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In recent times the catalytic oxidation of cyclohexene by (immobilized) metalloporphyrin complexes has been found to be an efficient way. [7] [8] In laboratory, cyclohexene oxide can also be prepared by reacting cyclohexene with magnesium monoperoxyphthalate (MMPP) in a mixture of isopropanol and water as solvent at room temperature. [9]
Aliquat 336 is used as a phase transfer catalyst, [2] including in the catalytic oxidation of cyclohexene to 1,6-hexanedioic acid. [3] This reaction is an example of green chemistry, as it is more environmentally friendly than the traditional method of oxidizing cyclohexanol or cyclohexanone with nitric acid or potassium permanganate, which produce hazardous wastes.
Benzene is converted to cyclohexylbenzene by acid-catalyzed alkylation with cyclohexene. [6] Cyclohexylbenzene is a precursor to both phenol and cyclohexanone. [7] Hydration of cyclohexene gives cyclohexanol, which can be dehydrogenated to give cyclohexanone, a precursor to caprolactam. [8] The oxidative cleavage of cyclohexene gives adipic acid.
Oxidation of 1-methylcyclohexene catalyzed by cytochrome P450 yields a 2:1 mixture of hydroxylation to epoxidation products. [4] The stereochemistry of hydroformylation has been examined using 1-methylcyclohexene. The main product has the formyl group on the less substituted alkene-carbon, trans with respect to the methyl substituent. [5]
Potassium permanganate will decompose into potassium manganate, manganese dioxide and oxygen gas: 2 KMnO 4 → K 2 MnO 4 + MnO 2 + O 2. This reaction is a laboratory method to prepare oxygen, but produces samples of potassium manganate contaminated with MnO 2. The former is soluble and the latter is not.
It has been found that the rate of oxidation of electron-deficient olefins can be accelerated by maintaining the pH of the reaction slightly acidic. [13] On the other hand, a high pH can increase the rate of oxidation of internal olefins, and also increase the enantiomeric excess (e.e.) for the oxidation of terminal olefins. [13]
The three phenomena of oxidation, as described in the article text. The model assumes that the oxidation reaction occurs at the interface between the oxide layer and the substrate material, rather than between the oxide and the ambient gas. [3] Thus, it considers three phenomena that the oxidizing species undergoes, in this order:
Depending on the conditions in which the titration is performed, the manganese is reduced from an oxidation of +7 to +2, +4, or +6. In most cases, permanganometry is performed in a very acidic solution in which the following electrochemical reaction occurs: [3] MnO − 4 + 8 H + + 5 e − → Mn 2+ + 4 H 2 O; E° = +1.51 V [4]