Na And S Chemical Formula

Chemical compound

Sodium sulfide

Names
Other names Disodium sulfide
Identifiers
CAS Number	1313-82-2 Y 1313-83-iii (pentahydrate) Y 1313-84-iv (nonahydrate) Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:76208 N
ChemSpider	14120 N
ECHA InfoCard	100.013.829
EC Number	215-211-5
PubChem CID	237873
RTECS number	WE1905000
UNII	YGR27ZW0Y7 Y 6U55N59SZ2 (pentahydrate) Y C02T02993U (nonahydrate) Y
Un number	1385 (anhydrous) 1849 (hydrate)
CompTox Dashboard (EPA)	DTXSID0029636
InChI InChI=1S/2Na.S/q2*+one;-2 North Central: GRVFOGOEDUUMBP-UHFFFAOYSA-N N InChI=one/2Na.S/q2*+1;-2 Primal: GRVFOGOEDUUMBP-UHFFFAOYAP
SMILES [Na+].[Na+].[Southward-two]
Properties
Chemic formula	Na2S
Molar mass	78.0452 m/mol (anhydrous) 240.eighteen one thousand/mol (nonahydrate)
Appearance	colorless, hygroscopic solid
Odor	none
Density	1.856 g/cm3 (anhydrous) one.58 g/cm3 (pentahydrate) 1.43 grand/cmthree (nonohydrate)
Melting point	1,176 °C (2,149 °F; 1,449 K) (anhydrous) 100 °C (pentahydrate) 50 °C (nonahydrate)
Solubility in h2o	12.four g/100 mL (0 °C) xviii.6 k/100 mL (20 °C) 39 g/100 mL (50 °C) (hydrolyses)
Solubility	insoluble in ether slightly soluble in alcohol[ane]
Magnetic susceptibility (χ)	−39.0·x−half-dozen cm3/mol
Structure
Crystal structure	Antifluorite (cubic), cF12
Space group	Fm3m, No. 225
Coordination geometry	Tetrahedral (Na+); cubic (S2−)
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Gamble statements	H302, H311, H314, H400
Precautionary statements	P260, P264, P270, P273, P280, P301+P312, P301+P330+P331, P302+P352, P303+P361+P353, P304+P340, P305+P351+P338, P310, P312, P321, P322, P330, P361, P363, P391, P405, P501
NFPA 704 (fire diamond)	3 ane one
Autoignition temperature	> 480 °C (896 °F; 753 K)
Condom data sheet (SDS)	ICSC 1047
Related compounds
Other anions	Sodium oxide Sodium selenide Sodium telluride Sodium polonide
Other cations	Lithium sulfide Potassium sulfide Rubidium sulfide Caesium sulfide
Related compounds	Sodium hydrosulfide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Nverify (what is Y Due north  ?) Infobox references

Chemical compound

Sodium sulfide is the chemical compound with the formula Na₂S, or more commonly its hydrate Na₂S·9H₂O. Both the anhydrous and the hydrated salts are colorless solids. They are h2o-soluble, giving strongly alkaline solutions. When exposed to moist air, Na_twoS and its hydrates emit hydrogen sulfide, an extremely toxic, flammable and corrosive gas which smells like rotten eggs.

Some commercial samples are specified as Na_twoS·xH₂O, where a weight percentage of Na₂S is specified. Commonly available grades take effectually 60% Na_iiS by weight, which ways that x is around 3. Such technical grades of sodium sulfide have a yellow appearance attributable to the presence of polysulfides. These grades of sodium sulfide are marketed equally 'sodium sulfide flakes'.

Structure [edit]

Na₂S adopts the antifluorite structure,^{[two] [iii]} which means that the Na⁺ centers occupy sites of the fluoride in the CaF_ii framework, and the larger S²⁻ occupy the sites for Ca²⁺.

Production [edit]

Industrially Na₂S is produced by carbothermic reduction of sodium sulfate often using coal:^[4]

Na₂Then₄ + 2 C → Na₂S + 2 CO₂

In the laboratory, the salt can be prepared by reduction of sulfur with sodium in anhydrous ammonia, or by sodium in dry THF with a catalytic amount of naphthalene (forming sodium naphthalenide):^[5]

2 Na + S → Na₂Southward

Reactions with inorganic reagents [edit]

The sulfide ion in sulfide salts such equally sodium sulfide can comprise a proton into the table salt by protonation:

S ^two−
+ H⁺ → SH ⁻

Considering of this capture of the proton (H⁺), sodium sulfide has basic character. Sodium sulfide is strongly bones, able to absorb two protons. Its conjugate acrid is sodium hydrosulfide (SH ⁻
). An aqueous solution contains a significant portion of sulfide ions that are singly protonated.

S ^two−
+ H₂O ${\displaystyle {\ce {<=>>}}}$ SH ⁻
+ OH⁻

SH ⁻
+ H₂O ${\displaystyle {\ce {<<=>}}}$ H₂South + OH⁻

Sodium sulfide is unstable in the presence of water due to the gradual loss of hydrogen sulfide into the atmosphere.

When heated with oxygen and carbon dioxide, sodium sulfide can oxidize to sodium carbonate and sulfur dioxide:

two Na₂S + 3 O₂ + 2 CO₂ → ii Na_iiCO₃ + 2 SO_ii

Oxidation with hydrogen peroxide gives sodium sulfate:^[6]

Na_iiS + 4 H_iiO₂ → 4 H₂O + Na₂And then₄

Upon handling with sulfur, polysulfides are formed:

2 Na₂S + Due south₈ → 2 Na₂S₅

Uses [edit]

Sodium sulfide is primarily used in the kraft procedure in the pulp and paper manufacture.

It is used in h2o treatment equally an oxygen scavenger agent and also as a metals precipitant; in chemical photography for toning black and white photographs; in the textile manufacture as a bleaching amanuensis, for desulfurising and as a dechlorinating amanuensis; and in the leather trade for the sulfitisation of tanning extracts. Information technology is used in chemical manufacturing as a sulfonation and sulfomethylation agent. It is used in the product of rubber chemicals, sulfur dyes and other chemical compounds. Information technology is used in other applications including ore flotation, oil recovery, making dyes, and detergent. It is also used during leather processing, as an unhairing agent in the liming operation.

Reagent in organic chemistry [edit]

Alkylation of sodium sulfide give thioethers:

Na₂South + 2 RX → R₂South + ii NaX

Even aryl halides participate in this reaction.^[7] Past a broadly similar process sodium sulfide can react with alkenes in the thiol-ene reaction to give thioethers. Sodium sulfide can be used every bit nucleophile in Sandmeyer type reactions.^[8] Sodium sulfide reduces1,iii-dinitrobenzene derivatives to the iii-nitroanilines.^[nine] Aqueous solution of sodium sulfide can be refluxed with nitro conveying azo dyes dissolved in dioxane and ethanol to selectively reduce the nitro groups to amine; while other reducible groups, e.m. azo group, remain intact.^[ten] Sulfide has besides been employed in photocatalytic applications.^[xi]

Sodium sulfide is the agile ingredient in Dr. Scholl'southward ingrown toenail pain treatment.

Rubber [edit]

Similar sodium hydroxide, sodium sulfide is strongly alkaline and tin cause chemic burns. Acids react with information technology to rapidly produce hydrogen sulfide, which is highly toxic.

References [edit]

1. ^ Kurzin, Alexander V.; Evdokimov, Andrey Northward.; Golikova, Valerija S.; Pavlova, Olesja S. (June 9, 2010). "Solubility of Sodium Sulfide in Alcohols". J. Chem. Eng. Data. 55 (9): 4080–4081. doi:10.1021/je100276c.
2. ^ Zintl, E; Harder, A; Dauth, B. (1934). "Gitterstruktur der oxyde, sulfide, selenide und telluride des lithiums, natriums und kaliums". Z. Elektrochem. Angew. Phys. Chem. 40: 588–93.
3. ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
4. ^ Holleman, A. F.; Wiberg, Eastward. "Inorganic Chemical science" Bookish Press: San Diego, 2001. ISBN 0-12-352651-v.
5. ^ And then, J.-H; Boudjouk, P; Hong, Harry H.; Weber, William P. (1992). Hexamethyldisilathiane. Inorg. Synth. Inorganic Syntheses. Vol. 29. p. xxx. doi:x.1002/9780470132609.ch11. ISBN978-0-470-13260-9.
6. ^ L. Lange, W. Triebel, "Sulfides, Polysulfides, and Sulfanes" in Ullmann's Encyclopedia of Industrial Chemistry 2000, Wiley-VCH, Weinheim. doi:10.1002/14356007.a25_443
7. ^ Charles C. Price, Gardner W. Stacy "p-Aminophenyldisulfide" Org. Synth. 1948, vol. 28, 14. doi:10.15227/orgsyn.028.0014
8. ^ Khazaei; et al. (2012). "synthesis of thiophenols". Synthesis Messages - Thieme Chemistry. 23 (13): 1893–1896. doi:x.1055/s-0032-1316557.
9. ^ Hartman, W. W.; Silloway, H. 50. (1955). "2-Amino-4-nitrophenol". Organic Syntheses. {{cite periodical}}: CS1 maint: multiple names: authors list (link); Collective Book, vol. 3, p. 82
10. ^ Yu; et al. (2006). "Syntheses of functionalized azobenzenes". Tetrahedron. 62 (44): 10303–10310. doi:x.1016/j.tet.2006.08.069.
11. ^ Savateev, A.; Dontsova, D.; Kurpil, B.; Antonietti, One thousand. (June 2017). "Highly crystalline poly(heptazine imides) past mechanochemical synthesis for photooxidation of various organic substrates using an intriguing electron acceptor – Elemental sulfur". Journal of Catalysis. 350: 203–211. doi:10.1016/j.jcat.2017.02.029.

Na And S Chemical Formula,

Source: https://en.wikipedia.org/wiki/Sodium_sulfide

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