Sodium polysulfide

Sodium polysulfide

Sodium pentasulfide, a representative component of sodium polysulfide
Names
Other names
Sodium sulfane; Viradon
Identifiers
1344-08-7
UN number UN3266
Properties
Na2Sx
Hazards
Safety data sheet AGFA
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazards (white): no codeNFPA 704 four-colored diamond
0
3
1
Flash point Non-combustible
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Sodium polysulfide is a general term for salts with the formula Na2Sx, where x = 2 to 5. The species Sx2-, called polysulfide anions, include disulfide (S22-), trisulfide (S32-), tetrasulfide (S42-), and pentasulfide (S52-). In principle, but not in practice, the chain lengths could be longer.[1] The salts are dark red solids that dissolve in water to give highly alkaline and corrosive solutions. In air, these salts oxidize, and they evolve hydrogen sulfide by hydrolysis.

Structure

The polysulfide anions form chains with S---S bond distances around 2 Å in length. The chains adopt skewed conformations. In the solid state, these salts are dense solids with strong association of the sodium cations with the anionic termini of the chains.[2]

S42- from the crystal structure, highlighting its skewed conformation.
S52- from the crystal structure, highlighting its skewed conformation.

Production and occurrence

Sodium polysulfide can produced by dissolving sulfur in a solution of sodium sulfide.[3] Alternatively they are produced by the redox reaction of aqueous sodium hydroxide with sulfur at elevated temperatures.[4] Finally they arise by the reduction of elemental sulfur with sodium, a reaction often conducted in anhydrous ammonia.

These salts are used in the production of polysulfide polymers, as a chemical fungicide, as a blackening agent on copper jewellery, as a component in a polysulfide bromide battery, as a toner in a photochemical solution, and in the tanning industry to remove hair from hides.

Reactions

As exploited in the sodium-sulfur battery, the polysulfides absorb and release reducing equivalents by breaking and making S-S bonds, respectively. An idealized reaction for sodium tetrasulfide is shown:

Na2S4 + 2 Na \overrightarrow{\leftarrow} 2 Na2S2

Alkylation gives organic polysulfides according to the following idealized equation:

Na2S4 + 2 RX → 2 NaX + R2S4

Alkylation with an organic dihalide gives polymers called thiokols.

Protonation of these salts gives hydrogen sulfide and elemental sulfur, as illustrated by the reaction of sodium pentasulfide:

Na2S5 + 2 H+ → H2S + 1/2 S8

References

  1. ↑ Elemental Sulfur and Sulfur-Rich Compounds volumes I and II, Steudel, R., Ed.; Springer-Verlag: Berlin, 2003.
  2. ↑ Rosén, E.; Tegman, R. "Preparative and X - ray powder diffraction study of the polysulfides Na2S2, Na2S4 and Na2S5" Acta Chemica Scandinavica 1988, volume 25, pp 3329-3336. doi:10.3891/acta.chem.scand.25-3329
  3. ↑ F. Fehér" Sodium Disulfide", "Sodium Tetrasulfide" "Sodium Pentasulfide" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 361-367.
  4. ↑ Lee, T.C.P. (1999). Properties and applications of elastomeric polysulfides. Rapra Technology. p. 4. ISBN 978-1859571583.
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