World Library  
Flag as Inappropriate
Email this Article


Article Id: WHEBN0000292444
Reproduction Date:

Title: Sulfide  
Author: World Heritage Encyclopedia
Language: English
Subject: Sulfur assimilation, Calcium sulfide, Qualitative inorganic analysis, Telluride (chemistry), Photocatalytic water splitting
Collection: Anions, Corrosion, Functional Groups, Sulfides
Publisher: World Heritage Encyclopedia


Formula of sulfide
Systematic IUPAC name
Sulfanediide[1] (substitutive)
Sulfide(2-)[1] (additive)
ChemSpider  Y
Jmol-3D images Image
Molar mass 32.06 g·mol−1
Related compounds
Other anions
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Sulfide (systematically named sulfanediide, and sulfide(2−)) is an anion of sulfur with the chemical formula S2−. It contributes no color to sulfide salts. As it is classified as a strong base, even dilute solutions of salts such as sodium sulfide (Na2S) are corrosive and can attack the skin. Sulfide is the simplest sulfur anion.


  • Nomenclature 1
  • Chemical properties 2
    • Basicity 2.1
    • Chemical reactions 2.2
  • Metal derivatives 3
  • Geology 4
  • Corrosion induced by sulfide 5
  • Organic chemistry 6
  • Disulfides 7
  • Examples 8
  • Preparation 9
  • Safety 10
  • See also 11
  • References 12


The systematic names sulfanediide and sulfide(2−), valid IUPAC names, are determined according to the substitutive and additive nomenclatures, respectively. However, the name sulfide is also used in compositional IUPAC nomenclature which does not take the nature of bonding involved. Examples of such naming are selenium disulfide and titanium sulfide, which contains no sulfide ions whatsoever.

Sulfide is also used non-systematically, to describe compounds which release hydrogen sulfide upon acidification, or a compound that otherwise incorporates sulfur in some form, such as dimethyl sulfide. "Hydrogen sulfide" is itself an example of a non-systematic name of this nature. However, it is also a trivial name, and the preferred IUPAC name for sulfane.

Chemical properties

Sulfide does not exist in appreciable concentrations even in highly alkaline water, being undetectable at pH < ~15 (8 M NaOH).[2]


The sulfide anion can assimilate a proton by recombination:

S2− + H+ → SH

Because of this capture of a proton (H+), sulfide has basic character. In aqueous solution, it has a pKb value of less than 0. Its conjugate acid is bisulfide (SH). In aqueous solution, most sulfide ions are neutralized.

S2− + H2O SH + OH

Chemical reactions

Upon treatment with a standard acid, sulfide converts to hydrogen sulfide (H2S) and a metal salt. Oxidation of sulfide gives sulfur or sulfate. Metal sulfides are mildly corroded by nonmetals including iodine, bromine, and chlorine forming sulfur and metal salts.

8 MgS + 8 I2 → S8 + 8 MgI2

Sulfur can also be prepared from a sulfide and an appropriate oxidizer:

16 HNO3 + 24 H2S → 16 NO + 3 S8 + 32 H2O

Metal derivatives

Aqueous solutions of cadmium yellow". The black tarnish formed on sterling silver is Ag2S. Such species are sometimes referred to as salts. In fact, the bonding in transition metal sulfides is highly covalent, which gives rise to their semiconductor properties, which in turn is related to the deep colors. Several have practical applications as pigments, in solar cells, and as catalysts. Aspergillus niger plays a role in the solubilization of heavy metal sulfides. [3]


Many important metal ores are sulfides.[4] Significant examples include: argentite (silver sulfide), cinnabar (mercury), galena (lead sulfide), molybdenite (molybdenum sulfide), pentlandite (nickel sulfide]), realgar (arsenic sulfide), and stibnite (antimony), sphalerite (zinc sulfide), and pyrite (iron disulfide), and chalcopyrite (iron-copper sulfide).

Corrosion induced by sulfide

Dissolved free sulfides (H2S, HS and S2−) are very aggressive species for the corrosion of many metals such as steel, stainless steel, and copper. Sulfides present in aqueous solution are responsible for stress corrosion cracking (SCC) of steel, and is also known as sulfide stress cracking. Corrosion is a major concern in many industrial installations processing sulfides: sulfide ore mills, deep oil wells, pipeline transporting soured oil, Kraft paper factories.

Microbially-induced corrosion (MIC) or biogenic sulfide corrosion are also caused by sulfate reducing bacteria producing sulfide that is emitted in the air and oxidized in sulfuric acid by sulfur oxidizing bacteria. Biogenic sulfuric acid reacts with sewerage materials and most generally causes mass loss, cracking of the sewer pipes and ultimately, structural collapse. This kind of deterioration is a major process affecting sewer systems worldwide and leading to very high rehabilitation costs.

Oxidation of sulfide can also form thiosulfate (S2O32−) an intermediate species responsible for severe problems of pitting corrosion of steel and stainless steel while the medium is also acidified by the production of sulfuric acid when oxidation is more advanced.

Organic chemistry

In thioether is less ambiguous. For example, the thioether dimethyl sulfide is CH3-S-CH3. Polyphenylene sulfide (see below) has the empirical formula C6H4S. Occasionally, the term sulfide refers to molecules containing the -SH functional group. For example, methyl sulfide can mean CH3-SH. The preferred descriptor for such SH-containing compounds is thiol or mercaptan, i.e. methanethiol, or methyl mercaptan.


Confusion arises from the different meanings of the term "disulfide". Molybdenum disulfide (MoS2) consists of separated sulfide centers, in association with molybdenum in the formal 4+ oxidation state (Mo4+). Iron disulfide (pyrite, FeS2) on the other hand consists of S22−, or S–S dianion, in association with divalent iron in the formal 2+ oxidation state (ferrous ion: Fe2+). Dimethyldisulfide has the chemical binding CH3-S–S-CH3, whereas carbon disulfide has no S–S bond, being S=C=S (linear molecule analog to CO2). Most often in sulfur chemistry and in biochemistry, the disulfide term is commonly ascribed to the sulfur analogue of the peroxide −O–O− bond. The disulfide bond (−S–S−) plays a major role in the conformation of proteins and in the catalytic activity of enzymes.


Formula Melting point (°C) Boiling point (°C) CAS number
H2S Hydrogen sulfide is a very toxic and corrosive gas characterised by a typical odour of "rotten egg". -85,7 -60,20 7783-06-4
CdS Cadmium sulfide can be used in photocells. 1750 1306-23-6
Calcium polysulfide ("lime sulfur") is a traditional fungicide in gardening.
CS2 Carbon disulfide is sometimes used as a solvent in industrial chemistry. -111.6 46 75-15-0
PbS Lead sulfide is used in infra-red sensors. 1114 1314-87-0
MoS2 Molybdenum disulfide, the mineral molybdenite, is used as a catalyst to remove sulfur from fossil fuels; also as lubricant for high-temperature and high-pressure applications. 1317-33-5
Cl-CH2CH2-S-CH2CH2-Cl Sulfur mustard (mustard gas) is an organosulfide (thioether) that has been used as a chemical weapon in the First World War, the chloride on the molecule acts as a leaving group when in the presence of water and forms a thioether-alcohol and HCl. 13 - 14 217 505-60-2
Ag2S Silver sulfide is formed on silver electrical contacts operating in an atmosphere rich in hydrogen sulfide. 21548-73-2
Na2S Sodium sulfide is an important industrial chemical, used in manufacture of kraft paper, dyes, leather tanning, crude petroleum processing, treatment of heavy metal pollution, and others. 920 1180 1313-82-2
ZnS Zinc sulfide is used for lenses and other optical devices in the infrared part of the spectrum. Zinc sulfide doped with silver is used in alpha detectors while zinc sulfide with traces of copper has applications in photoluminescent strips for emergency lighting and luminous watch dials. 1185 1314-98-3
MeS Several metal sulfides are used as pigments in art, although their use has declined somewhat due to their toxicity. Sulfide pigments include cadmium, mercury, and arsenic.
C6H4S Polyphenylene sulfide is a polymer commonly called "Sulfar". Its repeating units are bonded together by sulfide (thioether) linkages. 26125-40-6
SeS2 Selenium sulfide is an antifungal used in anti-dandruff preparations, such as Selsun Blue. The presence of the highly toxic selenium in healthcare and cosmetics products represents a general health and environmental concern. <100 7488-56-4
FeS2 The crystal lattice of pyrite is made of iron disulfide, in which iron is divalent and present as ferrous ion (Fe2+). 600 1317-66-4


Sulfide compounds can be prepared in several different ways:[5]

1. Direct combination of elements:

Example: Fe(s) + S(s) --> FeS(s)

2. Reduction of a sulfate:

Example: MgSO4(s) + 4C(s) --> MgS(s) + 4CO(g)

3. Precipitation of an insoluble sulfide:

Example: M2+ + H2S(g) --> MS(s) + 2H+(aq)


Many metal sulfides are so insoluble in water that they are probably not very toxic. Some metal sulfides, when exposed to a strong mineral acid, including gastric acids, will release toxic hydrogen sulfide.

Organic sulfides are highly flammable. When a sulfide burns it produces sulfur dioxide (SO2) gas.

Hydrogen sulfide, some of its salts, and almost all organic sulfides have a strong and putrid stench; rotting biomass releases these.

See also


  1. ^ a b "sulfide(2-) (CHEBI:15138)". Chemical Entities of Biological Interest (ChEBI). UK: European Bioinformatics Institute. 
  2. ^ Meyer, B; Ward, K; Koshlap, K; Peter, L (1983). "Second dissociation constant of hydrogen sulfide". Inorganic Chemistry 22: 2345.  
  3. ^ Harbhajan Singh. Mycoremediation: Fungal Bioremediation. p. 509. 
  4. ^ Vaughan, D. J.; Craig, J. R. “Mineral chemistry of metal sulfides" Cambridge University Press, Cambridge: 1978. ISBN 0-521-21489-0.
  5. ^ Atkins, Shriver. Inorganic Chemistry, Fifth Edition. W. H. Freeman and Company, New York; 2010; pp 413.
This article was sourced from Creative Commons Attribution-ShareAlike License; additional terms may apply. World Heritage Encyclopedia content is assembled from numerous content providers, Open Access Publishing, and in compliance with The Fair Access to Science and Technology Research Act (FASTR), Wikimedia Foundation, Inc., Public Library of Science, The Encyclopedia of Life, Open Book Publishers (OBP), PubMed, U.S. National Library of Medicine, National Center for Biotechnology Information, U.S. National Library of Medicine, National Institutes of Health (NIH), U.S. Department of Health & Human Services, and, which sources content from all federal, state, local, tribal, and territorial government publication portals (.gov, .mil, .edu). Funding for and content contributors is made possible from the U.S. Congress, E-Government Act of 2002.
Crowd sourced content that is contributed to World Heritage Encyclopedia is peer reviewed and edited by our editorial staff to ensure quality scholarly research articles.
By using this site, you agree to the Terms of Use and Privacy Policy. World Heritage Encyclopedia™ is a registered trademark of the World Public Library Association, a non-profit organization.

Copyright © World Library Foundation. All rights reserved. eBooks from Hawaii eBook Library are sponsored by the World Library Foundation,
a 501c(4) Member's Support Non-Profit Organization, and is NOT affiliated with any governmental agency or department.