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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]
Hydration is an important process in many other applications; one example is the production of Portland cement by the crosslinking of calcium oxides and silicates that is induced by water. Hydration is the process by which desiccants function. CuSO 4 ·5H 2 O is bright blue and has a rather different structure from its colourless anhydrous ...
Cyclohexene is a hydrocarbon with the formula (CH 2) 4 C 2 H 2. It is an example of a cycloalkene. At room temperature, cyclohexene is a colorless liquid with a sharp odor. Among its uses, it is an intermediate in the commercial synthesis of nylon. [3]
Cyclohexene derivatives, such as imines, epoxides, and halonium ions, react with nucleophiles in a stereoselective fashion, affording trans-diaxial addition products. The term “Trans-diaxial addition” describes the mechanism of the addition, however the products are likely to equilibrate by ring flip to the lower energy conformer, placing the new substituents in the equatorial position.
Heterogeneous OER is sensitive to the surface in which the reaction takes place and is also affected by the pH of the solution. The general mechanism for acidic and alkaline solutions is shown below. Under acidic conditions water binds to the surface with the irreversible removal of one electron and one proton to form a platinum hydroxide. [4]
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1-Methylcyclohexene an organic compound consisting of cyclohexene with a methyl group substituent attached to the alkene group. Two other structural isomers are known: 3-methylcyclohexene and 4-methylcyclohexene. All are colorless volatile liquids. They are specialized reagents.
Heating may be used to encourage oxidation, although the reaction temperature should never exceed 50 °C, to avoid decomposition of the dioxirane [1] Alkenes bound to both electron-withdrawing and -donating groups tend to behave like the former, requiring long oxidation times and occasionally some heating.