Polysulfane

Source: Wikipedia, the free encyclopedia.

A polysulfane is a chemical compound of formula H2Sn, where n > 1 (although disulfane (H2S2) is sometimes excluded).[1][2][3] Compounds containing 2 – 8 sulfur atoms have been isolated, longer chain compounds have been detected, but only in solution.[4] H2S2 is colourless, higher members are yellow with the colour increasing with the sulfur content. In the chemical literature the term polysulfanes is sometimes used for compounds containing −(S)n−, e.g. organic polysulfanes R1−(S)n−R2.

Structures

Polysulfanes consist of unbranched chains of sulfur atoms

terminated with hydrogen atoms. The branched isomer of tetrasulfane H2S4, in which the fourth sulfur is bonded to the central sulfur, would be described as trithiosulfurous acid, S=S(−SH)2. Computations suggests that it is less stable than the linear isomer HS−S−S−SH.[5] The S-S-S angles approach 90° in trisulfane H2S3 and higher polysulfanes.[4]

Reactions and properties

Polysulfanes can easily be

oxidised, and are thermodynamically unstable with respect to decomposition (disproportionation
) readily to H2S and sulfur:

8 H2Sn → 8 H2S + (n − 1) S8 (in this chemical reaction, S8 is cyclo-octasulfur, one of the allotropes of sulfur)

This

catalyzed by alkali. To suppress this behavior, containers for polysulfanes are often pretreated with acid to remove traces of alkali.[6]

In contrast to the

anions
form spontaneously by treatment of S2− with elemental sulfur:

S2− + (n − 1) S → [Sn]2−

Beyond H2S and H2S2, many higher polysulfanes H2Sn (n = 3 – 8) are known.[7] They have unbranched sulfur chains. Starting with disulfane H2S2, all known polysulfanes are liquids at room temperature. The density, boiling point and viscosity correlate with chain length. Physical properties of polysulfanes are given in the table below.[6]

Chemical formula Name Density at 20 °C (g/cm3)
Vapour pressure
Extrapolated boiling point
H2S Sulfane 1.363 g/dm3 (gas) 1740 (
kPa
, 21 °C) (gas) 		−60 °C (−76 °F)
H2S2
 Disulfane 1.334 87.7 mmHg (11,690 Pa) 70 °C (158 °F)
H2S3 Trisulfane 1.491 1.4 mmHg (190 Pa) 170 °C (338 °F)
H2S4 Tetrasulfane 1.582 0.035 mmHg (4.7 Pa) 240 °C (464 °F)
H2S5 Pentasulfane 1.644 0.0012 mmHg (0.16 Pa) 285 °C (545 °F)
H2S6 Hexasulfane 1.688 ? ?
H2S7 Heptasulfane 1.721 ? ?
H2S8 Octasulfane 1.747 ? ?

They also react with sulfite and cyanide producing thiosulfate and thiocyanate respectively.[6]

Polysulfanes can be made from polysulfides by pouring a solution of a polysulfide salt into cooled concentrated hydrochloric acid. A mixture of metastable polysulfanes separates as a yellow oil, from which individual compounds may be separated by fractional distillation. Other more selective syntheses are:

Na2Sn + 2 HCl → 2 NaCl + H2Sn (n = 4, 5, 6)
SnCl2 + 2 H2Sm → 2 HCl + H2Sn+2m

The reaction of polysulfanes with sulfur dichloride or disulfur dichloride produces long-chain dichloropolysulfanes:

2 SCl2 + H2Sn → 2 HCl + S2+nCl2
2 S2Cl2 + H2Sn → 2 HCl + S4+nCl2

The reaction with a sulfite salt (a base) quantitatively decomposes the polysulfane to produce thiosulfate and hydrogen sulfide:

(n − 1) SO2−3 + H2Sn → (n − 1) S2O2−3 + H2S

References

  1. doi:10.1351/goldbook.P04753
  2. OCLC 48056955.{{cite book}}: CS1 maint: location missing publisher (link
    )
  3. OCLC 48138330
    .
  4. ^
    doi:10.1007/b13182
  5. doi:10.1021/ja00237a012
    .
  6. ^ a b c Greenwood and Earnshaw, p. 683
  7. doi:10.1007/b13182
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