Hydrogen disulfide

Chemical compound

Hydrogen disulfide

Top (white): hydrogen, bottom (yellow): sulfur

Names
IUPAC name

Dihydrogen disulfide

Systematic IUPAC name

Disulfane

Other names

* Dithioperoxol
* Hydrogen disulphide
* Hydrogen persulfide
* Hydrogen persulphide
* Thiosulfenic acid

Identifiers

CAS Number

* 13465-07-1 Y

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:33114 Y

ChemSpider |

* 97274 Y

PubChem CID

* 108196

CompTox Dashboard (EPA)

* DTXSID10158844

InChI

* InChI=1S/H2S2/c1-2/h1-2H Y

Key: BWGNESOTFCXPMA-UHFFFAOYSA-N Y

* InChI=1/H2S2/c1-2/h1-2H

Key: BWGNESOTFCXPMA-UHFFFAOYAV

SMILES

* SS

Properties

Chemical formula

| H2S2
Molar mass | 66.14 g·mol−1
Appearance  | Pale yellow liquid
Density | 1.334 g/cm3
Melting point | −89.6 °C (−129.3 °F; 183.6 K)
Boiling point | 70.7 °C (159.3 °F; 343.8 K)
Hazards
Flash point | flammable
Related compounds

Related compounds

* Hydrogen sulfide
* Hydrogen peroxide
* Hydrogen diselenide
* Hydrogen ditelluride
* Disulfur dichloride

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Y verify (what is YN ?)

Infobox references

Chemical compound

Hydrogen disulfide is the inorganic compound with the formula H2S2. This hydrogen chalcogenide is a pale yellow volatile liquid with a camphor-like odor. It decomposes readily to hydrogen sulfide (H2S) and elemental sulfur.[1]

## Structure[edit]

The connection of atoms in the hydrogen disulfide molecule is H−S−S−H. The structure of hydrogen disulfide is similar to that of hydrogen peroxide, with C2 point group symmetry. Both molecules are distinctly nonplanar. The dihedral angle between the Ha−S−S and S−S−Hb planes is 90.6°, compared with 111.5° in H2O2. The H−S−S bond angle is 92°, close to 90° for unhybridized divalent sulfur.[1]

## Synthesis[edit]

Hydrogen disulfide can be synthesised by cracking polysulfanes (H2Sn) according to this idealized equation:

H2Sn → H2S2 \+ Sn−2

The main impurity is trisulfane (H2S3).[1] The precursor polysulfane is produced by the reaction of hydrochloric acid with aqueous sodium polysulfide. The polysulfane precipitates as an oil.[1][2]

## Reactions[edit]

Upon contact with water or alcohols, hydrogen disulfide readily decomposes under ambient conditions to hydrogen sulfide and sulfur.

It is more acidic than hydrogen sulfide, but the pKa has not been reported.[1]

In organosulfur chemistry, hydrogen disulfide adds to alkenes to give disulfides and thiols.[3]

## Quantum tunneling and its suppression in deuterium disulfide[edit]

The deuterated form of hydrogen disulfide, deuterium disulfide D−S−S−D (dideuterodisulfane), has a similar geometry to H−S−S−H, but its tunneling time is slower, making it a convenient test case for the quantum Zeno effect, in which frequent observation of a quantum system suppresses its normal evolution. Trost and Hornberger[4] have calculated that while an isolated D−S−S−D molecule would spontaneously oscillate between left and right chiral forms with a period of 5.6 milliseconds, the presence of a small amount of inert helium gas should stabilize the chiral states, the collisions of the helium atoms in effect "observing" the molecule's momentary chirality and so suppressing spontaneous evolution to the other chiral state.[5]

## Health effects[edit]

In high concentrations, it can cause dizziness, disorientation and ultimately unconsciousness.[6]

## Historic literature[edit]

* Walton, James H.; Parsons, Llewellyn B. (1921-12-01). "Preparation and Properties of the Persulfides of Hydrogen". J. Am. Chem. Soc. 43 (12): 2539–48. doi:10.1021/ja01445a008.
* Georg Brauer: Handbook of Preparative Inorganic Chemistry Volume I, page 391, Wiley, 1963.
* von Richter, Victor: Translated by Edgar F Smith, "A Text-Book of Inorganic Chemistry", Page 111, P. Blakiston, Son & Co., 1893

## References[edit]

1. ^ a b c d e R. Steudel "Inorganic Polysulfanes H2Sn with n > 1" in Elemental Sulfur and Sulfur-Rich Compounds II (Topics in Current Chemistry) 2003, Volume 231, pp 99–125. doi:10.1007/b13182
2. ^ De, A. K. (2001-01-15). A Text Book of Inorganic Chemistry. ISBN 978-81-224-1384-7.
3. ^ Hazardous Reagents, Robinson Brothers
4. ^ Trost, J.; Hornberger, K. (2009). "Hund's Paradox and the Collisional Stabilization of Chiral Molecules". Phys. Rev. Lett. 103 (2): 023202. arXiv:0811.2140. Bibcode:2009PhRvL.103b3202T. doi:10.1103/PhysRevLett.103.023202. PMID 19659202.
5. ^ Month-long calculation solves 82-year-old quantum paradox, Physics Today, September 2009, p. 16
6. ^ Stein, Wilkinson, G (2007). Seminars in general adult psychiatry. Royal College of Psychiatrists. ISBN 978-1-904671-44-2.

* v
* t
* e

Hydrogen compounds

* H3AsO3
* H3AsO4
* HArF
* HAt
* HSO3F
* HBF4
* HBr
* HBrO
* HBrO2
* HBrO3
* HBrO4
* HCl
* HClO
* HClO2
* HClO3
* HClO4
* HCN
* HCNO
* H2CrO4/H2Cr2O7
* H2CO3
* H2CS3
* HF
* HFO
* HI
* HIO
* HIO2
* HIO3
* HIO4
* HMnO4
* H2MnO4
* H2MoO4
* HNC
* NaHCO3
* HNCO
* HNO
* HNO2
* HNO3
* H2N2O2
* HNO5S
* H3NSO3
* H2O
* H2O2
* H2O3
* H

* H

* H3PO2
* H3PO3
* H3PO4
* H4P2O7
* H5P3O10
* H2PtCl6
* H2S
* H2S2
* H2Se
* H2SeO3
* H2SeO4
* H4SiO4
* H2SiF6
* HSCN
* HNCS
* H2SO3
* H2SO4
* H2SO5
* H2S2O3
* H

* H2S2O6
* H2S2O7
* H2S2O8
* CF3SO3H
* H2Te
* H2TeO3
* H6TeO6
* H4TiO4
* H2Po
* HCo(CO)4

* v
* t
* e

Binary compounds of hydrogen

Alkali metal
(Group 1) hydrides|

* LiH
* NaH
* KH
* RbH
* CsH

Alkaline
(Group 2)
earth hydrides|

| Monohydrides|

* BeH
* MgH
* CaH
* SrH
* BaH

|

Dihydrides|

* BeH2
* MgH2
* CaH2
* SrH2
* BaH2

|

Group 13
hydrides|

| Boranes|

* BH3
* BH
* B2H6
* B2H2
* B2H4
* B4H10
* B5H9
* B5H11
* B6H10
* B6H12
* B10H14
* B18H22

|

Alanes|

* AlH3
* Al2H6

|

Gallanes|

* GaH3
* Ga2H6

|

Indiganes|

* InH3
* In2H6

|

Thallanes|

* TlH3
* Tl2H6

|

Group 14 hydrides|

| Hydrocarbons|

* alkanes
* alkenes
* alkynes
* Cycloalkanes
* Cycloalkenes
* Cycloalkynes
* Annulenes

|

* CH
* CH2
* CH3
* C2H

Silanes|

* SiH4
* Si2H6
* Si3H8
* Si4H10
* Si5H12
* Si6H14
* Si7H16
* Si8H18
* Si9H20
* Si10H22
* more...

|

Silenes|

* Si2H4

|

Silynes|

* Si2H2
* SiH

|

Germanes|

* GeH4
* Ge2H6
* Ge3H8
* Ge4H10
* Ge5H12

|

Stannanes|

* SnH4
* Sn2H6

|

Plumbanes|

* PbH4

|

Pnictogen
(Group 15) hydrides|

| Azanes|

* NH3
* N2H4
* N3H5
* N4H6
* N5H7
* N6H8
* N7H9
* N8H10
* N9H11
* N10H12
* more...

|

Azenes|

* N2H2
* N3H3
* N4H4

|

Phosphanes|

* PH3
* P2H4
* P3H5
* P4H6
* P5H7
* P6H8
* P7H9
* P8H10
* P9H11
* P10H12
* more...

|

Phosphenes|

* P2H2
* P3H3
* P4H4

|

Arsanes|

* AsH3
* As2H4

|

Stibanes|

* SbH3

|

Bismuthanes|

* BiH3

|

* HN3
* NH
* HN5
* NH5

Hydrogen
chalcogenides
(Group 16 hydrides)|

| Polyoxidanes|

* H2O
* H2O2
* H2O3
* H2O4
* H2O5
* H2O6
* H2O7
* H2O8
* H2O9
* H2O10
* more...

|

Polysulfanes|

* H2S
* H2S2
* H2S3
* H2S4
* H2S5
* H2S6
* H2S7
* H2S8
* H2S9
* H2S10
* more...

|

Selanes|

* H2Se
* H2Se2

|

Tellanes|

* H2Te
* H2Te2

|

Polanes|

* PoH2

|

* HO
* HO2
* HO3
* H2O+–O–
* HS
* HDO
* D2O
* T2O

Hydrogen halides
(Group 17 hydrides)|

* HF
* HCl
* HBr
* HI
* HAt

Transition metal hydrides|

* ScH2
* YH2
* YH3
* YH6
* YH9
* LuH2
* LuH3
* TiH2
* TiH4
* ZrH2
* HfH2
* VH
* VH2
* NbH
* NbH2
* TaH
* CrH
* CrH2
* CrHx
* NiH
* PdHx (x < 1)
* IrH3
* FeH
* FeH2
* FeH5
* CoH2
* RhH2
* CuH
* ZnH2
* CdH2
* HgH2

Lanthanide hydrides|

* LaH2
* LaH3
* LaH10
* CeH2
* CeH3
* PrH2
* PrH3
* NdH2
* NdH3
* SmH2
* SmH3
* EuH2
* GdH2
* GdH3
* TbH2
* TbH3
* DyH2
* DyH3
* HoH2
* HoH3
* ErH2
* ErH3
* TmH2
* TmH3
* YbH2
* LuH2
* LuH3

Actinide hydrides|

* AcH2
* ThH2
* ThH4
* Th4H15
* PaH3
* UH3
* UH4
* NpH2
* NpH3
* PuH2
* PuH3
* AmH2
* AmH3
* CmH2

Exotic matter hydrides|

* PsH

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