| Revision as of 13:21, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,081 edits Saving copy of the {{chembox}} taken from revid 473626119 of page Carbon_tetrachloride for the Chem/Drugbox validation project (updated: ''). |
Latest revision as of 19:31, 21 January 2025 edit Marbletan (talk | contribs)Extended confirmed users5,633 editsNo edit summary |
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{{Short description|Carbon compound}} |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
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{{For|the chemokine|CCL4}} |
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{{chembox |
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{{chembox |
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| Watchedfields = changed |
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| Watchedfields = changed |
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| verifiedrevid = 410564234 |
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| verifiedrevid = 477000161 |
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| ImageFileL1 = Tetrachlormethan.svg |
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| ImageFileL1 = Tetrachlormethan.svg |
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| ImageClassL1 = skin-invert-image |
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| ImageNameL1 = Structural formula of carbon tetrachloride |
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| ImageFileR1 = Carbon-tetrachloride-3D-vdW.png |
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| ImageNameL1 = Structural formula of tetrachloride |
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| ImageNameR1 = Space-filling model carbon tetrachloride |
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| ImageFileR1 = Carbon-tetrachloride-3D-vdW.png |
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| ImageNameR1 = Space-filling model carbon tetrachloride |
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| IUPACName = Tetrachloromethane |
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| ImageFile2 = Carbon Tetrachloride.jpg |
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| OtherNames = Tetrachloromethane, Benziform, Benzinoform, Carbon chloride, Carbon tet, Freon 10, Halon 104, Methane tetrachloride, Perchloromethane, Tetraform, Tetrasol |
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| ImageName2 = Carbon tetrachloride |
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| Section1 = {{Chembox Identifiers |
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| PIN = Tetrachloromethane |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| OtherNames = Benzinoform<br />carbon(IV) chloride <br />carbon tet<br />''Carboneum Tetrachloratum / Carbonei tetrachloridum''<br />''Carboneum Chloratum / Carbonei chlorurum''<br /> |
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chloride of carbon<br />Freon-10<br />Halon-104 <br />methane tetrachloride <br />methyl tetrachloride <br />Necatorina <br />perchloromethane<br />Refrigerant-10<br />''Tetrachloretum Carbonicum''<br />Tetrachlorocarbon<br /> Tetraform<br />Tetrasol |
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| Section1 = {{Chembox Identifiers |
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| Abbreviations= CTC, TCM, PCM, R-10 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 5730 |
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| ChemSpiderID = 5730 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| StdInChIKey = VZGDMQKNWNREIO-UHFFFAOYSA-N |
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| StdInChIKey = VZGDMQKNWNREIO-UHFFFAOYSA-N |
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| CASNo = 56-23-5 |
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| CASNo = 56-23-5 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| EINECS = 200-262-8 |
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| EINECS = 200-262-8 |
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| PubChem = 5943 |
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| PubChem = 5943 |
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| SMILES = ClC(Cl)(Cl)Cl |
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| SMILES = ClC(Cl)(Cl)Cl |
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| InChI = 1/CCl4/c2-1(3,4)5 |
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| InChI = 1/CCl4/c2-1(3,4)5 |
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| RTECS = FG4900000 |
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| RTECS = FG4900000 |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI = 27385 |
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| ChEBI = 27385 |
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| KEGG_Ref = {{keggcite|correct|kegg}} |
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| KEGG_Ref = {{keggcite|correct|kegg}} |
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| KEGG = C07561 |
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| KEGG = C07561 |
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| UNNumber = 1846 |
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| UNNumber = 1846 |
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| Gmelin = 2347 |
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| Beilstein = 1098295 |
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}} |
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| Section2 = {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| C = 1 |
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| C=1 | Cl=4 |
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| Appearance = Colourless liquid |
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| Cl = 4 |
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| Odor = ]-like odor |
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| ExactMass = 153.872461 |
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| Density = {{ubl |
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| Appearance = colourless liquid |
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| 1.5867{{nbsp}}g·cm<sup>−3</sup> (liquid) |
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| Odor = ]-like odor |
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| Density = 1.5867 g cm<sup>−3</sup> (liquid)<br /> |
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| 1.831{{nbsp}}g·cm<sup>−3</sup> at −186{{nbsp}}°C (solid) |
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1.831 g cm<sup>−3</sup> at −186 °C (solid)<br /> |
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| 1.809{{nbsp}}g·cm<sup>−3</sup> at −80{{nbsp}}°C (solid) |
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}} |
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1.809 g cm<sup>−3</sup> at −80 °C (solid) |
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| MeltingPtC = -22.92 |
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| MeltingPtC = −22.92 |
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| BoilingPtC = 76.72 |
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| BoilingPtC = 76.72 |
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| Solubility = ?? g/100 mL (25 °C) |
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| Solubility = {{ubl |
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| 0.097{{nbsp}}g/100{{nnbsp}}mL (0{{nbsp}}°C) |
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| SolubleOther = soluble in ], ], ], ], ], ] |
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| 0.081{{nbsp}}g/100{{nnbsp}}mL (25{{nbsp}}°C) |
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| LogP = 2.64 |
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}} |
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| VaporPressure = 11.94 kPa at 20 °C |
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| SolubleOther = Soluble in ], ], ], ], ], ], ] |
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| HenryConstant = 2.76x10<sup>-2</sup> atm-cu m/mol |
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| RefractIndex = 1.4601 |
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| LogP = 2.64 |
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| VaporPressure = 11.94{{nbsp}}kPa at 20{{nbsp}}°C |
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| HenryConstant = 2.76×10<sup>−2</sup>{{nbsp}}atm·m{{sup|3}}/mol |
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| RefractIndex = 1.4607 |
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| Dipole = 0 D |
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| MagSus = −66.60×10<sup>−6</sup>{{nbsp}}cm<sup>3</sup>/mol |
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| ThermalConductivity = 0.1036{{nbsp}}W/m·K (300{{nbsp}}K)<ref>Touloukian, Y.S., Liley, P.E., and Saxena, S.C. Thermophysical properties of matter - the TPRC data series. Volume 3. Thermal conductivity - nonmetallic liquids and gases. Data book. 1970.</ref> |
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| Viscosity = 0.86{{nbsp}}mPa·s<ref>{{Citation|last1=Reid|first1=Robert C.|last2=Prausnitz|first2=John M.|last3=Poling|first3=Bruce E.|title=The Properties of Gases and Liquids|publisher=McGraw-Hill Book Company|year=1987|isbn=0-07-051799-1|page=442}}</ref> |
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}} |
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| Section3 = {{Chembox Structure |
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| Section3 = {{Chembox Structure |
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| CrystalStruct = ] |
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| CrystalStruct = ] |
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| Coordination = |
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| Coordination = Tetragonal |
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| MolShape = ] |
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| MolShape = ] |
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| Dipole = 0{{nbsp}}D |
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}} |
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| Section4 = {{Chembox Hazards |
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| Section5 = {{Chembox Thermochemistry |
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| DeltaHf = −95.6{{nbsp}}kJ/mol |
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| ExternalMSDS = |
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| DeltaGf = −87.34{{nbsp}}kJ/mol<ref>{{Cite web |title=Carbon tetrachloride |url=https://www.chemeo.com/cid/64-699-6/Carbon%20tetrachloride.pdf |access-date=14 Jun 2022 |website=Cheméo}}</ref> |
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| EUClass = ]<br />Toxic ('''T''')<br />Dangerous for the environment ('''N''') |
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| Entropy = 214.39{{nbsp}}J/mol·K |
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| EUIndex = 602-008-00-5 |
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| HeatCapacity = 132.6{{nbsp}}J/mol·K |
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| NFPA-H = 3 |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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| NFPA-O = |
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| RPhrases = {{R23/24/25}}, {{R40}}, {{R48/23}}, {{R59}}, {{R52/53}} |
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| SPhrases = {{S1/2}}, {{S23}}, {{S36/37}}, {{S45}}, {{S59}}, {{S61}} |
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| FlashPt = Not flammable |
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| Autoignition = 982 °C |
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| LD50 = 2350 mg/kg |
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}} |
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}} |
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| Section5 = {{Chembox Thermochemistry |
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| Section7 = {{Chembox Hazards |
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| MainHazards = extremely toxic to the liver and kidneys, potential occupational carcinogen, harmful to the ] |
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| DeltaHf = −135 kJ·mol<sup>−1</sup> |
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| ExternalSDS = |
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| Entropy = 216 J·mol<sup>−1</sup>·K<sup>−1</sup> |
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| NFPA-H = 3 |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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| NFPA-S = |
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| GHSPictograms = {{GHS06}} {{GHS08}} |
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| GHSSignalWord = Danger |
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| HPhrases = {{H-phrases|301|302|311|331|351|372|412|420}} |
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| PPhrases = {{P-phrases|201|202|260|261|264|270|271|273|280|281|301+310|302+352|304+340|308+313|311|312|314|321|322|330|361|363|403+233|405|501|502}} |
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| FlashPt = non-flammable |
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| AutoignitionPtC = |
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| LD50 =7749 mg/kg (oral, mouse); 5760 mg/kg (oral, rabbit); 2350 mg/kg (oral, rat)<ref></ref> |
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| PEL = TWA 10{{nbsp}}ppm C 25{{nbsp}}ppm 200{{nbsp}}ppm (5-minute maximum peak in any 4 hours)<ref name=PGCH>{{PGCH|0107}}</ref> |
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| IDLH = 200{{nbsp}}ppm<ref name=PGCH/> |
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| REL = Ca ST 2{{nbsp}}ppm (12.6{{nbsp}}mg/m<sup>3</sup>) <ref name=PGCH/> |
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| LC50 = {{ubl |
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| 5400{{nbsp}}ppm (mammal) |
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| 8000{{nbsp}}ppm (rat, 4{{nbsp}}hr) |
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| 9526{{nbsp}}ppm (mouse, 8{{nbsp}}hr)<ref name=IDLH>{{IDLH|56235|Carbon tetrachloride}}</ref> |
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}} |
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| LCLo = {{ubl |
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| 1000{{nbsp}}ppm (human) |
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| 20,000{{nbsp}}ppm (guinea pig, 2{{nbsp}}hr) |
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| 38,110{{nbsp}}ppm (cat, 2{{nbsp}}hr) |
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| 50,000{{nbsp}}ppm (human, 5{{nbsp}}min) |
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| 14,620{{nbsp}}ppm (dog, 8{{nbsp}}hr)<ref name=IDLH/> |
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}} |
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| Section8 = {{Chembox Related |
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| Function = chloromethanes |
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| OtherCations = ]<br />]<br />]<br />] |
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| OtherFunctn = ]<br />]<br />] |
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| OtherCpds = ]<br />]<br />] |
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| Section8 = {{Chembox Related |
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| OtherFunction_label = chloromethanes |
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| OtherAnions = ] <br> ] <br> ] |
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| OtherCations = ]<br />]<br />]<br />] |
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| OtherFunction = ]<br />]<br />] |
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| OtherCompounds = |
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}} |
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}} |
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'''Carbon tetrachloride''', also known by many other names (such as '''carbon tet''' for short and '''tetrachloromethane''', also ]), is a ] with the ] CCl<sub>4</sub>. It is a non-flammable, dense, colourless liquid with a "sweet" ]-like odour that can be detected at low levels. It was formerly widely used in ]s, as a precursor to ]s, an ] and a ], but has since been phased out because of environmental and safety concerns. Exposure to high concentrations of carbon tetrachloride can affect the ] and degenerate the liver and kidneys. Prolonged exposure can be fatal. |
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==Properties== |
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In the carbon tetrachloride ], four ] ]s are positioned symmetrically as corners in a ] configuration joined to a central ] atom by single ]s. Because of this symmetric geometry, CCl<sub>4</sub> is non-polar. ] has the same structure, making carbon tetrachloride a ]. As a ], it is well suited to dissolving other non-polar compounds such as fats and oils. It can also dissolve ]. It is ], giving off ]s with an odor characteristic of other chlorinated solvents, somewhat similar to the ] odor reminiscent of ]s' shops. |
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Solid tetrachloromethane has two ]: crystalline II below −47.5 °C (225.6 K) and crystalline I above −47.5 °C.<ref>{{cite web| url=http://webbook.nist.gov/cgi/cbook.cgi?ID=C56235&Units=SI&Mask=4#Thermo-Phase |title=Carbon Tetrachloride |website=webbook.nist.gov |access-date=28 April 2018 |url-status=live |archive-url=https://web.archive.org/web/20170630080210/http://webbook.nist.gov/cgi/cbook.cgi?ID=C56235&Units=SI&Mask=4#Thermo-Phase |archive-date=30 June 2017 }}</ref> At −47.3 °C it has ] crystal structure with space group ''C2/c'' and ] ''a'' = 20.3, ''b'' = 11.6, ''c'' = 19.9 (.10<sup>−1</sup> nm), β = 111°.<ref name="chtas">F. Brezina, J. Mollin, R. Pastorek, Z. Sindelar. ''Chemicke tabulky anorganickych sloucenin'' (''Chemical tables of inorganic compounds''). SNTL, 1986.</ref> |
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With a ] greater than 1, carbon tetrachloride will be present as a ] if sufficient quantities are spilt in the environment. |
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==Reactions== |
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Despite being generally inert, carbon tetrachloride can undergo various reactions. Hydrogen or an acid in the presence of an ] catalyst can reduce carbon tetrachloride to chloroform, dichloromethane, chloromethane and even methane.<ref>{{cite journal |last1=Johnson |first1=Timothy L. |last2=Fish |first2=William |last3=Gorby |first3=Yuri A. |last4=Tratnyek |first4=Paul G. |title=Degradation of carbon tetrachloride by iron metal: Complexation effects on the oxide surface |journal=Journal of Contaminant Hydrology |date=March 1998 |volume=29 |issue=4 |pages=379–398 |doi=10.1016/S0169-7722(97)00063-6 |bibcode=1998JCHyd..29..379J }}</ref> When its vapours are passed through a red-hot tube, carbon tetrachloride dechlorinates to ] and ].<ref>"Carbonic Dichloride". Tidy, C. M. (1887). Handbook of modern chemistry, inorganic and organic. UK: Smith, Elder & Company. p. 215</ref> |
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Carbon tetrachloride, when treated with ], gives various compounds such as ] (R-11), ] (R-12), ] (R-13) and ] with ] as the by-product: |
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:{{chem2 | CCl4 + HF -> CCl3F + HCl }} |
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:{{chem2 | CCl4 + 2 HF -> CCl2F2 + 2 HCl }} |
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:{{chem2 | CCl4 + 3 HF -> CClF3 + 3 HCl }} |
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:{{chem2 | CCl4 + 4 HF -> CF4 + 4 HCl }} |
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This was once one of the main uses of carbon tetrachloride, as R-11 and R-12 were widely used as refrigerants. |
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An alcohol solution of potassium hydroxide decomposes it to potassium chloride and potassium carbonate in water:<ref>Wislicenus, J., Strecker, A., Hodgkinson, W. R. E. (1882). Adolph Strecker's Short Text-book of Organic Chemistry. USA: D. Appleton.</ref> |
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:{{chem2 | CCl4 + 6 KOH -> 4 KCl + K2CO3 + 3 H2O }} |
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Carbon is sufficiently ] that many compounds react to give ]: |
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{{Table alignment}} |
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{| class="wikitable col1right col2center col3left col4right" |
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! Reactants !! !! Products !! Conditions<sup>cite</sup> |
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|- |
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| {{chem2|] + CCl4}} || → || {{chem2|2 COCl2}} || 350 °C<ref name=watts/> |
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|- |
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| {{Chem2|] + CCl4}} || → || {{chem2|COCl2 +}} {{frac|1|3}}{{chem2|C2Cl4|link=tetrachloroethylene}} || <ref name=watts/> |
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|- |
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| {{chem2|2 ] + CCl4}} || → || {{chem2|COCl2 + ]}} || <ref name=graham/> |
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| {{frac|1|3}}{{chem2|] + CCl4}} || → || {{chem2|COCl2 +}} {{frac|2|3}}{{chem2|POCl3|link=phosphoryl chloride}} || <ref name=graham/> |
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|- |
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| {{chem2|3 ] + 2 CCl4}} || → || {{chem2|COCl2 + CO2 + 3 ]}} || ZnO dry; 200 °C<ref name=watts>Watts, H. (1872). A Dictionary of Chemistry. UK: Longman, Green, Roberts & Green.</ref> |
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Reaction with ] gives ]:<ref name=graham>Graham-Otto's ausführliches Lehrbuch der Chemie. (1881). Germany: Vieweg.</ref> |
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:{{chem2 | CCl4 + H2S -> CCl2S + 2 HCl }} |
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==History and synthesis== |
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Carbon tetrachloride was originally synthesized in 1820 by ], who named it "protochloride of carbon", by decomposition of ] ("perchloride of carbon") which he synthesized by chlorination of ].<ref>{{Cite book| author=Faraday, Michael | title = Experimental Researches in Chemistry and Physics | page = 46 | year = 1859 | publisher=Taylor and Francis | url = https://archive.org/details/experimentalrese00fararich| isbn = 978-0-85066-841-4}}</ref><ref>Turner, Edward. Elements of Chemistry: Including the Recent Discoveries and Doctrines of the Science. United Kingdom, John Taylor, 1834. Page 247</ref> The protochloride of carbon has been previously misidentified as ] because it can be made with the same reaction of hexachloroethane. Later in the 19th century, the name "protochloride of carbon" was used for tetrachloroethylene, and carbon tetrachloride was called "bichloride of carbon" or "perchloride of carbon". ] developed another method to synthesise carbon tetrachloride from ], ] or ] with excess ] in 1839.<ref name=grahamwatts/> |
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Kolbe made carbon tetrachloride in 1845 by passing chlorine over carbon disulfide through a porcelain tube.<ref name=grahamwatts>Graham, T., Watts, H. (1850). Elements of Chemistry: Including the Applications of the Science in the Arts. USA: Baillière.</ref> Prior to the 1950s, carbon tetrachloride was manufactured by the chlorination of ] at 105 to 130 °C:<ref name=Ross/> |
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:CS<sub>2</sub> + 3 ] → CCl<sub>4</sub> + ] |
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But now it is mainly produced from ]: |
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:CH<sub>4</sub> + 4 Cl<sub>2</sub> → CCl<sub>4</sub> + 4 ] |
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The production often utilizes by-products of other ]s, such as from the syntheses of ] and ]. Higher chlorocarbons are also subjected to this process named "chlorinolysis": |
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:] + Cl<sub>2</sub> → 2 CCl<sub>4</sub> |
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The production of carbon tetrachloride has steeply declined since the 1980s because of environmental concerns and the decreased demand for ], which were derived from carbon tetrachloride. In 1992, production in the U.S./Europe/Japan was estimated at 720,000 tonnes.<ref name=Ross>Manfred Rossberg, Wilhelm Lendle, Gerhard Pfleiderer, Adolf Tögel, Eberhard-Ludwig Dreher, Ernst Langer, Heinz Jaerts, Peter Kleinschmidt, Heinz Strack, Richard Cook, Uwe Beck, Karl-August Lipper, Theodore R. Torkelson, Eckhard Löser, Klaus K. Beutel, "Chlorinated Hydrocarbons" in Ullmann's Encyclopedia of Industrial Chemistry, 2006 Wiley-VCH, Weinheim. {{doi|10.1002/14356007.a06_233.pub2}}</ref> |
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===Natural occurrence=== |
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Carbon tetrachloride was discovered along with chloromethane and chloroform in ], ] and ]es.<ref>{{cite journal | doi = 10.1021/np50088a001 | author = Gribble, G. W. | title = Naturally occurring organohalogen compounds – A comprehensive survey | journal = Progress in the Chemistry of Organic Natural Products | year = 1996 | volume = 68 | pages = 1–423 | pmid = 8795309 | issue = 10}}</ref> The natural emissions of carbon tetrachloride are too little compared to those from anthropogenic sources; for example, the ] Volcano in ] emits carbon tetrachloride at a flux of 82 grams per year while the global industrial emissions were at 2 × 10<sup>10</sup> grams per year.<ref name=natural/> |
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Carbon tetrachloride was found in ] ''] '' and '']''.<ref>Gribble, G. (2012). Progress in the Chemistry of Organic Natural Products. Austria: Springer Vienna.</ref> It was detected in Southern California ecosystems, ]s of ]n Steppe and a common ] in Czechia.<ref name=natural>Naturally Occurring Organohalogen Compounds. (2023). Springer Nature Switzerland.</ref> |
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==Safety== |
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At high temperatures in air, it decomposes or burns to produce poisonous ]. This was a common problem when carbon tetrachloride was used as a fire extinguisher<ref name="Burke">{{cite book |last=Burke |first=Robert |title=Fire Protection: Systems and Response |date=2007-11-06 |publisher=CRC Press |isbn=978-0-203-48499-9 |pages=209}}</ref> and there have been deaths due to its conversion to phosgene reported.<ref name="Fieldner Katz Kinney 1920">{{cite journal |last1=Fieldner |first1=A.C. |last2=Katz |first2=S.H. |last3=Kinney |first3=S.P. |last4=Longfellow |first4=E.S. |title=Poisonous gases from carbon tetrachloride fire extinguishers |journal=Journal of the Franklin Institute |date=October 1920 |volume=190 |issue=4 |pages=543–565 |doi=10.1016/S0016-0032(20)91494-1 }}</ref> |
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Carbon tetrachloride is a suspected human ] but there is no sufficient evidence of carcinogenicity in humans.<ref>{{cite web |title=Report on Carcinogens, Fourteenth Edition - Carbon Tetrachloride |url=https://ntp.niehs.nih.gov/ntp/roc/content/profiles/carbontetrachloride.pdf |publisher=ntp.niehs.nih.gov}}</ref> The ] reports carbon tetrachloride can induce ]s (hepatomas) in mice and rats. The doses inducing hepatic tumors in mice and rats are higher than those inducing cell toxicity.<ref>{{cite web |title=Environmental Health Criteria 208: CARBON TETRACHLORIDE |url=https://www.who.int/ipcs/publications/ehc/who_ehc_208.pdf?ua=1 |publisher=who.int}}</ref> The ] (IARC) classified this compound in ], "''possibly carcinogenic to humans''".<ref>{{cite web |title=Public Health Statement for Carbon Tetrachloride (Tetracloruro de Carbono) |url=https://www.atsdr.cdc.gov/phs/phs.asp?id=194&tid=35 |publisher=atsdr.cdc.gov}}</ref> |
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Carbon tetrachloride is one of the most potent ] (toxic to the liver), so much so that it is widely used in scientific research to evaluate hepatoprotective agents.<ref name=TemaNord/><ref name=Seifert/> Exposure to high concentrations of carbon tetrachloride (including vapor) can affect the ] and degenerate the liver<ref name=Seifert> |
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{{cite journal |
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|vauthors=Seifert WF, Bosma A, Brouwer A |
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|title=Vitamin A deficiency potentiates carbon tetrachloride-induced liver fibrosis in rats |
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|journal=Hepatology |
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|volume=19 |
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|issue=1 |
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|pages=193–201 |
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|date=January 1994 |
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|pmid=8276355 |
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|doi = 10.1002/hep.1840190129 |
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|s2cid=205863459 |
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| display-authors=etal |
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}}</ref> and kidneys,<ref> |
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{{cite journal |
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|vauthors=Liu KX, Kato Y, Yamazaki M, Higuchi O, Nakamura T, Sugiyama Y |
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|title=Decrease in the hepatic clearance of hepatocyte growth factor in carbon tetrachloride-intoxicated rats |
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|journal=Hepatology |
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|volume=17 |
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|issue=4 |
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|pages=651–60 |
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|date=April 1993 |
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|pmid=8477970 |
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|doi=10.1002/hep.1840170420 |
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|s2cid=25794501 |
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|doi-access=free |
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}}</ref> and prolonged exposure may lead to ] or death.<ref> |
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{{cite journal |
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| title = Mechanism of Carbon-tetrachloride Toxicity |
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| author1 = Recknagel R. O. |
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| author2 = Glende E. A. |
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| author3 = Dolak J. A. |
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| author4 = Waller R. L. |
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| journal = Pharmacology & Therapeutics |
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| issue = 43 |
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| pages = 139–154 |
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| year = 1989 |
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| doi = 10.1016/0163-7258(89)90050-8 |
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| volume = 43 |
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| pmid = 2675128 |
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}}</ref> Chronic exposure to carbon tetrachloride can cause ]<ref> |
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{{cite journal |
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|author=Recknagel R. O. |
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|title=Carbon tetrachloride hepatotoxicity |
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|journal=Pharmacol. Rev. |
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|volume=19 |
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|issue=2 |
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|pages=145–208 |
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|date=June 1967 |
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|pmid=4859860 |
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|url=http://pharmrev.aspetjournals.org/cgi/pmidlookup?view=long&pmid=4859860 |
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}}</ref><ref> |
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{{cite journal |
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|author = Masuda Y. |
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|title = |
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|language = ja |
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|journal = Yakugaku Zasshi |
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|volume = 126 |
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|issue = 10 |
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|pages = 885–99 |
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|date = October 2006 |
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|pmid = 17016019 |
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|doi = 10.1248/yakushi.126.885 |
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|doi-access= free |
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}}</ref> and ] and could result in ].<ref>{{cite journal |
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| vauthors=Rood AS, McGavran PD, Aanenson JW, Till JE|title=Stochastic estimates of exposure and cancer risk from carbon tetrachloride released to the air from the rocky flats plant |journal=Risk Anal. |volume=21 |issue=4 |pages=675–95 |date=August 2001 |pmid=11726020 |doi=10.1111/0272-4332.214143 |
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|bibcode=2001RiskA..21..675R |s2cid=31797685 }}</ref><ref> {{webarchive|url=https://web.archive.org/web/20100913043411/http://fscimage.fishersci.com/msds/90116.htm |date=2010-09-13 }} at Fisher Scientific.</ref> |
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Consumption of ] increases the toxic effects of carbon tetrachloride and may cause more severe organ damage, such as ], in heavy drinkers. The doses that can cause mild toxicity to non-drinkers can be fatal to drinkers.<ref name=toxprofile>Toxicological Profile for Carbon Tetrachloride. (2005). USA: Agency for Toxic Substances and Disease Registry.</ref> |
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The effects of carbon tetrachloride on human health and the environment have been assessed under ] in 2012 in the context of the substance evaluation by France.<ref>{{cite web |url=http://echa.europa.eu/information-on-chemicals/evaluation/community-rolling-action-plan/corap-table/-/substance-rev/3080/term |title=Substance evaluation - CoRAP - ECHA |website=echa.europa.eu |access-date=28 April 2018 |url-status=live |archive-url=https://web.archive.org/web/20160820174108/https://echa.europa.eu/information-on-chemicals/evaluation/community-rolling-action-plan/corap-table/-/substance-rev/3080/term |archive-date=20 August 2016}}</ref> |
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In 2008, a study of common cleaning products found the presence of carbon tetrachloride in "very high concentrations" (up to 101 mg/m<sup>3</sup>) as a result of manufacturers' mixing of surfactants or soap with ] (bleach).<ref> |
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{{cite journal |
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| author = Odabasi M. |
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| title = Halogenated Volatile Organic Compounds from the Use of Chlorine-Bleach-Containing Household Products |
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| journal = Environmental Science & Technology |
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| volume = 42 |
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| issue = 5 |
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| pages = 1445–51 |
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| year = 2008 |
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| doi = 10.1021/es702355u |
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| pmid = 18441786 |
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| bibcode = 2008EnST...42.1445O }}</ref> |
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Carbon tetrachloride is also both ]<ref>{{cite journal |
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| author = Fraser P. |
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| title = Chemistry of stratospheric ozone and ozone depletion |
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| journal = Australian Meteorological Magazine |
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| volume =46 |
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| issue =3 |
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| pages = 185–193 |
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| year = 1997 }}</ref> and a ].<ref>{{cite journal |
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| vauthors = Evans WF, Puckrin E |
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| title = A measurement of the greenhouse radiation associated with carbon tetrachloride (CCl<sub>4</sub>) |
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| journal = Geophysical Research Letters |
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| volume = 23 |
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| issue = 14 |
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| pages = 1769–72 |
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| year = 1996 |
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| doi = 10.1029/96GL01258 |
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| bibcode=1996GeoRL..23.1769E |
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}}</ref> However, since 1992<ref>{{cite journal |
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| author = Walker, S. J. |
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| author2 = Weiss R. F. |
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| author3 = Salameh P. K. |
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| name-list-style = amp |
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| year = 2000 |
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| title = Reconstructed histories of the annual mean atmospheric mole fractions for the halocarbons CFC-11, CFC-12, CFC-113 and carbon tetrachloride |
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| journal = Journal of Geophysical Research |
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| volume =105 |
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| issue = C6 |
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| pages = 14285–96 |
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| doi = 10.1029/1999JC900273 |
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| bibcode=2000JGR...10514285W |
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| doi-access = free |
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}}</ref> its atmospheric concentrations have been in decline for the reasons described above (see atmospheric concentration graphs in the ]). CCl<sub>4</sub> has an ] of 85 years.<ref>The Atlas of Climate Change (2006) by ] and Thomas E. Downing {{ISBN|978-0-520-25558-6}}</ref> |
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==Uses== |
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In ], carbon tetrachloride serves as a source of chlorine in the ]. |
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:]{{clear-left}} |
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Carbon tetrachloride made from heavy ] has been used in the detection of ]s and ]s. ] used carbon tetrachloride in his experiments to detect antineutrinos.<ref>{{cite journal | doi = 10.1103/PhysRev.97.766 | title = Attempt to Detect the Antineutrinos from a Nuclear Reactor by the Cl<sup>37</sup> (𝜈,𝑒<sup>−</sup>) A<sup>37</sup> Reaction | date = 1955 | last1 = Davis | first1 = Raymond | journal = Physical Review | volume = 97 | issue = 3 | pages = 766–769 }}</ref> |
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==Historical uses== |
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Carbon tetrachloride was widely used as a ] solvent, as a ], and in ]s.<ref>{{cite journal |title= A History of the Production and Use of Carbon Tetrachloride, Tetrachloroethylene, Trichloroethylene and 1,1,1-Trichloroethane in the United States: Part 1—Historical Background; Carbon Tetrachloride and Tetrachloroethylene |author=Doherty R. E. |issue=2 |year=2000 |pages=69–81 |doi=10.1006/enfo.2000.0010 |journal=Environmental Forensics | volume=1|bibcode=2000EnvFo...1...69D |s2cid=97680726 }}</ref> In the last case, carbon tetrachloride is a key ingredient that adds weight to the otherwise buoyant wax. |
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One speciality use of carbon tetrachloride was in ], to reveal ]s on postage stamps without damaging them. A small amount of the liquid is placed on the back of a stamp, sitting in a black glass or obsidian tray. The letters or design of the watermark can then be seen clearly. Today, this is done on lit tables without using carbon tetrachloride. |
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===Cleaning=== |
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Being a good solvent for many materials (such as grease and tar), carbon tetrachloride was widely used as a cleaning fluid for nearly 70 years. It is nonflammable and nonexplosive and did not leave any odour on the cleaned material, unlike ], which was also used for cleaning at the time. It was used as a "safe" alternative to gasoline. It was first marketed as '''Katharin''', in 1890<ref name=recommended/> or 1892<ref>Neueste Erfindungen und Erfahrungen Auf Den Gebieten Der Praktischen Technik, Elektrotechnik, Der Gewerbe, Industrie, Chemie, Der Land und Hauswirthschaft. (1895). Austria: (n.p.).</ref> and as '''Benzinoform''' later. |
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] |
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Carbon tetrachloride was recommended for regularly cleaning the type slugs of typewriters in office settings in the 1940s.<ref>{{cite journal |last1=Kasten |first1=R. M. |title=First Aid for Typewriters |journal=Popular Science Monthly |date=1941 |volume=138 |issue=5 |pages=156–160 |access-date=21 October 2024 |url=https://books.google.com/books?id=hycDAAAAMBAJ&dq=popular%20science%201941%20%22the%20handy%20man%22%20typewriter&pg=PA156}}</ref> |
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Carbon tetrachloride was the first chlorinated solvent to be used in ] and was used until the 1950s.<ref name=drycleaning/> It had the downsides of being corrosive to the dry-cleaning equipment and causing illness among dry-cleaning operators, and was replaced by ], ]<ref name="drycleaning"></ref> and ] (trichloroethane).<ref>Health and Safety Guide for Laundries and Dry Cleaners. (1975) U.S. Department of Health, Education, and Welfare, Public Health Service, Center for Disease Control, National Institute for Occupational Safety and Health, Division of Technical Services.</ref> |
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Carbon tetrachloride was also used as an alternative to petrol (gasoline) in ]s, from the beginning of 1903 to the 1930s. Several women had fainted from its fumes during the hair wash in barber shops, the hairdressers often used ]s to blow the fumes away. In 1909, a ]'s daughter, Helenora Elphinstone-Dalrymple (aged 29), died after having her hair shampooed with carbon tetrachloride.<ref>Pharmaceutical Journal: A Weekly Record of Pharmacy and Allied Sciences. (1909). UK: J. Churchill.</ref><ref>Meeker, R., Hamilton, A. (1915). Industrial Poisons Used in the Rubber Industry. U.S. Government Printing Office.</ref> |
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It is assumed that carbon tetrachloride was still used as a dry cleaning solvent in ] as of 2006.<ref>Report of the TEAP, May 2006 Progress Report. (2006). Kenya: United Nations Environment Programme Ozone Secretariat.</ref> |
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=== Medical uses === |
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====Anaesthetic and analgesic==== |
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Carbon tetrachloride was briefly used as a volatile inhalation anaesthetic and analgesic for intense ] pains and headaches in the mid-19th century.<ref name=p302>"The Tetrachloride of Carbon as an Anaesthetic", Dr Protheroe Smith, British Journal of Dental Science and Prosthetics (1867). UK: J. P. Segg & Company, page 302</ref> Its anaesthetic effects were known as early as 1847 or 1848.<ref>''On the Anaesthetic Use of Terchloride and Protochloride of Carbon'' The Lancet. UK, J. Onwhyn, 1848.</ref><ref>''Mr Nunneley on Anaesthesia and Anaesthetic Substances'' Edinburgh medical and surgical journal (1849). UK</ref> |
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It was introduced as a safer alternative to ] by the doctor Protheroe Smith in 1864.<ref>"A New Anaesthetic", British Journal of Dental Science and Prosthetics (1867). UK: J. P. Segg & Company, page 239</ref> In December 1865, the Scottish obstetrician who discovered the anaesthetic effects of chloroform on humans, ], had experimented with carbon tetrachloride as an anaesthetic.<ref name=Bichloride>Notes on the anaesthetic properties of the Bichloride of Carbon by Arthur Ernest Sansom, Transactions of the Obstetrical Society of London. (1867) UK: Longmans, Green and Company.</ref> Simpson named the compound "Chlorocarbon" for its similarity to chloroform. His experiments involved injecting carbon tetrachloride into two women's vaginas. Simpson orally consumed carbon tetrachloride and described it as having "the same effect as swallowing a capsule of chloroform".<ref>Pages 170-173, "Anaesthetic and Sedative Properties of Bichloride of Carbon, or Chlorocarbon" (December 1865), Simpson, J. Y., Anaesthesia, Hospitalism, Hermaphroditism, and a Proposal to Stamp Out Small-pox and Other Contagious Diseases. (1871( UK: Adam and Charles Black.</ref> |
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Because of the higher amount of chlorine atoms (compared to chloroform) in its molecule, carbon tetrachloride has a stronger anaesthetic effect than chloroform and required a smaller amount.<ref name=p302/> Its anaesthetic action was likened to ], rather than the related chloroform.<ref name=Bichloride/> It is less volatile than chloroform, therefore it was more difficult to apply and needed warm water to evaporate.<ref name=Bichloride/> Its smell has been described as "fruity",<ref name=Bichloride/> quince-like<ref name=PSmith>Protheroe Smith, Dental Cosmos. (1867). USA: S. S. White Dental Manufacturing Company, page 673</ref> and "more pleasant than chloroform",<ref name=p302/> and had a "pleasant taste".<ref name=Bichloride/> Carbon tetrachloride for anaesthetic use was made by the chlorination of ]. It was used on at least 50 patients, of which most were women in labour.<ref>"The Tetrachloride of Carbon as an Anaesthetic", Dr Protheroe Smith, British Journal of Dental Science and Prosthetics (1867). UK: J. P. Segg & Company, page 260</ref> During anaesthesia, carbon tetrachloride has caused such violent muscular contractions and negative effects on the heart in some patients that it had to be replaced with chloroform or ether.<ref name=Bichloride/><ref name="Andrews">Am J Dent Sci. 1868 Jan; 1(9): 462–463. |
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"Trial of Tetrachloride of Carbon as an Anaesthetic.—Dangerous Effects" E. Andrews |
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</ref> Such use was experimental and the anaesthetic use of carbon tetrachloride never gained popularity due to its potential toxicity. |
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====Parasite medication==== |
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] |
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The veterinary doctor Maurice Crowther Hall (1881-1938) discovered in 1921 that carbon tetrachloride was incredibly effective as an anthelminthic in eradicating hookworm via ingestion. In one of the clinical trials of carbon tetrachloride, it was tested on criminals to determine its safety for use in human beings.<ref>Browning, E. (1940). Modern Drugs in General Practice.</ref> Beginning in 1922, capsules of pure carbon tetrachloride were marketed by ] under the name '''Necatorina''' (variants include '''Neo-necatorina''' and '''Necatorine'''). Necatorina was used as a medication against parasitic diseases in humans. This medication was most prevalently used in ] countries.<ref>Tropical Diseases Bulletin (1927) UK: Bureau of Hygiene and Tropical Diseases.</ref><ref>Taeger, H. (2013) Die Klinik der entschädigungspflichtigen Berufskrankheiten. Germany: Springer Berlin Heidelberg.</ref> Its toxicity was not well understood at the time and toxic effects were attributed to impurities in the capsules rather than carbon tetrachloride itself.<ref>Tropical Diseases Bulletin (1925) UK: Bureau of Hygiene and Tropical Diseases.</ref> Due to carbon tetrachloride's toxicity, ] (which was also investigated by Hall in 1925) replaced its use as an anthelmintic by the 1940s.<ref>Manson-Bahr, P. H., Manson, P. (1954). Manson's Tropical Diseases: A Manual of the Diseases of Warm Climates.</ref> |
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]. Note the "perfectly harmless" statement for carbon tetrachloride and the claims of toxic impurities in other companies' preparations.]] |
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===Solvent=== |
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It once was a popular ] in organic chemistry, but because of its adverse health effects, it is rarely used today.<ref name=TemaNord/> It is sometimes useful as a solvent for ], because there are no significant absorption bands above 1600 cm<sup>−1</sup>. Because carbon tetrachloride does not have any hydrogen atoms, it was historically used in proton ]. In addition to being toxic, its dissolving power is low.<ref>{{cite web |url=http://www.cem.msu.edu/~reusch/VirtualText/Spectrpy/nmr/nmr1.htm |title=Introduction to Nuclear Magnetic Resonance Spectroscopy |publisher=] |author=W. Reusch |work=Virtual Textbook of Organic Chemistry |url-status=dead |archive-url=https://web.archive.org/web/20060831170638/http://www.cem.msu.edu/~reusch/VirtualText/Spectrpy/nmr/nmr1.htm |archive-date=August 31, 2006 }}</ref> Its use in NMR spectroscopy has been largely superseded by ] (mainly ]). The use of carbon tetrachloride in the determination of oil has been replaced by various other solvents, such as ].<ref name=TemaNord> {{webarchive |url=https://web.archive.org/web/20080227052412/http://www.norden.org/pub/ebook/2003-516.pdf |date=February 27, 2008 }}</ref> Because it has no C–H bonds, carbon tetrachloride does not easily undergo ]s. It is a useful solvent for ]s either by the elemental ] or by a halogenation reagent such as ] (these conditions are known as ]).{{cn|date=January 2024}} |
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===Fire suppression=== |
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] |
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] |
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Between 1902 and 1908, carbon tetrachloride-based fire extinguishers began to appear in the United States, years after Europe.<ref name=recommended/> |
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In 1910, the Pyrene Manufacturing Company of Delaware filed a patent to use carbon tetrachloride to extinguish fires.<ref>{{US patent|1010870}}, filed April 5, 1910.</ref> The liquid was vaporized by the heat of combustion and extinguished flames, an early form of ]. At the time it was believed the gas displaced oxygen in the area near the fire, but later research found that the gas inhibited the chemical chain reaction of the combustion process.{{Citation needed|date=July 2021}} |
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In 1911, Pyrene patented a small, portable extinguisher that used the chemical.<ref>{{US patent|1105263}}, filed Jan 7, 1911.</ref> The extinguisher consisted of a ] bottle with an integrated hand-pump that was used to expel a jet of liquid toward the fire. As the container was unpressurized, it could easily be refilled after use.<ref>{{cite web |
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|publisher = Vintage Fire Extinguishers |
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|title = Pyrene Fire Extinguishers |
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|url = http://www.vintagefe.com/pyrene.html |
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|access-date = 23 December 2009 |
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|url-status = dead |
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|archive-url = https://web.archive.org/web/20100325160709/http://www.vintagefe.com/pyrene.html |
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|archive-date = 25 March 2010 |
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}} |
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</ref> Carbon tetrachloride was suitable for liquid and electrical fires and the extinguishers were often carried on aircraft or motor vehicles. However, as early as 1920, there were reports of fatalities caused by the chemical when used to fight a fire in a confined space.<ref name="Fieldner Katz Kinney 1920"/> |
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In the first half of the 20th century, another common fire extinguisher was a single-use, sealed glass globe, a "fire grenade, " filled with carbon tetrachloride or salt water. The bulb could be thrown at the base of the flames to quench the fire. The carbon tetrachloride type could also be installed in a spring-loaded wall fixture with a ]-based restraint. When the solder melted by high heat, the spring would either break the globe or launch it out of the bracket, allowing the extinguishing agent to be automatically dispersed into the fire.<ref>{{Cite book |last=Burke |first=Robert |url=https://books.google.com/books?id=R8ahgLlUTLEC&dq=carbon+tetrachloride+fire+extinguisher&pg=PA209 |title=Fire Protection: Systems and Response |date=2007-11-06 |publisher=CRC Press |isbn=978-0-203-48499-9 |pages=209 |language=en}}</ref> |
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] |
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A well-known brand of fire grenade was the "Red Comet", which was variously manufactured with other fire-fighting equipment in the Denver, Colorado area by the Red Comet Manufacturing Company from its founding in 1919 until manufacturing operations were closed in the early 1980s.<ref>{{cite web |
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|publisher = City of Littleton, CO |
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|title = Red Comet Manufacturing Company |
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|url = http://www.littletongov.org/my-littleton/littleton-history/other-topics/red-comet-manufacturing |
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|access-date = 30 September 2016 |
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|url-status = live |
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|archive-url = https://web.archive.org/web/20161001211637/http://www.littletongov.org/my-littleton/littleton-history/other-topics/red-comet-manufacturing |
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|archive-date = 1 October 2016 |
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}} |
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}} |
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</ref>{{dead link|date=February 2024}} |
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Since carbon tetrachloride freezes at –23 °C, the fire extinguishers would contain only 89-90% carbon tetrachloride and 10% ] (] –85 °C) or ] (m.p. –63 °C) for lowering the extinguishing mixture's freezing point down to temperatures as low as –45 °C. The extinguishers with 10% trichloroethylene would contain 1% ] as a stabiliser.<ref name=recommended>Hazards of Carbon Tetrachloride Fire Extinguishers: Recommended Practices Number 3. USA, The Council, 1967.</ref> |
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=== Refrigerants === |
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Prior to the ], large quantities of carbon tetrachloride were used to produce the ] refrigerants R-11 (]) and R-12 (]). However, these refrigerants play a role in ] and have been phased out. Carbon tetrachloride is still used to manufacture less destructive refrigerants.{{cn|date=January 2024}} |
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===Fumigant=== |
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Carbon tetrachloride was widely used as a ] to kill insect pests in stored grain.<ref>{{Cite web |date=2018-08-09 |title=ACSH Explains: What's The Story On Carbon Tetrachloride? |url=https://www.acsh.org/news/2018/08/09/acsh-explains-whats-story-carbon-tetrachloride-13292 |access-date=2022-02-03 |website=American Council on Science and Health |language=en}}</ref> It was employed in a mixture known as 80/20, that was 80% carbon tetrachloride and 20% ].<ref>{{Cite journal |last1=Peters |first1=H. A. |last2=Levine |first2=R. L. |last3=Matthews |first3=C. G. |last4=Sauter |first4=S. |last5=Chapman |first5=L. |date=1986 |title=Synergistic neurotoxicity of carbon tetrachloride/carbon disulfide (80/20 fumigants) and other pesticides in grain storage workers |url=https://pubmed.ncbi.nlm.nih.gov/3535379/ |access-date=2022-02-03 |journal=Acta Pharmacologica et Toxicologica |volume=59 |pages=535–546 |doi=10.1111/j.1600-0773.1986.tb02820.x |pmid=3535379}}</ref> The ] banned its use in 1985.<ref>{{Cite news |last=Darst |first=Guy |date=1985-02-12 |title=Manufacturers Take Grain Fumigant Off Market in Face of EPA Testing |language=en |work=AP News|url=https://apnews.com/article/baee5a0b83efd39fc92f08db6b4a58ee |access-date=2022-02-03}}</ref> |
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Another carbon tetrachloride fumigant preparation mixture contained ]. Carbon tetrachloride reduced the flammability of the mixture. Most common trade names for the preparation were ''Acritet'', ''Carbacryl'' and ''Acrylofume''.<ref>''COMMERCIAL PRODUCTS'' Morgan, D. P. (1996). Recognition and Management of Pesticide Poisonings. (n.p.): DIANE Publishing Company.</ref> The most common preparation, ''Acritet'', was prepared with 34 percent acrylonitrile and 66 percent carbon tetrachloride.<ref>Hearings, Reports and Prints of the Senate Committee on Government Operations (1964). U.S. Government Printing Office.</ref><ref>Plant Protection and Quarantine Treatment Manual. (1976). U.S. Department of Agriculture, Animal and Plant Health Inspection Service, Plant Protection and Quarantine Programs.</ref> |
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==Society and culture== |
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* The French writer ] intoxicated himself by inhalation of carbon tetrachloride which he used to kill the beetles he collected, to "encounter other worlds" by voluntarily plunging himself into intoxications close to comatose states.<ref name=Libe2011>{{cite web | title=Le cercle des «phrères» disparus | author1=Frédérique Roussel | year=2011 | url=https://www.liberation.fr/culture/2011/08/25/le-cercle-des-phreres-disparus_756766/ }}</ref> |
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* Carbon tetrachloride is listed (along with ], ], ], ], ], ], ] and "BHA") as an ingredient in Peter Parker's (]) custom web fluid formula in the book ''The Wakanda Files: A Technological Exploration of the Avengers and Beyond''.<ref>{{ cite web | title= Marvel Official MCU Spider-Man Web Fluid Formula| date=23 October 2020| url=https://thedirect.com/article/marvel-official-mcu-spider-man-web-fluid-formula}}</ref> |
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* Australian YouTuber Tom of ''Explosions&Fire'' and ''Extractions&Ire'' made a video on extracting carbon tetrachloride from an old fire extinguisher in 2019,<ref>{{cite web |url= https://youtube.com/watch?v=piN0fDkivG0 |title= Illegal Chemical from a Vintage 1960s Extinguisher|last= de Prinse|first= Tom|date= 22 September 2019|website= YouTube}}</ref> and later experimenting with it by mixing it with ],<ref>{{cite web |url= https://youtube.com/watch?v=psUc_oBXE6c |title= Mixing Sodium and Chlorinated Solvents is Real Bad (Carbon Tetrachloride and Sodium)|last= de Prinse|first= Tom|date= 27 March 2020|website= YouTube |publisher= |access-date= |quote=}}</ref> and the chemical gained a ] called "''Tet Gang''" on social media (especially on ]). The channel owner later used carbon tetrachloride-themed designs in the channel's merch. |
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* In the ] song "]" released in 1977, the narrator says that ] the vapours of ''Carbona'', a carbon tetrachloride-based stain remover, was better than huffing glue. They later removed the song from the album as ] was a corporate trademark.<ref>Bessman, Jim (1993). ''Ramones: An American Band.'' St. Martin's Griffin. p74.</ref> |
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===Famous deaths from carbon tetrachloride poisoning=== |
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* ] (1917–1944), British actress who died from accidentally drinking carbon tetrachloride after mistaking it for her drink while working in a photographic darkroom.<ref>{{cite web | url=http://www.bostock.net/tree/bostgen/names/king/evelyn1917.html | title=Evelyn Hermia (1917 - 1944) }}</ref> |
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* ] (1887–1952), an American director who died from carbon tetrachloride poisoning shortly after directing his first television production.<ref>{{cite book | last = Okuda | first = Ted | authorlink = Ted Okuda |author2=Watz, Edward | title = The Columbia Comedy Shorts | publisher = McFarland & Company, Inc., Publishers | year = 1986 | pages = 214 | isbn = 0-89950-181-8}}</ref> |
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* ] (1910–1956), American musician and activist who died from accidentally drinking a glass full of carbon tetrachloride-based typewriter cleaning fluid that she mistook for water.<ref>{{Cite book|title=Highlander: No Ordinary School, 2nd ed.|last=Glen|first=John M.|publisher=University of Tennessee Press|year=1996|location=Knoxville|pages=138}}</ref> |
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* ] (1911–1955), American stage director who was exposed to the fumes of carbon tetrachloride that was used to clean off paint from a carpet. She died a week later from kidney failure.<ref>{{Cite news |title=Margo Jones Theatre To Suspend on Dec. 15 | work=The New York Times |url=http://timesmachine.nytimes.com/timesmachine/1959/12/07/89308262.html?pageNumber=42 |access-date=2022-03-23 |language=en}}</ref> |
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* ] (1919–1956), American record producer, died after exposure to carbon tetrachloride fumes while cleaning recording equipment.<ref>''Certificate of Death: James A. Beck,'' Texas Department of Health, Bureau of Vital Statistics, File #24027</ref> |
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* ] (1933–1982), American blues singer, died after using carbon tetrachloride in floor refinishing.<ref>{{cite web|url=http://www.soulfulkindamusic.net/ttucker.htm |title=Tommy Tucker|publisher=Soulfulkindamusic.net |accessdate=June 13, 2014}}</ref><ref>{{cite news |title=Robert Higginbotham, Singer Of Blues and Jazz, Dead at 48 |url=https://www.nytimes.com/1982/01/25/nyregion/robert-higginbotham-singer-of-blues-and-jazz-dead-at-48.html |quote=Robert Higginbotham, a blues and jazz singer who performed under the name Tommy Tucker, died Friday at College Hospital in Newark. Mr. Higginbotham, who lived in East Orange, N.J., was 48 years old. ... A native of Springfield, Ohio, he had lived in East Orange for 17 years. He was a licensed real-estate broker and had been an amateur prize fighter as a young man. |newspaper=] |date=January 25, 1982 |accessdate=August 20, 2012 }}</ref> |
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<!--you.--> |
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==Gallery== |
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<gallery class="center"> |
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File:CCl4_mm.png|CCl<sub>4</sub> measured by the Advanced Global Atmospheric Gases Experiment () in the lower atmosphere (]) at stations around the world. Abundances are given as pollution-free monthly mean mole fractions in ]. |
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File:Hats ccl4 global.png|Hemispheric and Global mean concentrations of CCl<sub>4</sub> (NOAA/ESRL). |
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Image:AYool CCl4 history.png|Time-series of atmospheric concentrations of CCl<sub>4</sub> (Walker ''et al.'', 2000). |
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</gallery> |
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==References== |
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{{reflist|30em}} |
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==External links== |
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* {{ICSC|0024|00}} |
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* {{PGCH|0107}} |
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* {{cite journal |title=Carbon Tetrachloride (Group 2B) |journal=International Agency for Research on Cancer (IARC) – Summaries & Evaluations |volume=71 |page=401 |year=1999 |url=http://www.inchem.org/documents/iarc/vol71/011-carbontetrac.html}} |
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{{Halomethanes}} |
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{{Carbon compounds}} |
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{{Chlorides}} |
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{{Authority control}} |
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{{DEFAULTSORT:Carbon Tetrachloride}} |
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