Deuterated chloroform

(Redirected from CDCl3)

Deuterated chloroform, also known as chloroform-d, is the organic compound with the formula CDCl3. Deuterated chloroform is a common solvent used in NMR spectroscopy.[2] The properties of CDCl3 and ordinary CHCl3 (chloroform) are virtually identical.

Deuterated chloroform
Stereo, skeletal formula of deuterated chloroform
Stereo, skeletal formula of deuterated chloroform
Spacefill model of deuterated chloroform
Spacefill model of deuterated chloroform
Names
IUPAC name
trichloro(deuterio)methane[1]
Other names
Chloroform-d
Deuterochloroform
Identifiers
3D model (JSmol)
1697633
ChEBI
ChemSpider
ECHA InfoCard 100.011.585 Edit this at Wikidata
EC Number
  • 212-742-4
UNII
UN number 1888
  • InChI=1S/CHCl3/c2-1(3)4/h1H/i1D checkY
    Key: HEDRZPFGACZZDS-MICDWDOJSA-N checkY
  • InChI=1/CHCl3/c2-1(3)4/h1H/i1D
    Key: HEDRZPFGACZZDS-MICDWDOJEH
  • [2H]C(Cl)(Cl)Cl
Properties
CDCl3
Molar mass 120.384 g/mol
Appearance Colorless liquid
Odor chloroform-like
Density 1.500 g/cm3
Melting point −64 °C (−83 °F; 209 K)
Boiling point 61 °C (142 °F; 334 K)
Hazards
GHS labelling:
GHS05: CorrosiveGHS07: Exclamation markGHS08: Health hazard
Danger
H302, H315, H319, H331, H336, H351, H361, H372, H373
P201, P202, P260, P261, P264, P270, P271, P280, P281, P301+P312, P302+P352, P304+P340, P305+P351+P338, P308+P313, P311, P312, P314, P321, P330, P332+P313, P337+P313, P362, P403+P233, P405, P501
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 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Related compounds
Related compounds
Chloroform

Deuterated dichloromethane

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 ?)

Deuterochloroform was first made in 1935 during the years of research on deuterium.[3]

Preparation

edit

Deuterated chloroform is commercially available. It is more easily produced and less expensive than deuterated dichloromethane.[4] Deuterochloroform is produced by the reaction of hexachloroacetone with deuterium oxide, using pyridine as a catalyst. The large difference in boiling points between the starting material and product facilitate purification by distillation.[5][6]

O=C(CCl3)2 + D2O → 2 CDCl3 + CO2

Treating chloral with sodium deuteroxide (NaOD) gives deuterated chloroform.[7][8]

NMR solvent

edit

In proton NMR spectroscopy, deuterated solvent (enriched to >99% deuterium) is typically used to avoid recording a large interfering signal or signals from the proton(s) (i.e., hydrogen-1) present in the solvent itself. If nondeuterated chloroform (containing a full equivalent of protium) were used as solvent, the solvent signal would almost certainly overwhelm and obscure any nearby analyte signals. In addition, modern instruments usually require the presence of deuterated solvent, as the field frequency is locked using the deuterium signal of the solvent to prevent frequency drift. Commercial chloroform-d does, however, still contain a small amount (0.2% or less) of non-deuterated chloroform; this results in a small singlet at 7.26 ppm, known as the residual solvent peak, which is frequently used as an internal chemical shift reference.

In carbon-13 NMR spectroscopy, the sole carbon in deuterated chloroform shows a triplet at a chemical shift of 77.16 ppm with the three peaks being about equal size, resulting from splitting by spin coupling to the attached spin-1 deuterium atom (CHCl3 has a chemical shift of 77.36 ppm).[4]

Deuterated chloroform is a general purpose NMR solvent, as it is not very chemically reactive and unlikely to exchange its deuterium with its solute,[9] and its low boiling point allows for easy sample recovery. It, however, it is incompatible with strongly basic, nucleophilic, or reducing analytes, including many organometallic compounds.

Hazards

edit

Chloroform reacts photochemically with oxygen to form chlorine, phosgene and hydrogen chloride. To slow this process and reduce the acidity of the solvent, chloroform-d is stored in brown-tinted bottles, often over copper chips or silver foil as stabilizer. Instead of metals, a small amount of a neutralizing base like potassium carbonate may be added.[10] It is less toxic to the liver and kidneys than CHCl3 due to the stronger C−D bond as compared to the C−H bond, making it somewhat less prone to form the destructive trichloromethyl radical (•CCl3).[11][12]

References

edit
  1. ^ "Chloroform-d".
  2. ^ Fulmer, Gregory R.; Miller, Alexander J. M.; Sherden, Nathaniel H.; Gottlieb, Hugo E.; Nudelman, Abraham; Stoltz, Brian M.; Bercaw, John E.; Goldberg, Karen I. (2010). "NMR Chemical Shifts of Trace Impurities: Common Laboratory Solvents, Organics, and Gases in Deuterated Solvents Relevant to the Organometallic Chemist" (PDF). Organometallics. 29 (9): 2176–2179. doi:10.1021/om100106e.
  3. ^ Chloroform-d (Deuteriochloroform), F. W. Breuer , J. Am. Chem. Soc. 1935, 57, 11, 2236–2237 (November 1, 1935) [1]
  4. ^ a b "The Theory of NMR – Solvents for NMR spectroscopy". Archived from the original on 2016-03-03. Retrieved 2014-01-23.
  5. ^ Paulsen, P. J.; Cooke, W. D. (1 September 1963). "Preparation of Deuterated Solvents for Nuclear Magnetic Resonance Spectrometry". Analytical Chemistry. 35 (10): 1560. doi:10.1021/ac60203a072.
  6. ^ Zaharani, Lia; Johan, Mohd Rafie Bin; Khaligh, Nader Ghaffari (2022). "Cost and Energy Saving Process for the Laboratory-Scale Production of Chloroform-d". Organic Process Research & Development. 26 (11): 3126–3129. doi:10.1021/acs.oprd.2c00260. S2CID 253071632.
  7. ^ Kluger, Ronald (1964). "A Convenient Preparation of Chloroform-d1". The Journal of Organic Chemistry. 29 (7): 2045-2046. doi:10.1021/jo01030a526.
  8. ^ Breuer, F. W. (1935). "Chloroform-d (Deuteriochloroform)1". Journal of the American Chemical Society. 57 (11): 2236-2237. doi:10.1021/ja01314a058.
  9. ^ Sabot, Cyrille; Kumar, Kanduluru Ananda; Antheaume, Cyril; Mioskowski, Charles (2007-06-01). "Triazabicyclodecene: An Effective Isotope Exchange Catalyst in CDCl3". The Journal of Organic Chemistry. 72 (13): 5001–5004. doi:10.1021/jo070307h. ISSN 0022-3263. PMID 17530896.
  10. ^ Teipel, Jan; Gottstein, Vera; Hölzle, Eva; Kaltenbach, Katja; Lachenmeier, Dirk W.; Kuballa, Thomas (2022). "An Easy and Reliable Method for the Mitigation of Deuterated Chloroform Decomposition to Stabilise Susceptible NMR Samples". Chemistry. 4 (3): 776–785. doi:10.3390/chemistry4030055. ISSN 2624-8549.
  11. ^ Goldstein, Robin S. (2013). Toxic interactions. Hewitt, William R., Hook, Jerry B. Burlington: Elsevier Science. ISBN 978-1-4832-6970-2. OCLC 896796140.
  12. ^ Ahmadizadeh, M.; Kuo, C.-H.; Hook, J.B. (1981-07-01). "Nephrotoxicity and hepatotoxicity of chloroform in mice: Effect of deuterium substitution". Journal of Toxicology and Environmental Health. 8 (1–2): 105–111. Bibcode:1981JTEH....8..105A. doi:10.1080/15287398109530054. ISSN 0098-4108. PMID 7328696.