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Carbonyl group

For carboxyl as a ligand, see Metal carbonyl. For the web browser, see Carbonyl (web browser).
A ketone compound containing a carbonyl group (C=O)

For organic chemistry, a carbonyl group is a functional group with the formula C=O, composed of a carbon atom double-bonded to an oxygen atom, and it is divalent at the C atom. It is common to several classes of organic compounds (such as aldehydes, ketones and carboxylic acids), as part of many larger functional groups. A compound containing a carbonyl group is often referred to as a carbonyl compound.[1]

The term carbonyl can also refer to carbon monoxide as a ligand in an inorganic or organometallic complex (a metal carbonyl, e.g. nickel carbonyl).

The remainder of this article concerns itself with the organic chemistry definition of carbonyl, such that carbon and oxygen share a double bond.

Carbonyl compounds

See also: α,β-Unsaturated carbonyl compound

In organic chemistry, a carbonyl group characterizes the following types of compounds:

Compound Aldehyde Ketone Carboxylic acid Carboxylate ester Amide
Structure Aldehyde Ketone Carboxylic acid Ester Amide
General formula RCHO RCOR' RCOOH RCOOR' RCONR'R''
Compound Enone Acyl halide Acid anhydride Imide
Structure Enone Acyl chloride Acid anhydride Imide
General formula RC(O)C(R')CR''R''' RCOX (RCO)2O RC(O)N(R')C(O)R''
Carbon dioxide

Other organic carbonyls are urea and the carbamates, the derivatives of acyl chlorides chloroformates and phosgene, carbonate esters, thioesters, lactones, lactams, hydroxamates, and isocyanates. Examples of inorganic carbonyl compounds are carbon dioxide and carbonyl sulfide.[citation needed]

A special group of carbonyl compounds are dicarbonyl compounds, which can exhibit special properties.

Structure and reactivity

For organic compounds, the length of the C-O bond does not vary widely from 120 picometers. Inorganic carbonyls have shorter C-O distances: CO, 113; CO2, 116; and COCl2, 116 pm.[2]

The carbonyl carbon is typically electrophilic. A qualitative order of electrophilicity is RCHO (aldehydes) > R2CO (ketones) > RCO2R' (esters) > RCONH2 (amides). A variety of nucleophiles attack, breaking the carbon-oxygen double bond.

Interactions between carbonyl groups and other substituents were found in a study of collagen.[3] Substituents can affect carbonyl groups by addition or subtraction of electron density by means of a sigma bond.[4] ΔHσ values are much greater when the substituents on the carbonyl group are more electronegative than carbon.[4]

A carbonyl compound

The polarity of C=O bond also enhances the acidity of any adjacent C-H bonds. Due to the positive charge on carbon and the negative charge on oxygen, carbonyl groups are subject to additions and/or nucleophilic attacks. A variety of nucleophiles attack, breaking the carbon-oxygen double bond, and leading to addition-elimination reactions. Nucleophiliic reactivity is often proportional to the basicity of the nucleophile and as nucleophilicity increases, the stability within a carbonyl compound decreases.[5] The pKa values of acetaldehyde and acetone are 16.7 and 19 respectively,[6]

Spectroscopy

  • Infrared spectroscopy: the C=O double bond absorbs infrared light at wavenumbers between approximately 1600–1900 cm−1(5263 nm to 6250 nm). The exact location of the absorption is well understood with respect to the geometry of the molecule. This absorption is known as the "carbonyl stretch" when displayed on an infrared absorption spectrum.[7] In addition, the ultraviolet-visible spectra of propanone in water gives an absorption of carbonyl at 257 nm.[8]
  • Nuclear magnetic resonance: the C=O double-bond exhibits different resonances depending on surrounding atoms, generally a downfield shift. The 13C NMR of a carbonyl carbon is in the range of 160–220 ppm.[9]

See also

References

  1. ^ Saul Patai, ed. (1966). The Carbonyl Group. PATAI'S Chemistry of Functional Groups. Vol. 1. John Wiley & Sons. doi:10.1002/9780470771051. ISBN 9780470771051.Jacob Zabicky, ed. (1970). The Carbonyl Group. PATAI'S Chemistry of Functional Groups. Vol. 2. John Wiley & Sons. doi:10.1002/9780470771228. ISBN 9780470771228.
  2. ^ G. Berthier, J. Serre (1966). "General and Theoretical Aspects of the Carbonyl Group". In Saul Patai (ed.). The Carbonyl Group. PATAI'S Chemistry of Functional Groups. Vol. 1. John Wiley & Sons. pp. 1–77. doi:10.1002/9780470771051.ch1. ISBN 9780470771051.
  3. ^ Newberry, Robert W.; Raines, Ronald T. (2017-08-15). "The n→π* Interaction". Accounts of Chemical Research. 50 (8): 1838–1846. doi:10.1021/acs.accounts.7b00121. ISSN 0001-4842. PMC 5559721. PMID 28735540.
  4. ^ a b Wiberg, Kenneth B. (1999-11-01). "The Interaction of Carbonyl Groups with Substituents". Accounts of Chemical Research. 32 (11): 922–929. doi:10.1021/ar990008h. ISSN 0001-4842.
  5. ^ Lienhard, Gustav E.; Jencks, William P. (September 1966). "Thiol Addition to the Carbonyl Group. Equilibria and Kinetics1". Journal of the American Chemical Society. 88 (17): 3982–3995. doi:10.1021/ja00969a017. ISSN 0002-7863. PMID 5915153.
  6. ^ Ouellette, R.J. and Rawn, J.D. "Organic Chemistry" 1st Ed. Prentice-Hall, Inc., 1996: New Jersey. ISBN 0-02-390171-3
  7. ^ Mayo D.W., Miller F.A and Hannah R.W “Course Notes On The Interpretation of Infrared and Raman Spectra” 1st Ed. John Wiley & Sons Inc, 2004: New Jersey. ISBN 0-471-24823-1.
  8. ^ "Archived copy" (PDF). Archived from the original (PDF) on 2015-08-24. Retrieved 2015-07-11.{{cite web}}: CS1 maint: archived copy as title (link)
  9. ^ "NMR Spectroscopy. 13C NMR". organicchemistrydata.org. 20 October 2021. Archived from the original on 6 January 2024. Retrieved 6 January 2024.

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