1313-82-2 Usage
Chemical Properties
Different sources of media describe the Chemical Properties of 1313-82-2 differently. You can refer to the following data:
1. Sodium sulfide is the chemical compound with the formula Na?S, or more commonly its hydrate Na?S·9H?O. Both are colorless water-soluble salts that give strongly alkaline solutions. When exposed to moist air, Na?S and its hydrates emit hydrogen sulfide, which smells like rotten eggs. Sodium sulfide, anhydrous is a yellow to brick red crystalline mass or fused solid. If exposed to moist air, it absorbs moisture from the air, and it is liable to spontaneous heating and may cause ignition of nearby combustible material. The industrial sodium sulfide often exhibits pink, reddish brown or yellowish brown color for containing impurities.
2. It is pale yellow flakes with the main features being the iron (Fe2O3) content is lower than 30 mg/kg. See other properties in sodium sulfide.
3. Sodium sulfide,Na2S, also known as sodium sulfuret,is an irritating, water-soluble, yellowish to reddish, deliquescent powder that melts at 1180°C (2156 °F). Sodium sulfide is used as a chemical intermediate and solvent,in conversion of wood into paper pulp, as a photographic and analytical reagent,as a source of sulfide,as a reducing agent,in organic reactions, as a depilatory, and in sheep dips.
Sodium sulfide
Sodium sulfide is also known as smelly soda and stinky base. At room temperature, the pure product is colorless or slightly purple prismatic crystal. The industrial sodium sulfide often exhibits pink, reddish brown or yellowish brown color for containing impurities. It has rotten egg smell and is corrosive and toxic. Its density is 2.427. It will be subject to decomposition at 920 ℃. It is soluble in cool water and easily soluble in hot water with dissolving in water almost fully being hydrolyzed into sodium hydroxide and sodium hydrosulfide (at 10 ℃, the solubility is 15.4; while the solubility is 57.2 g at 90 ℃). The aqueous water exhibits strongly alkalinity and is corrosive on copper, wood, skin, etc. It is slightly soluble in ethanol but insoluble in ether. When being encountered strong acid, the sodium sulfide will release hydrogen sulfide. It will be subject to deliquescence in air and is easily oxidized into sodium thiosulfate. Sodium sulfide is mainly used as the raw materials of hides depilatories, pulp cooking agent, and sulfur dye, the reducing agents of dye intermediates, fabric dyeing mordant, and ore flotation agent. It can also be used as viscose fiber desulfurizer and the raw material for production of sodium hydrosulfide and sodium polysulfide.
The sodium sulfide in our county was originated in the 1830s. The production of it was earliest started from a chemical plant in Dalian, Liaoning in small-scale. Upon entering into the mid-1980s to the 1990s, with the vigorous development of the international chemical industry, the domestic industry had undergone a fundamental transformation with both the number and scale of production being dramatically increased with rapid development. The production area of sodium sulfide centered in Shanxi Yuncheng has quickly expanded to a dozen of other provinces or cities including Yunnan, Xinjiang, Inner Mongolia, Gansu, Qinghai, Ningxia, and Shaanxi. The national annual production capacity has increased from the value of 420,000 tons by the end of the 80s to a value of 640,000 tons in mid-1990s. The region with the fastest growing includes Inner Mongolia, Gansu, and Xinjiang region at northwest of China. The production capacity has reached 200,000 tons in Inner Mongolia, which has become the largest production base of sodium sulfide in China.
Figure 1 is a picture of yellow flaky sodium sulfide
The above information is edited by the lookchem of Dai Xiongfeng.
Industrial sodium sulfide
Industrial sodium sulfide is generally a mixture with different numbers of crystalline water; the molecular formula is Na2S ? nH2O; it exhibits as yellow or reddish-brown massive, flaky and granular and is mainly used in paper, dyes, mineral processing, printing and dyeing industries.
GB/T 10500-2000 standard has classified the industrial sodium sulfide products into three categories: Category 1 is ordinary sodium sulfide (commonly known as red base); Class 2 is low-iron sodium sulfide (commonly known as the yellow base); Class 3 is sodium sulfide of high content.
Figure 2 the reference quality indicators of industrial sodium sulfide
Packing, storage and shipping: sodium sulfide belongs to alkaline corrosive substances, classification: GB 8.2 class, number:82011. It is packed with a tight leakproof iron drums with the net weight per barrel being 25.50 kg or 100 kg. The packaging should contain obvious "drugs" and "corrosive substance" signs. It should be stored in a dry, airy shed asbestos with the container must be intact. It can’t be stored and shipped together with acidic materials and oxidizing agents.
Toxicity
Sodium sulfide is strongly corrosive to the skin. Worker subjecting to contact with a solution of sodium sulfide has their hand skin get ruffling and redness. During the operation, you should note that: upon inadvertently contact with skin, you should rinse with water. After the sodium sulfide droplets or small pieces falling into eyes, immediately wash with water for 15 min and send to hospital for treatment. To protect the skin, it is recommended to wash hands with a weak acetic acid solution and then coated with oily ointment. Pay attention to the protection of eye.
Preparation of polyarylene sulfide
We can take industrial sodium sulfide and poly-halogenated aromatic compounds as raw materials; apply multi-component composite catalyst or additive and carry out segmented poly-condensation at normal pressure in high-boiling polar organic solvent (such as hempa) for generating linear high molecular weight polyarylene sulfide. The reaction conversion rate is high with the product being white granular and with excellent mechanical properties, thermal properties and thermal processing stability. Additionally supplement of a certain amount of cross-linking agent can generate higher molecular weight branched or cross-linked polyarylene sulfide.
Uses
Different sources of media describe the Uses of 1313-82-2 differently. You can refer to the following data:
1. It can be used for the production of high-grade sulfur dye and high-quality leather. It can be used in the production of high-grade paper production in the paper industry.
In the dye industry, it can be used for the production of sulfur dye and is the raw material of sulfur green and sulfur blue. In the printing and dyeing industry, it can be used as a facilitator agent for dissolving sulfur dye. In the tanning industry, it can be used for the hydrolysis for hair removal of raw skin and also used for the preparation of sodium polysulfide to help accelerate soaking and softening of dry skin. It can also be used as the cooking agent of papermaking industry. In fiber textile industry, it is used for the denitrofication of artificial fiber textile as well as the reduction of nitration as well as the mordant for cotton fabric dyeing. In the pharmaceutical industry, it is mainly used for the production of antipyretic drugs such as phenacetin. In addition, it can also be used for making sodium thiosulfate, sodium hydrosulfide, and sodium polysulfide.
It can be used for analysis reagents and leather depilatory
It can be used for the manufacture of dyes, sulfide, and used as ore flotation agent, depilatory rawhide, and the cooking agent of paper.
2. These yellow flakes were made by fusing sodium carbonate with
sulfur. Soluble in water but less so in alcohol, sodium sulfide
was lovingly called “stink” by those who used it for toning
prints or intensifying negatives because of its sulfurous smell.
3. used in sulfur dyes, used as reductant, mordant, floatation agent, depilatory for leather, digestion auxiliary in paper-making, and used in textile, pigment and rubber
4. It is used for H2S therapy, to study its effect on the prevention of diabetes in animals.
5. Sodium sulfide (Na2S) is used in the dye industry, in the oxidation process of gold, lead, and
cooper metal ores, as a sheep dip, and to process paper.
Production method
Pulverized coal reduction method: put mirabilite and coal powder in a mixing ratio of 100: (21 to 22.5) (weight ratio) for calcination and reduction at 800~1100 ℃. The resultant after cooling is molten into a liquid. After standing for clarification, the upper portion of the alkaline solution was concentrated to obtain a solid sulfide. The flake (or granules)-like sodium sulfide is made through the transition tank and flaking. The reaction equation is as below:
Na2SO4 + 2C → Na2S + 2CO2
Absorption method: use 380~420 g/L sodium hydroxide solution to absorb H2S> 85% containing hydrogen sulfide waste gas; the resulting product was concentrated by evaporation to obtain sodium sulfide products. Its reaction equation is as below:
H2S + 2NaOH → Na2S + 2H2O
Barium sulfide method: use sodium sulfide and barium sulfide for cross-metathesis reaction to get precipitated barium sulfate. During this process, we can get the byproduct sodium sulfide. The reaction formula is as below:
BaS + Na2SO4 → Na2S + BaSO4 ↓
Gas reduction method: in the presence of iron catalyst, put hydrogen (or carbon monoxide, coal gas, methane gas) into boiling furnace for reaction with sodium sulfate, we can obtain high-quality anhydrous granular sodium sulfide (containing Na2S: 95%~97% ). Its reaction equation is:
Na2SO4 + 4CO → Na2S + 4CO2
Na2SO4 + 4H2 → Na2S + 4H2O
Refined method using the byproduct (4% of sodium sulfide) during the production of precipitated barium sulfate as raw material, pump it into dual-effect evaporator for concentration into 23%; it further enters into the mixing tank for removing iron as well as carbon; pump it into the evaporator (manufactured by pure nickel material) to evaporate the lye into a certain concentration and further send it into the roller squeezing apparatus for flaking and further obtain the finished product after screening and packaging.
Pulverized coal reduction method is the traditional production method for making sodium sulfide. During the manufacturing process, improve the equipment and materials and increase the iron removal process so that the products can meet standards.
Toxicity grading
highly toxic
Acute toxicity
oral-rat LD50: 208 mg/kg; Oral-Mouse LD50: 205 mg/kg
Hazardous characteristics of explosive
it is explosive upon heating and collision.
Flammability and hazard characteristics
it release toxic hydrogen sulfide gas upon acids; anhydrous sodium sulfide is flammable; heating can release toxic fumes of sulfur oxides
Storage characteristics
Treasury: ventilation, low-temperature and dry; store it separately from oxidants and acids
Extinguishing agent
water, sand
Physical properties
White cubic crystal; hygroscopic; density 1.856 g/cm3; melts at 1,172°C; soluble in water 18.6 g/100mL at 20°C and 39 g/100mL at 50°C; aqueous solutions strongly alkaline; slightly soluble in alcohol; insoluble in ether.The pentahydrate consists of flat, shiny prismatic crystals; density 1.58 g/cm3; loses three water molecules at 100°C; melts at 120°C losing all water molecules; soluble in water and alcohol; aqueous solutions strongly alkaline; insoluble in ether.The nonahydrate is a yellowish-white crystalline solid; tetragonal crystals; odor of hydrogen sulfide; the color changes on exposure to light and air, first turning to yellow and then becoming brownish-black, deliquescent; density 1.43 g/cm3; decomposes at about 50°C; very soluble in water; aqueous solution strongly alkaline; slightly soluble in alcohol; insoluble in ether.
Definition
Different sources of media describe the Definition of 1313-82-2 differently. You can refer to the following data:
1. ChEBI: A sulfide salt with formula Na2S. The pentahydrate and (particularly) the nonahydrate are also known. In gel form, sodium sulfide is used to soften toenails to assist in trimming (and so relive pain) of ingrowing toenails.
2. A yellow-red solid, Na2S, formed by the reduction of sodium sulphate with carbon (coke) at elevated temperatures. It is a corrosive and readily oxidized material of variable composition and usually contains polysulphides of the type Na2S2, Na2S3, and Na2S4, which cause the variety of colours. It is known in an anhydrous form (r.d. 1.85; m.p. 1180°C) and as a nonahydrate, Na2S·9H2O (r.d. 1.43; decomposes at 920°C). Other hydrates of sodium sulphide have been reported. The compound is deliquescent, soluble in water with extensive hydrolysis, and slightly soluble in alcohol. It is used in wood pulping, dyestuffs manufacture, and metallurgy on account of its reducing properties. It has also been used for the production of sodium thiosulphate (for the photographic industry) and as a depilatory agent in leather preparation. It is a strong skin irritant.
Preparation
Sodium sulfide is prepared by heating sodium bisulfate with sodium chloride and coal above 950°C. The product mixture is extracted with water and the hydrated sulfide is obtained from the solution by crystallization: NaHSO4 + NaCl + 2C → Na2S + 2CO2↑ + HCl↑Sodium sulfide also is produced from its elements in liquid ammonia: Na + 2S → Na2S.
General Description
Sodium sulfide is a yellow to brick red crystalline mass or fused solid with an odor of rotten eggs. If exposed to moist air Sodium sulfide is liable to spontaneous heating and may cause ignition of nearby combustible material. Sodium sulfide absorbs moisture from the air.
Air & Water Reactions
Aqueous solutions of sodium sulfide when exposed to air slowly convert to sodium hydroxide and sodium thiosulfate. The crystalline form upon exposure to air forms hydrogen sulfide and sodium carbonate [Merck 11th ed. 1989].
Reactivity Profile
SODIUM SULFIDE is a white to yellow crystalline material, flammable. Can explode on rapid heating or when shocked. Violent reaction with carbon, charcoal, diazonium salts, N,N-dichloromethylamine, strong oxidizers, water. On contact with acids Sodium sulfide liberates highly toxic and flammable hydrogen sulfide gas. When heated to decomposition Sodium sulfide emits toxic fumes of sodium oxide, and oxides of sulfur [Bretherick, 5th ed., 1995, p. 1729].
Hazard
Flammable, dangerous fire and explosion
risk. Strong irritant to skin and tissue, liberates toxic
hydrogen sulfide on contact with acids.
Health Hazard
Caustic action on skin and eyes. If ingested may liberate hydrogen sulfide in stomach.
Fire Hazard
Special Hazards of Combustion Products: Irritating sulfur dioxide is produced in fire.
Flammability and Explosibility
Nonflammable
Industrial uses
Different sources of media describe the Industrial uses of 1313-82-2 differently. You can refer to the following data:
1. In non-metallic flotation, sodium sulfide is also used as a depressant and for collector
desorption, in particular, fatty acids from monazite, pyrochlore, zircon and microcline.
As a depressant for quartz, sodium sulfide is an excellent depressant for iron-activated
quartz as well as non-activated quartz.
2. Sodium sulfide (Na2S·9H2O) is a hygroscopic substance with a specific gravity of 1.864
and a melting temperature of 1180 °C. The reagent is soluble in water. The aqueous solution
of sodium sulfide has a highly alkaline reaction resulting from its hydrolysis:
Na2S + H2O ? NaOH + NaHS
Safety Profile
A poison by ingestion and intraperitoneal routes. Flammable when exposed to heat or flame. Unstable and can explode on rapid heating or percussion. Reacts violently with carbon, diazonium salts, n,n-dichloromethylamine, onitroaniline diazonium salt, water. When heated to decomposition it emits toxic fumes of SOx and Na2O. See also SULFIDES
Purification Methods
Some purification of the hydrated salt can be achieved by selecting large crystals and removing the surface layer (contaminated with oxidation products) by washing with distilled water. Other metal ions can be removed from Na2S solutions by passage through a column of Dowex ion-exchange A-1 resin, Na+-form. The hydrated salt can be rendered anhydrous by heating it in a stream of H2 or N2 until water is no longer evolved. (The resulting cake should not be heated to fusion because it is readily oxidised.) Recrystallise it from distilled water [Anderson & Azowlay J Chem Soc, Dalton Trans 469 1986]. Note that sodium sulfide hydrolyses in H2O to form NaHS + H2O, and is therefore alkaline. A 0.1N solution in H2O is 86% hydrolysed at room temperature. Its solubility in H2O is 8% at 0o, 12% at 20o and 30% at 50o. The anhydrous salt is obtained by allowing it to stand in a vacuum over conc H2SO4 or P2O5 at 45o to start with, then at 30-35o when the salt contains 4% of water. The last traces of water are removed by heating to 700o in a glass or porcelain tube in a stream of H2 to give pure H2S. [Fehér in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I pp 358-360 1963.]
Check Digit Verification of cas no
The CAS Registry Mumber 1313-82-2 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 1,3,1 and 3 respectively; the second part has 2 digits, 8 and 2 respectively.
Calculate Digit Verification of CAS Registry Number 1313-82:
(6*1)+(5*3)+(4*1)+(3*3)+(2*8)+(1*2)=52
52 % 10 = 2
So 1313-82-2 is a valid CAS Registry Number.
InChI:InChI=1/2Na.S/rNa2S/c1-3-2
1313-82-2Relevant articles and documents
Complex Hydroxides of Chromium: Na9[Cr(OH)6]2(OH)3 ? 6 H2O and Na4[Cr(OH)6]X ? H2O (X = Cl, (S2)1/2) - Synthesis, Crystal Structure, and Thermal Behaviour
Hinz, Dirk
, p. 1004 - 1011 (2000)
Green plate-like crystals of Na9[Cr(OH)6]2(OH)3 · 6H2O (triclinic, P1?, a = 872.9(1) pm, b = 1142.0(1) pm, c = 1166.0(1) pm, α = 74.27(1)°, β = 87.54(1)°, γ = 70.69(1)°) are obtained upon slow cooling of a hot saturated solution of CrIII in cone. NaOH (50 wt%) at room temperature. In the presence of chloride or disulfide the reaction yields green prismatic crystals of Na4[Cr(OH)6]Cl · H2O (monoclinic, C2/c, a = 1138.8(2) pm, b = 1360.4(1) pm, c = 583.20(7) pm, β = 105.9(1)°) or green elongated plates of Na4[Cr(OH)6](S2)1/2 · H2O (monoclinic, P21/c, a = 580.8(1) pm, b = 1366.5(3) pm, c = 1115.0(2) pm, β = 103.71(2)°), respeclively. The latter compounds crystallize in related structures. All compounds can be described as distorted cubic closest packings of the anions and the crystal water molecules with the cations occupying octahedral sites in an ordered way. The thermal decomposition of the compounds was investigated by DSC/TG or DTA/TG and high temperature X-ray powder diffraction measurements. In all cases the final decomposition product is NaCrO2.
Caldwell, W. E.,Krauskopf, F. C.
, p. 2936 - 2942 (1929)
Na3+xMxP1?xS4 (M = Ge4+, Ti4+, Sn4+) enables high rate all-solid-state Na-ion batteries Na2+2δFe2?δ(SO4)3|Na3+xMxP1?xS4|Na2Ti3O7
Rao, Rayavarapu Prasada,Chen, Haomin,Wong, Lee Loong,Adams, Stefan
, p. 3377 - 3388 (2017)
Electrolytes in current Na-ion batteries are mostly based on the same fundamental chemistry as those in Li-ion batteries-a mixture of flammable liquid cyclic and linear organic carbonates leading to the same safety concerns especially during fast charging. All-solid-state Na-ion rechargeable batteries utilizing non-flammable ceramic Na superionic conductor electrolytes are a promising alternative. Among the known sodium conducting electrolytes the cubic Na3PS4 phase has relatively high sodium ion conductivity exceeding 10?4 S cm?1 at room temperature. Here we systematically study the doping of Na3PS4 with Ge4+, Ti4+, Sn4+ and optimise the processing of these phases. A maximum ionic conductivity of 2.5 × 10?4 S cm?1 is achieved for Na3.1Sn0.1P0.9S4. Utilising this fast Na+ ion conductor, a new class of all-solid-state Na2+2δFe2?δ(SO4)3|Na3+xMxP1?xS4 (M = Ge4+, Ti4+, Sn4+) (x = 0, 0.1)|Na2Ti3O7 sodium-ion secondary batteries is demonstrated that is based on earth-abundant safe materials and features high rate capability even at room temperature. All-solid-state Na2+2δFe2?δ(SO4)3|Na3+xMxP1?xS4|Na2Ti3O7 cells with the newly prepared electrolyte exhibited charge-discharge cycles at room temperature between 1.5 V and 4.0 V. At low rates the initial capacity matches the theoretical capacity of ca. 113 mA h g?1. At 2C rate the first discharge capacity at room temperature is still 83 mA h per gram of Na2+2δFe2?δ(SO4)3 and at 80 °C it rises to 109 mA h per gram with 80% capacity retention over 100 cycles.
Aromatic hydrocarbon-catalyzed direct reaction of sulfur and sodium in a heterogeneous system: Selective and facile synthesis of sodium monosulfide and disulfide
Takata, Toshikazu,Saeki, Daisaku,Makita, Yoshimasa,Yamada, Nobuo,Kihara, Nobuhiro
, p. 3712 - 3714 (2003)
Sodium disulfide and monosulfide were selectively formed via the direct reaction of sulfur and an equimolar amount of sodium in 1,2-dimethoxyethane at 70 °C in the presence of a catalytic amount of aromatic hydrocarbons and ketone.
Preparation of alkali-metal hypothiophosphates in an alcoholic solution
Svirskaya,Lupeiko,Pakhomov,Medvedeva
, p. 762 - 765 (2011)
A procedure was developed for preparation of lithium and sodium hypothiophosphates from the corresponding alkali-metal and phosphorus sulfides in ethanol. The possibility was explored for preparation of tin(II) hypothiophosphate in an alcoholic solution by an exchange reaction between sodium hypothiophosphate and tin(II) chloride.
DETERMINATION OF GIBBS ENERGY OF THE EXCHANGE REACTION OF SULPHIDES USING BETA-ALUMINA SOLID ELECTROLYTE.
Itoh, Mitsuru,Kozuka, Tetsuya Yamamoto Zensaku
, (1988)
EMF measurements of the cell Na(l)/ beta prime -alumina/Na//2S plus Ag//2S plus Ag were carried out in the temperature range 463. 4 to 843. 7 K. The results are represented by the equation E/V ( plus or minus 0. 00057) equals 1. 75793( plus or minus 0. 00
Solvent-thermal preparation of nanocrystalline tin chalcogenide
Qian,Zhang,Wang,Wang,Xie,Qian
, p. 415 - 417 (1999)
Nanocrystalline β-SnS2 has been successfully prepared by the reaction between SnCl4 and anhydrous Na2S using a solvent-thermal method at 150 °C, which is similar to the well-known hydrothermal process except that toluene is substituted for water. X-ray diffraction analysis indicates that the product is the β-SnS2 phase, and no Sn-O vibrations are found in the IR spectra. Transmission electron microscopy shows that the average particle size is about 12 nm.
Topochemical anion metathesis routes to the Zr2N2S phases and the Na2S and ACL derivatives (A = Na, K, Rb)
Stoltz,Ramesha,Sirchio,Goenen,Eichhorn,Salamanca-Riba,Gopalakrishnan
, p. 4285 - 4292 (2003)
Anion metathesis reactions between ZrNCl and A2S (A = Na, K, Rb) in the solid state follow three different pathways depending on reaction temperature and reactant stoichiometry: (1) the reaction of ZrNCl with A2S in the 2:1 stoichiometry at 800 °C/72 h/in vacuo yields α-Zr2N2S with the expected layered structure of La2O2S. Above 850 °C, α-Zr2N2S (P3m1; a = 3.605(1) A, c = 6.421(3) A) neatly transforms to β-Zr2N2S (P63/mmc: a = 3.602(1) A, c = 12.817(1) A). The structures of the α- and β-forms are related by an a/2 shift of successive Zr2N2 layers. (2) The same reaction at low temperatures (300-400 °C) yields ACl intercalated phases of the formula AxZr2N2SClx (0 a ZrNCl-type structure. The S and Cl ions are disordered and the c lattice parameters are alkali dependent (R3m, a ～ 3.6 A, c ～ 28.4 (Na), 28.9 (K), and 30.5 A (Rb). AxZr2N2SClx phases are hygroscopic and reversibly absorb water to give monohydrates. (3) Reaction of ZrNCl with excess A2S at 400-1000 °C gives A2S intercalated phases of the formula A2xZr2N2S1+x (0 a ZrNCl type structure (R3m, a ～ 3.64 A, c ～ 29.48 A). Structural characterization of the new phases and implications of the results are described.
Selective and Facile Synthesis of Sodium Sulfide and Sodium Disulfide Polymorphs
El-Shinawi, Hany,Cussen, Edmund J.,Corr, Serena A.
, p. 7499 - 7502 (2018)
Na2S and Na2S2 were selectively synthesized using a microwave-assisted thermal treatment of a Na+/S solution in tetraglyme between 100 and 200 °C, considerably lower than that of current routes. This novel synthetic pathway yields the Na2S phase in high purity and allows for good selectivity between the polymorphs of Na2S2 (α and β phases). These materials show promising electrochemical properties and are particularly interesting for the continued development of Na-S batteries.
Flux Synthesis of LiAuS and NaAuS: Chicken-Wire-Like Layer Formation by Interweaving of (AuS)nn- Threads. Comparison with α-HgS and AAuS (A = K, Rb)
Axtell III, Enos A.,Liao, Ju-Hsiou,Kanatzidis, Mercouri G.
, p. 5583 - 5587 (1998)
From the reaction of Au with alkali metal polysulfide liquids, LiAuS and NaAuS were discovered. Orange crystals of LiAuS crystallize in the monoclinic space group C2/c, (no. 15), with a = 8.994(2) ?, b = 8.956(2) ?, c = 7.201(3) ?, β= 128.68(1)°, and Z = 8. Light-yellow planks of NaAuS crystallize in the orthorhombic space group Ccca, (no. 68), with a = 14.658(5) ?, b = 21.043(7) ?, c = 7.118(4) ?, and Z = 32. Both compounds contain infinite one-dimensional (AuS)nn- chains, featuring alternating sulfide anions and linear coordinated Au centers. In LiAuS, the chains are zigzag and fully extended and they pack in two mutually perpendicular sets. In NaAuS, the same chains coil in an unusual fashion so that they become interwoven to form layers reminiscent of chicken-wire . This novel coiling mode allows Au-Au contacts to form, which help to stabilize the structure. The structural relationships between LiAuS, NaAuS, Na7Au5S6, AAuQ (A = K, Rb, Cs; Q = S, Se), and α-HgS are explored.
Kinetics and Mechanism of the Reaction of the Ammoniated Electron with Sodium Thiosulfate in Liquid Ammonia
Lau, Nathanielo,Dewald, Robert R.
, p. 2348 - 2350 (1980)
The reaction of sodium with thiosulfate in liquid ammonia was found to be second order, first order with respect to both the sodium and thiosulfate concentration.The sodium ion concentration was found to have a dominant influence on the net reaction rate, and a mechanism involving ion-paired species is proposed.The stoichiometry and reaction products were also determined.
Synthesis in molten alkali metal polythiophosphate fluxes. The new quaternary bismuth and antimony thiophosphates ABiP2S7 (A = K, Rb), A3M(PS4)2 (A = K, Rb, Cs; M = Sb, Bi), Cs3Bi2(PS4)3, and Na0.16Bi1.28P2S6
McCarthy,Kanatzidis
, p. 70 - 85 (1996)
The molten alkali metal polychalcogenide flux method was used to prepare the new compounds ABiP2S7 (A = K, Rb), A3M(PS4)2 (A = K, Rb, Cs; M = Sb, Bi), Cs3Bi2 (PS4)3, and Na0.16Bi1.28P2S6. The structural diversity in this family of compounds ranges from the one-dimensional non-centrosymmetric chains of A3M(PS4)2 and the layered compounds, ABiP2S7 and Cs3Bi2 (PS4)2, to the dense three-dimensional framework of Na0.16Bi1.28P2S6. Their synthesis, structural characterization, optical absorption and thermal properties are reported.
Na2EuAs2S5, NaEuAsS4, and Na4Eu(AsS4)2: Controlling the valency of arsenic in polysulfide fluxes
Bera, Tarun K.,Kanatzidis, Mercouri G.
, p. 4293 - 4299 (2012)
The reactivity of europium with As species in Lewis basic alkali-metal polysulfide fluxes was investigated along with compound formation and the As3+/As5+ interplay vis-a-vis changes in the flux basicity. The compound Na2EuAs2S5 containing trivalent As3+ is stabilized from an arsenic-rich polysulfide flux. It crystallizes in the monoclinic centrosymmetric space group P21/c. Na2EuAs2S5 has [As2S 5]4- units, built of corner sharing AsS3 pyramids, which are coordinated to Eu2+ ions to give a two-dimensional (2D) layered structure. A sodium polysulfide flux with comparatively less arsenic led to the As5+ containing compounds NaEuAsS4 (orthorhombic, Ama2) and Na4Eu(AsS 4)2 (triclinic, P1) depending on Na2S/S ratio. The NaEuAsS4 and Na4Eu(AsS4)2 have a three-dimensional (3D) structure built of [AsS4]3- tetrahedra coordinated to Eu2+ ions. All compounds are semiconductors with optical energy gaps of ～2 eV.
Kingzett
, p. 456 - 456 (1873)
Kraus, C. A.,Ridderhof, J. A.
, p. 79 - 86 (1934)
Mixed thio/oxo orthovanadates Na3[VSxO4-x] (x = 2, 3): Synthesis - crystal structures - properties
Schnabel, Simone,R?hr, Caroline
, p. 479 - 490 (2005)
Mixed sodium thio/oxo orthovanadates(V), dark red Na3[VS 3O] and orange red Na3[VS2O2], were synthesized via reactions in the melt starting from V, Na, Na2S, Na2O and sulfur. The structure of the low temperature phase of Na3[VS3O] (space group Pnma, a = 589.5(3), b = 962.8(5), c = 1186.6(6) pm, Z = 4, R1 = 0.0494) contains anions [VS3O] 3- almost identical to those known from the high temperature form, β-Na3[VS3O] (space group Cmc21, a = 968.4(4), b = 1194.6(4), c = 590.5(2) pm, Z = 4, R1 = 0.0291). The second order phase transition between these two forms at 536°C was studied by temperature dependent powder diffraction and explained on the basis of a comparison of the anion packing in the two related structures. The packing of the dithiodioxovanadate anions in Na3[VS2O2] (space group Pbca, a = 1162.7(2), b = 592.71(12), c = 1766.7(4) pm, Z = 8, R1 = 0.0312) is also closely related. The chemical bonding in the anions [VS 3O]3- and [VS2O2]3- of approximately ideal C3v and C2v symmetry is discussed on the basis of FP-LAPW band structure calculations and force constants obtained from Raman spectroscopy. The decrease of the calculated band gaps with increasing S content x in Na3[VSxO4-x] is in accordance with the optical properties showing a gradually deepening of the crystal and solution colour. Discernible trends in the chemical bonding in this series of mixed thio-oxo anions also include the amount of π bonding of the V-O and V-S bonds and the corresponding variation of force constants and V-O/V-S distances.
An efficient method for synthesizing dimethylsulfonio-34S-propionate hydrochloride from 34S8
Wirth, Joseph S.,Whitman, William B.
, p. 52 - 58 (2019/01/04)
Dimethylsulfoniopropionate (DMSP, (2-carboxyethyl)dimethylsulfonium) is a highly abundant compound in marine environments. As a precursor to the climatically active gas, dimethylsulfide (DMS), DMSP connects the marine and terrestrial sulfur cycles. However, the fate of DMSP in microbial biomass is not well understood as only a few studies have performed isotopic labeling experiments. A previously published method synthesized 34S-labeled DMSP from 34S8, but the efficiency was only 26% and required five separate reactions, expensive reagents, and purification of the products of each reaction. In this study, a method of synthesizing 34S-labeled DMSP from 34S8 is described. Improvements include elemental steps, inexpensive reagents, purification of only one intermediate, and less time to complete. The efficiency of this method is 65% and results in pure DMSP with more than 98% isotope enrichment as determined by 1H-nuclear magnetic resonance (NMR) and gas chromatography–mass spectrometry (GC–MS).
