Carbon disulfide

Carbon disulfide  Carbon disulfide

Names
IUPAC name

Carbon disulfide

Systematic IUPAC name

Methanedithione

Other names

Carbon bisulfide
Dithiocarbonic anhydride[1]

Identifiers

CAS Number

* 75-15-0 Y

3D model (JSmol)

* Interactive image

Beilstein Reference

| 1098293
ChEBI |

* CHEBI:23012 Y

ChEMBL |

* ChEMBL1365180

ChemSpider |

* 6108 Y

EC Number |

* 200-843-6

KEGG |

* C19033 Y

PubChem CID

* 6348

RTECS number |

* FF6650000

UNII |

* S54S8B99E8 Y

UN number | 1131

InChI

* InChI=1S/CS2/c2-1-3 Y

Key: QGJOPFRUJISHPQ-UHFFFAOYSA-N Y

* InChI=1/CS2/c2-1-3

Key: QGJOPFRUJISHPQ-UHFFFAOYAS

SMILES

* S=C=S

Properties

Chemical formula

| CS2
Molar mass | 76.13 g·mol−1
Appearance  | Colorless liquid
Impure: light-yellow
Odor | Pleasant, ether\- or chloroform-like
Commercial: Foul, like rotten radish
Density | 1.539 g/cm3 (−186°C)
1.2927 g/cm3 (0 °C)
1.266 g/cm3 (25 °C)[2]
Melting point |  −111.61 °C (−168.90 °F; 161.54 K)
Boiling point |  46.24 °C (115.23 °F; 319.39 K)

Solubility in water

| 2.58 g/L (0 °C)
2.39 g/L (10 °C)
2.17 g/L (20 °C)[3]
0.14 g/L (50 °C)[2]
Solubility | Soluble in alcohol, ether, benzene, oil, CHCl3, CCl4
Solubility in formic acid | 4.66 g/100 g[2]
Solubility in dimethyl sulfoxide | 45 g/100 g (20.3 °C)[2]
Vapor pressure | 48.1 kPa (25 °C)
82.4 kPa (40 °C)[4]

Magnetic susceptibility (χ)

| −42.2·10−6 cm3/mol

Refractive index (nD)

| 1.627[5]
Viscosity | 0.436 cP (0 °C)
0.363 cP (20 °C)
Structure

Molecular shape

| Linear

Dipole moment

| 0 D (20 °C)[2]
Thermochemistry

Heat capacity (C)

| 75.73 J/(mol·K)[2]

Std molar
entropy (S ~~o~~ 298)

| 151 J/(mol·K)[2]

Std enthalpy of
formation (ΔfH⦵298)

| 88.7 kJ/mol[2]

Gibbs free energy (ΔfG˚)

| 64.4 kJ/mol[2]

Std enthalpy of
combustion (ΔcH⦵298)

| 1687.2 kJ/mol[4]
Hazards
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H225, H315, H319, H332, H361fd, H372

GHS precautionary statements

| P202, P210, P281, P303+361+353, P304+340+312Script error: No such module "Preview warning".Category:GHS errors, P305+351+338, P308+313
ICSC 0022
Inhalation hazard | Irritant; neurotoxin
Eye hazard | Irritant
Skin hazard | Irritant
NFPA 704 (fire diamond)  |

Flash point |  −43 °C (−45 °F; 230 K)[2]

Autoignition
temperature

|  102 °C (216 °F; 375 K)[2]
Explosive limits | 1.3–50%[6]
Lethal dose or concentration (LD, LC):

LD50 (median dose)

| 3188 mg/kg (rat, oral)

LC50 (median concentration)

| >1670 ppm (rat, 1 h)
15500 ppm (rat, 1 h)
3000 ppm (rat, 4 h)
3500 ppm (rat, 4 h)
7911 ppm (rat, 2 h)
3165 ppm (mouse, 2 h)[7]

LCLo (lowest published)

| 4000 ppm (human, 30 min)[7]
NIOSH (US health exposure limits):

PEL (Permissible)

| TWA 20 ppm C 30 ppm 100 ppm (30-minute maximum peak)[6]

REL (Recommended)

| TWA 1 ppm (3 mg/m3) ST 10 ppm (30 mg/m3) [skin][6]

IDLH (Immediate danger)

| 500 ppm[6]
Related compounds

Related compounds

| Carbon dioxide
Carbonyl sulfide
Carbon diselenide

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

N verify (what is YN ?)
Infobox references

Tracking categories (test):

* SizeSet

Carbon disulfide (also spelled as carbon disulphide) is an inorganic compound with the chemical formula CS
2 and structure S=C=S. It is also considered as the anhydride of thiocarbonic acid.[9] It is a colorless, flammable, neurotoxic liquid that is used as a building block in organic synthesis. Pure carbon disulfide has a pleasant, ether\- or chloroform-like odor, but commercial samples are usually yellowish and are typically contaminated with foul-smelling impurities.[10]

## Contents

* 1 History
* 2 Occurrence, manufacture, properties
* 2.1 Solvent
* 2.2 Extraterrestrial
* 3 Reactions
* 3.1 With nucleophiles
* 3.2 Reduction
* 3.3 Chlorination
* 3.4 Coordination chemistry
* 4 Polymerization
* 5 Uses
* 5.1 Niche uses
* 6 Health effects
* 6.1 Environmental sources
* 6.2 Incidence of exposure
* 7 See also
* 8 References
* 9 External links

## History

In 1796, the German chemist Wilhelm August Lampadius (1772–1842) first prepared carbon disulfide by heating pyrite with moist charcoal. He called it "liquid sulfur" (flüssig Schwefel).[11] The composition of carbon disulfide was finally determined in 1813 by the team of the Swedish chemist Jöns Jacob Berzelius (1779–1848) and the Swiss-British chemist Alexander Marcet (1770–1822).[12] Their analysis was consistent with an empirical formula of CS2.[13]

## Occurrence, manufacture, properties

Small amounts of carbon disulfide are released by volcanic eruptions and marshes. CS2 once was manufactured by combining carbon (or coke) and sulfur at 800–1000 °C.[14]

C + 2S → CS2

A lower-temperature reaction, requiring only 600 °C, utilizes natural gas as the carbon source in the presence of silica gel or alumina catalysts:[10]

2 CH4 \+ S8 → 2 CS2 \+ 4 H2S

The reaction is analogous to the combustion of methane.

Global production/consumption of carbon disulfide is approximately one million tonnes, with China consuming 49%, followed by India at 13%, mostly for the production of rayon fiber.[15] United States production in 2007 was 56,000 tonnes.[16]

### Solvent

Carbon disulfide can dissolve a variety of nonpolar chemicals including phosphorus, sulfur, selenium, bromine, iodine, fats, resins, rubber, and asphalt.[17]

### Extraterrestrial

In March 2024, possible traces of CS2 were detected in the atmosphere of the temperate mini-Neptune planet TOI-270 d by the James Webb Space Telescope.[18]

## Reactions

Combustion of CS2 affords sulfur dioxide according to this ideal stoichiometry:

CS2 \+ 3 O2 → CO2 \+ 2 SO2

### With nucleophiles

Compared to the isoelectronic carbon dioxide, CS2 is a weaker electrophile. While, however, reactions of nucleophiles with CO2 are highly reversible and products are only isolated with very strong nucleophiles, the reactions with CS2 are thermodynamically more favored allowing the formation of products with less reactive nucleophiles.[19]

For example, amines afford dithiocarbamates:[20]

2 R2NH + CS2 → [R2NH2+][R2NCS2−]

Xanthates form similarly from alkoxides:[20]

RONa + CS2 → [Na+][ROCS2−]

This reaction is the basis of the manufacture of regenerated cellulose, the main ingredient of viscose, rayon, and cellophane. Both xanthates and the related thioxanthates (derived from treatment of CS2 with sodium thiolates) are used as flotation agents in mineral processing.

Upon treatment with sodium sulfide, carbon disulfide affords trithiocarbonate:[20]

Na2S + CS2 → [Na+]2[CS32−]

Carbon disulfide does not hydrolyze readily, although the process is catalyzed by an enzyme.

### Reduction

Reduction of carbon disulfide with sodium affords sodium 1,3-dithiole-2-thione-4,5-dithiolate together with sodium trithiocarbonate:[21]

4 Na + 4 CS2 → Na2C3S5 \+ Na2CS3

### Chlorination

Chlorination of CS2 provides a route to carbon tetrachloride:[10]

CS2 \+ 3 Cl2 → CCl4 \+ S2Cl2

This conversion proceeds via the intermediacy of thiophosgene, CSCl2.

### Coordination chemistry

Main article: Chemistry:Transition metal complexes of carbon disulfide

CS2 is a ligand for many metal complexes, forming pi complexes. One example is CpCo(η2-CS2)(PMe3).[22]

## Polymerization

CS2 polymerizes upon photolysis or under high pressure to give an insoluble material called car-sul or "Bridgman's black", named after the discoverer of the polymer, Percy Williams Bridgman.[23] Trithiocarbonate (-S-C(S)-S-) linkages comprise, in part, the backbone of the polymer, which is a semiconductor.[24]

## Uses

The principal industrial uses of carbon disulfide, consuming 75% of the annual production in 2000, are the manufacture of viscose rayon and cellophane film.[25]

It is also a valued intermediate in chemical synthesis of carbon tetrachloride. It is widely used in the synthesis of organosulfur compounds such as xanthates, which are used in froth flotation, a method for extracting metals from their ores. Carbon disulfide is also a precursor to dithiocarbamates, which are used as drugs (e.g. Metam sodium) and rubber chemistry.

### Niche uses

Carbon disulfide insecticide ad from the 1896 issue of The American Elevator and Grain Trade magazine

It can be used in fumigation of airtight storage warehouses, airtight flat storage, bins, grain elevators, railroad box cars, ship holds, barges, and cereal mills.[26] Carbon disulfide is also used as an insecticide for the fumigation of grains, nursery stock, in fresh fruit conservation, and as a soil disinfectant against insects and nematodes.[27]

It can also be used for the Barking dog reaction.

## Health effects

Carbon disulfide has been linked to both acute and chronic forms of poisoning, with a diverse range of symptoms.[28]

Concentrations of 500–3000 mg/m3 cause acute and subacute poisoning. These include a set of mostly neurological and psychiatric symptoms, called encephalopathia sulfocarbonica. Symptoms include acute psychosis (manic delirium, hallucinations), paranoic ideas, loss of appetite, gastrointestinal and sexual disorders, polyneuritis, myopathy, and mood changes (including irritability and anger). Effects observed at lower concentrations include neurological problems (encephalopathy, psychomotor and psychological disturbances, polyneuritis, abnormalities in nerve conduction), hearing problems, vision problems (burning eyes, abnormal light reactions, increased ophthalmic pressure), heart problems (increased deaths for heart disease, angina pectoris, high blood pressure), reproductive problems (increased miscarriages, immobile or deformed sperm), and decreased immune response.[29][30]

Occupational exposure to carbon disulfide is also associated with cardiovascular disease, particularly stroke.[31]

In 2000, the World Health Organization (WHO) considered that health harms were unlikely at levels below 100 μg/m3 over an averaging time of 24 hours, and recommended this as a guideline level.[32] Carbon disulfide can be smelled at levels above 200 μg/m3, and the WHO recommended a sensory guideline of below 20 μg/m3. Exposure to carbon disulfide is well-established to be harmful to health in concentrations at or above 30 mg/m3. Changes in the function of the central nervous system have been observed at concentrations of 20–25 mg/m3. There are also reports of harms to health at 10 mg/m3, for exposures of 10–15 years, but the lack of good data on past exposure levels make the association of these harms with concentrations of 10 mg/m3 findings uncertain. The measured concentration of 10 mg/m3 may be equivalent to a concentration in the general environment of 1 mg/m3.[29]

### Environmental sources

The primary source of carbon disulfide in the environment is rayon factories.[29] Most global carbon disulfide emissions come from rayon production, as of 2008.[33] Other sources include the production of cellophane, carbon tetrachloride,[33] carbon black, and sulfur recovery. Carbon disulfide production also emits hydrogen sulfide.[34]

As of 2004[update], about 250 g of carbon disulfide is emitted per kilogram of rayon produced. About 30 g of carbon disulfide is emitted per kilogram of carbon black produced. About 0.341 g of carbon disulfide is emitted per kilogram of sulfur recovered.[34]

Japan has reduced carbon disulfide emissions per kilogram of rayon produced, but in other rayon-producing countries, including China, emissions are assumed to be uncontrolled (based on global modelling and large-scale free-air concentration measurements). Rayon production is steady or decreasing except in China, where it is increasing, as of 2004[update].[34] Carbon black production in Japan and Korea uses incinerators to destroy about 99% of the carbon disulfide that would otherwise be emitted.[34] When used as a solvent, Japanese emissions are about 40% of the carbon disulfide used; elsewhere, the average is about 80%.[34]

Most rayon production uses carbon sulfide.[35][36] One exception is rayon made using the lyocell process, which uses a different solvent; as of 2018[update] the lyocell process is not widely used, because it is more expensive than the viscose process.[37][38] Cuprammonium rayon also does not use carbon disulfide.

### Incidence of exposure

Industrial workers working with carbon disulfide are at high risk. Emissions may also harm the health of people living near rayon plants.[29]

Concerns about carbon disulfide exposure have a long history.[25][39][40]: 79 Around 1900, carbon disulfide came to be widely used in the production of vulcanized rubber. The psychosis produced by high exposures was soon apparent (it has been reported with 6 months of exposure[29]). Sir Thomas Oliver told a story about a rubber factory that put bars on its windows so that the workers would not leap out to their deaths.[40]: 17 Carbon disulfide use in the US as a heavier-than-air burrow poison for Richardson's ground squirrel also led to reports of psychosis. No systematic medical study of the issue was published, and knowledge was not transferred to the rayon industry.[35]

The first large epidemiological study of rayon workers was done in the US in the late 1930s, and found fairly severe effects in 30% of the workers. Data on increased risks of heart attacks and strokes came out in the late 1960s.[41] Courtaulds, a major rayon manufacturer, worked hard to prevent publication of this data in the UK.[35] Average concentrations in sampled rayon plants were reduced from about 250 mg/m3 in 1955–1965 to about 20–30 mg/m3 in the 1980s (US figures only? ).[29] Rayon production has since largely moved to the developing world, especially China, Indonesia and India.[36][35]

Rates of disability in factories are unknown as of 2016[update].[36][42] Manufacturers using the viscose process do not provide any information on harm to their workers.[35][36]

## See also

* Carbon monosulfide
* Ethenedithione
* Carbon subsulfide
* Carbon diselenide
* Carbon dioxide
* 1949 Holland Tunnel fire, accident with truck carrying carbon disulfide.

## References

1. ↑ "Carbon disulfide chemistry". PubChem. https://webbook.nist.gov/cgi/cbook.cgi?ID=C75150&Mask=80:~:text=Dithiocarbonic Anhydride.
2. ↑ 2.00 2.01 2.02 2.03 2.04 2.05 2.06 2.07 2.08 2.09 2.10 "Properties of substance: carbon disulfide". http://chemister.ru/Database/properties-en.php?dbid=1&id=1955.
3. ↑ Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand.
4. ↑ 4.0 4.1 Carbon disulfide in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD), http://webbook.nist.gov (retrieved 2014-05-27).
5. ↑ 5.0 5.1 Sigma-Aldrich Co., [www.sigmaaldrich.com/product/sigald/180173 Carbon disulfide]. Retrieved on 2024-10-23.
6. ↑ 6.0 6.1 6.2 6.3 NIOSH Pocket Guide to Chemical Hazards. "#0104". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0104.html.
7. ↑ 7.0 7.1 "Carbon disulfide". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/75150.html.
8. ↑ [1]
9. ↑ Informatics, NIST Office of Data and. "Carbon disulfide" (in en). https://webbook.nist.gov/cgi/cbook.cgi?ID=C75150&Mask=80.
10. ↑ 10.0 10.1 10.2 Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils, ed., Inorganic Chemistry, San Diego/Berlin: Academic Press/De Gruyter, ISBN 0-12-352651-5 .
11. ↑ Lampadius (1796). "Etwas über flüssigen Schwefel, und Schwefel-Leberluft" (in de). Chemische Annalen für die Freunde der Naturlehre, Arzneygelährtheit, Haushaltungskunst und Manufacturen (Chemical Annals for the Friends of Science, Medicine, Economics, and Manufactures) (2): 136–137. https://books.google.com/books?id=gqk5AAAAcAAJ&pg=PA136.
12. ↑ Berzelius, J.; Marcet, Alexander (1813). "Experiments on the alcohol of sulphur, or sulphuret of carbon". Philosophical Transactions of the Royal Society of London (103): 171–199. doi:10.1098/rstl.1813.0026.
13. ↑ (Berzelius and Marcet, 1813), p. 187.
14. ↑ Warnecke, Friedrich (1941). "Die gewerbliche Schwefelkohlenstoffvergiftung" (in de). Archiv für Gewerbepathologie und Gewerbehygiene (Springer Science and Business Media LLC) 11 (2): 198–248. doi:10.1007/bf02122927. ISSN 0340-0131. Bibcode: 1941ArGG...11..198W.
15. ↑ "Carbon Disulfide report from IHS Chemical". http://www.ihs.com/products/chemical/planning/ceh/carbon-disulfide.aspx.
16. ↑ "Chemical profile: carbon disulfide from ICIS.com". http://www.icis.com/Articles/2008/09/08/9154319/chemical-profile-carbon-disulfide.html.
17. ↑ "Carbon Disulfide". Akzo Nobel. http://www.akzonobel.com/sulfurderivatives/products/carbon_disulfide/.
18. ↑ Benneke, Björn; Roy, Pierre-Alexis; Coulombe, Louis-Philippe; Radica, Michael; Piaulet, Caroline; Ahrer, Eva-Maria; Pierrehumbert, Raymond; Krissansen-Totton, Joshua; Schlichting, Hilke E. (2024-03-05). "JWST Reveals CH$_4$, CO$_2$, and H$_2$O in a Metal-rich Miscible Atmosphere on a Two-Earth-Radius Exoplanet". arXiv:2403.03325 [astro-ph.EP].
19. ↑ Li, Zhen; Mayer, Robert J.; Ofial, Armin R.; Mayr, Herbert (2020-04-27). "From Carbodiimides to Carbon Dioxide: Quantification of the Electrophilic Reactivities of Heteroallenes". Journal of the American Chemical Society 142 (18): 8383–8402. doi:10.1021/jacs.0c01960. PMID 32338511. Bibcode: 2020JAChS.142.8383L.
20. ↑ 20.0 20.1 20.2 Yokoyama, Masataka; Imamoto, Tsuneo (1984). "Organic Reactions of Carbon Disulfide". Synthesis (Georg Thieme Verlag KG) 1984 (10): 797–824. doi:10.1055/s-1984-30978. ISSN 0039-7881.
21. ↑ "4,5-Dibenzoyl-1,3-dithiole-1-thione". Org. Synth. 73: 270. 1996. doi:10.15227/orgsyn.073.0270.
22. ↑ Werner, Helmut (1982). "Novel Coordination Compounds formed from CS2 and Heteroallenes". Coordination Chemistry Reviews 43: 165–185. doi:10.1016/S0010-8545(00)82095-0.
23. ↑ Bridgman, P.W. (1941). "Explorations toward the limit of utilizable pressures". Journal of Applied Physics 12 (6): 461–469. doi:10.1063/1.1712926. Bibcode: 1941JAP....12..461B.
24. ↑ Ochiai, Bungo; Endo, Takeshi (2005). "Carbon dioxide and carbon disulfide as resources for functional polymers". Progress in Polymer Science 30 (2): 183–215. doi:10.1016/j.progpolymsci.2005.01.005.
25. ↑ 25.0 25.1 Lay, Manchiu D. S.; Sauerhoff, Mitchell W.; Saunders, Donald R.; "Carbon Disulfide", in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2000 doi: 10.1002/14356007.a05_185
26. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
27. ↑ Worthing, Charles R.; Hance, Raymond J. (1991). The Pesticide Manual, A World Compendium (9th ed.). British Crop Protection Council. ISBN 9780948404429. https://archive.org/details/pesticidemanualw0000unse.
28. ↑ "ATSDR - Public Health Statement: Carbon Disulfide". https://www.atsdr.cdc.gov/phs/phs.asp?id=472&tid=84#bookmark05.
29. ↑ 29.0 29.1 29.2 29.3 29.4 29.5 "Chapter 5.4 : Carbon disulfide". Air Quality Guidelines (2 ed.). WHO Regional Office for Europe, Copenhagen, Denmark. 2000. https://www.euro.who.int/__data/assets/pdf_file/0019/123058/AQG2ndEd_5_4carbodisulfide.PDF. Retrieved 31 July 2021.
30. ↑ (in en) ﻿Preventing hearing loss caused by chemical (ototoxicity) and noise exposure.﻿ (Report). U.S. Department of Health and Human Services, Public Health Service, Centers for Disease Control and Prevention, National Institute for Occupational Safety and Health. 2018-03-01. doi:10.26616/nioshpub2018124. https://www.cdc.gov/niosh/docs/2018-124/.
31. ↑ "Occupational health and safety – chemical exposure" (in en). Swedish Agency for Health Technology Assessment and Assessment of Social Services (SBU). http://www.sbu.se/en/publications/sbu-assesses/occupational-health-and-safety--chemical-exposure/.
32. ↑ Air quality guidelines for Europe. WHO regional publications. European series (2nd ed.). Copenhagen: World Health Organization, Regional Office for Europe. 2000. pp. 71–74. ISBN 978-92-890-1358-1.
33. ↑ 33.0 33.1 "Carbon Disulfide Health Effects Assessment for HEAC Discussion April 2008". State of California Department of Industrial Relations. April 2008. https://www.dir.ca.gov/dosh/DoshReg/CarbonDisulfide5155-4-08.doc.
34. ↑ 34.0 34.1 34.2 34.3 34.4 Blake, Nicola J. (2004). "Carbonyl sulfide and carbon disulfide: Large-scale distributions over the western Pacific and emissions from Asia during TRACE-P". Journal of Geophysical Research 109 (D15): D15S05. doi:10.1029/2003JD004259. Bibcode: 2004JGRD..10915S05B. https://scholars.unh.edu/cgi/viewcontent.cgi?article=1072&context=earthsci_facpub.
35. ↑ 35.0 35.1 35.2 35.3 35.4 Swan, Norman; Blanc, Paul (20 February 2017). "The health burden of viscose rayon" (in en). ABC Radio National. http://www.abc.net.au/radionational/programs/healthreport/the-health-burden-of-viscose-rayon/8286870.
36. ↑ 36.0 36.1 36.2 36.3 Nijhuis, Michelle (2009). "Bamboo Boom: Is This Material for You?". Scientific American Special Editions 19 (2): 60–65. Bibcode: 2009SciAm..19f..60N. https://www.scientificamerican.com/article/bamboo-boom/. Retrieved 24 March 2023.
37. ↑ "Regenerated cellulose by the Lyocell process, a brief review of the process and properties :: BioResources". BioRes. 2018. https://bioresources.cnr.ncsu.edu/resources/regenerated-cellulose-by-the-lyocell-process-a-brief-review-of-the-process-and-properties/.
38. ↑ Tierney, John William (2005). Kinetics of Cellulose Dissolution in N-MethylMorpholine-N-Oxide and Evaporative Processes of Similar Solutions (Thesis).
39. ↑ St. Clair, Kassia (2018). The Golden Thread: How Fabric Changed History. London: John Murray. pp. 213–215. ISBN 978-1-4736-5903-2. OCLC 1057250632.
40. ↑ 40.0 40.1 Blanc, M.D., Paul David (15 November 2016). Fake Silk / The Lethal History of Viscose Rayon. Yale University Press. ISBN 9780300204667. https://yalebooks.yale.edu/book/9780300204667/fake-silk. Retrieved 17 December 2020. "in 1915,...[of 16] carbon disulfide poisoning cases....one worker had been briefly committed to an asylum and several others had experienced nervous system complaints..."
41. ↑ Tiller, J. R.; Schilling, R. S.; Morris, J. N. (1968-11-16). "Occupational toxic factor in mortality from coronary heart disease". British Medical Journal 4 (5628): 407–411. doi:10.1136/bmj.4.5628.407. ISSN 0007-1447. PMID 5687604.
42. ↑ Monosson, Emily (2016). "Toxic textiles". Science 354 (6315): 977. doi:10.1126/science.aak9834. PMID 27884997. Bibcode: 2016Sci...354..977M.

## External links

| Wikisource has the text of the 1911 Encyclopædia Britannica article Carbon Bisulphide.

|

* Australian National Pollutant Inventory: Carbon disulfide
* CDC - NIOSH Pocket Guide to Chemical Hazards - Carbon Disulfide
* Inno Motion Engineering
* Agency for Toxic Substances & Disease Registry Public Health Statement for Carbon Disulfide , 1996.
* Resources on Carbon Disulfide by the National Institute for Occupational Safety and Health
* Blanc, Paul David (2016). Fake silk : the lethal history of viscose rayon. New Haven: Yale University Press. pp. 328. ISBN 9780300204667. https://yalebooks.yale.edu/book/9780300204667/fake-silk.

* v
* t
* e

Inorganic compounds of carbon and related ions

Compounds|

* CBr4
* CCl4
* CF
* CF4
* CI4
* CO
* CO2
* CO3
* COS
* CS
* CS2
* CSe2
* C3O2
* C3S2
* SiC

Carbon ions|

* Carbides [:C≡C:]2-, [::C::]4-, [:C=C=C:]4-
* Cyanides [:C≡N:]-
* Cyanates [:O-C≡N:]-
* Thiocyanates [:S-C≡N:]-
* Fulminates [:C≡N-O:]-
* Thiofulminates [:C≡N-S:]-

Oxides and related|

* Oxides
* Metal carbonyls
* Carbonic acid
* Bicarbonates
* Carbonates

* v
* t
* e

Sulfides

| H2S
H2S2 |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  | He

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Li2S | BeS |  |  |  |  |  |  |  |  |  |  | B2S3 | CS2
COS | (NH4)SH | O | F | Ne
Na2S
Na2Sx | MgS |  |  |  |  |  |  |  |  |  |  | Al2S3 | SiS
SiS2 | PxSy | S | Cl | Ar
K2S | CaS | Sc2S3 | TiS2 | V | CrS
Cr2S3 | MnS
MnS2 | FeS
Fe3S4 | CoS | NiS | Cu2S
CuS | ZnS | GaS
Ga2S3 | GeS
GeS2 | As2S3
As4S3 | SeS2 | Br | Kr
Rb2S | SrS | Y2S3 | ZrS2 | NbS2 | MoS2 | Tc | Ru | Rh2S3 | PdS | Ag2S | CdS | In2S3 | SnS
SnS2 | Sb2S3
Sb2S5 | TeS2 | I | Xe
Cs2S | BaS | *  | HfS2 | TaS2 | WS2
WS3 | ReS2
Re2S7 | Os | Ir2S3
IrS2 | PtS
PtS2 | Au2S
Au2S3 | HgS | Tl2S | PbS
PbS2 | Bi2S3 | Po | At | Rn
Fr | Ra | **  | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og |  |  |  |  |  |  |  |
|  | ↓ |  |  |  |  |  |  |  |  |  |  |  |  |  |  |
| * | La2S3 | CeS
Ce2S3 | Pr2S3 | Nd2S3 | Pm2S3 | SmS
Sm2S3 | Eu2S3 | Gd2S3 | Tb2S3 | Dy2S3 | Ho2S3 | Er2S3 | Tm2S3 | Yb2S3 | Lu2S3 |
| ** | Ac | ThS2 | Pa | US2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr |

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Original source: https://en.wikipedia.org/wiki/Carbon disulfide. Read more

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Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Carbon_disulfide&oldid=4531682"
*[CID]: Compound ID
*[H225]: Highly flammable liquid and vapour
*[H315]: Causes skin irritation
*[H319]: Causes serious eye irritation
*[H332]: Harmful if inhaled
*[H361fd]: Suspected of damaging fertility. Suspected of damaging the unborn child.
*[H372]: Causes damage to organs through prolonged or repeated exposure
*[P202]: Do not handle until all safety precautions have been read and understood
*[P210]: Keep away from heat/sparks/open flames/hot surfaces – No smoking
*[P281]: Use personal protective equipment as required
*[P303+361+353]: IF ON SKIN (or hair): Remove/Take off immediately all contaminated clothing. Rinse skin with water/shower
*[P305+351+338]: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do – continue rinsing
*[P308+313]: IF exposed or concerned: Get medical advice/attention
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