Dimethyl sulfoxide

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Dimethyl sulfoxide
DMSO-2D-dimensions.svg
Stereo structural formula of dimethyl sulfoxide with an explicit electron pair and assorted dimensions Dimethyl-sulfoxide-3D-balls-A.png
Stereo structural formula of dimethyl sulfoxide with an explicit electron pair and assorted dimensions
Spacefill model of dimethyl sulfoxide DMSO-3D-vdW.png
Spacefill model of dimethyl sulfoxide
Sample of Dimethyl sulfoxide 01.jpg
A sample of dimethyl sulfoxide
Names
Preferred IUPAC name
(Methanesulfinyl)methane
Systematic IUPAC name
(Methanesulfinyl)methane (substitutive)
Dimethyl(oxido)sulfur (additive)
Other names
Methylsulfinylmethane
Methyl sulfoxide (2:1), Dermasorb [1]
Identifiers
3D model (JSmol)
AbbreviationsDMSO, Me2SO
506008
ChEBI
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.000.604 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 200-664-3
1556
KEGG
MeSH Dimethyl+sulfoxide
PubChem CID
RTECS number
  • PV6210000
UNII
  • InChI=1S/C2H6OS/c1-4(2)3/h1-2H3 Yes check.svgY
    Key: IAZDPXIOMUYVGZ-UHFFFAOYSA-N Yes check.svgY
  • InChI=1/C2H6OS/c1-4(2)3/h1-2H3
    Key: IAZDPXIOMUYVGZ-UHFFFAOYAR
  • CS(=O)C
  • CS(C)=O
Properties
C2H6OS
Molar mass 78.13 g·mol−1
AppearanceColourless liquid
Density 1.1004 g⋅cm−3
Melting point 19 °C (66 °F; 292 K)
Boiling point 189 °C (372 °F; 462 K)
Miscible
Solubility in Diethyl ether Not soluble
Vapor pressure 0.556 millibars or 0.0556 kPa at 20 °C [2]
Acidity (pKa)35 [3]
1.479
εr = 48
Viscosity 1.996  cP at 20 °C
Structure
Cs
Trigonal pyramidal
3.96  D
Pharmacology
G04BX13 ( WHO ) M02AX03 ( WHO )
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Irritant
NFPA 704 (fire diamond)
NFPA 704.svgHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 2: Must be moderately heated or exposed to relatively high ambient temperature before ignition can occur. Flash point between 38 and 93 °C (100 and 200 °F). E.g. diesel fuelInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
2
0
Flash point 89 °C (192 °F; 362 K)
Safety data sheet (SDS) Oxford MSDS
Related compounds
Related sulfoxides
Diethyl sulfoxide
Related compounds
Supplementary data page
Dimethyl sulfoxide (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Yes check.svgY  verify  (what is  Yes check.svgYX mark.svgN ?)

Dimethyl sulfoxide (DMSO) is an organosulfur compound with the formula (CH3)2 S O . This colorless liquid is the sulfoxide most widely used commercially. It is an important polar aprotic solvent that dissolves both polar and nonpolar compounds and is miscible in a wide range of organic solvents as well as water. It has a relatively high boiling point. DMSO is metabolised to compounds that leave a garlic-like taste in the mouth after DMSO is absorbed by skin. [4]

Contents

In terms of chemical structure, the molecule has idealized Cs symmetry. It has a trigonal pyramidal molecular geometry consistent with other three-coordinate S(IV) compounds, [5] with a nonbonded electron pair on the approximately tetrahedral sulfur atom.

Synthesis and production

Dimethyl sulfoxide was first synthesized in 1866 by the Russian scientist Alexander Zaytsev, who reported his findings in 1867. [6] Its modern use as an industrial solvent began through popularization by Thor Smedslund at the Stepan Chemical Company. [7] Dimethyl sulfoxide is produced industrially from dimethyl sulfide, a by-product of the Kraft process, by oxidation with oxygen or nitrogen dioxide. [8]

Reactions

Reactions with electrophiles

The sulfur center in DMSO is nucleophilic toward soft electrophiles and the oxygen is nucleophilic toward hard electrophiles. With methyl iodide it forms trimethylsulfoxonium iodide, [(CH3)3SO]I:

(CH3)2SO + CH3I → [(CH3)3SO]I

This salt can be deprotonated with sodium hydride to form the sulfur ylide:

[(CH3)3SO]I + NaH → (CH3)2S(CH2)O + NaI + H2

Acidity

The methyl groups of DMSO are only weakly acidic, with a pKa = 35. For this reason, the basicities of many weakly basic organic compounds have been examined in this solvent.

Deprotonation of DMSO requires strong bases like lithium diisopropylamide and sodium hydride. Stabilization of the resultant carbanion is provided by the S(O)R group. The sodium derivative of DMSO formed in this way is referred to as dimsyl sodium . It is a base, e.g., for the deprotonation of ketones to form sodium enolates, phosphonium salts to form Wittig reagents, and formamidinium salts to form diaminocarbenes. It is also a potent nucleophile.

Oxidant

In organic synthesis, DMSO is used as a mild oxidant. [9] It forms the basis of several selective sulfonium-based oxidation reactions including the Pfitzner–Moffatt oxidation, Corey–Kim oxidation and the Swern oxidation. [10] The Kornblum oxidation is conceptually similar. These all involve formation of an intermediate sulfonium species (R2S+X where X is a heteroatom)

Ligand and Lewis base

Related to its ability to dissolve many salts, DMSO is a common ligand in coordination chemistry. [11] Illustrative is the complex dichlorotetrakis(dimethyl sulfoxide)ruthenium(II) (RuCl2(dmso)4). In this complex, three DMSO ligands are bonded to ruthenium through sulfur. The fourth DMSO is bonded through oxygen. In general, the oxygen-bonded mode is more common.

In carbon tetrachloride solutions DMSO functions as a Lewis base with a variety of Lewis acids such as I2, phenols, trimethyltin chloride, metalloporphyrins, and the dimer Rh2Cl2(CO)4. The donor properties are discussed in the ECW model. The relative donor strength of DMSO toward a series of acids, versus other Lewis bases, can be illustrated by C-B plots. [12] [13]

Applications

Solvent

Distillation of DMSO requires a partial vacuum to achieve a lower boiling point. Vacuum distillation of DMSO at 70C.jpg
Distillation of DMSO requires a partial vacuum to achieve a lower boiling point.

DMSO is a polar aprotic solvent and is less toxic than other members of this class, such as dimethylformamide, dimethylacetamide, N-methyl-2-pyrrolidone, and hexamethylphosphoramide (HMPA). DMSO is frequently used as a solvent for chemical reactions involving salts, most notably Finkelstein reactions and other nucleophilic substitutions. It is also extensively used as an extractant in biochemistry and cell biology. [14] Because DMSO is only weakly acidic, it tolerates relatively strong bases and as such has been extensively used in the study of carbanions. A set of non-aqueous pKa values (C-H, O-H, S-H and N-H acidities) for thousands of organic compounds have been determined in DMSO solution. [15] [16]

Because of its high boiling point, 189 °C (372 °F), DMSO evaporates slowly at normal atmospheric pressure. Samples dissolved in DMSO cannot as easily be recovered compared to other solvents, as it is very difficult to remove all traces of DMSO by conventional rotary evaporation. One technique to fully recover samples is removal of the organic solvent by evaporation followed by addition of water (to dissolve DMSO) and cryodesiccation to remove both DMSO and water. Reactions conducted in DMSO are often diluted with water to precipitate or phase-separate products. The relatively high freezing point of DMSO, 18.5 °C (65.3 °F), means that at, or just below, room temperature it is a solid, which can limit its utility in some chemical processes (e.g. crystallization with cooling).

In its deuterated form (DMSO-d6), it is a useful solvent for NMR spectroscopy, again due to its ability to dissolve a wide range of analytes, the simplicity of its own spectrum, and its suitability for high-temperature NMR spectroscopic studies. Disadvantages to the use of DMSO-d6 are its high viscosity, which broadens signals, and its hygroscopicity, which leads to an overwhelming H2O resonance in the 1H-NMR spectrum. It is often mixed with CDCl3 or CD2Cl2 for lower viscosity and melting points.

MIC microbroth dilution.jpg
Lightmatter lab mice.jpg
DMSO is used as a solvent in in vitro and in vivo drug testing.

DMSO is used to dissolve test compounds in in vitro drug discovery [17] [18] and drug design [19] screening programs, including high-throughput screening programs. [18] [19] This is because it is able to dissolve both polar and nonpolar compounds, [17] [19] can be used to maintain stock solutions of test compounds (important when working with a large chemical library), [18] is readily miscible with water and cell culture media, and has a high boiling point (this improves the accuracy of test compound concentrations by reducing room temperature evaporation). [17] One limitation with DMSO is that it can affect cell line growth and viability, with low DMSO concentrations sometimes stimulating cell growth, and high DMSO concentrations sometimes inhibiting or killing cells. [17]

DMSO is used as a vehicle in in vivo studies of test compounds. It has, for example, been employed as a co-solvent to assist absorption of the flavonol glycoside Icariin in the nematode worm Caenorhabditis elegans . [20] As with its use in in vitro studies, DMSO has some limitations in animal models. [21] [22] Pleiotropic effects can occur and, if DMSO control groups are not carefully planned, then solvent effects can falsely be attributed to the prospective drug. [21] For example, even a very low dose of DMSO has a powerful protective effect against paracetamol (acetaminophen)-induced liver injury in mice. [22]

DMSO is finding increased use in manufacturing processes to produce microelectronic devices. [23] It is widely used to strip photoresist in TFT-LCD 'flat panel' displays and advanced packaging applications (such as wafer-level packaging / solder bump patterning). DMSO is an effective paint stripper, being safer than many of the others such as nitromethane and dichloromethane.

Biology

DMSO is used in polymerase chain reaction (PCR) to inhibit secondary structures in the DNA template or the DNA primers. It is added to the PCR mix before reacting, where it interferes with the self-complementarity of the DNA, minimizing interfering reactions. [24]

DMSO in a PCR is applicable for supercoiled plasmids (to relax before amplification) or DNA templates with high GC-content (to decrease thermostability). For example, 10% final concentration of DMSO in the PCR mixture with Phusion decreases primer annealing temperature (i.e. primer melting temperature) by 5.5–6.0 °C (9.9–10.8 °F). [25]

It is well known as a reversible cell cycle arrester at phase G1 of human lymphoid cells. [26]

DMSO may also be used as a cryoprotectant, added to cell media to reduce ice formation and thereby prevent cell death during the freezing process. [27] Approximately 10% may be used with a slow-freeze method, and the cells may be frozen at −80 °C (−112 °F) or stored in liquid nitrogen safely.

In cell culture, DMSO is used to induce differentiation of P19 embryonic carcinoma cells into cardiomyocytes and skeletal muscle cells.

Medicine

Use of DMSO in medicine dates from around 1963, when an Oregon Health & Science University Medical School team, headed by Stanley Jacob, discovered it could penetrate the skin and other membranes without damaging them and could carry other compounds into a biological system. In medicine, DMSO is predominantly used as a topical analgesic, a vehicle for topical application of pharmaceuticals, as an anti-inflammatory, and an antioxidant. [28] Because DMSO increases the rate of absorption of some compounds through biological tissues, including skin, it is used in some transdermal drug delivery systems. Its effect may be enhanced with the addition of EDTA. It is frequently compounded with antifungal medications, enabling them to penetrate not just skin but also toenails and fingernails. [29]

DMSO has been examined for the treatment of numerous conditions and ailments, but the U.S. Food and Drug Administration (FDA) has approved its use only for the symptomatic relief of patients with interstitial cystitis. [30] A 1978 study concluded that DMSO brought significant relief to the majority of the 213 patients with inflammatory genitourinary disorders that were studied. [31] The authors recommended DMSO for genitourinary inflammatory conditions not caused by infection or tumor in which symptoms were severe or patients failed to respond to conventional therapy.

In interventional radiology, DMSO is used as a solvent for ethylene vinyl alcohol in the Onyx liquid embolic agent, which is used in embolization, the therapeutic occlusion of blood vessels.

In cryobiology DMSO has been used as a cryoprotectant and is still an important constituent of cryoprotectant vitrification mixtures used to preserve organs, tissues, and cell suspensions. Without it, up to 90% of frozen cells will become inactive. It is particularly important in the freezing and long-term storage of embryonic stem cells and hematopoietic stem cells, which are often frozen in a mixture of 10% DMSO, a freezing medium, and 30% fetal bovine serum. In the cryogenic freezing of heteroploid cell lines (MDCK, VERO, etc.) a mixture of 10% DMSO with 90%  EMEM (70% EMEM + 30% fetal bovine serum + antibiotic mixture) is used. As part of an autologous bone marrow transplant the DMSO is re-infused along with the patient's own hematopoietic stem cells.

DMSO is metabolized by disproportionation to dimethyl sulfide and dimethyl sulfone. It is subject to renal and pulmonary excretion. A possible side effect of DMSO is therefore elevated blood dimethyl sulfide, which may cause a blood borne halitosis symptom.

Alternative medicine

DMSO's popularity as an alternative medicine is stated to stem from a March 1980 60 Minutes documentary "The Riddle of DMSO" [32] and April 1980 Time magazine article [33] covering the treatments of ardent DMSO advocate Dr. Stanley Jacob beginning in the 1960s. [34]

The use of DMSO as an alternative treatment for cancer is of particular concern, as it has been shown to interfere with a variety of chemotherapy drugs, including cisplatin, carboplatin, and oxaliplatin. [35] There is insufficient evidence to support the hypothesis that DMSO has any effect, [36] and most sources agree that its history of side effects when tested warrants caution when using it as a dietary supplement, for which it is marketed heavily with the usual disclaimer. DMSO is an ingredient in some products listed by the U.S. FDA as fake cancer cures [37] and the FDA has had a running battle with distributors. [32] One such distributor is Mildred Miller, who promoted DMSO for a variety of disorders and was consequently convicted of Medicare fraud. [32]

Veterinary medicine

DMSO is commonly used in veterinary medicine as a liniment for horses, alone or in combination with other ingredients. In the latter case, often, the intended function of the DMSO is as a solvent, to carry the other ingredients across the skin. Also in horses, DMSO is used intravenously, again alone or in combination with other drugs. It is used alone for the treatment of increased intracranial pressure and/or cerebral edema in horses.[ citation needed ]

Taste

The perceived garlic taste upon skin contact with DMSO may be due to nonolfactory activation of TRPA1 receptors in trigeminal ganglia. [38] Unlike dimethyl and diallyl disulfides (which have odors resembling garlic), mono- and tri- sulfides (which typically have foul odors), and similar odiferous sulfur compounds, the pure chemical DMSO is odorless.

Safety

Toxicity

DMSO is a non-toxic solvent with a median lethal dose higher than ethanol (DMSO: LD50, oral, rat, 14,500 mg/kg; [39] [40] ethanol: LD50, oral, rat, 7,060 mg/kg [41] ).

DMSO can cause contaminants, toxins, and medicines to be absorbed through the skin, which may cause unexpected effects. DMSO is thought to increase the effects of blood thinners, steroids, heart medicines, sedatives, and other drugs. In some cases this could be harmful or dangerous. [42]

Because DMSO easily penetrates the skin, substances dissolved in DMSO may quickly be absorbed. Glove selection is important when working with DMSO. Butyl rubber, fluoroelastomer, neoprene, or thick (15  mil / 0.4  mm) latex gloves are recommended. [43] Nitrile gloves, which are very commonly used in chemical laboratories, may protect from brief contact but have been found to degrade rapidly with exposure to DMSO. [44]

Regulation

In Australia, it is listed as a Schedule 4 (S4) Drug, and a company has been prosecuted for adding it to products as a preservative. [45]

Clinical safety

Early clinical trials with DMSO were stopped because of questions about its safety, especially its ability to harm the eye. The most commonly reported side effects include headaches and burning and itching on contact with the skin. Strong allergic reactions have been reported.[ full citation needed ]

On September 9, 1965, The Wall Street Journal reported that a manufacturer of the chemical warned that the death of an Irish woman after undergoing DMSO treatment for a sprained wrist may have been due to the treatment, although no autopsy was done, nor was a causal relationship established. [46] Clinical research using DMSO was halted and did not begin again until the National Academy of Sciences (NAS) published findings in favor of DMSO in 1972. [47] In 1978, the US FDA approved DMSO for treating interstitial cystitis. In 1980, the US Congress held hearings on claims that the FDA was slow in approving DMSO for other medical uses. In 2007, the US FDA granted "fast track" designation on clinical studies of DMSO's use in reducing brain tissue swelling following traumatic brain injury. [47]

DMSO exposure to developing mouse brains can produce brain degeneration. This neurotoxicity could be detected at doses as low as 0.3 mL/kg, a level exceeded in children exposed to DMSO during bone marrow transplant. [48]

Odor problem

DMSO disposed into sewers can cause odor problems in municipal effluents: waste water bacteria transform DMSO under hypoxic (anoxic) conditions into dimethyl sulfide (DMS) that has a strong disagreeable odor, similar to rotten cabbage. [49] However, chemically pure DMSO is odorless because of the lack of C-S-C (sulfide) and C-S-H (mercaptan) linkages. Deodorization of DMSO is achieved by removing the odorous impurities it contains. [50]

Explosion hazard

Dimethyl sulfoxide can produce an explosive reaction when exposed to acyl chlorides; at a low temperature, this reaction produces the oxidant for Swern oxidation.

DMSO can decompose at the boiling temperature of 189 °C at normal pressure, possibly leading to an explosion. The decomposition is catalyzed by acids and bases and therefore can be relevant at even lower temperatures. A strong to explosive reaction also takes place in combination with halogen compounds, metal nitrides, metal perchlorates, sodium hydride, periodic acid and fluorinating agents. [51]

See also

Related Research Articles

<span class="mw-page-title-main">Toluene</span> Chemical compound

Toluene, also known as toluol, is a substituted aromatic hydrocarbon with the chemical formula C6H5CH3, often abbreviated as PhCH3, where Ph stands for the phenyl group. It is a colorless, water-insoluble liquid with the odor associated with paint thinners. It is a mono-substituted benzene derivative, consisting of a methyl group (CH3) attached to a phenyl group by a single bond. As such, its systematic IUPAC name is methylbenzene. Toluene is predominantly used as an industrial feedstock and a solvent.

In organic chemistry, the Swern oxidation, named after Daniel Swern, is a chemical reaction whereby a primary or secondary alcohol is oxidized to an aldehyde or ketone using oxalyl chloride, dimethyl sulfoxide (DMSO) and an organic base, such as triethylamine. It is one of the many oxidation reactions commonly referred to as 'activated DMSO' oxidations. The reaction is known for its mild character and wide tolerance of functional groups.

<span class="mw-page-title-main">Organic sulfide</span> Organic compound with an –S– group

In organic chemistry, a sulfide or thioether is an organosulfur functional group with the connectivity R−S−R' as shown on right. Like many other sulfur-containing compounds, volatile sulfides have foul odors. A sulfide is similar to an ether except that it contains a sulfur atom in place of the oxygen. The grouping of oxygen and sulfur in the periodic table suggests that the chemical properties of ethers and sulfides are somewhat similar, though the extent to which this is true in practice varies depending on the application.

Sulfide (also sulphide in British English ) is an inorganic anion of sulfur with the chemical formula S2− or a compound containing one or more S2− ions. Solutions of sulfide salts are corrosive. Sulfide also refers to large families of inorganic and organic compounds, e.g. lead sulfide and dimethyl sulfide. Hydrogen sulfide (H2S) and bisulfide (SH−) are the conjugate acids of sulfide.

In organic chemistry, a carbanion is an anion in which carbon is negatively charged.

<span class="mw-page-title-main">Methylsulfonylmethane</span> Chemical compound

Dimethyl sulfone (DMSO2) is an organosulfur compound with the formula (CH3)2SO2. It is also known by several other names including methyl sulfone and (especially in alternative medicine) methylsulfonylmethane (MSM). This colorless solid features the sulfonyl functional group and is the simplest of the sulfones. It is relatively inert chemically and is able to resist decomposition at elevated temperatures. It occurs naturally in some primitive plants, is present in small amounts in many foods and beverages, and is marketed (under the MSM name) as a dietary supplement. It is sometimes used as a cutting agent for illicitly manufactured methamphetamine. It is also commonly found in the atmosphere above marine areas, where it is used as a carbon source by the airborne bacteria Afipia. Oxidation of dimethyl sulfoxide produces the sulfone, both under laboratory conditions and metabolically.

Organosulfur chemistry is the study of the properties and synthesis of organosulfur compounds, which are organic compounds that contain sulfur. They are often associated with foul odors, but many of the sweetest compounds known are organosulfur derivatives, e.g., saccharin. Nature is abound with organosulfur compounds—sulfur is vital for life. Of the 20 common amino acids, two are organosulfur compounds, and the antibiotics penicillin and sulfa drugs both contain sulfur. While sulfur-containing antibiotics save many lives, sulfur mustard is a deadly chemical warfare agent. Fossil fuels, coal, petroleum, and natural gas, which are derived from ancient organisms, necessarily contain organosulfur compounds, the removal of which is a major focus of oil refineries.

<span class="mw-page-title-main">Carbodiimide</span> Class of organic compounds with general structure RN=C=NR

In organic chemistry, a carbodiimide is a functional group with the formula RN=C=NR. On Earth they are exclusively synthetic, but in interstellar space the parent compound HN=C=NH has been detected by its maser emissions.

<span class="mw-page-title-main">Dimethyl sulfate</span> Chemical compound

Dimethyl sulfate (DMS) is a chemical compound with formula (CH3O)2SO2. As the diester of methanol and sulfuric acid, its formula is often written as (CH3)2SO4 or Me2SO4, where CH3 or Me is methyl. Me2SO4 is mainly used as a methylating agent in organic synthesis. Me2SO4 is a colourless oily liquid with a slight onion-like odour. Like all strong alkylating agents, Me2SO4 is toxic. Its use as a laboratory reagent has been superseded to some extent by methyl triflate, CF3SO3CH3, the methyl ester of trifluoromethanesulfonic acid.

<span class="mw-page-title-main">Sulfoxide</span> Organic compound containing a sulfinyl group (>SO)

In organic chemistry, a sulfoxide, also called a sulphoxide, is an organosulfur compound containing a sulfinyl functional group attached to two carbon atoms. It is a polar functional group. Sulfoxides are oxidized derivatives of sulfides. Examples of important sulfoxides are alliin, a precursor to the compound that gives freshly crushed garlic its aroma, and dimethyl sulfoxide (DMSO), a common solvent.

<span class="mw-page-title-main">Dimethyl sulfide</span> Chemical compound

Dimethyl sulfide (DMS) or methylthiomethane is an organosulfur compound with the formula (CH3)2S. It is the simplest thioether and has a characteristic disagreeable odor. It is a flammable liquid that boils at 37 °C (99 °F). It is a component of the smell produced from cooking of certain vegetables and seafoods. It is also an indication of bacterial contamination in malt production and brewing. It is a breakdown product of dimethylsulfoniopropionate (DMSP), and is also produced by the bacterial metabolism of methanethiol.

Sulfur compounds are chemical compounds formed the element sulfur (S). Common oxidation states of sulfur range from −2 to +6. Sulfur forms stable compounds with all elements except the noble gases.

<span class="mw-page-title-main">Phosphorus pentasulfide</span> Chemical compound

Phosphorus pentasulfide is the inorganic compound with the formula P2S5 (empirical) or P4S10 (molecular). This yellow solid is the one of two phosphorus sulfides of commercial value. Samples often appear greenish-gray due to impurities. It is soluble in carbon disulfide but reacts with many other solvents such as alcohols, DMSO, and DMF.

The Pfitzner–Moffatt oxidation, sometimes referred to as simply the Moffatt oxidation, is a chemical reaction for the oxidation of primary and secondary alcohols to aldehydes and ketones, respectively. The oxidant is a combination of dimethyl sulfoxide (DMSO) and dicyclohexylcarbodiimide (DCC). The reaction was first reported by J. Moffatt and his student K. Pfitzner in 1963.

The Corey–Kim oxidation is an oxidation reaction used to synthesize aldehydes and ketones from primary and secondary alcohols. It is named for American chemist and Nobel Laureate Elias James Corey and Korean-American chemist Choung Un Kim.

<span class="mw-page-title-main">Deuterated DMSO</span> Chemical compound

Deuterated DMSO, also known as dimethyl sulfoxide-d6, is an isotopologue of dimethyl sulfoxide (DMSO, (CH3)2S=O)) with chemical formula ((CD3)2S=O) in which the hydrogen atoms ("H") are replaced with their isotope deuterium ("D"). Deuterated DMSO is a common solvent used in NMR spectroscopy.

<span class="mw-page-title-main">Sodium methylsulfinylmethylide</span> Chemical compound

Sodium methylsulfinylmethylide is the sodium salt of the conjugate base of dimethyl sulfoxide. This unusual salt has some uses in organic chemistry as a base and nucleophile.

The Parikh–Doering oxidation is an oxidation reaction that transforms primary and secondary alcohols into aldehydes and ketones, respectively. The procedure uses dimethyl sulfoxide (DMSO) as the oxidant and the solvent, activated by the sulfur trioxide pyridine complex (SO3•C5H5N) in the presence of triethylamine or diisopropylethylamine as base. Dichloromethane is frequently used as a cosolvent for the reaction.

<span class="mw-page-title-main">Thiosulfinate</span> Functional group

In organosulfur chemistry, thiosulfinate is a functional group consisting of the linkage R-S(O)-S-R. Thiolsulfinates are also named as alkanethiosulfinic acid esters.

<span class="mw-page-title-main">Transition metal sulfoxide complex</span> Class of coordination compounds containing sulfoxide ligands)

A transition metal sulfoxide complex is a coordination complex containing one or more sulfoxide ligands. The inventory is large.

References

  1. ↑ DMSO (medication)
  2. ↑ "Dimethyl Sulfoxide (DMSO) -- Technical". Atofina Chemicals, inc. Retrieved 26 May 2007.
  3. ↑ Matthews WS, Bares JE, Bartmess JE, Bordwell FG, Cornforth FJ, Drucker GE, Margolin Z, McCallum RJ, McCollum GJ, Vanier NR (1975). "Equilibrium acidities of carbon acids. VI. Establishment of an absolute scale of acidities in dimethyl sulfoxide solution". J. Am. Chem. Soc. 97 (24): 7006–7014. doi:10.1021/ja00857a010.
  4. ↑ Novak KM, ed. (2002). Drug Facts and Comparisons (56th ed.). St. Louis, Missouri: Wolters Kluwer Health. p.  2345. ISBN   978-1-57439-110-7.
  5. ↑ Thomas R, Shoemaker CB, Eriks K (1966). "The Molecular and Crystal Structure of Dimethyl Sulfoxide, (H3C)2SO". Acta Crystallogr. 21 (1): 12–20. Bibcode:1966AcCry..21...12T. doi:10.1107/S0365110X66002263.
  6. ↑ von Demselben (1867). "Ueber die Einwirkung von Saltpetersäure auf Schwefelmethyl und Schwefeläthyl" [On the effect of nitric acid on methyl sulfide and ethyl sulfide]. In Erlenmeyer, E.; Rieckher, T.; Volhard, J.; Liebig, J.; Wöhler, F. (eds.). Annalen der Pharmacie (in German). Meyer ; Winter. p. 148.
  7. ↑ Gergel, Max G. (March 1977). Excuse me sir, would you like to buy a kilo of isopropyl bromide?. Pierce Chemical. p. 145.
  8. ↑ Roy, Kathrin-Maria (15 June 2000), "Sulfones and Sulfoxides", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim, Germany: Wiley-VCH Verlag GmbH & Co. KGaA, doi:10.1002/14356007.a25_487, ISBN   3527306730
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  12. ↑ Laurence, Christian; Gal, Jean-François (2010). Lewis basicity and affinity scales : data and measurement. Chichester, West Sussex, U.K.: John Wiley. pp. 50–51. ISBN   978-0-470-74957-9. OCLC   428031803.
  13. ↑ Cramer, R. E.; Bopp, T. T. (1977). "Graphical display of the enthalpies of adduct formation for Lewis acids and bases". Journal of Chemical Education. 54: 612–613. doi:10.1021/ed054p612. The plots shown in this paper used older parameters. Improved E&C parameters are listed in ECW model.
  14. ↑ "DMSO". exactantigen.com. Archived from the original on 2009-10-05. Retrieved 2009-10-02.
  15. ↑ Bordwell FG (1988). "Equilibrium acidities in dimethyl sulfoxide solution". Accounts of Chemical Research . 21 (12): 456–463. doi:10.1021/ar00156a004. S2CID   26624076.
  16. ↑ "Bordwell pKa Table (Acidity in DMSO)". Archived from the original on 9 October 2008. Retrieved 23 April 2019.
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