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Sulfide

Names
Systematic IUPAC name Sulfanediide[1] (substitutive) Sulfide(2−)[1] (additive)
Identifiers
CAS Number	18496-25-8 Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:15138
ChemSpider	27079 Y
PubChem CID	29109
InChI InChI=1S/S/q-2 Y Key: UCKMPCXJQFINFW-UHFFFAOYSA-N Y
SMILES [S--]
Properties
Chemical formula	S2−
Molar mass	32.06 g·mol−1
Conjugate acid	Bisulfide
Related compounds
Other anions	Telluride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Sulfide (systematically named sulfanediide, and sulfide(2−)) (British English sulphide) is an inorganic anion of sulfur with the chemical formula S²⁻ or a compound containing one or more S²⁻ ions. 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

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

It has been confirmed that the sulfide ion, S²⁻, does not exist even in hyper-concentrated aqueous alkaline solutions of Na₂S.^[2] Thus, the dissociation reaction

SH⁻ (aq) → S²⁻ + H⁺

does not occur in aqueous solution at any concentration of sulphide. The sulphide ion, S²⁻, was previously reported to be undetectable at concentrations up to 5 M NaOH.^[3] However, the sulfide ion may be produced when a solid is formed. For example cadmium sulphide precipitates in group 2 of qualitative analysis.

H₂S (g) + Cd²⁺ (aq) + 2OH⁻ → CdS↓ (s) + 2H₂O

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 react with 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:

Metal derivatives

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.^[4]

Geology

Many important metal ores are sulfides.^[5] 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, 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
₂O²⁻
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.

Organic chemistry

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.

Disulfides

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.

Examples

Preparation

Sulfide compounds can be prepared in several different ways:^[6]

1. Direct combination of elements:
   

   Example: Fe_(s) + S_(s) → FeS_(s)



2. Reduction of a sulfate:
   

   Example: MgSO_4(s) + 4C_(s) → MgS_(s) + 4CO_(g)



3. Precipitation of an insoluble sulfide:
   

   Example: M²⁺ + H₂S_(g) → MS_(s) + 2H⁺_(aq)

Safety

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

• Dithionite


• Sulfate


• Sulfide stress cracking


• Sulfite


• Tetrathionate


• Thioether


• Thiosulfate

References