Allotropes of sulfur
The element sulfur exists as many allotropes. In terms of large number of allotropes, sulfur is second only to carbon. In addition to the allotropes, each allotrope often exists in polymorphs, delineated by Greek prefixes (α, β, etc.).
Furthermore, because elemental sulfur has been an item of commerce for centuries, its various forms are given traditional names. Early workers identified some forms that have later proved to be single or mixtures of allotropes. Some forms have been named for their appearance, e.g. "mother of pearl sulfur", or alternatively named for a chemist who was pre-eminent in identifying them, e.g. "Muthmann's sulfur I" or "Engel's sulfur".
The most commonly encountered form of sulphur is the orthorhombic polymorph of S
8, which adopts a puckered ring – or "crown" – structure. Two other polymorphs are known, also with nearly identical molecular structures. In addition to S8, sulfur rings of 6, 7, 9–15, 18 and 20 atoms are known. At least five allotropes are uniquely formed at high pressures, two of which are metallic.
The number of sulfur allotropes reflects the relatively strong S−S bond of 265 kJ/mol. Furthermore, unlike most elements, the allotropes of sulfur can be manipulated in solutions of organic solvents and is amenable to analysis by HPLC.
Phase diagram for sulfurEdit
The pressure-temperature (P-T) phase diagram for sulfur is complex (see image). The region labeled I (a solid region), is α-sulfur. See the legend for further identifications and information, and see the section on high pressure forms for information on these phases.
High pressure solid allotropesEdit
In a high-pressure study at ambient temperatures, four new solid forms, termed II, III, IV, V have been characterized, where α-sulfur is form I. Solid forms II and III are polymeric, while IV and V are metallic (and are superconductive below 10 K and 17 K, respectively). Laser irradiation of solid samples produces three sulfur forms below 200–300 kbar (20–30 GPa).
Solid cyclo allotrope preparationEdit
Two methods exist for the preparation of the cyclo-sulfur allotropes. One of the methods, which is most famous for preparing hexasulfur, is to react hydrogen polysulfides with polysulfur dichloride:
- H2Sx + SyCl2 → cyclo-Sx+y + 2 HCl
- [NH4]2[S5] + (C5H5)2TiCl2 → (C5H5)2TiS5 + 2 NH4Cl
Then the resulting pentasulfur-titanocene complex is allowed to react with polysulfur dichloride to give the desired cyclo-sulfur in the series:
- (C5H5)2TiS5 + SyCl2 → cyclo-Sy+5 + (C5H5)2TiCl2
Solid cyclo-sulfur allotropesEdit
This has not been isolated, but has been detected in the vapour phase.
This was first prepared by M. R. Engel in 1891 by reacting HCl with thiosulfate, HS2O3−. Cyclo-S6 is orange-red and forms a rhombohedral crystal. It is called ρ-sulfur, ε-sulfur, Engel's sulfur and Aten's sulfur. Another method of preparation involves reacting a polysulfane with sulfur monochloride:
- H2S4 + S2Cl2 → cyclo-S6 + 2 HCl (dilute solution in diethyl ether)
It is a bright yellow solid. Four (α-, β-, γ-, δ-) forms of cyclo-heptasulfur are known. Two forms (γ-, δ-)have been characterized. The cyclo-S7 ring has an unusual range of bond lengths of 199.3–218.1 pm. It is said to be the least stable of all of the sulfur allotropes.
α-Sulfur, see image, is the form most commonly found in nature. When pure it has a greenish-yellow colour (traces of cyclo-S7 in commercially available samples make it appear yellower). It is practically insoluble in water and is a good electrical insulator with poor thermal conductivity. It is quite soluble in carbon disulfide: 35.5 g/100 g solvent at 25 °C. It has an orthorhombic crystal structure. This is the predominant form found in "flowers of sulfur", "roll sulfur" and "milk of sulfur". It contains S8 puckered rings, alternatively called a crown shape. The S-S bond lengths are all 203.7 pm and the S-S-S angles are 107.8° with a dihedral angle of 98°. At 95.3 °C, α-sulfur converts to β-sulfur.
This is a yellow solid with a monoclinic crystal form and is less dense than α-sulfur. Like the α- form it contains puckered S8 rings and only differs from it in the way the rings are packed in the crystal. It is unusual because it is only stable above 95.3 °C, below this it converts to α-sulfur. It can be prepared by crystallising at 100 °C and cooling rapidly to slow down formation of α-sulfur. It has a melting point variously quoted as 119.6 °C and 119.8 °C but as it decomposes to other forms at around this temperature the observed melting point can vary from this. The 119 °C melting point has been termed the "ideal melting point" and the typical lower value (114.5 °C) when decomposition occurs, the "natural melting point".
This form, first prepared by F.W. Muthmann in 1890, is sometimes called "nacreous sulfur" or "mother of pearl sulfur" because of its appearance. It crystallises in pale yellow monoclinic needles. It contains puckered S8 rings like α-sulfur and β-sulfur and only differs from them in the way that these rings are packed. It is the densest form of the three. It can be prepared by slowly cooling molten sulfur that has been heated above 150 °C or by chilling solutions of sulfur in carbon disulfide, ethyl alcohol or hydrocarbons. It is found in nature as the mineral rosickyite.
Cyclo-Sn (n = 9–15, 18, 20)Edit
- (η5-C5H5)2TiS5 + Sn−5Cl2 → cyclo-Sn
- Sn−mCl2 + H2Sm → cyclo-Sn
Cyclo-S12 is the most stable cyclo-allotrope. Its structure can be visualised as having sulfur atoms in three parallel planes, 3 in the top, 6 in the middle and three in the bottom.
Two forms (α-, β-) of cyclo-S9 are known, one of which has been characterized.
Two forms of cyclo-S18 are known where the conformation of the ring is different. To differentiate these structures, rather than using the normal crystallographic convention of α-, β-, etc., which in other cyclo-Sn compounds refer to different packings of essentially the same conformer, these two conformers have been termed endo- and exo-.
This is produced from a solution of cyclo-S6 and cyclo-S10 in CS2. It has a density midway between cyclo-S6 and cyclo-S10. The crystal consists of alternate layers of cyclo-S6 and cyclo-S10. For all the elements this may be the only allotrope which contains molecules of different sizes.
Solid catena allotropesEdit
The production of pure forms of catena-sulfur has proved to be extremely difficult. Complicating factors include the purity of the starting material and the thermal history of the sample.
This form, also called fibrous sulfur or ω1-sulfur, has been well characterized. It has a density of 2.01 g·cm−3 (α-sulfur 2.069 g·cm−3) and decomposes around its melting point of 104 °C. It consists of parallel helical sulfur chains. These chains have both left and right-handed "twists" and a radius of 95 pm. The S-S bond length is 206.6 pm, the S-S-S bond angle is 106° and the dihedral angle is 85.3°, (comparable figures for α-sulfur are 203.7 pm, 107.8° and 98.3°).
This has not been well characterized but is believed to consist of criss-crossed helices. It is also called χ-sulfur or ω2-sulfur.
Catena sulfur formsEdit
The naming of the different forms is very confusing and care has to be taken to determine what is being described as the same names are used interchangeably.
This is the quenched product of sulfur melts above 160 °C (at this point the properties of the liquid melt change remarkably, e.g. large increase in viscosity). Its form changes from an initial plastic form gradually to a glassy form, hence its other names of plastic, glassy or vitreous sulfur. It is also called χ-sulfur. It contains a complex mixture of catena-sulfur forms mixed with cyclo-forms.
Fibrous (φ-) sulfurEdit
This is a mixture of the allotropic ψ- form and γ-cycloS8.
This is a commercially available product prepared from amorphous sulfur that has not been stretched prior to extraction of soluble forms with CS2. It sometimes called "white sulfur of Das" or supersublimated sulfur. It is a mixture of ψ-sulfur and lamina sulfur. The composition depends on the exact method of production and the samples history. One well known commercial form is "Crystex". ω-sulfur is used in the vulcanization of rubber.
This name is given to the molten sulfur immediately after melting, cooling this gives predominantly β-sulfur.
This name is applied to solid insoluble sulfur and the melt prior to quenching.
Dark-coloured liquid formed when λ-sulfur is left to stay molten. Contains mixture of Sn rings.
Biradical catena (S∞) chainsEdit
This term is applied to biradical catena- chains in sulfur melts or the chains in the solid.
List of allotropes and formsEdit
Allotropes are in Bold.
|Formula/name||Common name||Other names||Notes|
|S2||disulfur||A diatomic gas with a triplet ground state like dioxygen.|
|S3||trisulfur||A cherry red triatomic gas with a bent ozone-like structure.|
|S4||tetrasulfur||Structure not determined but calculations indicate it to be cyclo-S4.|
|cyclo-S5||cyclo-pentasulfur||Not yet isolated, only detected in sulfur vapour.|
|cyclo-S6||ρ-sulfur||cyclo-hexasulfur, "ε-sulfur", "Engel's" sulfur, "Aten's sulfur"||The ring adopts a chair form in the solid.|
|cyclo-S6/cyclo-S10 adduct||A mixed crystal with alternating layers of cyclo-S6 and cyclo-S10.|
|cyclo-S7||α-, β-, γ-, δ- cycloheptasulfur||Four forms known, two(γ-, δ- ) characterized.|
|cyclo-S8||α-sulfur||"orthorhombic sulfur" "rhombic sulfur", "flowers of sulfur", "roll sulfur" "milk of sulfur", "Muthmann's sulfur I"||Yellow solid consisting of S8 puckered rings. The thermodynamically stable form at ordinary temperatures.|
|cyclo-S8||β-sulfur||"monoclinic sulfur" "prismatic sulfur" "Muthmann's sulfur II"||Yellow crystalline solid, consisting of S8 puckered rings. Only stable above 95.3 °C, it reverts to α-sulfur at room temperature.|
|cyclo-S8||γ-sulfur||"nacreous sulfur" "mother of pearl sulfur" "Gernez’s sulfur" or "Muthmann's sulfur III".||Light yellow solid, crystal monoclinic, consisting of S8 puckered rings. Found in nature as the rare mineral rosickyite.|
n = 9–15, 18, 20
|cyclo-(nona; deca; undeca; dodeca; trideca; tetradeca; pentadeca; octadeca; eicosa)sulfur||Pure forms all allotropes, cyclo-S9 has four forms, cyclo-S18 has two forms. Generally synthesised rather than obtained by treatment of another form of elemental sulfur.|
|catena-Sx||fibrous (ψ) sulfur||Well characterized, contains parallel helical sulfur chains and is difficult to obtain pure.|
|catena-Sx||lamina sulfur||Not well characterized, contains helical chains partially crossed.|
|amorphous sulfur||"plastic sulfur"||Quenched molten sulfur at first solidifies to amorphous or glassy sulfur. Consists of a mixture of catena sulfur and cyclo sulfur.|
|insoluble sulfur||Quenched liquid sulfur with soluble species extracted with CS2. Sometimes called polymeric sulfur, μ-S or ω-S.|
|φ-sulfur||A mixture of allotropic ψ-sulfur and cyclo forms mainly γ-cyclo-S8.|
|ω-sulfur||insoluble sulfur||A mixture of chains with a minimum of soluble species.|
|λ-sulfur||Light yellow mobile liquid formed when β-sulfur first melts at 119.6 °C. Consists of S8 rings.|
|μ-sulfur||The dark-coloured viscous liquid formed when π-sulfur is heated and the solid when cooled. Contains a mixture of polymeric chains.|
|π-sulfur||Dark-coloured liquid that develops as λ-sulfur is left molten. Contains mixture of Sn rings.|
|High-pressure forms of α-sulfur||S-II, S-III, S-IV, S-V and others||Four high-pressure phases (at ambient temperature) including two that are metallic and become superconducting at low temperature and some additional phases photo-induced below 20–30 GPa.|
High-temperature gaseous allotropesEdit
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Disulfur, S2, is the predominant species in sulfur vapour above 720 °C (a temperature above that shown in the phase diagram); at low pressure (1 mmHg) at 530 °C, it comprises 99% of the vapor. It is a triplet diradical (like dioxygen and sulfur monoxide), with an S−S bond length of 188.7 pm. The blue colour of burning sulfur is due to the emission of light by the S2 molecule produced in the flame.
The S2 molecule has been trapped in the compound [S2I4][EF6]2 (E = As, Sb) for crystallographic measurements, produced by reacting elemental sulfur with excess iodine in liquid sulfur dioxide. The [S2I4]2+ cation has an "open-book" structure, in which each [I2]+ ion donates the unpaired electron in the π* molecular orbital to a vacant orbital of the S2 molecule.
This has been detected in the vapour phase but has not been fully characterized; various forms, (e.g. chains, branched chains and rings) have been proposed. A primary research result based on theoretical calculations suggests that it has a ring structure.[non-primary source needed]
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