Wikipedia

Isophorone

This article is about α-isophorone. For its isomer, see β-isophorone.

Isophorone is an α,β-unsaturated cyclic ketone. It is a colorless liquid with a characteristic peppermint-like odor, although commercial samples can appear yellowish. Used as a solvent and as a precursor to polymers, it is produced on a large scale industrially.[4]

Isophorone[1]
Isophorone
Names
Preferred IUPAC name
3,5,5-Trimethylcyclohex-2-en-1-one
Other names
3,5,5-Trimethyl-2-cyclohexene-1-one
1,1,3-Trimethyl-3-cyclohexene-5-one
Isoforone
Isoacetophorone
IP
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.001.024 Edit this at Wikidata
EC Number
  • 201-126-0
KEGG
UNII
  • InChI=1S/C9H14O/c1-7-4-8(10)6-9(2,3)5-7/h4H,5-6H2,1-3H3 checkY
    Key: HJOVHMDZYOCNQW-UHFFFAOYSA-N checkY
  • InChI=1/C9H14O/c1-7-4-8(10)6-9(2,3)5-7/h4H,5-6H2,1-3H3
    Key: HJOVHMDZYOCNQW-UHFFFAOYAC
  • O=C1\C=C(/CC(C)(C)C1)C
Properties
C9H14O
Molar mass 138.210 g·mol−1
Appearance Colorless to white liquid
Odor Peppermint-like[2]
Density 0.9255 g/cm3
Melting point −8.1 °C (17.4 °F; 265.0 K)
Boiling point 215.32 °C (419.58 °F; 488.47 K)
1.2 g/100 mL
Solubility ether, acetone, hexane, dichloromethane, benzene, toluene, alcohol
Vapor pressure 0.3 mmHg (20°C)[2]
1.4766
Viscosity 2.62 cP
Thermochemistry
43.4 kJ/mol
Hazards
Flash point 84 °C (183 °F; 357 K)
460 °C (860 °F; 733 K)
Explosive limits 0.8–3.8%[2]
Lethal dose or concentration (LD, LC):
2280 mg/kg (rat, oral)[citation needed]
2330 mg/kg (rat, oral)
2690 mg/kg (mouse, oral)[3]
4600 ppm (guinea pig, 8 hr)[3]
885 ppm (rat, 6 hr)
1840 ppm (rat, 4 hr)[3]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 25 ppm (140 mg/m3)[2]
REL (Recommended)
 TWA 4 ppm (23 mg/m3)[2]
IDLH (Immediate danger)
 200 ppm[2]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Structure and reactivity

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Isophorone undergoes reactions characteristic of an α,β-unsaturated ketone. Hydrogenation gives the cyclohexanone derivative. Epoxidation with basic hydrogen peroxide affords the oxide.[5]

Isophorone is degraded by attack of hydroxyl radicals.[6]

Photodimerization

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When exposed to sunlight in aqueous solutions, isophorone undergoes 2+2 photocycloaddition to give three isomeric photodimers (Figure). These "diketomers" are cis-syn-cis, head to tail (HT), cys-anti-cys (HT), and head-head (HH). The formation of HH photodimers is favored over HT photodimers with increasing polarity of the medium.[7]

 

Natural occurrence

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Isophorone occurs naturally in cranberries.[8]

Synthesis

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Isophorone is produced on a multi-thousand ton scale by the aldol condensation of acetone using KOH. Diacetone alcohol, mesityl oxide, and 3-hydroxy-3,5,5-trimethylcyclohexan-1-one are intermediates. A side product is beta-isophorone, where the C=C group is not conjugated with the ketone.[4]

 

Applications

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The partly hydrogenated derivative trimethylcyclohexanone is used in production of polycarbonates. It condenses with phenol to give an analogue of bisphenol A. Polycarbonates produced by phosgenation of these two diols produces a polymer with improved thermal stability.[9] Trimethyladipic acid and 2,2,4-trimethylhexamethylenediamine are produced from trimethylcyclohexanone and trimethylcyclohexanol. They are used to make specialty polyamides. Hydrocyanation gives the nitrile followed by reductive amination gives isophorone diamine. This diamine is used to produce isophorone diisocyanate which has certain niche applications.[4]

 
Isophorone diisocyanate is used to produce specialty polyurethanes.

Full hydrogenation gives 3,3,5-Trimethylcyclohexanol, a precursor to both sunscreens and chemical weapons.

Safety

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The LD50 value of isophorone in rats and rabbits by oral exposure is around 2.00 g/kg.[10] The safety aspects of isophorone have been subject to several studies.[11]

History

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The use of isophorone as a solvent resulted from the search for ways to dispose of or recycle acetone, which is a waste product of phenol synthesis by the Hock method.[12]

See also

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References

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  1. ^ Merck Index, 13th Edition, 5215.
  2. ^ a b c d e f NIOSH Pocket Guide to Chemical Hazards. "#0355". National Institute for Occupational Safety and Health (NIOSH).
  3. ^ a b c "Isophorone". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  4. ^ a b c Hardo Siegel; Manfred Eggersdorfer (2005). "Ketones". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a15_077. ISBN 978-3-527-30673-2.
  5. ^ Richard L. Wasson; Herbert O. House (1957). "Isophorone Oxide". Org. Synth. 37: 58. doi:10.15227/orgsyn.037.0058.
  6. ^ "TOXNET". toxnet.nlm.nih.gov. Archived from the original on 2017-10-24. Retrieved 2016-03-11.
  7. ^ Gonçalves, Huguette; Robinet, Germaine; Barthelat, Michèle; Lattes, Armand (1998-01-28). "Supramolecularity and Photodimerization of Isophorone: FTIR and Molecular Mechanics Studies". The Journal of Physical Chemistry A. 102 (8): 1279–1287. Bibcode:1998JPCA..102.1279G. doi:10.1021/jp9729270.
  8. ^ "Isophorone".
  9. ^ Volker Serini (2000). "Polycarbonates". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a21_207. ISBN 978-3-527-30673-2.
  10. ^ "Toxicity Effects". tools.niehs.nih.gov. Retrieved 2016-03-11.
  11. ^ W. Morton Grant, Joel S. Schuman M.D (11 February 2016). "Toxicology of the Eye: Effects on the Eyes and Visual System from Chemicals, Drugs, Metals and Minerals, Plants, Toxins, and Venoms; Also, Systemic Side Effects from Eye". Med (2-Volume Set) 4th Edition, Page 863.
  12. ^ Isophorone history at Degussa
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