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Sulfur dioxide
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Sulfur dioxide
Names
IUPAC name
Sulfur dioxide
Other names
Sulfurous anhydride
Sulfur(IV) oxide
Identifiers
CAS Number
7446-09-5 Y
3D model (JSmol)
Interactive image
Beilstein Reference
3535237
ChEBI
CHEBI:18422 Y
ChEMBL
ChEMBL1235997
ChemSpider
1087 Y
ECHA InfoCard 100.028.359
EC Number 231-195-2
E number E220 (preservatives)
Gmelin Reference
1443
KEGG
D05961 Y
MeSH Sulfur+dioxide
PubChem CID
1119
RTECS number WS4550000
UNII
0UZA3422Q4 Y
UN number 1079, 2037
InChI[show]
InChI=1S/O2S/c1-3-2 Y
Key: RAHZWNYVWXNFOC-UHFFFAOYSA-N Y
InChI=1/O2S/c1-3-2
Key: RAHZWNYVWXNFOC-UHFFFAOYAT
SMILES[show]
O=S=O
Properties
Chemical formula
SO
2
Molar mass 64.066 g mol−1
Appearance Colorless gas
Odor Pungent; similar to a just-struck match[1]
Density 2.6288 kg m−3
Melting point −72 °C; −98 °F; 201 K
Boiling point −10 °C (14 °F; 263 K)
Solubility in water
94 g/L[2]
forms sulfurous acid
Vapor pressure 237.2 kPa
Acidity (pKa) 1.81
Basicity (pKb) 12.19
Magnetic susceptibility (χ)
−18.2·10−6 cm3/mol
Viscosity 0.403 cP (at 0 °C)
Structure
Point group
C2v
Coordination geometry
Digonal
Molecular shape
Dihedral
Dipole moment
1.62 D
Thermochemistry
Std molar
entropy (So298)
248.223 J K−1 mol−1
Std enthalpy of
formation (ΔfHo298)
−296.81 kJ mol−1
Hazards
EU classification (DSD) (outdated)
T
R-phrases (outdated) R23, R34, R50
S-phrases (outdated) (S1/2), S9, S26, S36/37/39, S45
NFPA 704
0
3
0
Lethal dose or concentration (LD, LC):
LC50 (median concentration)
3000 ppm (mouse, 30 min)
2520 ppm (rat, 1 hr)[4]
LCLo (lowest published)
993 ppm (rat, 20 min)
611 ppm (rat, 5 hr)
764 ppm (mouse, 20 min)
1000 ppm (human, 10 min)
3000 ppm (human, 5 min)[4]
US health exposure limits (NIOSH):
PEL (Permissible)
TWA 5 ppm (13 mg/m3)[3]
REL (Recommended)
TWA 2 ppm (5 mg/m3) ST 5 ppm (13 mg/m3)[3]
IDLH (Immediate danger)
100 ppm[3]
Related compounds
Related sulfur oxides
Sulfur monoxide
Sulfur trioxide
Related compounds
Ozone
Selenium dioxide
Sulfurous acid
Tellurium dioxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
verify (what is Y ?)
Infobox references
Sulfur dioxide (also sulphur dioxide in British English) is the chemical compound with the formula SO
2. It is a toxic gas with a pungent, irritating smell. It is released naturally by volcanic activity and is produced as a by-product of the burning of fossil fuels contaminated with sulfur compounds.
Contents
[hide]
1 Structure and bonding
2 Occurrence
3 Production
3.1 Combustion routes
3.2 Reduction of higher oxides
3.3 From sulfite
4 Reactions
4.1 Industrial reactions
4.2 Laboratory reactions
5 Uses
5.1 Precursor to sulfuric acid
5.2 As a preservative
5.3 In winemaking
5.4 As a reducing agent
5.5 Biochemical and biomedical roles
5.6 As a refrigerant
5.7 As a reagent and solvent in the laboratory
5.8 Proposed use in climate engineering
6 As an air pollutant
7 Safety
7.1 Inhalation
7.2 Ingestion
8 See also
9 References
10 External links
Structure and bonding[edit]
SO2 is a bent molecule with C2v 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.
Two resonance structures of sulfur dioxide
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.[5] In terms of electron-counting formalism, the sulfur atom has an oxidation state of +4 and a formal charge of +1.
Occurrence[edit]
The blue auroral glows of Io's upper atmosphere are caused by volcanic sulfur dioxide.
It is found on Earth and exists in very small concentrations and in the atmosphere at about 1 ppm.[6][7][clarification needed]
On other planets, it can be found in various concentrations, the most significant being the atmosphere of Venus, where it is the third-most significant atmospheric gas at 150 ppm. There, it condenses to form clouds, and is a key component of chemical reactions in the planet's atmosphere and contributes to global warming.[8] 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,[9] 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 is 90% sulfur dioxide[10] and trace amounts are thought to also exist in the atmosphere of Jupiter.
As an ice, it is thought to exist in abundance on the Galilean moons—as sublimating ice or frost on the trailing hemisphere of Io, a natural satellite of Jupiter[11] and in the crust and mantle of Europa, Ganymede, and Callisto, possibly also in liquid form and readily reacting with water.[12]
Production[edit]
Sulfur dioxide is primarily produced for sulfuric acid manufacture (see contact process). In the United States in 1979, 23.6 million tonnes (26,014,547 US short tons) of sulfur dioxide were used in this way, compared with 150 thousand tonnes (165,347 US 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.[13]
Play media
An experiment showing burning of sulfur in oxygen. 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 a reaction.
Combustion routes[edit]
Sulfur dioxide is the product of the burning of sulfur or of burning materials that contain sulfur:
S + O2 → SO2, ΔH = −297 kJ/mol
To aid combustion, liquefied sulfur (140–150 °C, 284-302 °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 1000–1600 °C, 1832-2912 °F). The significant amount of heat produced is recovered by steam generation that can subsequently be converted to electricity.[13]
The combustion of hydrogen sulfide and organosulfur compounds proceeds similarly. For example:
2 H2S + 3 O2 → 2 H2O + 2 SO2
The roasting of sulfide ores such as pyrite, sphalerite, and cinnabar (mercury sulfide) also releases SO2:[14]
4 FeS2 + 11 O2 → 2 Fe2O3 + 8 SO2
2 ZnS + 3 O2 → 2 ZnO + 2 SO2
HgS + O2 → Hg + SO2
4 FeS + 7O2 → 2 Fe2O3 + 4 SO2
A combination of these reactions is responsible for the largest source of sulfur dioxide, volcanic eruptions. These events can release millions of tonnes of SO2.
Reduction of higher oxides[edit]
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 CaSO4 + 2 SiO2 + C → 2 CaSiO3 + 2 SO2 + 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.[15]
On a laboratory scale, the action of hot concentrated sulfuric acid on copper turnings produces sulfur dioxide.
Cu + 2 H2SO4 → CuSO4 + SO2 + 2 H2O
From sulfite[edit]
Sulfite results from the reaction of aqueous base and sulfur dioxide. The reverse reaction involves acidification of sodium metabisulfite:
H2SO4 + Na2S2O5 → 2 SO2 + Na2SO4 + H2O
Reactions[edit]
Industrial reactions[edit]
Treatment of basic solutions with sulfur dioxide affords sulfite salts (e.g. sodium sulfite):
SO2 + 2 NaOH → Na2SO3 + H2O
Featuring sulfur in the +4 oxidation state, sulfur dioxide is a reducing agent. It is oxidized by halogens to give the sulfuryl halides, such as sulfuryl chloride:
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:
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.
2 SO2 + 2 H2O + O2 → 2 H2SO4
Laboratory reactions[edit]
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.[citation needed]
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.
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.[16]
Uses[edit]
Precursor to sulfuric acid[edit]
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 billion kilograms are produced annually for this purpose.
As a preservative[edit]
Sulfur dioxide is sometimes used as a preservative for dried apricots, dried figs, and other dried fruits, owing to its antimicrobial properties, and is called E220[17] when used in this way in Europe. As a preservative, it maintains the colorful appearance of the fruit and prevents rotting. It is also added to sulfured molasses.
In winemaking[edit]
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.[18]
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.[19] 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.[20][21] 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]
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 the risk of cork taint,[22] 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.[23]
As a reducing agent[edit]
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.[24]
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+
Biochemical and biomedical roles[edit]
Sulfur dioxide is toxic in large amounts. It 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.[25] Sulfur dioxide blocks nerve signals from the pulmonary stretch receptors and abolishes the Hering–Breuer inflation reflex.
It was shown that endogenous sulfur dioxide plays a role in diminishing an experimental lung damage caused by oleic acid. Endogenous sulfur dioxide lowered lipid peroxidation, free radical formation, oxidative stress and inflammation during an experimental lung damage. Conversely, a successful lung damage caused a significant lowering of endogenous sulfur dioxide production, and an increase in lipid peroxidation, free radical formation, oxidative stress and inflammation. Moreover, blockade of an enzyme that produces endogenous SO2 significantly increased the amount of lung tissue damage in the experiment. Conversely, adding acetylcysteine or glutathione to the rat diet increased the amount of endogenous SO2 produced and decreased the lung damage, the free radical formation, oxidative stress, inflammation and apoptosis.[26]
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, stenocardia.[27]
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.[28]
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.[29] 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.[30]
Endogenous sulfur dioxide also diminishes myocardial damage, caused by isoproterenol adrenergic hyperstimulation, and strengthens the myocardial antioxidant defense reserve.[31]
As a refrigerant[edit]
Being easily condensed and possessing a high heat of evaporation, sulfur dioxide is a candidate material for refrigerants. Prior to the development of chlorofluorocarbons, sulfur dioxide was used as a refrigerant in home refrigerators.
As a reagent and solvent in the laboratory[edit]
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:[32]
Proposed use in climate engineering[edit]
Injections of sulfur dioxide in the stratosphere has been proposed in climate engineering. The cooling effect would be similar to what has been observed after the large explosive volcano eruption of Mount Pinatubo in 1991. However this form of geoengineering would have uncertain regional consequences on rainfall patterns, for example in monsoon regions.[33]
As an air pollutant[edit]
A sulfur dioxide plume from the Halemaʻumaʻu vent, glows at night
Sulfur dioxide is a noticeable component in the atmosphere, especially following volcanic eruptions.[34] According to the United States Environmental Protection Agency,[35] the amount of sulfur dioxide released in the U.S. per year was:
A collection of estimates of past and future anthropogenic global sulphur dioxide emissions. The Cofala et al. estimates are for sensitivity studies on SO2 emission policies, CLE: Current Legislation, MFR: Maximum Feasible Reductions. RCPs (Representative Concentration Pathways) are used in CMIP5 simulations for latest (2013–2014) IPCC 5th assessment report.
Year
SO2
1970 31,161,000 short tons (28.3 Mt)
1980 25,905,000 short tons (23.5 Mt)
1990 23,678,000 short tons (21.5 Mt)
1996 18,859,000 short tons (17.1 Mt)
1997 19,363,000 short tons (17.6 Mt)
1998 19,491,000 short tons (17.7 Mt)
1999 18,867,000 short tons (17.1 Mt)
Sulfur dioxide is a major air pollutant and has significant impacts upon human health.[36] In addition, the concentration of sulfur dioxide in the atmosphere can influence the habitat suitability for plant communities, as well as animal life.[37] Sulfur dioxide emissions are a precursor to acid rain and atmospheric particulates. Due largely to the US EPA’s Acid Rain Program, the U.S. has had a 33% decrease in emissions between 1983 and 2002. 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 oil. 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.
Sulfur can be removed from coal during burning by using limestone as a bed material in fluidized bed combustion.[38]
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[39] or Sulferox.[40]
Sulfur dioxide in the world on April 15th, 2017. Note that sulfur dioxide moves through the atmosphere with prevailing winds and thus local sulfur dioxide distributions vary day to day with weather patterns and seasonality.
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.[41]
As of 2006, China was the world's largest sulfur dioxide polluter, with 2005 emissions estimated to be 25,490,000 short tons (23.1 Mt). This amount represents a 27% increase since 2000, and is roughly comparable with U.S. emissions in 1980.[42]
Safety[edit]
Inhalation[edit]
Inhaling sulfur dioxide is associated with increased respiratory symptoms and disease, difficulty in breathing, and premature death.[43] In 2008, the American Conference of Governmental Industrial Hygienists reduced the short-term exposure limit to 0.25 parts per million (ppm). The OSHA PEL is currently set at 5 ppm (13 mg/m3) time-weighted average. NIOSH has set the IDLH at 100 ppm.[44] 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."[45]
A 2011 systematic review concluded that exposure to sulfur dioxide is associated with preterm birth.[46]
Ingestion[edit]
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.[47] Symptoms of sensitivity to sulfiting agents, including sulfur dioxide, manifest as potentially life-threatening trouble breathing within minutes of ingestion.[48]
See also[edit]
Sulfur trioxide
Sulfur–iodine cycle
National Ambient Air Quality Standards
References[edit]
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Jump up ^ "NIOSH Pocket Guide to Chemical Hazards".
Jump up ^ http://www.epa.gov/airquality/sulfurdioxide/
Jump up ^ Shah PS, Balkhair T, Knowledge Synthesis Group on Determinants of Preterm/LBW Births (2011). "Air pollution and birth outcomes: a systematic review". Environ Int. 37 (2): 498–516. doi:10.1016/j.envint.2010.10.009. PMID 21112090. CS1 maint: Multiple names: authors list (link)
Jump up ^ "Center for Science in the Public Interest – Chemical Cuisine". Retrieved March 17, 2010.
Jump up ^ "California Department of Public Health: Food and Drug Branch: Sulfites" (PDF). Archived from the original (PDF) on July 23, 2012. Retrieved September 27, 2013.
External links[edit]
Wikimedia Commons has media related to sulfur dioxide.
Global map of sulfur dioxide distribution
United States Environmental Protection Agency Sulfur Dioxide page
International Chemical Safety Card 0074
IARC Monographs. "Sulfur Dioxide and some Sulfites, Bisulfites and Metabisulfites" v54. 1992. p131.
NIOSH Pocket Guide to Chemical Hazards
CDC – Sulfure Dioxide – NIOSH Workplace Safety and Health Topic
Sulfur Dioxide, Molecule of the Month
[show]
v
t
e
Oxides
Mixed oxidation states
Antimony tetroxide (Sb2O4)
Cobalt(II,III) oxide (Co3O4)
Europium(II,III) oxide (Eu3O4)
Iron(II,III) oxide (Fe3O4)
Lead(II,IV) oxide (Pb3O4)
Manganese(II,III) oxide (Mn3O4)
Silver(I,III) oxide (Ag2O2)
Triuranium octoxide (U3O8)
Carbon suboxide (C3O2)
Mellitic anhydride (C12O9)
Praseodymium(III,IV) oxide (Pr6O11)
Terbium(III,IV) oxide (Tb4O7)
+1 oxidation state
Copper(I) oxide (Cu2O)
Dicarbon monoxide (C2O)
Dichlorine monoxide (Cl2O)
Gallium(I) oxide (Ga2O)
Lithium oxide (Li2O)
Potassium oxide (K2O)
Rubidium oxide (Rb2O)
Silver oxide (Ag2O)
Thallium(I) oxide (Tl2O)
Sodium oxide (Na2O)
Water (hydrogen oxide) (H2O)
+2 oxidation state
Aluminium(II) oxide (AlO)
Barium oxide (BaO)
Beryllium oxide (BeO)
Cadmium oxide (CdO)
Calcium oxide (CaO)
Carbon monoxide (CO)
Chromium(II) oxide (CrO)
Cobalt(II) oxide (CoO)
Copper(II) oxide (CuO)
Europium(II) oxide (EuO)
Germanium monoxide (GeO))
Iron(II) oxide (FeO)
Lead(II) oxide (PbO)
Magnesium oxide (MgO)
Manganese(II) oxide (MnO)
Mercury(II) oxide (HgO)
Nickel(II) oxide (NiO)
Nitric oxide (NO)
Palladium(II) oxide (PdO)
Silicon monoxide (SiO)
Strontium oxide (SrO)
Sulfur monoxide (SO)
Disulfur dioxide (S2O2)
Tin(II) oxide (SnO)
Titanium(II) oxide (TiO)
Vanadium(II) oxide (VO)
Zinc oxide (ZnO)
+3 oxidation state
Aluminium oxide (Al2O3)
Antimony trioxide (Sb2O3)
Arsenic trioxide (As2O3)
Bismuth(III) oxide (Bi2O3)
Boron trioxide (B2O3)
Cerium(III) oxide (Ce2O3)
Dibromine trioxide (Br2O3)
Chromium(III) oxide (Cr2O3)
Dinitrogen trioxide (N2O3)
Dysprosium(III) oxide (Dy2O3)
Erbium(III) oxide (Er2O3)
Europium(III) oxide (Eu2O3)
Gadolinium(III) oxide (Gd2O3)
Gallium(III) oxide (Ga2O3)
Holmium(III) oxide (Ho2O3)
Indium(III) oxide (In2O3)
Iron(III) oxide (Fe2O3)
Lanthanum oxide (La2O3)
Lutetium(III) oxide (Lu2O3)
Manganese(III) oxide (Mn2O3)
Neodymium(III) oxide (Nd2O3)
Nickel(III) oxide (Ni2O3)
Phosphorus trioxide (P4O6)
Praseodymium(III) oxide (Pr2O3)
Promethium(III) oxide (Pm2O3)
Rhodium(III) oxide (Rh2O3)
Samarium(III) oxide (Sm2O3)
Scandium oxide (Sc2O3)
Terbium(III) oxide (Tb2O3)
Thallium(III) oxide (Tl2O3)
Thulium(III) oxide (Tm2O3)
Titanium(III) oxide (Ti2O3)
Tungsten(III) oxide (W2O3)
Vanadium(III) oxide (V2O3)
Ytterbium(III) oxide (Yb2O3)
Yttrium(III) oxide (Y2O3)
+4 oxidation state
Americium dioxide (AmO2)
Carbon dioxide (CO2)
Carbon trioxide (CO3)
Cerium(IV) oxide (CeO2)
Chlorine dioxide (ClO2)
Chromium(IV) oxide (CrO2)
Dinitrogen tetroxide (N2O4)
Germanium dioxide (GeO2)
Hafnium(IV) oxide (HfO2)
Lead dioxide (PbO2)
Manganese dioxide (MnO2)
Neptunium(IV) oxide (NpO2)
Nitrogen dioxide (NO2)
Osmium dioxide (OsO2)
Plutonium(IV) oxide (PuO2)
Praseodymium(IV) oxide (PrO2)
Protactinium(IV) oxide (PaO2)
Rhodium(IV) oxide (RhO2)
Ruthenium(IV) oxide (RuO2)
Selenium dioxide (SeO2)
Silicon dioxide (SiO2)
Sulfur dioxide (SO2)
Tellurium dioxide (TeO2)
Terbium(IV) oxide (TbO2)
Thorium dioxide (ThO2)
Tin dioxide (SnO2)
Titanium dioxide (TiO2)
Tungsten(IV) oxide (WO2)
Uranium dioxide (UO2)
Vanadium(IV) oxide (VO2)
Zirconium dioxide (ZrO2)
+5 oxidation state
Antimony pentoxide (Sb2O5)
Arsenic pentoxide (As2O5)
Dinitrogen pentoxide (N2O5)
Niobium pentoxide (Nb2O5)
Phosphorus pentoxide (P2O5)
Protactinium(V) oxide (Pa2O5)
Tantalum pentoxide (Ta2O5)
Vanadium(V) oxide (V2O5)
+6 oxidation state
Chromium trioxide (CrO3)
Molybdenum trioxide (MoO3)
Rhenium trioxide (ReO3)
Selenium trioxide (SeO3)
Sulfur trioxide (SO3)
Tellurium trioxide (TeO3)
Tungsten trioxide (WO3)
Uranium trioxide (UO3)
Xenon trioxide (XeO3)
Iridium trioxide (IrO3)
+7 oxidation state
Dichlorine heptoxide (Cl2O7)
Manganese heptoxide (Mn2O7)
Rhenium(VII) oxide (Re2O7)
Technetium(VII) oxide (Tc2O7)
+8 oxidation state
Osmium tetroxide (OsO4)
Ruthenium tetroxide (RuO4)
Xenon tetroxide (XeO4)
Iridium tetroxide (IrO4)
Hassium tetroxide (HsO4)
Related
Oxocarbon
Suboxide
Oxyanion
Ozonide
Peroxide
Superoxide
Oxides are sorted by oxidation state. Category:Oxides
[show]
v
t
e
Molecules detected in outer space
Molecules
Diatomic
Aluminium monochloride
Aluminium monofluoride
Aluminium monoxide
Argonium
Carbon monophosphide
Carbon monosulfide
Carbon monoxide
Carborundum
Cyanogen radical
Diatomic carbon
Fluoromethylidynium
Hydrogen chloride
Hydrogen fluoride
Hydrogen (molecular)
Hydroxyl radical
Iron(II) oxide
Magnesium monohydride cation
Methylidyne radical
Nitric oxide
Nitrogen (molecular)
Nitrogen monohydride
Nitrogen sulfide
Oxygen (molecular)
Phosphorus monoxide
Phosphorus mononitride
Potassium chloride
Silicon carbide
Silicon mononitride
Silicon monoxide
Silicon monosulfide
Sodium chloride
Sodium iodide
Sulfur monohydride
Sulfur monoxide
Titanium oxide

Triatomic
Aluminium hydroxide
Aluminium isocyanide
Amino radical
Carbon dioxide
Carbonyl sulfide
CCP radical
Chloronium
Diazenylium
Dicarbon monoxide
Disilicon carbide
Ethynyl radical
Formyl radical
Hydrogen cyanide (HCN)
Hydrogen isocyanide (HNC)
Hydrogen sulfide
Hydroperoxyl
Iron cyanide
Isoformyl
Magnesium cyanide
Magnesium isocyanide
Methylene radical
N2H+
Nitrous oxide
Nitroxyl
Ozone
Phosphaethyne
Potassium cyanide
Protonated molecular hydrogen
Sodium cyanide
Sodium hydroxide
Silicon carbonitride
c-Silicon dicarbide
Silicon naphthalocyanine
Sulfur dioxide
Thioformyl
Thioxoethenylidene
Titanium dioxide
Tricarbon
Water
Four
atoms
Acetylene
Ammonia
Cyanic acid
Cyanoethynyl
Cyclopropynylidyne
Formaldehyde
Fulminic acid
HCCN
Hydrogen peroxide
Hydromagnesium isocyanide
Isocyanic acid
Isothiocyanic acid
Ketenyl
Methylene amidogen
Methyl radical
Propynylidyne
Protonated carbon dioxide
Protonated hydrogen cyanide
Silicon tricarbide
Thioformaldehyde
Tricarbon monoxide
Tricarbon sulfide
Thiocyanic acid
Five
atoms
Ammonium ion
Butadiynyl
Carbodiimide
Cyanamide
Cyanoacetylene
Cyanoformaldehyde
Cyanomethyl
Cyclopropenylidene
Formic acid
Isocyanoacetylene
Ketene
Methane
Methoxy radical
Methylenimine
Propadienylidene
Protonated formaldehyde
Protonated formaldehyde
Silane
Silicon-carbide cluster
Six
atoms
Acetonitrile
Cyanobutadiynyl radical
E-Cyanomethanimine
Cyclopropenone
Diacetylene
Ethylene
Formamide
HC4N
Ketenimine
Methanethiol
Methanol
Methyl isocyanide
Pentynylidyne
Propynal
Protonated cyanoacetylene
Seven
atoms
Acetaldehyde
Acrylonitrile
Vinyl cyanide
Cyanodiacetylene
Ethylene oxide
Hexatriynyl radical
Methylacetylene
Methylamine
Methyl isocyanate
Vinyl alcohol
Eight
atoms
Acetic acid
Aminoacetonitrile
Cyanoallene
Ethanimine
Glycolaldehyde
Heptatrienyl radical
Hexapentaenylidene
Methylcyanoacetylene
Methyl formate
Propenal
Nine
atoms
Acetamide
Cyanohexatriyne
Cyanotriacetylene
Dimethyl ether
Ethanol
Methyldiacetylene
Octatetraynyl radical
Propene
Propionitrile
Ten
atoms
or more
Acetone
Benzene
Benzonitrile
Buckminsterfullerene (C60 fullerene, buckyball)
C70 fullerene
Cyanodecapentayne
Cyanopentaacetylene
Cyanotetra-acetylene
Ethylene glycol
Ethyl formate
Methyl acetate
Methyl-cyano-diacetylene
Methyltriacetylene
Propanal
n-Propyl cyanide
Pyrimidine
Deuterated
molecules
Ammonia
Ammonium ion
Formaldehyde
Formyl radical
Heavy water
Hydrogen cyanide
Hydrogen deuteride
Hydrogen isocyanide
Methylacetylene
N2D+
Trihydrogen cation
Unconfirmed
Anthracene
Dihydroxyacetone
Ethyl methyl ether
Glycine
Graphene
H2NCO+
Linear C5
Naphthalene cation
Phosphine
Pyrene
Silylidine
Related
Abiogenesis
Astrobiology
Astrochemistry
Atomic and molecular astrophysics
Chemical formula
Circumstellar envelope
Cosmic dust
Cosmic ray
Cosmochemistry
Diffuse interstellar band
Earliest known life forms
Extraterrestrial life
Extraterrestrial liquid water
Forbidden mechanism
Helium hydride ion
Homochirality
Intergalactic dust
Interplanetary medium
Interstellar medium
Photodissociation region
Iron–sulfur world theory
Kerogen
Molecules in stars
Nexus for Exoplanet System Science
Organic compound
Outer space
PAH world hypothesis
Panspermia
Polycyclic aromatic hydrocarbon (PAH)
RNA world hypothesis
Spectroscopy
Tholin
Book:Chemistry
Category:Astrochemistry
Category:Molecules
Portal:Astrobiology
Portal:Astronomy
Portal:Chemistry
[show]
v
t
e
Sulfur compounds
Al2S3
As2S2
As2S3
As5S2
As4S4
Au2S3
B2S3
BaS
BeS
Bi2S3
Br2S
Br2S2
CS2
C3S2
CaS
CdS
CeS
SCl2
S2Cl2
CoS
Cr2S3
CuS
D2S
Dy2S3
Er2S3
EuS
SF4
SF6
FeS2
GaS
H2S
HfS2
HgS
InS
I2S
LaS
LiS
MgS
MoS3
NiS
SO2
SO3
P4S7
PbS
PbS2
PtS
ReS2
SrS
TlS
SV
SeS2
S2U
WS2
Sb2S3
Sb2S5
Sm2S3
Y2S3
Ag2SO4
SOBr2
CSTe
C2H4S
C2H6S3
C4H4S
CaSO4
C32H66S2
CuFeS2
H2SO4
H2SO3
F2OS
NaHS
K2SO3
O3S3Sb4
Yb2(SO4)3
AlKO8S2
CHCl3S
KSCN
CdSO3
PSCl3
SOCl2
Cs2O4S
Re2S7
Na2S
K2S
H2S2O7
H2SO5
NH5S
HgSO4
K2SO4
RaSO4
SnSO4
SrSO4
Zr(SO4)2
Ti(SO4)2
Tm2(SO4)3
AlNa(SO4)2
Er2(SO4)3
Eu2(SO4)3
CHNS
Co(SCN)2
C2H3SN
PSI3
ZrS2
SiS
CSSe
Chemical formulas
Authority control
GND: 4180392-9
NDL: 00568537
Retrieved from "https://en.wikipedia.org/w/index.php?title=Sulfur_dioxide&oldid=843187743"
Categories:
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values: Flammability code 0: Will not burn. E.g., water

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Diazonium salt

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text:
Have Some Madeira M'Dear
From Wikipedia, the free encyclopedia
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"Have Some Madeira M'Dear"
Writers Flanders and Swann
Song by Flanders and Swann
Genre
Novelty song
Composer(s)
Michael Flanders
Lyricist(s)
Donald Swann
"Have Some Madeira M'Dear", also titled "Madeira, M'Dear?",[n 1] is a darkly comic song by Flanders and Swann.[2] It is a song about seduction and alcohol, containing complex and witty wordplay.
Madeira wine
The lyrics[3] tell of an elderly rake who "slyly inveigles" an attractive young girl of seventeen to his flat where he offers her a glass of Madeira, a fortified Portuguese wine. The girl enthusiastically drains her glass, becoming slightly drunk in the process. Sensing victory, the rake offers the young girl another glass of wine, which she accepts. However, before raising it to her lips, she recalls her dying mother's warning to avoid red wine. With a cry, the girl drops the glass and flees the apartment, the old roué's pleas for her to remain echoing in her ears. The following morning, however, the young lady awakens in bed with a hangover and a beard tickling her ear.
The song contains three much-quoted instances of syllepsis:[4][5] "And he said as he hastened to put out the cat, the wine, his cigar and the lamps" "She lowered her standards by raising her glass, her courage, her eyes and his hopes" "She made no reply, up her mind and a dash for the door."[6]
The song has been covered by other groups, including most notably The Limeliters (performed by Lou Gottlieb). The lyrics were also recited as a poem by Tony Randall in episode #922 of The Carol Burnett Show which first aired 02/21/1976.
Sam Leith has referred to it as a "hilarious song about date rape".[7]
Notes and references[edit]
Notes
Jump up ^ The shorter title is used on the original LP records of the show; the longer is adopted in the 1977 collected songs of Flanders and Swann, edited by Flanders's widow Claudia.[1]
References
Jump up ^ Parlophone LPs PMC 1033 (1957) and PCS 3001 (1959); and Flanders and Swann, p. 143
Jump up ^ Blocker, Jack S.; David M. Fahey; Ian R. Tyrrell (2003). Alcohol and temperance in modern history: an international encyclopedia, Volume 1. ABC-CLIO. p. 210. ISBN 978-1-57607-833-4.
Jump up ^ http://sniff.numachi.com/pages/tiMADERA.html
Jump up ^ Oliver, A. (2001). "Strategies for a Logic of Plurals". The Philosophical Quarterly. 51 (204): 289. doi:10.1111/j.0031-8094.2001.00231.x.
Jump up ^ Everett, Anthony (2005). "Recent Defenses of Descriptivism". Mind & Language. 20: 103. doi:10.1111/j.0268-1064.2005.00279.x.
Jump up ^ Flanders and Swann, pp. 143–145
Jump up ^ You Talkin' To Me?: Rhetoric from Aristotle to Obama, by Sam Leith; published Oct 20, 2011, by Profile Books; via Google Books
Sources[edit]
Flanders, Michael; Donald Swann; Claudia Flanders (1977). The Songs of Michael Flanders and Donald Swann. London: Elm Tree Books and Saint George's Press. ISBN 0241897386.
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"Have Some Madeira M'Dear"
Retrieved from "https://en.wikipedia.org/w/index.php?title=Have_Some_Madeira_M%27Dear&oldid=854684351"
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