Isocyanic acid
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| Names | |
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| IUPAC name
Isocyanic acid
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| Other names
Carbimide[1]
Carbonic imide | |
| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.109.068 |
PubChem CID
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| UNII |
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CompTox Dashboard (EPA)
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| Properties | |
| HNCO | |
| Molar mass | 43.025 g·mol−1 |
| Appearance | Colorless gas (condenses near room temperature) |
| Density | 1.14 g/cm3[2] |
| Melting point | |
| Boiling point | 23.5 °C (74.3 °F; 296.6 K) (extrapolated)[2] |
| Dissolves; polymerizes if concentrated | |
| Solubility | Soluble in benzene, toluene, diethyl ether |
| Acidity (pKa) | 3.7[4] |
| Conjugate acid | Oxomethaniminium[5] |
| Conjugate base | Cyanate |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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Poisonous |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Isocyanic acid is a chemical compound with the structural formula HNCO, which is often written as H−N=C=O. It is a colourless, volatile and poisonous gas, condensing at 23.5 °C. It is the predominant tautomer and an isomer of cyanic acid (aka. cyanol) (H−O−C≡N), and the monomer of cyanuric acid.
The derived anion of isocyanic acid is the same as the derived anion of cyanic acid, and that anion is [N=C=O]−, which is called cyanate. The related functional group −N=C=O is isocyanate; it is distinct from cyanate (−O−C≡N), fulminate (−O−N+≡C−), and nitrile oxide (−C≡N+−O−).[6]
Isocyanic acid was discovered in 1830 by Justus von Liebig and Friedrich Wöhler.[7]
Isocyanic acid is the simplest stable chemical compound that contains carbon, hydrogen, nitrogen, and oxygen, the four most commonly found elements in organic chemistry and biology. It is the only fairly stable one of the four linear isomers with molecular formula HOCN that have been synthesized, the others being cyanic acid (cyanol, H−O−C≡N) and the elusive fulminic acid (H−C≡N+−O−)[8] and isofulminic acid H−O−N+≡C−.[6][9]
Structure
[edit]Isocyanic acid (HNCO)
[edit]Although the electronic structure according to valence bond theory can be written as H−N=C=O, the vibrational spectrum has a band at 2268.8 cm−1 in the gas phase, which some say indicates a carbon–nitrogen triple bond.[10][11] If so, then the canonical form H−N+≡C−O− is the major resonance structure.
However, classic vibrational analysis would indicate that the 2268.8 cm−1 is the asymmetric N=C=O stretch, as per Colthup et al.,[12] as well as the NIST Chemistry WebBook,[13] which also reports the corresponding symmetric N=C=O stretch (weak in infrared, but strong in Raman) to be 1327 cm−1. Based on these classic assignments, there is no need to invoke a full charged state for the N and O atoms, to explain the vibrational spectral data.
Cyanic acid (HOCN)
[edit]The tautomer, known as cyanic acid, HOCN, in which the oxygen atom is protonated exists in equilibrium with isocyanic acid to the extent of about 3%.[citation needed][dubious – discuss] The vibrational spectrum is indicative of the presence of a triple bond between the nitrogen and carbon atoms.[11]
Properties
[edit]In aqueous solution it is a weak acid, having a pKa of 3.7:[4]
- HNCO ⇌ H+ + NCO−
Isocyanic acid hydrolyses to carbon dioxide and ammonia:
- HNCO + H2O → CO2 + NH3
Dilute solutions of isocyanic acid are stable in inert solvents, e.g. ether and chlorinated hydrocarbons.[2]
At high concentrations, isocyanic acid oligomerizes to give the trimer cyanuric acid and cyamelide, a polymer. These species usually are easily separated from liquid- or gas-phase reaction products.[2]
Isocyanic acid reacts with amines to give ureas (carbamides):
- HNCO + RNH2 → RNHC(O)NH2
This reaction is called carbamylation. Excess isocyanic acid can react with the ureas to give allophanates.[2]
HNCO adds across electron-rich double bonds, such as vinylethers, to give the corresponding isocyanates.
Isocyanic acid, HNCO, is a Lewis acid whose free energy, enthalpy and entropy changes for its 1:1 association with a number of bases in carbon tetrachloride solution at 25 °C have been reported.[14] The acceptor properties of HNCO are compared with other Lewis acid in the ECW model.
Low-temperature photolysis of solids containing HNCO creates the tautomer cyanic acid H−O−C≡N, also called hydrogen cyanate.[15] Pure cyanic acid has not been isolated, and isocyanic acid is the predominant form in all solvents.[2] Sometimes information presented for cyanic acid in reference books is actually for isocyanic acid.[citation needed]
Preparation
[edit]Isocyanic acid can be made by protonation of the cyanate anion, such as from salts like potassium cyanate, by either gaseous hydrogen chloride or acids such as oxalic acid.[16]
- H+ + NCO− → HNCO
HNCO also can be made by the high-temperature thermal decomposition of the trimer cyanuric acid:
- C3H3N3O3 → 3 HNCO
In all cases the resulting acid must be kept very cold or in gaseous form, as concentrated isocyanic acid polymerizes rapidly above −20 °C.[2]
In the reverse of the famous synthesis of urea by Friedrich Wöhler,
- CO(NH2)2 → HNCO + NH3
isocyanic acid is produced and rapidly trimerizes to cyanuric acid.
Occurrence
[edit]Isocyanic acid has been detected in many kinds of interstellar environments.[9]
Isocyanic acid is also present in various forms of smoke, including smog and cigarette smoke. It was detected using mass spectrometry, and easily dissolves in water, posing a health risk to the lungs.[17]
See also
[edit]References
[edit]- ^ Cyanamide also has this name, and for which it is more systematically correct
- ^ a b c d e f g h Narula, Acharan S.; Ramachandran, Kishore (2001). "Isocyanic Acid". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.ri072m. ISBN 0-471-93623-5.
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- ^ a b Pettit, Gwyneth; Pettit, Leslie. "SC-Database" (proprietary database). Timble, Yorks: Academic Software — via proprietary executable.
- ^ "Oxomethaniminium | CH2NO | ChemSpider". www.chemspider.com. Retrieved 27 January 2019.
- ^ a b Martin, William R.; Ball, David W. (2019). "Small organic fulminates as high energy materials. Fulminates of acetylene, ethylene, and allene". Journal of Energetic Materials. 37 (1): 70–79. Bibcode:2019JEnM...37...70M. doi:10.1080/07370652.2018.1531089.
- ^ Liebig, J.; Wöhler, F. (1830). "Untersuchungen über die Cyansäuren". Ann. Phys. 20 (11): 394. Bibcode:1830AnP....96..369L. doi:10.1002/andp.18300961102.
- ^ Kurzer, Frederick (2000). "Fulminic Acid in the History of Organic Chemistry". Journal of Chemical Education. 77 (7): 851–857. Bibcode:2000JChEd..77..851K. doi:10.1021/ed077p851.
- ^ a b Quan, Donghui; Herbst, Eric; Osamura, Yoshihiro; Roueff, Evelyne (2010). "Gas-Grain Modeling of Isocyanic Acid (Hnco), Cyanic Acid (Hocn), Fulminic Acid (Hcno), and Isofulminic Acid (Honc) in Assorted Interstellar Environments". The Astrophysical Journal. 725 (2): 2101–2109. Bibcode:2010ApJ...725.2101Q. doi:10.1088/0004-637X/725/2/2101. hdl:1811/47796.
- ^ Nakamoto, part A, p 190
- ^ a b Teles, Joaquim Henrique; Maier, Günther; Andes Hess, B.; Schaad, Lawrence J.; Winnewisser, Manfred; Winnewisser, Brenda P. (1989). "The CHNO Isomers". Chemische Berichte. 122 (4): 753–766. doi:10.1002/cber.19891220425.
- ^ Colthup, Norman B.; Daly, Lawrence H.; Wiberley, Stephen E. (1990). Introduction to Infrared and Raman Spectroscopy. Academic Press (Elsevier). ISBN 978-0-12-182554-6.
- ^ "Isocyanic acid". National Institute of Standards and Technology (U.S. Department of Commerce). Retrieved 2023-04-20.
- ^ Nelson, J. (1970) Hydrogen-bonded complexes of isocyanic acid: Infrared spectra and thermodynamic measurements. Spectrochimica Acta Part A: Molecular Spectroscopy 26,109-120.
- ^ Jacox, M.E.; Milligan, D.E. (1964). "Low-Temperature Infrared Study of Intermediates in the Photolysis of HNCO and DNCO". Journal of Chemical Physics. 40 (9): 2457–2460. Bibcode:1964JChPh..40.2457J. doi:10.1063/1.1725546.
- ^ Fischer, G.; Geith, J.; Klapötke, T. M.; Krumm B. (2002). "Synthesis, Properties and Dimerization Study of Isocyanic Acid" (PDF). Z. Naturforsch. 57b (1): 19–25. doi:10.1515/znb-2002-0103. S2CID 37461221.
- ^ Preidt, Robert. "Chemical in Smoke May Pose Health Risk". MyOptumHealth. AccuWeather. Retrieved 14 September 2011.
External links
[edit]- Walter, Wolfgang (1997). Organic Chemistry: A Comprehensive Degree Text and Source Book. Chichester: Albion Publishing. p. 364. ISBN 978-1-898563-37-2. Retrieved 2008-06-21.
- Cyanic acid from NIST Chemistry WebBook (accessed 2006-09-09)
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