratosphere, depletion of dinitrogen pentoxide in the middle stratosphere associated with its reactivity to the aerosols can promote ozone formation. Injection of sulfur dioxide and large amounts of water vapor into the stratosphere following the 2022 eruption of Hunga Tonga-Hunga Haʻapai resulted in altered atmospheric circulation that promoted a decrease in ozone in the southern latitudes but an increase in the tropics.{{cite web|url=https://www.chemistry.harvard.edu/news/new-research-massive-2022-eruption-reduced-ozone-levels|title=New research: Massive 2022 eruption reduced ozone levels|website=Department of Chemistry and Chemical Biology|publisher=Harvard University|date=21 November 2023|access-date=7 January 2025}}{{cite journal|last1=Wilmouth|first1=D.M.|last2=Østerstrøm|first2=F.F.|last3=Smith|first3=J.B.|last4=Anderson|first4=J.G.|last5=Salawitch|first5=R.J.|title=Impact of the Hunga Tonga volcanic eruption on stratospheric composition|journal=Proceedings of the National Academy of Sciences of the United States of America|volume=120|issue=46|id=Art. No. e2301994120|doi=10.1073/pnas.2301994120|doi-access=free|year=2023|pages=e2301994120 |pmid=37903247 |pmc=10655571}} The additional presence of hydrochloric acid in eruptions can result in net ozone depletion.

{{excerpt|Global dimming#History|paragraph=2}}

{{excerpt|Global dimming#Causes|paragraph=1|hat=no|files=no}}

File:Physical Drivers of climate change.svg, including the cooling provided by sulfate aerosols and the dimming they cause. The large error bar shows that there are still substantial unresolved uncertainties.]]

{{excerpt|Global dimming#Future|paragraphs=1,3|hat=no|files=no}}

File:SPICE SRM overview.jpg into the stratosphere]]

As the real world had shown the importance of sulfate aerosol concentrations to the global climate, research into the subject accelerated. Formation of the aerosols and their effects on the atmosphere can be studied in the lab, with methods like ion-chromatography and mass spectrometry{{Cite journal |last1=Kobayashi |first1=Yuya |last2=Ide |first2=Yu |last3=Takegawa |first3=Nobuyuki |date=3 April 2021 |title=Development of a novel particle mass spectrometer for online measurements of refractory sulfate aerosols |url=https://doi.org/10.1080/02786826.2020.1852168 |journal=Aerosol Science and Technology |volume=55 |issue=4 |pages=371–386 |doi=10.1080/02786826.2020.1852168 |bibcode=2021AerST..55..371K |s2cid=229506768 |issn=0278-6826}} Samples of actual particles can be recovered from the stratosphere using balloons or aircraft,{{cite journal |url=https://www.researchgate.net/publication/234296252_DUSTER_Aerosol_collection_in_the_stratosphere |journal=Societa Astronomica Italiana |title=The DUSTER experiment: collection and analysis of aerosol in the high stratosphere |author1=Palumbo, P. |author2= A. Rotundi |author3=V. Della Corte |author4=A. Ciucci |author5=L. Colangeli |author6=F. Esposito |author7=E. Mazzotta Epifani |author8=V. Mennella |author9=J.R. Brucato |author10=F.J.M. Rietmeijer |author11=G. J. Flynn |author12=J.-B. Renard |author13=J.R. Stephens |author14=E. Zona |access-date=19 February 2009 }} and remote satellites were also used for observation.{{Cite journal |last1=Myhre |first1=Gunnar |last2=Stordal |first2=Frode |last3=Berglen |first3=Tore F. |last4=Sundet |first4=Jostein K. |last5=Isaksen |first5=Ivar S. A. |date=1 March 2004 |title=Uncertainties in the Radiative Forcing Due to Sulfate Aerosols |journal=Journal of the Atmospheric Sciences |language=EN |volume=61 |issue=5 |pages=485–498 |doi=10.1175/1520-0469(2004)061<0485:UITRFD>2.0.CO;2 |bibcode=2004JAtS...61..485M |s2cid=55623817 |issn=0022-4928|doi-access=free }} This data is fed into the climate models,{{Cite journal |last1=Zhang |first1=Jie |last2=Furtado |first2=Kalli |last3=Turnock |first3=Steven T. |last4=Mulcahy |first4=Jane P. |last5=Wilcox |first5=Laura J. |last6=Booth |first6=Ben B. |last7=Sexton |first7=David |last8=Wu |first8=Tongwen |last9=Zhang |first9=Fang |last10=Liu |first10=Qianxia |date=22 December 2021 |title=The role of anthropogenic aerosols in the anomalous cooling from 1960 to 1990 in the CMIP6 Earth system models |url=https://acp.copernicus.org/articles/21/18609/2021/ |journal=Atmospheric Chemistry and Physics |volume=21 |issue=4 |pages=18609–18627 |language=en |doi=10.5194/acp-21-18609-2021 |bibcode=2021ACP....2118609Z |doi-access=free }} as the necessity of accounting for aerosol cooling to truly understand the rate and evolution of warming had long been apparent, with the IPCC Second Assessment Report being the first to include an estimate of their impact on climate, and every major model able to simulate them by the time IPCC Fourth Assessment Report was published in 2007.{{cite web|url=https://earthobservatory.nasa.gov/features/Aerosols/page3.php|title=Aerosols and Incoming Sunlight (Direct Effects)|publisher=NASA|date=2 November 2010}} Many scientists also see the other side of this research, which is learning how to cause the same effect artificially.{{cite web |url=https://www.sciencedaily.com/releases/2006/09/060914182715.htm |title=Stratospheric Injections Could Help Cool Earth, Computer Model Shows | access-date=19 February 2009 |publisher=ScienceDaily |date=15 September 2006 }} While discussed around the 1990s, if not earlier,{{cite journal |journal=Phil. Trans. R. Soc. A |year=1996 |volume=366 |pages=4039–56 |title=Global and Arctic climate engineering: numerical model studies |doi=10.1098/rsta.2008.0132 |author1=Launder B. |author2=J.M.T. Thompson |pmid=18757275 |issue=1882 |bibcode=2008RSPTA.366.4039C|doi-access=free }} stratospheric aerosol injection as a solar geoengineering method is best associated with Paul Crutzen's detailed 2006 proposal.{{Cite journal|last1=Crutzen|first1=P. J.|year=2006|title=Albedo Enhancement by Stratospheric Sulfur Injections: A Contribution to Resolve a Policy Dilemma?|journal=Climatic Change|volume=77|issue=3–4|pages=211–220|bibcode=2006ClCh...77..211C|doi=10.1007/s10584-006-9101-y|doi-access=free}} Deploying in the stratosphere ensures that the aerosols are at their most effective, and that the progress of clean air measures would not be reversed: more recent research estimated that even under the highest-emission scenario RCP 8.5, the addition of stratospheric sulfur required to avoid {{convert|4|C-change|F-change}} relative to now (and {{convert|5|C-change|F-change}} relative to the preindustrial) would be effectively offset by the future controls on tropospheric sulfate pollution, and the amount required would be even less for less drastic warming scenarios.{{Cite journal|last1=Visioni|first1=Daniele|last2=Slessarev|first2=Eric |last3=MacMartin|first3=Douglas G|last4=Mahowald|first4=Natalie M|last5=Goodale|first5=Christine L|last6=Xia|first6=Lili|date=1 September 2020|title=What goes up must come down: impacts of deposition in a sulfate geoengineering scenario|journal=Environmental Research Letters|volume=15|issue=9|pages=094063|doi=10.1088/1748-9326/ab94eb|bibcode=2020ERL....15i4063V|issn=1748-9326|doi-access=free}} This spurred a detailed look at its costs and benefits,{{cite web |url=http://www.met.reading.ac.uk/pg-research/downloads/2009/pgr-charlton.pdf |title=Costs and benefits of geo-engineering in the Stratosphere |author1=Andrew Charlton-Perez |author2=Eleanor Highwood |access-date=17 February 2009 |archive-date=14 January 2017 |archive-url=https://web.archive.org/web/20170114032949/http://www.met.reading.ac.uk/pg-research/downloads/2009/pgr-charlton.pdf |url-status=dead }} but even with hundreds of studies into the subject completed by the early 2020s, some notable uncertainties remain.{{Cite journal |last1=Trisos |first1=Christopher H. |last2=Geden |first2=Oliver |last3=Seneviratne |first3=Sonia I. |last4=Sugiyama |first4=Masahiro |last5=van Aalst |first5=Maarten |last6=Bala |first6=Govindasamy |last7=Mach |first7=Katharine J. |last8=Ginzburg |first8=Veronika |last9=de Coninck |first9=Heleen |last10=Patt |first10=Anthony |title=Cross-Working Group Box SRM: Solar Radiation Modification |url=https://www.ipcc.ch/report/ar6/wg2/downloads/report/IPCC_AR6_WGII_Chapter16.pdf |journal=Climate Change 2021: The Physical Science Basis. Contribution of Working Group I to the Sixth Assessment Report of the Intergovernmental Panel on Climate Change |year=2021 |volume=2021 |pages=1238 |doi=10.1017/9781009157896.007|bibcode=2021AGUFM.U13B..05K }}

Table of thermal and physical properties of saturated liquid sulfur dioxide:{{Cite book |last=Holman |first=Jack P. |title=Heat Transfer |publisher=McGraw-Hill Companies, Inc. |year=2002 |isbn=9780072406559 |edition=9th |location=New York, NY |pages=600–606 |language=English}}{{Cite book |last1=Incropera |last2=Dewitt |last3=Bergman |last4=Lavigne |first1=rank P. |first2=David P. |first3=Theodore L. |first4=Adrienne S. |title=Fundamentals of Heat and Mass Transfer |publisher=John Wiley and Sons, Inc. |year=2007 |isbn=9780471457282 |edition=6th |location=Hoboken, NJ |pages=941–950 |language=English}}

• Bunker fuel
• National Ambient Air Quality Standards
• Sulfur trioxide
• Sulfur–iodine cycle

{{Reflist|30em}}

{{Commons category|Sulfur dioxide|lcfirst=yes}}

• [https://earth.nullschool.net/#current/chem/surface/level/overlay=so2smass/winkel3 Global map of sulfur dioxide distribution]
• [https://www.epa.gov/so2-pollution United States Environmental Protection Agency Sulfur Dioxide page]
• [https://inchem.org/documents/icsc/icsc/eics0074.htm International Chemical Safety Card 0074]
• [https://web.archive.org/web/20090325155828/http://monographs.iarc.fr/ENG/Monographs/vol54/volume54.pdf IARC Monographs. "Sulfur Dioxide and some Sulfites, Bisulfites and Metabisulfites". vol. 54. 1992. p. 131.]
• [https://www.cdc.gov/niosh/npg/npgd0575.html NIOSH Pocket Guide to Chemical Hazards]
• [https://www.cdc.gov/niosh/topics/SulfurDioxide/ CDC – Sulfure Dioxide – NIOSH Workplace Safety and Health Topic]
• [http://www.chm.bris.ac.uk/motm/so2/so2h.htm Sulfur Dioxide, Molecule of the Month]

{{Oxides}}

{{Molecules detected in outer space}}

{{sulfur compounds}}

{{Authority control}}

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