7704-34-9

Basic information

• Product Name: Sulfur
• Synonyms: MICROTHIOL SPECIAL;RASULF;SULFUR;SULFUR, AAS STANDARD SOLUTION;Atomic sulfur;atomicsulfur;Bensulfoid;Biosulphur powder
• CAS NO: 7704-34-9
• Molecular Formula: S8
• Molecular Weight: 256.52
• EINECS: 231-722-6
• Product Categories: Sulfur;Rubber Chemicals;Nonmetallic Element;Inorganics;FUNGICIDE;Essential Chemicals;Reagent Grade;Routine Reagents;AcaricidesMicro/Nanoelectronics;Electronic Chemicals;Pure Elements;InorganicsPesticides&Metabolites;AcaricidesPesticides;Alpha sort;Fungicides;Pesticides;Pesticides&Metabolites;Q-ZAlphabetic;S;SN - SZ;metal or element;rubber vulcanizing agent
• Mol File: 7704-34-9.mol
• Article Data: 2983

Chemical Properties

• Melting Point: 114 °C
• Boiling Point: 445 °C
• Flash Point: 168 °C
• Appearance: Yellow/powder
• Density: 2.36
• Vapor Density: 8.9 (vs air)
• Vapor Pressure: 1 mm Hg ( 183.8 °C)
• Solubility: carbon disulfide: in accordance1g/5mL
• Water Solubility: Insoluble
• Merck: 13,9059 / 13,9067
• CAS DataBase Reference: Sulfur(CAS DataBase Reference)
• NIST Chemistry Reference: Sulfur(7704-34-9)
• EPA Substance Registry System: Sulfur(7704-34-9)

Safety Data

• Hazard Codes: F,Xi
• Statements: 11-38
• Safety Statements: 16-26-46
• RIDADR: UN 1350 4.1/PG 3
• WGK Germany: 1
• RTECS: WS4250000
• TSCA: Yes
• HazardClass: 4.1
• PackingGroup: III
• Hazardous Substances Data: 7704-34-9(Hazardous Substances Data)

Usage

Chemical Description

Different sources of media describe the Chemical Description of 7704-34-9 differently. You can refer to the following data:
1. Sulfur is a chemical element.
2. Sulfur is a yellow solid that is used in the production of sulfuric acid.
3. Sulfur is a nonmetallic element that is often used in organic synthesis as a reducing agent or to promote cyclization reactions.
4. Sulfur and chloranil are used in attempts to dehydrogenate some of the addition products, while bromine is used in the synthesis of tetrabromide of 1,4-diphenylbutadiene.
5. Sulfur is used as a reagent in the reactions to form the sulfur-containing rings.

Description

Sulfur belongs to a nonmetallic chemical element (pure product: yellow crystalline solid) under the symbol S. It can actively react with many other elements. It exists in various kinds of forms and compound such as sulfide and sulfate minerals which can be found everywhere around the universe and earth. It is also a key element for all life as the major component of amino acids, vitamins and many other cofactors. Sulfur has applications in various kinds of fields. For example, one of its biggest applications is for the production of sulfuric acid for sulfate and phosphate fertilizers. It is also used for the manufacturing of insecticides, fungicides, and bactericides. In pharmaceutical, it can be used for the manufacturing of many kinds of sulfur-containing antibiotics.

Chemical Properties

Different sources of media describe the Chemical Properties of 7704-34-9 differently. You can refer to the following data:
1. Sulfur, S, is a nonmetallic element that exists in a crystalline or amorphous form and in four stable isotopes. Sulfur melts at temperatures rangingfrom 112.8°C (234 °F) for the rhombic form to 120.0°C(248 °F) for amorphous sulfur,and all forms boil at 444.7°C (835°F). Sulfur occurs as free sulfur in many volcanic areas and is often associated with gypsum and limestone. It is used as a chemical intermediate and fungicide and in the vulcanization of rubber.
2. Sulfur is a yellow crystalline solid or powder. Often transported in the molten state.

Physical properties

Sulfur is considered a nonmetallic solid. It is found in three allotropic crystal forms:1. Orthorhombic (or rhombic) octahedral lemon-yellow crystals, which are also called“brimstone” and referred to as “alpha” sulfur. The density of this form of sulfur is 2.06g/cm3, with a melting point of 95.5°C.2. Monoclinic, prismatic crystals, which are light-yellow in color. This allotrope is referredto as “beta” sulfur. Its density is 1.96 g/cm3, with a melting point of 119.3°C.3. Amorphous sulfur is formed when molten sulfur is quickly cooled. Amorphous sulfur issoft and elastic, and as it cools, it reverts back to the orthorhombic allotropic form.Sulfur, in its elemental form, is rather common and does not have a taste or odor except whenin contact with oxygen, when it forms small amounts of sulfur dioxide.

Isotopes

There are a total of 24 isotopes of sulfur; all but four of these are radioactive.The four stable isotopes and their contribution to sulfur’s total abundance on Earth areas follows: S-32 contributes 95.02% to the abundance of sulfur; S-33, just 0.75%; S-34,4.21%; and S-36, 0.02%.

Origin of Name

From the Sanskrit word sulvere and the Latin word sulphurim.

Occurrence

Sulfur has been known since ancient times primarily because it is a rather common substance.It is the 15th most common element in the universe, and though it is not found in allregions of the Earth, there are significant deposits in south Texas and Louisiana, as well in allvolcanoes. Sulfur makes up about 1% of the Earth’s crust.Sulfur is an element found in many common minerals, such as galena (PbS), pyrite(fool’s gold, FeS2), sphalerite (ZnS), cinnabar (HgS), and celestite (SrSO4), among others.About 1/4 of all sulfur procured today is recovered from petroleum production. Themajority of sulfur is the result of or a by-product of mining other minerals from the orescontaining sulfur.Sulfur is mined by the recovery method known as the Frasch process, which was inventedby Herman Frasch in Germany in the early 1900s. This process forces superheated water,under pressure, into deep underground sulfur deposits. Compressed air then forces the moltensulfur to the surface, where it is cooled. There are other methods for mining sulfur, but theFrasch process is the most important and most economical.Sulfur is found in Sicily, Canada, Central Europe, and the Arabian oil states, as well as inthe southern United States in Texas and Louisiana and offshore beneath the Gulf of Mexico.

Characteristics

Sulfur exhibits a remarkable array of unique characteristics. Today, there are chemistsdevoting large portions of their careers to studying this unusual element. For example, whensulfur is melted, its viscosity increases, and it turns reddish-black as it is heated. Beyond200°C, the color begins to lighten, and it flows as a thinner liquid.Sulfur burns with a beautiful subdued blue flame. The old English name for sulfur was“brimstone,” which means “a stone that burns.” This is the origin of the term “fire and brimstone”when referring to great heat. Above 445°C, sulfur turns to a gas, which is dark orangeyellowbut which becomes lighter in color as the temperature rises.Sulfur is an oxidizing agent and has the ability to combine with most other elements toform compounds.

History

Different sources of media describe the History of 7704-34-9 differently. You can refer to the following data:
1. Sulfur was known to the alchemists from ancient times as brimstone. Lavoisier in 1772 proved sulfur to be an element. The element derived its name from both the Sanskrit and Latin names Sulvere and Sulfurium, respectively. Sulfur is widely distributed in nature, in earth's crust, ocean, meteorites, the moon, sun, and certain stars. It also is found in volcanic gases, natural gases, petroleum crudes, and hot springs. It is found in practically all plant and animal life. Most natural sulfur is in iron sulfides in the deep earth mantle. The abundance of sulfur in earth’s crust is about 350 mg/kg. Its average concentration in seawater is estimated to be about 0.09%. Sulfur occurs in earth’s crust as elemental sulfur (often found in the vicinity of volcanoes), sulfides, and sulfates. The most important sulfur-containing ores are iron pyrite, FeS2; chalcopyrite, CuFeS2; sphalerite, ZnS; galena, PbS; cinnabar HgS; gypsum CaSO4?2H2O; anhydrite CaSO4; kieserite, MgSO4?H2O; celestite, SrSO4; barite, BaSO4; and. stibnite, Sb2S3.
2. Sulfur is found in meteorites. A dark area near the crater Aristarchus on the moon has been studied by R. W. Wood with ultraviolet light. This study suggests strongly that it is a sulfur deposit. Sulfur occurs native in the vicinity of volcanoes and hot springs. It is widely distributed in nature as iron pyrites, galena, sphalerite, cinnabar, stibnite, gypsum, Epsom salts, celestite, barite, etc. Sulfur is commercially recovered from wells sunk into the salt domes along the Gulf Coast of the U.S. It is obtained from these wells by the Frasch process, which forces heated water into the wells to melt the sulfur, which is then brought to the surface. Sulfur also occurs in natural gas and petroleum crudes and must be removed from these products. Formerly this was done chemically, which wasted the sulfur. New processes now permit recovery, and these sources promise to be very important. Large amounts of sulfur are being recovered from Alberta gas fields. Sulfur is a pale yellow, odorless, brittle solid that is insoluble in water but soluble in carbon disulfide. In every state, whether gas, liquid or solid, elemental sulfur occurs in more than one allotropic form or modification; these present a confusing multitude of forms whose relations are not yet fully understood. Amorphous or “plastic” sulfur is obtained by fast cooling of the crystalline form. X-ray studies indicate that amorphous sulfur may have a helical structure with eight atoms per spiral. Crystalline sulfur seems to be made of rings, each containing eight sulfur atoms that fit together to give a normal X-ray pattern. Twenty-one isotopes of sulfur are now recognized. Four occur in natural sulfur, none of which is radioactive. A finely divided form of sulfur, known as flowers of sulfur, is obtained by sublimation. Sulfur readily forms sulfides with many elements. Sulfur is a component of black gunpowder, and is used in the vulcanization of natural rubber and a fungicide. It is also used extensively is making phosphatic fertilizers. A tremendous tonnage is used to produce sulfuric acid, the most important manufactured chemical. It is used in making sulfite paper and other papers, as a fumigant, and in the bleaching of dried fruits. The element is a good electrical insulator. Organic compounds containing sulfur are very important. Calcium sulfate, ammonium sulfate, carbon disulfide, sulfur dioxide, and hydrogen sulfide are but a few of the many other important compounds of sulfur. Sulfur is essential to life. It is a minor constituent of fats, body fluids, and skeletal minerals. Carbon disulfide, hydrogen sulfide, and sulfur dioxide should be handled carefully. Hydrogen sulfide in small concentrations can be metabolized, but in higher concentrations it can quickly cause death by respiratory paralysis. It is insidious in that it quickly deadens the sense of smell. Sulfur dioxide is a dangerous component in atmospheric pollution. Sulfur (99.999%) costs about $575/kg.

Uses

Different sources of media describe the Uses of 7704-34-9 differently. You can refer to the following data:
1. sulfur (colloidal) reduces oil-gland activity and dissolves the skin’s surface layer of dry, dead cells. This ingredient is commonly used in acne soaps and lotions, and is a major component in many acne preparations. It can cause allergic skin reactions.
2. sulfur is a mild anti-septic used in acne creams and lotions. It stimulates healing when used on skin rashes. Sulfur may cause skin irritation.
3. Elemental sulfur is used for vulcanizing rubber; making black gunpowder; as a soil conditioner; as a fungicide; preparing a number of metal sulfides; and producing carbon disulfide. It also is used in matches; bleaching wood pulp, straw, silk, and wool; and in synthesis of many dyes. Pharmaceutical grade precipitated and sublimed sulfurs are used as scabicides and as antiseptics in lotions and ointments. Important sulfur compounds include sulfuric acid, sulfur dioxide, hydrogen 890 SULFUR sulfide, sulfur trioxide, and a number of metal sulfides and metal oxo- salts such as sulfates, bisulfates, and sulfites. Numerous organic compounds contain sulfur, such as mercaptans, thiophenes, thiophenols, sulfate esters, sulfones, and carbon disulfide.
4. Sulfur is one of the four major commodities of the chemical industry. The other three arelimestone, coal, and salt. Most sulfur that is produced is used to manufacture sulfuric acid(H2SO4). Forty million tons are produced each year in the manufacture of fertilizers, lead-acidbatteries, gunpowder, desiccants (drying agent), matches, soaps, plastics, bleaching agents,rubber, road asphalt binders, insecticides, paint, dyes, medical ointment, and other pharmaceuticalproducts, among many, many other uses. Sulfur is essential to life.

Definition

sulphur: Symbol S. A yellow nonmetallic element belonging to group 16 (formerly VIB) of the periodic table; a.n. 16; r.a.m. 32.06; r.d. 2.07 (rhombic); m.p. 112.8°C; b.p. 444.674°C. The element occurs in many sulphide and sulphate minerals and native sulphur is also found in Sicily and the USA (obtained by the Frasch process). It can also be obtained from hydrogen sulphide by the Claus process.Sulphur has various allotropic forms. Below 95.6°C the stable crystal form is rhombic; above this temperature the element transforms into a triclinic form. These crystalline forms both contain cyclic S8 molecules. At temperatures just above its melting point, molten sulphur is a yellow liquid containing S8 rings (as in the solid form). At about 160°C,the sulphur atoms form chains and the liquid becomes more viscous and dark brown. If the molten sulphur is cooled quickly from this temperature (e.g. by pouring into cold water) a reddish-brown solid known as plastic sulphur is obtained. Above 200°C the viscosity decreases. Sulphur vapour contains a mixture of S2, S4, S6, and S8 molecules. Flowers of sulphur is a yellow powder obtained by subliming the vapour. It is used as a plant fungicide. The element is also used to produce sulphuric acid and other sulphur compounds.Sulphur is an essential element in living organisms, occurring in the amino acids cysteine and methionine and therefore in many proteins. It is also a constituent of various cell metabolites, e.g. coenzyme A. Sulphur is absorbed by plants from the soil as the sulphate ion (SO42–).

Production Methods

Elemental sulfur is recovered from its ore deposits found throughout the world. It is obtained commercially by the Frasch process, recovery from wells sunk into salt domes. Heated water under pressure is forced into the underground deposits to melt sulfur. Liquid sulfur is then brought to the surface. Sulfur is recovered by distillation. Often the ore is concentrated by froth flotation. Elemental sulfur also is recovered as a by-product in processing natural gas and petroleum. Refining operations of natural gas and petroleum crude produce hydrogen sulfide, which also may occur naturally. Hydrogen sulfide is separated from hydrocarbon gases by absorption in an aqueous solution of alkaline solvent such as monoethanol amine. Hydrogen sulfide is concentrated in this solvent and gas is stripped out and oxidized by air at high temperature in the presence of a catalyst (Claus process). Elemental sulfur also may be obtained by smelting sulfide ores with a reducing agent, such as coke or natural gas, or by reduction of sulfur dioxide.

Reactions

Sulfur forms two oxides, sulfur dioxide, SO2, and the trioxide, SO3. It burns in oxygen at about 250°C or in air above 260°C, forming sulfur dioxide. In excess oxygen the trioxide is obtained. Sulfur reacts with hydrogen at 260 to 350°C forming hydrogen sulfide. The reaction is slow at this temperature and does not go to completion. The reaction is catalyzed by activated alumina. Reactions with excess chlorine or fluorine yield sulfur tetrachloride, SCl4, or hexafluoride, SF6. These reactions occur under cold conditions. Sulfur reacts with sulfur dioxide in an electric discharge to form disulfuroxide, S2O. Sulfur reacts with aqueous sulfide to form polysulfides: S + Na2S → Na2S2 With aqueous solution of sulfite the product is thiosulfate: S + SO32– → S2O32– Thiosulfate also is obtained by heating sulfur with powdered sulfite: S + Na2SO3 → Na2S2O3 When heated with alkali cyanide, thiocyanate salt is obtained: S + KCN → KSCN A similar reaction occurs in the aqueous phase in which thiocyanate is obtained by evaporation and crystallization. Sulfur combines with alkali metals, copper, silver, and mercury on cold contact with the solid, forming sulfides. Reactions with magnesium, zinc, and cadmium occur to a small degree at ordinary temperatures, but rapidly on heating. Sulfur reacts with phosphorus, arsenic, antimony, bismuth, and silicon at their melting points and with other elements at elevated temperatures forming binary sulfides. Sulfides of tellurium, gold, platinum, and iridium are difficult to obtain even at elevated temperatures. Sulfur does not react with inert gases, nitrogen, and iodine.

Brand name

Liquamat (Galderma ); Sastid (Stiefel); Sulfur Soap (Stiefel).

General Description

A pale yellow crystalline solid with a faint odor of rotten eggs. Insoluble in water. A fire and explosion risk above 450° F. Transported as a yellow to red liquid. Handled at elevated temperature (typically 290°F) to prevent solidification and makes transfers easier. Hot enough that plastic or rubber may melt or lose strength. Causes thermal burns to skin on contact. Cools rapidly and solidifies if released. Equipment designed to protect against ordinary chemical exposure is ineffective against the thermal hazard. Exercise caution walking on the surface of a spill to avoid breakthrough into pockets of molten sulfur below the crust. Do not attempt to remove sulfur impregnated clothing because of the danger of tearing flesh if a burn has resulted. May be irritatin to skin, eyes and mucous membranes. Used in sulfuric acid production, petroleum refining, and pulp and paper manufacturing.

Air & Water Reactions

Flammable. Insoluble in water.

Reactivity Profile

SULFUR reacts violently with strong oxidizing agents causing fire and explosion hazards [Handling Chemicals Safely 1980 p. 871]. Reacts with iron to give pyrophoric compounds. Attacks copper, silver and mercury. Reacts with bromine trifluoride, even at 10°C [Mellor 2:113. 1946-47]. Ignites in fluorine gas at ordinary temperatures [Mellor 2:11-13 1946-47]. Reacts to incandescence with heated with thorium [Mellor 7:208 1946-47]. Can react with ammonia to form explosive sulfur nitride. Reacts with calcium phosphide incandescently at about 300°C. Reacts violently with phosphorus trioxide [Chem. Eng. News 27:2144 1949]. Mixtures with ammonium nitrate or with metal powders can be exploded by shock [Kirk and Othmer 8:644]. Combinations of finely divided sulfur with finely divided bromates, chlorates, or iodates of barium, calcium, magnesium, potassium, sodium, or zinc can explode with heat, friction, percussion, and sometimes light [Mellor 2 Supp.1:763. 1956]. A mixture with barium carbide heated to 150°C becomes incandescent. Reacts incandescently with calcium carbide or strontium carbide at 500°C. Attacks heated lithium, or heated selenium carbide with incandescence [Mellor 5:862 1946-47]. Reacts explosively if warmed with powdered zinc [Mellor 4:476. 1946-47]. Reacts vigorously with tin [Mellor 7:328. 1946-47]. A mixture with potassium nitrate and arsenic trisulfide is a known pyrotechnic formulation [Ellern 1968 p. 135]. Mixtures with any perchlorate can explode on impact [ACS 146:211-212]. A mixture of damp sulfur and calcium hypochlorite produces a brilliant crimson flash with scatter of molten sulfur [Chem. Eng. News 46(28):9 1968]. Takes fire spontaneously in chlorine dioxide and may produce an explosion [Mellor 2:289 (1946-47)]. Ignites if heated with chromic anhydride ignite and can explode, [Mellor 10:102 (1946-47)]. Even small percentages of hydrocarbons in contact with molten sulfur generate hydrogen sulfide and carbon disulfide, which may accumulate in explosive concentrations. Sulfur reacts with Group I metal nitrides to form flammable mixtures, evolving flammable and toxic NH3 and H2S gasses if water is present. (Mellor, 1940, Vol. 8, 99).

Hazard

Many of the sulfur compounds are toxic but essential for life. The gas from elemental sulfurand from most of the compounds of sulfur is poisonous when inhaled and deadly wheningested. This is the reason that sulfur compounds are effective for rat and mice exterminationas well an ingredient of insecticides. Sulfa drugs (sulfanilamide and sufadiazine), althoughtoxic, were used as medical antibiotics during World War II before the development of penicillin.They are still used today in veterinary medicine.

Health Hazard

Can cause eye irritation; may rarely irritate skin. If recovered sulfur, refer to hydrogen sulfide.*

Flammability and Explosibility

Nonflammable

Agricultural Uses

Different sources of media describe the Agricultural Uses of 7704-34-9 differently. You can refer to the following data:
1. Brimstone is coarsely ground sulphur which is used to increase the acidity of soil and correct sulphur deficiency inplants.
2. Sulphur (S) is a yellow, non-metallic element belonging to Group 16 (formerly VI B) of the Periodic Table. It is a macronutrient required by plants in relatively large amounts. Potato, cereals and grasses require about 20 kg/ha sulphur, while its ideal dosage for the Brassiceae family of crops is 50 kg/ha. Soil-sulphur reactions are similar to soil-nitrogen reactions, and are dominated by organic or microbial fractions in the soil. Approximately 90% sulphur required by plants is for the synthesis of amino acids (namely, cysteine, cystine and methionhe) which are essential components of proteins and contain 6 to 8% S. One of the main functions of sulphur in proteins is to form sulphur-sulphur (-S-S-) bonds between polypeptide chains which are essential for the protein conformation relevant to its catalytic or structural properties. Depending on their sulphur requirement, crops are divided into three groups. The first includes crops with a high sulphur requirement - in a range 20 to 80 kg/ha. Crucifers and Brassiceae fall in this group. The second group requires sulphur in a moderate range - 10 to 50 kg/ha and includes plantation crops. The third group needs sulphur in small quantities - 5 to 25 kg/ha and includes cereals, forages and other field crops. As a rule, sulphur requirement is 3 to 4 kg/ton of grains, 8 kg/ton of grain legumes and 12 kg/ton of oil seeds. Soil can lose sulphur by (a) its removal by crops, (b) leaching and erosion, (c) sulphate adsorption and retention by clays, and (d) cultivation. Decomposition of organic matter is accelerated by cultivation, which improves soil segregation and aeration. The oxidation of organic matter causes a decline in organic sulphur. Sulphur is needed for the synthesis of co-enzyme A, biotin, thiamine and glutathione. It is also present in substances like sulphur-adenosyl methionhe, formyl methionhe, lipoic acid and sulfolipid. Sulphur plays an important role in chlorophyll synthesis. It is part of ferridoxins, a type of non-heme iron-sulphur (Fe-S) protein occurring in chloroplasts and involved in the reduction of nitrite and sulphate, and in the assimilation of nitrogen by bacteria. Sulphur enhances the formation of oil in crops like soybean and flax. Plant roots absorb sulphur as sulphate ions. Small quantities of sulphur dioxide (SO2) can be absorbed through plant leaves and used in the plant. The concentration of sulphur in plants is 0.1 to 4% which is equal to, or less than, the amount of phosphorus in wheat, corn, beans and potato but is more than the phosphorus content in alfalfa, cabbage and turnip. There is a close relationship between organic C, total N and total S in soils. The C: N: S ratio in most welldrained, non-calcareous soils is approximately 120: 10: 1.4. Generally, the C: S ratio varies much more than the N: S ratio, the latter falling within a narrow range of 6 to 8.1. Sulphur may be immobilized in soils whenthe C: S or N: S ratio is large.

Safety Profile

Poison by ingestion, intravenous, and intraperitoneal routes. A human eye irritant. A fungcide. Chronic inhalation can cause irritation of mucous membranes. Combustible when exposed to heat or flame or by chemical reaction with oxidzers. Explosive in the form of dust when exposed to flame. Can react violently with halogens, carbides, halogenates, halogenites, zinc, uranium, tin, sodium, lithium, nickel, palladium, phosphorus, potassium, indum, calcium, boron, aluminum, (aluminum + niobium pentoxide), ammonia, ammonium nitrate, ammonium perchlorate, BrF5, BrF3, (Ca + VO + H20), Ca(OCl)2, Cad%, Cs3N, charcoal, (Cu + chlorates), ClO2, Cl0, ClF3, CrO3, Cr(OCl)2, hydrocarbons, IF5,IO5, Pb02, Hg(NO3)2, HgO, Hg20, NO2, P2O3, (KNO3 + As2S3), K3N, KMn04, AgNO3, Ag20, NaH, (NaNO3 + charcoal), (Na + SnI4), SCl2, T12O3, F2. Can react with oxidzing materials. To fight fire, use water or special mixtures of dry chemical. When heated it burns and emits highly toxic fumes of SOX. See also NUISANCE DUSTS.

Potential Exposure

Widely used in manufacture of sulfuric acid; carbon bisulfide; drugs, fungicides, gunpowder, wood pulp; rubber, and other products.

Shipping

UN1350 Sulfur, Hazard Class: 4.1; Labels: 4.1-Flammable solid (International). NA1350 Sulfur, Hazard class: 9; Labels: 9-Miscellaneous hazardous material (Domestic). UN2448 Sulfur, molten, Hazard Class: 4.1; Labels: 4.1-Flammable solid (International). NA 2448 Sulfur, molten Hazard class: 9; Labels: 9-Miscellaneous hazardous material (Domestic).

Purification Methods

Murphy, Clabaugh & Gilchrist [J Res Nat Bur Stand 64A 355 1960] have obtained sulfur of about 99.999% purity by the following procedure: Roll sulfur was melted and filtered through a coarse-porosity glass filter funnel into a 2L round-bottomed Pyrex flask with two necks. Conc H2SO4 (300mL) was added to the sulfur (2.5kg), and the mixture was heated to 150o, stirring continuously for 2hours. Over the next 6hours, conc HNO3 was added in about 2mL portions at 10-15minutes intervals to the heated mixture. It was then allowed to cool to room temperature and the acid was poured off. The sulfur was rinsed several times with distilled water, then remelted, cooled, and rinsed several times with distilled water again, this process being repeated four or five times to remove most of the acid entrapped in the sulfur. An air-cooled reflux tube (ca 40cm long) was attached to one of the necks of the flask, and a gas delivery tube (the lower end about 2.5cm above the bottom of the flask) was inserted into the other. While the sulfur was boiled under reflux, a stream of helium or N2 was passed through to remove any water, HNO3 or H2SO4, as vapours. After 4hours, the sulfur was cooled so that the reflux tube could be replaced by a bent air-cooled condenser. The sulfur was then distilled, rejecting the first and the final 100mL portions, and transferred in 200mL portions to 400mL glass cylinder ampoules (which were placed on their sides during solidification). After adding about 80mL of water, displacing the air with N2, the ampoule was cooled, and the water was titrated with 0.02M NaOH, the process being repeated until the acid content was negligible. Finally, entrapped water was removed by alternate evacuation to 10mm Hg and refilling with N2 while the sulfur was kept molten. The ampoules were then sealed. Other purifications include crystallisation from CS2 (which is less satisfactory because the sulfur retains appreciable amounts of organic material), *benzene or *benzene/acetone, followed by melting and degassing. It has also been boiled with 1% MgO, then decanted, and dried under a vacuum at 40o for 2days over P2O5. [For the purification of S6, “recrystallised S8” and “Bacon-Fanelli sulfur” see Bartlett et al. J Am Chem Soc 83 103, 109 1961.]

Incompatibilities

Widely used in manufacture of sulfuric acid; carbon bisulfide; drugs, fungicides, gunpowder, wood pulp; rubber, and other products.

Waste Disposal

Salvage for reprocessing or dump to landfill.

References

https://en.wikipedia.org/wiki/Sulfur#Applications http://geology.com/minerals/sulfur.shtml http://www.wisegeek.org/what-is-sulfur.htm

InChI:InChI=1/S

Synthetic route

sulfur dioxide (7446-09-5) + water (7732-18-5) → sulfuric acid (7664-93-9) + sulfur (7704-34-9)

Conditions	Yield
at 170-180°C; in very dilute soln. complete decompn. in 2 h, incomplete decompn. in concd. solns.;	A n/a B 100%
byproducts: H2S4O6;
sodium thiosulfate In water 100°C;

carbon monoxide (201230-82-2) + sulfur dioxide (7446-09-5) → sulfur (7704-34-9)

Conditions	Yield
With catalyst: CeO2.Co3O4 284-465°C, metal oxide mixture catalysts activity: CuCo2O4;	100%
With catalyst: CuCo2O4 284-465°C, metal oxide mixture catalysts activity: CuCo2O4;	100%
With catalyst: LaCoO3 284-465°C, metal oxide mixture catalysts activity: CuCo2O4;	100%

vanadium sulfate → hydrogen (1333-74-0) + sulfur (7704-34-9)

Conditions	Yield
1690°C complete decompn.;	A 100% B n/a
red heat;	A 7% B n/a
400°C;

barium dithionate → barium sulfate + sulfur (7704-34-9)

Conditions	Yield
With water In water byproducts: H2SO4; 6-8 h at 150-180°C;	A 100% B n/a
With H2O In water byproducts: H2SO4; 6-8 h at 150-180°C;	A 100% B n/a
With water In water byproducts: H2SO4, SO2; incomplete decompn.;
With H2O In water byproducts: H2SO4, SO2; incomplete decompn.;

tungsten(IV) sulfide → sulfur (7704-34-9) + tungsten (7440-33-7)

Conditions	Yield
2000°C, fast react.;	A n/a B 100%
2000°C, fast react.;	A n/a B 100%
1200°C, 2 h;	A n/a B 60%
1200°C, 2 h;	A n/a B 60%

cadmium(II) dithionate → cadmium sulfate + sulfur (7704-34-9)

Conditions	Yield
With water byproducts: H2SO4; 150-180°C under N2;	A 100% B n/a
With H2O byproducts: H2SO4; 150-180°C under N2;	A 100% B n/a

ammonium thiosulfate + hydrogen sulfide (7783-06-4) → water (7732-18-5) + sulfur (7704-34-9)

Conditions	Yield
In water Kinetics; Reduction of (NH4)2S2O3 (c=0.4 mole/liter) by H2S in aq. soln. (50°C, pH=5, p(H2S)=0.08 MPa) in presence of Si-based catalyst.; Gravimetrical determination of S.;	A n/a B 99.7%
In water Kinetics; Reduction of (NH4)2S2O3 (c=1.0 mole/liter) by H2S in aq. soln. (50°C, pH=5, p(H2S)=0.08 MPa) in presence of Si-based catalyst.; Gravimetrical determination of S.;	A n/a B 99.87%
In water Kinetics; Reduction of (NH4)2S2O3 (c=1.0 mole/liter) by H2S in aq. soln. (50°C, pH=5, p(H2S)=0.08 MPa).; Gravimetrical determination of S.;	A n/a B 76.1%
In water Kinetics; Reduction of (NH4)2S2O3 (c=0.4 mole/liter) by H2S in aq. soln. (50°C, pH=5, p(H2S)=0.08 MPa).; Gravimetrical determination of S.;	A n/a B 71.5%

hydrogen sulfide (7783-06-4) + sulfur dioxide (7446-09-5) → water (7732-18-5) + sulfur (7704-34-9)

Conditions	Yield
In hydrogenchloride 20°C;satd. solns.; molar ratio 2 : 1; 15 % HCl soln., ,30 min;; S coagulated by addn. of gelatine or Al2(SO4)3;	A n/a B 99.7%
In hydrogenchloride 20°C;satd. solns.; molar ratio 2 : 1; 15 % HCl soln., ,30 min;; S coagulated by addn. of gelatine or Al2(SO4)3;	A n/a B 99.7%
In hydrogenchloride 20°C; satd. solns.; molar ratio 2 : 1; 3.5 % HCl soln.;; S coagulated by addn. of gelatine or Al2(SO4)3;;	A n/a B 93.5%

sulfur dioxide (7446-09-5) → sulfuric acid (7664-93-9) + sulfur (7704-34-9)

Conditions	Yield
In not given Electrolysis; Pt anode, graphite cathode, area of the electrodes 30 cm^2, 1 A, 20 min, 0.208 mg/l SO2 soln.;	A 98.16% B 70.87%
In not given Electrolysis; Pt anode, graphite cathode, area of the electrodes 30 cm^2, 1 A, 20 min, 0.420 mg/l SO2 soln.;	A 98.52% B 74.28%
In not given Electrolysis; Pt anode, graphite cathode, area of the electrodes 30 cm^2, 1 A, 20 min, 1.123 mg/l SO2 soln.;	A 98.86% B 74.2%

hydrgensulfide(1-) + hydrogen sulfite → Sulfate (14808-79-8) + thiosulphate ion (14383-50-7) + sulfur (7704-34-9)

Conditions	Yield
In water byproducts: H2O; at ambient temp., molar ratio HS(1-) : HSO3(1-) = 1 : 2 must be adjusted as exactly as possible;; only small amts. of S and sulfate form;;	A n/a B 98% C n/a
In water byproducts: H2O; at ambient temp., molar ratio HS(1-) : HSO3(1-) = 1 : 2 must be adjusted as exactly as possible;; only small amts. of S and sulfate form;;	A n/a B 98% C n/a

2,2,4,4,6,6-hexamethyl-1,3,5,2,4,6-trithiatristanninane (16892-64-1) + N-chloro-p-chlorobenzenesulfonamide sodium salt (30066-82-1) → CH3OSn(CH3)2S(NSO2C6H4Cl)Sn(CH3)2SSn(CH3)2NHSO2C6H4Cl (206008-10-8) + sulfur (7704-34-9) + sodium chloride (7647-14-5)

Conditions	Yield
In methanol soln. of N-compd. addn. to soln. of Sn compd. (vacuum, stirring), heating (50°C, 30 min); mixture cooling (ice bath), ppt. filtration off and extracting with water to remove NaCl and with acetone to remove S, alcoholic filtrate vacuumevapn., residue treating with diethyl ether, soln. decanting and vacuum evapn.; elem. anal.;	A 92% B 33% C 98%

bis(tetraethylammonium)-bis[di-(thiophenolato)-(μ-sulfido)ferrate(III)] + nitrogen(II) oxide (10102-43-9) → (NEt4)[Fe(NO)2(thiophenol)2(-2H)] (106709-47-1) + sulfur (7704-34-9)

Conditions	Yield
In acetonitrile at 20℃; for 1.5h; Inert atmosphere; Schlenk technique;	A 81% B 98%

hydrogen sulfide (7783-06-4) → sulfur (7704-34-9)

Conditions	Yield
With catalyst: bauxite; H2SO4, SO3, oleum or HSO3Cl In gas byproducts: H2O; two steps: 300°C and 200°C;	97%
With catalyst: bauxite; H2SO4, SO3, oleum or HSO3Cl In neat (no solvent, gas phase) byproducts: H2O; two steps: 300°C and 200°C;	97%
With oxygen at 180℃; for 30h; Catalytic behavior; Activation energy; Reagent/catalyst; Temperature; Flow reactor;	95%

hydrgensulfide(1-) + hydrogen cation + sulfite(2-) (14265-45-3) + hydrogen sulfite → water (7732-18-5) + thiosulphate ion (14383-50-7) + sulfur (7704-34-9)

Conditions	Yield
In not given equimolar amts. of HSO3(1-) and SO3(2-);	A n/a B 96% C 0%
In not given equimolar amts. of HSO3(1-) and SO3(2-);	A n/a B 96% C 0%

sulfuryl dichloride (7791-25-5) + cadmium(II) sulphide → sulfur dioxide (7446-09-5) + sulfur (7704-34-9) + cadmium(II) chloride (10108-64-2)

Conditions	Yield
3-4 h at 350°C in a sealed bombe tube;	A n/a B n/a C 95%
3-4 h at 350°C in a sealed bombe tube;	A n/a B n/a C 95%
16 h at 250°C in a sealed bombe tube;	A n/a B n/a C 94%

carbon monoxide (201230-82-2) + sulfur dioxide (7446-09-5) → carbon oxide sulfide (463-58-1) + sulfur (7704-34-9)

Conditions	Yield
With catalyst: La2O3-TiO2 highest activity with 1:1 La:Ti ratio; 500°C, 1 atm, in the presence of N2;	A <1 B 95%
With catalyst: Fe-Al2O3 byproducts: CO2; highest SO2 reduction with 40 % Fe in the catalyst, maximum COS yield at 400°C;
With catalyst: Cu-Al2O3 H2O vapour diminishes catalyst activity;

carbon monoxide (201230-82-2) + sulfur dioxide (7446-09-5) → carbon dioxide (124-38-9) + sulfur (7704-34-9)

Conditions	Yield
La-doped ceria above 550°C;	A n/a B 95%
cerium(IV) oxide catalyst exposition to SO2/CO/He mixt. at space velocity 10000 ml/(h*g catalyst) and temp. increase rate 10 K/min; gas chromy.;
Ca-doped cerium oxide catalyst exposition to SO2/CO/He mixt. at space velocity 10000 ml/(h*g catalyst) and temp. increase rate 10 K/min; gas chromy.;

chloroauric acid + Sodium thiosulfate pentahydrate → gold(I) sulfide + Na3Au(thiosulfate)2*2water + gold (I) hydroxide + sulfur (7704-34-9)

Conditions	Yield
With sodium hydroxide; nitric acid In water 0.1 mol H{AuCl4}; 40% NaOH soln.; excess of 0.4 mol Na2S2O3*5H2O; 4 m HNO3 soln.; stirring; filtration; dissolving in alc. and H2O; decompn. with alc.; evapn.; drying in vac. dessicator above H2SO4 in dark 1 d;	A n/a B 95% C n/a D n/a
With NaOH; HNO3 In water 0.1 mol H{AuCl4}; 40% NaOH soln.; excess of 0.4 mol Na2S2O3*5H2O; 4 m HNO3 soln.; stirring; filtration; dissolving in alc. and H2O; decompn. with alc.; evapn.; drying in vac. dessicator above H2SO4 in dark 1 d;	A n/a B 95% C n/a D n/a

manganese(II) sulfide + ammonium tetrathionate → ammonium thiosulfate + manganese sulfite + manganese thiosulfate + hydrogen sulfide (7783-06-4) + sulfur (7704-34-9)

Conditions	Yield
21 hours;	A n/a B n/a C 95% D n/a E n/a
21 hours;	A n/a B n/a C 95% D n/a E n/a
1/2 hours;	A n/a B n/a C 56% D n/a E n/a
1/2 hours;	A n/a B n/a C 56% D n/a E n/a

pyrite → sulfur (7704-34-9) + iron(II) chloride

Conditions	Yield
With chlorine at 600°C;	A 94.7% B n/a
With Cl2 at 600°C;	A 94.7% B n/a

sulfur dioxide (7446-09-5) → sulfur (7704-34-9)

Conditions	Yield
With pyrographite	90%
With hydrogen sulfide In further solvent(s) in glycol with NaOOCCH2CH2COONa;	82%
With hydrogen sulfide In further solvent(s) in glycol with p-H2NC6H4COOK;	73%

hydrogen sulfide (7783-06-4) → sulfur (7704-34-9) + sodium thiosulfate

Conditions	Yield
With phosphate buffer; oxygen In water Kinetics; byproducts: H2O; at pH=8.4-9.0, temp. 25°C, O2 pressure 101 kPa, H2S concn. (2.4-7.2)E-2 M; catalyst Co(II)phthalocyanine(SO3Na)4+MnCl2; not isolated, detd. by iodometry, lead indicator paper, spectrophotometry;	A 90% B n/a
With phosphate buffer; oxygen; cobalt(II) phthalocyaninetetrasulfonate sodium salt In water Kinetics; byproducts: H2O; at pH=8.0-10.2, temp. 25°C, O2 pressure 101 kPa, H2S concn. (2.4-7.2)E-2 M; not isolated, detd. by iodometry, lead indicator paper, spectrophotometry;	A 60% B 40%
With phosphate buffer; oxygen; sodium salt of cobalt disulfophthalocyanine In water Kinetics; byproducts: H2O; at pH=8.0-10.2, temp. 25°C, O2 pressure 101 kPa, H2S concn. (2.4-7.2)E-2 M; not isolated, detd. by iodometry, lead indicator paper, spectrophotometry;	A 60% B 40%
With phosphate buffer; oxygen; manganese(II) sulfate In water Kinetics; byproducts: H2O; at pH=11.3, temp. 25°C, O2 pressure 101 kPa, H2S concn. (2.4-7.2)E-2 M; not isolated, detd. by iodometry, lead indicator paper, spectrophotometry;
With phosphate buffer; oxygen In water Kinetics; byproducts: H2O; at pH=11.3-11.85, temp. 25°C, O2 pressure 101 kPa, H2S concn. (2.4-7.2)E-2 M; catalyst Co(II)phthalocyanine(SO3Na)4+MnSO4; not isolated, detd. by iodometry, lead indicator paper, spectrophotometry;

ammonium bisulfite → trithionate (15579-17-6) + Sulfate (14808-79-8) + dithionate + sulfur (7704-34-9)

Conditions	Yield
In water in concd. soln. in closed tube for 4 years by light;	A <1 B 90% C 0% D n/a

sodium hydrogensulfite → sulfur (7704-34-9)

Conditions	Yield
selenium In not given 70-80°C for about 24 h;	90%
In not given standing for a longtime;
potassium pentathionate In not given 70°C in closed pot;
selenium In not given 70-80°C for about 30 h;
In not given in closed tube at 100°C for 22 h or at 150°C for 7 h;	0%

dimethoxy disulfide (28752-21-8) → iodine (7553-56-2) + sulfur (7704-34-9)

Conditions	Yield
With hydrogenchloride byproducts: H2O, H2S, SO2; in presence of KI;	A 90% B n/a
With HCl byproducts: H2O, H2S, SO2; in presence of KI;	A 90% B n/a

bis(tetraethylammonium)-bis[di-(thiophenolato)-(μ-sulfido)ferrate(III)] + nitrogen(II) oxide (10102-43-9) → (NEt4)[Fe(NO)2(thiophenol)2(-2H)] (106709-47-1) + hydrogen sulfide (7783-06-4) + sulfur (7704-34-9)

Conditions	Yield
With ethanethiol In acetonitrile at 20℃; for 1h; Reagent/catalyst; Inert atmosphere; Schlenk technique;	A 83% B 88% C 6.8%

magnesium sulfate (7487-88-9) → magnesium oxide + sulfur (7704-34-9)

Conditions	Yield
With acetylene In neat (no solvent) redn. with acetylene in a stream of CO2 at 700°C;; MgO containes coal;;	A n/a B 87.5%
With benzene In neat (no solvent) redn. with benzene in a stream of CO2 at 700°C;; MgO containes coal;;	A n/a B 19.2%

tetrabutylammonium hexasulfide (85533-96-6) + tetramethlyammonium chloride (75-57-0) + silver nitrate → n{Ag(S5)(1-)}(Me4N(1+)) (126032-36-8) + sulfur (7704-34-9)

Conditions	Yield
In methanol; acetonitrile oxygen exclusion; treatment of (Bu4N)2S6 with MeCN and methanolic Me4NCl, addn. of AgNO3 in acetonitrile (stirring); cooling (-20°C, 24 h), sulphur removal, standing (room temp.) crystals collection, washing (MeCN), drying (vac.); elem. anal.;	A 83% B n/a

rongalite (149-44-0) → trithioformaldehyde (36069-03-1) + sulfur dioxide (7446-09-5) + Sulfate (14808-79-8) + sulphurous acid (7782-99-2) + sulfur (7704-34-9)

Conditions	Yield
With hydrogenchloride In not given byproducts: H2O, polythionic acids; digesting with HCl-soln.;	A n/a B 82% C 0% D n/a E 82%
With HCl In not given byproducts: H2O, polythionic acids; digesting with HCl-soln.;	A n/a B 82% C 0% D n/a E 82%

sodium sulfide + sulphurous acid (7782-99-2) → water (7732-18-5) + sulfur (7704-34-9) + sodium thiosulfate

Conditions	Yield
In water pure SO2 is introduced into concd. Na2S soln. at 60°C;;	A n/a B n/a C 80%
In water at 20°C, aq. SO2 soln., diluted Na2S soln.;

bismuth (7440-69-9) + sulfur (7704-34-9) → bismuth(III) sulfide

Conditions	Yield
In neat (no solvent) under dry N2 atm. in vac. glovebox; mixt. of Bi and S was transferred inquartz tube, with was flame sealed under vac.; tube was heated to 650.d egree.C for 48 h; stayed at 650°C for 2 ds; cooled to 50°Cin 10 h; ground into powder;	100%
In melt by melting at possible min. temp.;
In melt addition of S to molten Bi at 600-700°C;; Bi content 1 - 2 %;;

antimony (7440-36-0) + sulfur (7704-34-9) → antimony(III) sulfide

Conditions	Yield
In melt melting of Sb and S at 450-500 °C gives complete reaction; slow cooling;;	100%
heating;
mixt. fusing (evac. quartz ampoule); vac. sublimation;

sulfur (7704-34-9) + sodium nitrite (7632-00-0) → sodium thiosulfate

Conditions	Yield
In N,N-dimethyl-formamide byproducts: N2O; at about 80°C, under N2 or CO2, cooling, separation of Na2S2O3;; washing with acetone, analytically pure;;	100%
In further solvent(s) byproducts: N2O; solvent: dimethyl acetamide, at about 80°C, under N2 or CO2, cooling, separation of Na2S2O3;; washing with acetone, analytically pure;;	100%

sulfur (7704-34-9) + phosphorus trichloride (7719-12-2, 52843-90-0) → trichlorothiophosphine (3982-91-0)

Conditions	Yield
With disulfur dichloride; iron(III) chloride In neat (no solvent) addn. of a mixt. of 140 g PCl3 and 1.7 g S2Cl2 drop by drop to a hot mixt. of 160 g PSCl3, 2 g anhydrous FeCl3 and 38 g S on stirring and refluxing (4.5 h); refluxing for 1 h, distg. off PSCl3;;	100%
In neat (no solvent) react. molten S with PCl3 at 124-126 °C at ambient pressure; use of a catalyst formed on melting S with active carbon and boiling in PSCl3 at 200 °C;;
disulfur dichloride In not given react. with S2Cl2 as catalyst;;

bis(perfluorophenyl) selenide (973-18-2) + sulfur (7704-34-9) → pentafluorophenyl sulfide (1043-50-1)

Conditions	Yield
at 230°C;	100%
at 230°C;	100%

bismuth (7440-69-9) + potassium (7440-09-7) + sulfur (7704-34-9) → potassium metathiobismuthite

Conditions	Yield
In neat (no solvent)	100%
differential thermal anal.;	100%

bromine (7726-95-6) + sulfur (7704-34-9) + molybdenum (7439-98-7) → Mo3(12+)*S(2-)*3S2(2-)*4Br(1-)=Mo3S7Br4

Conditions	Yield
In neat (no solvent) reactants placing into Mo-glass ampule, cooling (liquid N2), evacuation,sealing, gradual increasing temperature and heating (280°C, 14 h ; 400°C, 40 h), cooling, excess Br2 removing; remaining solid washing (CHCl3), vacuum drying (50°C, 6 h); elem.anal.;	100%

chromium chloride hexahydrate + tetraphenylphosphonium bromide (2751-90-8) + sulfur (7704-34-9) + ethylenediamine (107-15-3) → [(C6H5)4P](1+)*[Cr(NH2CH2CH2NH2)(S5)2](1-)=[(C6H5)4P][Cr(NH2CH2CH2NH2)(S5)2] (236386-04-2)

Conditions	Yield
In water stoichiometric amts., 10% en in H2O, heating (398 K, 7 d);	100%

tin (7440-31-5) + nickel (7440-02-0) + sulfur (7704-34-9) + 1,2-diaminopropan (78-90-0, 10424-38-1) → [Ni(1,2-diaminopropane)3]2Sn2S6*2H2O

Conditions	Yield
In further solvent(s) High Pressure; prepd. under solvothermal conditions; reactants weighted in ratio of 1 Ni:1 Sn:3 S, heated in sealed Teflon-lined steel autoclave in pure 1,2-diaminopropane for 7 d at 140°C; elem. anal.;	100%

2-phenyl-4,5-[1,2(1,2-dicarba-closo-dodecaborano)]-1,3-diselena-2-phospha-cyclopentane (1017605-86-5) + sulfur (7704-34-9) → 2-phenyl-2-thio-4,5-[1,2(1,2-dicarba-closo-dodecaborano)]-1,3-diselena-2-λ5-phospha-cyclopentane (1017605-87-6)

Conditions	Yield
In dichloromethane-d2 S added to B-compound in CD2Cl2; mixt. stirred overnight; crystallized from CH2Cl2 at room temp.;	100%

bis[1,3-dihydro-1-methyl-3-(1-methylethyl)-2H-imidazol-2-ylidene]iodocopper + sulfur (7704-34-9) → 1,3-dihydro-1-methyl-3-(1-methylethyl)-2H-imidazol-2-thione (61640-29-7)

Conditions	Yield
In chloroform at 20℃; for 4h; Inert atmosphere;	100%

bis(1-[2,6-bis(1-methylethyl)phenyl]-1,3-dihydro-3-methyl-2-H-imidazol-2-ylidene)copper(1+) hexafluorophosphate(1-) (1:1) + sulfur (7704-34-9) → 1,3-dihydro-1-[2,6-bis(1-methylethyl)phenyl]-3-methyl-2H-imidazol-2.thione (1184635-07-1)

Conditions	Yield
In chloroform at 20℃; for 16h; Inert atmosphere;	100%

lanthanum(III) oxide + tungsten(VI) oxide + cobalt (7440-48-4) + sulfur (7704-34-9) + tungsten (7440-33-7) → La3CoS3(6+)*WO6(6-)=La3CoWS3O6

Conditions	Yield
In melt stoich. amts. of La2O3, S, W, WO3, Co mixed with KCl flux; sealed in carbon coated SiO2 ampoule under vac.; heated from 200 to 400°C in 24 h; held for 48 h; heated to 950°C in 12 h; held for 120 h; cooled to room temp. within 24 h; soaked in H2O overnight; washed with H2O; detn. by EDX, XRD;	100%

tellurium + cesium azide (22750-57-8) + sulfur (7704-34-9) → cesium thiotellurate(II)

Conditions	Yield
In neat (no solvent) at 500℃; for 96h;	100%

tellurium + cesium azide (22750-57-8) + sulfur (7704-34-9) → cesium thiotellurate(IV)

Conditions	Yield
In neat (no solvent) at 500℃; for 96h;	100%

sodium sulfide + uranium + tetraphosphorus decasulfide (15857-57-5) + sulfur (7704-34-9) → P2S7(4-)*U(4+)

Conditions	Yield
In neat (no solvent) at 130 - 700℃; for 348h; Sealed tube;	100%

uranium + tetraphosphorus decasulfide (15857-57-5) + sulfur (7704-34-9) → P2S6(4-)*U(4+)

Conditions	Yield
In neat (no solvent) at 130 - 700℃; for 348h; Sealed tube;	100%

uranium + tetraphosphorus decasulfide (15857-57-5) + sulfur (7704-34-9) → P2S7(4-)*U(4+)

Conditions	Yield
In neat (no solvent) at 130 - 700℃; for 348h; Sealed tube;	100%

C33H38GeN2OSeSi + sulfur (7704-34-9) → C33H38GeN2OSSi

Conditions	Yield
In tetrahydrofuran at 20℃; for 10h;	100%

C33H38GeN2OSi + sulfur (7704-34-9) → C33H38GeN2OSSi

Conditions	Yield
In tetrahydrofuran at 20℃; for 2h;	100%

bismuth (7440-69-9) + tin (7440-31-5) + lithium sulfide + sulfur (7704-34-9) → Li0.97Sn2.06Bi4.97S10

Conditions	Yield
Stage #1: bismuth; tin; lithium sulfide; sulfur at 800℃; under 0.00150015 Torr; for 10h; Inert atmosphere; Glovebox; Sealed tube; Stage #2: at 800℃; for 26h;	100%

yttrium(III) oxysulfide + terbium dioxosulfide + silica gel (112926-00-8, 7631-86-9) + sulfur (7704-34-9) + silicon (7440-21-3) → (Y0.98Tb0.02)4S3(Si2O7)

Conditions	Yield
With cesium chloride at 1100℃; for 12h; Milling; Sealed tube;	100%

yttrium(III) oxysulfide + terbium dioxosulfide + silica gel (112926-00-8, 7631-86-9) + sulfur (7704-34-9) + silicon (7440-21-3) → (Y0.96Tb0.04)4S3(Si2O7)

Conditions	Yield
With cesium chloride at 1100℃; for 12h; Milling; Sealed tube;	100%

yttrium(III) oxysulfide + europium oxysulfide + silica gel (112926-00-8, 7631-86-9) + sulfur (7704-34-9) + silicon (7440-21-3) → (Y0.99Eu0.01)4S3(Si2O7)

Conditions	Yield
With cesium chloride at 1100℃; for 12h; Milling; Sealed tube;	100%

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