Sulfide (British English sulphide) is an inorganic anion of sulfur with the chemical formula S2− or a compound containing one or more S2− ions. Solutions of sulfide salts are corrosive. Sulfide also refers to chemical compounds large families of inorganic and organic compounds, e.g. lead sulfide and dimethyl sulfide. Hydrogen sulfide (H2S) and bisulfide (SH−) are the conjugate acids of sulfide.
|Systematic IUPAC name|
3D model (JSmol)
|Molar mass||32.06 g·mol−1|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
- S2− + H2O → SH− + OH−
Upon treatment with an acid, sulfide salts convert to hydrogen sulfide:
- S2− + H+ → SH−
- SH− + H+ → H2S
Oxidation of sulfide is a complicated process. Depending on the conditions, the oxidation can produce elemental sulfur, polysulfides, polythionates, sulfite, or sulfate. Metal sulfides react with halogens, forming sulfur and metal salts.
- 8 MgS + 8 I2 → S8 + 8 MgI2
Aqueous solutions of transition metals cations react with sulfide sources (H2S, NaHS, Na2S) to precipitate solid sulfides. Such inorganic sulfides typically have very low solubility in water, and many are related to minerals with the same composition (see below). One famous example is the bright yellow species CdS or "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. The fungus Aspergillus niger plays a role in the solubilization of heavy metal sulfides.
Many important metal ores are sulfides. Significant examples include: argentite (silver sulfide), cinnabar (mercury sulfide), 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 sulfideEdit
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, pipelines 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 (S
3) 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.
In organic chemistry, "sulfide" usually refers to the linkage C–S–C, although the term 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 (that is, Mo4+ and two S2−). Iron disulfide (pyrite, FeS2) on the other hand consists of S2−
2, 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 a precursor to organosulfur compounds.||−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 organosulfur compound (thioether) that was used as a chemical weapon in the First World War.||13–14||217||505-60-2|
|Ag2S||Silver sulfide is a component of silver tarnish.||21548-73-2|
|Na2S||Sodium sulfide, as the hydrate, is used in manufacture of kraft paper and as a precursor to organosulfur compounds.||920||1180||1313-82-2|
|ZnS||Zinc sulfide is used for lenses and other optical devices in the infrared part of the spectrum. ZnS-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|
|C6H4S||Polyphenylene sulfide is a polymer commonly called "Sulfar". Its repeating units are bonded together by sulfide (thioether) linkages.||26125-40-6 |
|SeS2||Selenium disulfide 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||Known as "fool's gold", pyrite, is a common mineral.||600||1317-66-4|
Sulfide compounds can be prepared in several different ways:
- Direct combination of elements:
- Example: Fe(s) + S(s) → FeS(s)
- Reduction of a sulfate:
- Example: MgSO4(s) + 4C(s) → MgS(s) + 4CO(g)
- 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.
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(2−) (CHEBI:15138)". Chemical Entities of Biological Interest (ChEBI). UK: European Bioinformatics Institute.
- May, P.M.; Batka, D.; Hefter, G.; Könignberger, E.; Rowland, D. (2018). "Goodbye to S2-". Chem. Comm. doi:10.1039/c8cc00187a.
- Meyer, B; Ward, K; Koshlap, K; Peter, L (1983). "Second dissociation constant of hydrogen sulfide". Inorganic Chemistry. 22: 2345. doi:10.1021/ic00158a027.
- Harbhajan Singh. Mycoremediation: Fungal Bioremediation. p. 509.
- Vaughan, D. J.; Craig, J. R. “Mineral chemistry of metal sulfides" Cambridge University Press, Cambridge: 1978. ISBN 0-521-21489-0.
- Atkins; Shriver (2010). Inorganic Chemistry (5th ed.). New York: W. H. Freeman & Co. p. 413.