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'''Chloromethane''', also called '''methyl chloride''', '''Refrigerant-40''', '''R-40''' or '''HCC 40''', is an [[organic compound]] with the chemical formula {{chem2|CH3Cl}}. One of the [[haloalkane]]s, it is a colorless, sweet-smelling, flammable gas. Methyl chloride is a crucial [[reagent]] in industrial chemistry, although it is rarely present in consumer products,<ref name=Ross/> and was formerly utilized as a [[refrigerant]].
'''Chloromethane''', also called '''methyl chloride''', '''Refrigerant-40''', '''R-40''' or '''HCC 40''', is an [[organic compound]] with the chemical formula {{chem2|CH3Cl}}. One of the [[haloalkane]]s, it is a colorless, sweet-smelling, flammable gas. Methyl chloride is a crucial [[reagent]] in industrial chemistry, although it is rarely present in consumer products,<ref name=Ross/> and was formerly utilized as a [[refrigerant]]. Most chloromethane is biogenic.


==Occurrence==
==Occurrence==
Chloromethane is an abundant [[organohalogen]], anthropogenic or natural, in the atmosphere.<ref>{{cite journal|journal=Int. J. Environ. Sci. Technol.|year=2017|pages=1355–1370|doi=10.1007/s13762-016-1219-5|title=REVIEW: Halocarbon Emissions from Marine Phytoplankton and Climate Change|first1=Y.-K.|last1=Lim|first2=S.-M.|last2=Phang|first3=N. Abdul |last3=Rahman|first4=W. T.|last4=Sturges|first5= G.|last5=Malin|s2cid=99300836}}</ref>
Chloromethane is an abundant [[organohalogen]], anthropogenic or natural, in the atmosphere. Natural sources produce an estimated 4,100,000,000 kg/yr.<ref>{{cite book|title=Naturally Occurring Organohalogen Compounds|editor=
Kinghorn, A. Douglas.; Falk, Heinz, Gibbons, Simon; Asakawa, Yoshinori; Liu, Ji-Kai; Dirsch, Verena M. Cham|publisher=Springer Nature|location=Switzerland|year=2023|
ISBN= 3-031-26629-3|author=Gribble, Gordon|series=Progress in the Chemistry of Organic Natural Products }}</ref>
===Marine===
===Marine===
Laboratory cultures of marine [[phytoplankton]] (''Phaeodactylum tricornutum'', ''Phaeocystis'' sp., ''Thalassiosira weissflogii'', ''Chaetoceros calcitrans'', ''Isochrysis'' sp., ''Porphyridium'' sp., ''Synechococcus'' sp., ''Tetraselmis'' sp., ''Prorocentrum'' sp., and ''Emiliana huxleyi'') produce CH<sub>3</sub>Cl, but in relatively insignificant amounts.<ref>{{cite journal |vauthors=Scarratt MG, Moore RM| year = 1996 | title = Production of Methyl Chloride and Methyl Bromide in Laboratory Cultures of Marine Phytoplankton | journal = Mar Chem | volume = 54 | pages = 263–272 | doi = 10.1016/0304-4203(96)00036-9 | issue = 3–4| bibcode = 1996MarCh..54..263S }}</ref><ref>{{cite journal |vauthors=Scarratt MG, Moore RM| year = 1998 | title = Production of Methyl Bromide and Methyl Chloride in Laboratory Cultures of Marine Phytoplankton II | journal = Mar Chem | volume = 59 | pages = 311–320 | doi = 10.1016/S0304-4203(97)00092-3 | issue = 3–4| bibcode = 1998MarCh..59..311S }}</ref> An extensive study of 30 species of polar macroalgae revealed the release of significant amounts of CH<sub>3</sub>Cl in only ''Gigartina skottsbergii'' and ''Gymnogongrus antarcticus''.<ref>{{cite journal | author = Laturnus F | year = 2001 | title = Marine Macroalgae in Polar Regions as Natural Sources for Volatile Organohalogens | journal = Environ Sci Pollut Res | volume = 8 | pages = 103–108 | doi = 10.1007/BF02987302 | pmid = 11400635 | issue = 2| s2cid = 570389 }}</ref>
Laboratory cultures of marine [[phytoplankton]] (''Phaeodactylum tricornutum'', ''Phaeocystis'' sp., ''Thalassiosira weissflogii'', ''Chaetoceros calcitrans'', ''Isochrysis'' sp., ''Porphyridium'' sp., ''Synechococcus'' sp., ''Tetraselmis'' sp., ''Prorocentrum'' sp., and ''Emiliana huxleyi'') produce CH<sub>3</sub>Cl, but in relatively insignificant amounts.<ref>{{cite journal |vauthors=Scarratt MG, Moore RM| year = 1996 | title = Production of Methyl Chloride and Methyl Bromide in Laboratory Cultures of Marine Phytoplankton | journal = Mar Chem | volume = 54 | pages = 263–272 | doi = 10.1016/0304-4203(96)00036-9 | issue = 3–4| bibcode = 1996MarCh..54..263S }}</ref><ref>{{cite journal |vauthors=Scarratt MG, Moore RM| year = 1998 | title = Production of Methyl Bromide and Methyl Chloride in Laboratory Cultures of Marine Phytoplankton II | journal = Mar Chem | volume = 59 | pages = 311–320 | doi = 10.1016/S0304-4203(97)00092-3 | issue = 3–4| bibcode = 1998MarCh..59..311S }}</ref> An extensive study of 30 species of polar macroalgae revealed the release of significant amounts of CH<sub>3</sub>Cl in only ''Gigartina skottsbergii'' and ''Gymnogongrus antarcticus''.<ref>{{cite journal | author = Laturnus F | year = 2001 | title = Marine Macroalgae in Polar Regions as Natural Sources for Volatile Organohalogens | journal = Environ Sci Pollut Res | volume = 8 | pages = 103–108 | doi = 10.1007/BF02987302 | pmid = 11400635 | issue = 2| s2cid = 570389 }}</ref>

Revision as of 22:08, 25 November 2023

Chloromethane
Stereo, skeletal formula of chloromethane with all explicit hydrogens added
Ball and stick model of chloromethane
Ball and stick model of chloromethane
Spacefill model of chloromethane
Spacefill model of chloromethane
Names
Preferred IUPAC name
Chloromethane[2]
Other names
  • Refrigerant-40
  • R-40[1]
  • Methyl chloride[1]
  • Monochloromethane[1]
Identifiers
3D model (JSmol)
1696839
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.000.744 Edit this at Wikidata
EC Number
  • 200-817-4
24898
KEGG
MeSH Methyl+Chloride
RTECS number
  • PA6300000
UNII
UN number 1063
  • InChI=1S/CH3Cl/c1-2/h1H3 checkY
    Key: NEHMKBQYUWJMIP-UHFFFAOYSA-N checkY
  • CCl
Properties
CH3Cl
Molar mass 50.49 g·mol−1
Appearance Colorless gas
Odor Faint, sweet odor[3]
Density 1.003 g/mL (-23.8 °C, liquid)[1] 2.3065 g/L (0 °C, gas)[1]
Melting point −97.4 °C (−143.3 °F; 175.8 K)[1]
Boiling point −23.8 °C (−10.8 °F; 249.3 K)[1]
5.325 g L−1
log P 1.113
Vapor pressure 506.09 kPa (at 20 °C (68 °F))
940 nmol Pa−1 kg−1
-32.0·10−6 cm3/mol
Structure
Tetragonal
Tetrahedron
1.9 D
Thermochemistry
234.36 J K−1 mol−1
−83.68 kJ mol−1
−764.5–−763.5 kJ mol−1
Hazards
GHS labelling:
GHS02: Flammable GHS08: Health hazard
Danger
H220, H351, H373
P210, P281, P410+P403
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propaneInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
4
0
Flash point −20 °C (−4 °F; 253 K)[1]
625 °C (1,157 °F; 898 K)[1]
Explosive limits 8.1%-17.4%[3]
Lethal dose or concentration (LD, LC):
150-180 mg/kg (oral, rat)[1]
5.3 mg/L/4 h (inhalation, rat)[1]
72,000 ppm (rat, 30 min)
2200 ppm (mouse, 6 hr)
2760 ppm (mammal, 4 hr)
2524 ppm (rat, 4 hr)[4]
20,000 ppm (guinea pig, 2 hr)
14,661 ppm (dog, 6 hr)[4]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 100 ppm C 200 ppm 300 ppm (5-minute maximum peak in any 3 hours)[3]
REL (Recommended)
 Ca[3]
IDLH (Immediate danger)
 Ca [2000 ppm][3]
Related compounds
Related alkanes
Related compounds
 2-Chloroethanol
Supplementary data page
Chloromethane (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Chloromethane, also called methyl chloride, Refrigerant-40, R-40 or HCC 40, is an organic compound with the chemical formula CH3Cl. One of the haloalkanes, it is a colorless, sweet-smelling, flammable gas. Methyl chloride is a crucial reagent in industrial chemistry, although it is rarely present in consumer products,[5] and was formerly utilized as a refrigerant. Most chloromethane is biogenic.

Occurrence

Chloromethane is an abundant organohalogen, anthropogenic or natural, in the atmosphere. Natural sources produce an estimated 4,100,000,000 kg/yr.[6]

Marine

Laboratory cultures of marine phytoplankton (Phaeodactylum tricornutum, Phaeocystis sp., Thalassiosira weissflogii, Chaetoceros calcitrans, Isochrysis sp., Porphyridium sp., Synechococcus sp., Tetraselmis sp., Prorocentrum sp., and Emiliana huxleyi) produce CH3Cl, but in relatively insignificant amounts.[7][8] An extensive study of 30 species of polar macroalgae revealed the release of significant amounts of CH3Cl in only Gigartina skottsbergii and Gymnogongrus antarcticus.[9]

Biogenesis

The salt marsh plant Batis maritima contains the enzyme methyl chloride transferase that catalyzes the synthesis of CH3Cl from S-adenosine-L-methionine and chloride.[10] This protein has been purified and expressed in E. coli, and seems to be present in other organisms such as white rot fungi (Phellinus pomaceus), red algae (Endocladia muricata), and the ice plant (Mesembryanthemum crystallinum), each of which is a known CH3Cl producer.[10][11]

Sugarcane and the emission of methyl chloride

In the sugarcane industry, the organic waste is usually burned in the power cogeneration process. When contaminated by chloride, this waste burns, releasing methyl chloride in the atmosphere.[12]

Interstellar detections

Chloromethane has been detected in the low-mass Class 0 protostellar binary, IRAS 16293–2422, using the Atacama Large Millimeter Array (ALMA). It was also detected in the comet 67P/Churyumov–Gerasimenko (67P/C-G) using the Rosetta Orbiter Spectrometer for Ion and Neutral Analysis (ROSINA) instrument on the Rosetta spacecraft.[13] The detections reveal that chloromethane can be formed in star-forming regions before planets or life is formed.[citation needed]

Chloromethane has been detected in space.[14]

Production

Chloromethane was first synthesized by the French chemists Jean-Baptiste Dumas and Eugene Peligot in 1835 by boiling a mixture of methanol, sulfuric acid, and sodium chloride. This method is the forerunner for that used today, which uses hydrogen chloride instead of sulfuric acid and sodium chloride.[15]

Chloromethane is produced commercially by treating methanol with hydrochloric acid or hydrogen chloride, according to the chemical equation:[5]

CH3OH + HCl → CH3Cl + H2O

A smaller amount of chloromethane is produced by treating a mixture of methane with chlorine at elevated temperatures. This method, however, also produces more highly chlorinated compounds such as dichloromethane, chloroform, and carbon tetrachloride. For this reason, methane chlorination is usually only practiced when these other products are also desired. This chlorination method also cogenerates hydrogen chloride, which poses a disposal problem.[5]

CH4 + Cl2 → CH3Cl + HCl
CH3Cl + Cl2 → CH2Cl2 + HCl
CH2Cl2 + Cl2 → CHCl3 + HCl
CHCl3 + Cl2 → CCl4 + HCl

Dispersion in the environment

CH3Cl measured by the Advanced Global Atmospheric Gases Experiment (AGAGE) in the lower atmosphere (troposphere) at stations around the world. Abundances are given as pollution free monthly mean mole fractions in parts-per-trillion.

Most of the methyl chloride present in the environment ends up being released to the atmosphere. After being released into the air, the atmospheric lifetime of this substance is about 10 months with multiple natural sinks, such as ocean, transport to the stratosphere, soil, etc.[16][17][18]

On the other hand, when the methyl chloride emitted is released to water, it will be rapidly lost by volatilization. The half-life of this substance in terms of volatilization in the river, lagoon and lake is 2.1 h, 25 h and 18 days, respectively.[19][20]

The amount of methyl chloride in the stratosphere is estimated to be 2 x 106 tonnes per year, representing 20-25% of the total amount of chlorine that is emitted to the stratosphere annually.[21][22]

Uses

Large scale use of chloromethane is for the production of dimethyldichlorosilane and related organosilicon compounds.[5] These compounds arise via the direct process. The relevant reactions are (Me = CH3):

x MeCl + Si → Me3SiCl, Me2SiCl2, MeSiCl3, Me4Si2Cl2, ...

Dimethyldichlorosilane (Me2SiCl2) is of particular value as a precursor to silicones, but trimethylsilyl chloride (Me3SiCl) and methyltrichlorosilane (MeSiCl3) are also valuable. Smaller quantities are used as a solvent in the manufacture of butyl rubber and in petroleum refining.

Chloromethane is employed as a methylating and chlorinating agent, e.g. the production of methylcellulose. It is also used in a variety of other fields: as an extractant for greases, oils, and resins, as a propellant and blowing agent in polystyrene foam production, as a local anesthetic, as an intermediate in drug manufacturing, as a catalyst carrier in low-temperature polymerization, as a fluid for thermometric and thermostatic equipment, and as a herbicide.

Obsolete applications

Chloromethane was a widely used refrigerant, but its use has been discontinued. Chloromethane was also once used for producing lead-based gasoline additives (tetramethyllead).

Safety

Inhalation of chloromethane gas produces central nervous system effects similar to alcohol intoxication. The TLV is 50 ppm and the MAC is the same. Prolonged exposure may have mutagenic effects.[5]

See also

References

  1. ^ a b c d e f g h i j k Record in the GESTIS Substance Database of the Institute for Occupational Safety and Health
  2. ^ International Union of Pure and Applied Chemistry (2014). Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013. The Royal Society of Chemistry. p. 1033. doi:10.1039/9781849733069. ISBN 978-0-85404-182-4.
  3. ^ a b c d e NIOSH Pocket Guide to Chemical Hazards. "#0403". National Institute for Occupational Safety and Health (NIOSH).
  4. ^ a b "Methyl chloride". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  5. ^ a b c d e Rossberg, M.; Lendle, W.; Pfleiderer, G.; Tögel, A.; Dreher, E. L.; Langer, E.; Rassaerts, H.; Kleinschmidt, P.; Strack, H.; Cook, R.; Beck, U.; Lipper, K.-A.; Torkelson, T.R.; Löser, E.; Beutel, K.K.; Mann, T. (2006). "Chlorinated Hydrocarbons". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a06_233.pub2. ISBN 3527306730.
  6. ^ Gribble, Gordon (2023). Kinghorn, A. Douglas.; Falk, Heinz, Gibbons, Simon; Asakawa, Yoshinori; Liu, Ji-Kai; Dirsch, Verena M. Cham (ed.). Naturally Occurring Organohalogen Compounds. Progress in the Chemistry of Organic Natural Products. Switzerland: Springer Nature. ISBN 3-031-26629-3.{{cite book}}: CS1 maint: multiple names: editors list (link)
  7. ^ Scarratt MG, Moore RM (1996). "Production of Methyl Chloride and Methyl Bromide in Laboratory Cultures of Marine Phytoplankton". Mar Chem. 54 (3–4): 263–272. Bibcode:1996MarCh..54..263S. doi:10.1016/0304-4203(96)00036-9.
  8. ^ Scarratt MG, Moore RM (1998). "Production of Methyl Bromide and Methyl Chloride in Laboratory Cultures of Marine Phytoplankton II". Mar Chem. 59 (3–4): 311–320. Bibcode:1998MarCh..59..311S. doi:10.1016/S0304-4203(97)00092-3.
  9. ^ Laturnus F (2001). "Marine Macroalgae in Polar Regions as Natural Sources for Volatile Organohalogens". Environ Sci Pollut Res. 8 (2): 103–108. doi:10.1007/BF02987302. PMID 11400635. S2CID 570389.
  10. ^ a b Ni X, Hager LP (1998). "cDNA Cloning of Batis maritima Methyl Chloride Transferase and Purification of the Enzyme". Proc Natl Acad Sci USA. 95 (22): 12866–71. Bibcode:1998PNAS...9512866N. doi:10.1073/pnas.95.22.12866. PMC 23635. PMID 9789006.
  11. ^ Ni X, Hager LP (1999). "Expression of Batis maritima Methyl Chloride Transferase in Escherichia coli". Proc Natl Acad Sci USA. 96 (7): 3611–5. Bibcode:1999PNAS...96.3611N. doi:10.1073/pnas.96.7.3611. PMC 22342. PMID 10097085.
  12. ^ Lobert, Jurgen; Keene, Willian; Yevich, Jennifer (1999). "Global chlorine emissions from biomass burning: Reactive Chlorine Emissions Inventory". Journal of Geophysical Research: Atmospheres. 104 (D7): 8373–8389. Bibcode:1999JGR...104.8373L. doi:10.1029/1998JD100077.
  13. ^ "ALMA and Rosetta Detect Freon-40 in Space".
  14. ^ "ALMA and Rosetta Detect Freon-40 in Space - Dashing Hopes that Molecule May be Marker of Life". eso.org. Retrieved 3 October 2017.
  15. ^ "Chloromethane". American Chemical Society. Retrieved 2022-05-13.
  16. ^ Fabian P, Borchers R, Leifer R, Subbaraya BH, Lal S, Boy M (1996). "Global stratospheric distribution of halocarbons". Atmospheric Environment. 30 (10/11): 1787–1796. Bibcode:1996AtmEn..30.1787F. doi:10.1016/1352-2310(95)00387-8.
  17. ^ Zhang W, Jiao Y, Zhu R, Rhew RC (2020). "Methyl Chloride and Methyl Bromide Production and Consumption in Coastal Antarctic Tundra Soils Subject to Sea Animal Activities". Environmental Science & Technology. 54 (20): 13354–13363. Bibcode:2020EnST...5413354Z. doi:10.1021/acs.est.0c04257. PMID 32935983. S2CID 221745138.
  18. ^ Carpenter LJ, Reimann S, Burkholder JB, Clerbaux C, Hall BD, Hossaini R, Laube JC, Yvon-Lewis SA (2014). "Update on ODSs and Other Gases of Interest to the Montreal Protocol". WMO (World Meteorological Organization), Scientific Assessment of Ozone Depletion: 2014, Global Ozone Research and Monitoring Project.
  19. ^ Lyman, Warren; Rosenblatt, David; Reehl, William (1982). Handbook of chemical property estimation methods. McGraw-Hill. ISBN 9780070391758.
  20. ^ Agency for Toxic Substances and Disease Registry (ATSDR) (1990). "Toxicological profile for chloromethane". {{cite journal}}: Cite journal requires |journal= (help)
  21. ^ Borchers R, Gunawardena R, Rasmussen RA (1994). "Long term trend of selected halogenated hydrocarbons": 259–262. {{cite journal}}: Cite journal requires |journal= (help)
  22. ^ Crutzen PJ, Gidel LT (1983). "The tropospheric budgets of the anthropogenic chlorocarbons CO, CH4, CH3Cl and the effect of various NOx sources on tropospheric ozone". Journal of Geophysical Research. 88: 6641–6661. doi:10.1029/JC088iC11p06641.
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