10312-83-1

Basic information

• Product Name: METHOXYACETALDEHYDE
• Synonyms: 2-methoxy-acetaldehyd;2-Methoxyacetaldehyde;Acetaldehyde, 2-methoxy-;alpha-Methoxyacetaldehyde;methoxy-acetaldehyd;Methoxyethanal;METHOXYACETALDEHYDE;Acetaldehyde, methoxy- (8ci,9ci)
• CAS NO: 10312-83-1
• Molecular Formula: C₃H₆O₂
• Molecular Weight: 74.08
• EINECS: 233-693-5
• Mol File: 10312-83-1.mol
• Article Data: 63

Chemical Properties

• Boiling Point: 99-101℃
• Flash Point: -38.9±13.4℃
• Appearance: /
• Density: 0.906±0.06 g/cm3 (20 ºC 760 Torr)
• Vapor Pressure: 406mmHg at 25°C
• Refractive Index: 1.3950 (589.3 nm 20℃)
• CAS DataBase Reference: METHOXYACETALDEHYDE(CAS DataBase Reference)
• NIST Chemistry Reference: METHOXYACETALDEHYDE(10312-83-1)
• EPA Substance Registry System: METHOXYACETALDEHYDE(10312-83-1)

Safety Data

• Hazard Codes: Xn
• Statements: 11-36/37/38-43-36-22
• Safety Statements: 16-33-36/37/39-36/37-26
• RIDADR: 1993
• RTECS: AB2940000
• Hazardous Substances Data: 10312-83-1(Hazardous Substances Data)

Usage

Definition

A highly reactive aldehyde derivative available in 77% aqueous solution. Clear colorless liquid with odor characteristic of lower aldehydes, miscible with water and many organic solvents. Resembles butyraldehyde in structure and some properties. Claimed as possible antimicrobial agent, preservative, and polymer modifier.

InChI:InChI=1/C3H6O2/c1-5-3-2-4/h2H,3H2,1H3

Upstream product

• 22805-71-6 (E)-1,4-dimethoxy-2-butene 
• 557-17-5 methyl propyl ether 
• 14315-97-0 1,1,3-trimethoxypropane 
• 110-71-4 1,2-dimethoxyethane 
• 109-86-4 2-methoxy-ethanol 
• 7664-93-9 sulfuric acid 
• 623-39-2 glycerol 1-monomethyl ether 
• 7732-18-5 water 
• 127-09-3 sodium acetate 
• 96747-12-5 oxo-phenyl-acetic acid 2-methoxy-ethyl ester 
• 41649-14-3 cis-1,4-dimethoxy-2-butene 
• 67-56-1 methanol 
• 6832-13-9 diazoacetaldehyde 
• 24332-20-5 methoxyacetaldehyde dimethylacetal 

Downstream Products

• 625-45-6 2-methoxyacetic acid 
• 7510-55-6 methoxy-acetaldehyde-(4-nitro-phenylhydrazone) 
• 36638-43-4 (2,4-dinitrophenyl)hydrazone of methoxyacetaldehyde 
• 192652-10-1 C₁₇H₂₀O₃ 
• 55854-60-9 1-methoxymethyl-β-carboline 
• 5928-67-6 (S)-(+)-benzoin 
• 50650-38-9 1-(2'-methoxy-ethylidene-amino)-2,6-dimethylbenzene 
• 50563-55-8 2,6-dimethyl-N-(2'-methoxyethyl)-aniline 
• 1115878-45-9 (R)-3-cyclohexenyl-2-hydroxy-1-methoxypropan-3-one 
• 141-46-8 Glycolaldehyde 
• 189245-01-0 C₂₇H₃₄N₄O₈ 
• 925932-14-5 Methyl 4-methoxy-2-N-acetylaminobut-2-enoate 
• 857017-62-0 2-hydroxy-4-(2-methoxy-ethylamino)-benzoic acid 

Relevant articles and documents

Kinetics and Mechanism of the Oxidation of Primary Alcohols by N-bromoacetamide in Alkaline Solution

The kinetics of the oxidation of seven primary alcohols by N-bromoacetamide has been studied in alkaline solution.The main product of the oxidation is the corresponding aldehyde.The reaction first order with respect to the oxidant and alcohol.The oxidation of ethanol indicates an absence of a primary kinetic isotope effect.The rate decreases with the increase in the concentration of hydroxide ion.Addition of acetamide decreases the reaction rate.The rates were determined at five different temperatures and the activation parameters were evaluated.The activation enthalpies and entropies of the oxidation of seven alcohols are linearly related.Hypobromite ion has been postulated as the reactive oxidizing species.A mechanism involving rate-determining nucleophilic attack of hypobromite ion on the alcohol molecule has been proposed.

Kinetics and Mechanism of the Oxidation of Primary Alcohols by N-Bromoacetamide in Acid Medium

The kinetics of the oxidation of ten primary alcohols by N-bromoacetamide (NBA) has been studied in acid medium.The main product of the oxidation is the corresponding aldehyde.The reaction is first order in alcohol, NBA, and H(+).The oxidation of ethanol-1,1-d2 indicates no primary kinetic isotope effect.A solvent isotope effect, k(D2O)/k(H2O)= 1.16, was observed at 308 K.The rates were determined at four different temperatures and the activation parameters were evaluated.Addition of acetamide decreases the rate. (H2OBr)(+) has been postulated as the oxidizing species.A mechanism involving formation of a hypobromite ester in the rate-determining step has been proposed.The reaction constant, ρ*, has a value of -1.53 at 303 K.

STUDY OF THE KINETICS AND MECHANISM OF THE ACID-BASE CATALYZED ENOLIZATION OF HYDROXYACETALDEHYDE AND METHOXYACETALDEHYDE

In acid and alkaline media, glycolaldehyde (hydroxyacetaldehyde) exists in equilibrium with its enediol form, which is quantitatively oxidized to glyoxal by an excess of Methylene Blue.In acid and alkaline media, the enol form of methoxyacetaldehyde is formed.In alkaline medium, this enol is stable; in acid, it undergoes hydrolysis to glycolaldehyde.The kinetics of enolization of glycolaldehyde and methoxyacetaldehyde were studied polarographically.The mechanisms of enolization of glycolaldehyde and acid hydrolysis of methoxyacetaldehyde were established both from kinetic data and from deuterium-incorporation data.The proposed mechanisms were confirmed by quantum-mechanical calculation of the charge distribution in the two compounds studied and their reaction intermediates.The glyoxal obtained in the oxidation was isolated as quinoxaline and analyzed by mass spectrometry.

The lifetime of formylcarbene determined by transient absorption and transient grating spectroscopy

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DEHYDROGENATION OF SUBSTITUTED ALCOHOLS TO ALDEHYDES ON ZINC OXIDE-CHROMIUM OXIDE CATALYSTS

Sixteen primary alcohols of the structure RCH2OH (R = CH3, C2H5, (CH3)2CH, (CH3)3CCH2, HOCH2, CH3OCH2, C6H5, C6H5CH2, C6H5OCH2, ClCH2, BrCH2, F3C, CNCH2, (CH3)2NCH2, (C2H5)2NCH2 and tetrahydrofurfuryl) were explored for the possibility of obtaining the corresponding aldehydes by dehydrogenation on solid catalysts.Various catalysts were tested and two zinc oxide-chromium oxide catalysts were selected for further work because their activity and selectivity was satisfactory; moreover, the selectivity could be improved by addition of sodium into the catalysts and of water into the feed.The reaction was performed in the temperature range 250 - 450 deg C and at atmospheric pressure. 2-Chloroethanol, 2-bromoethanol, ethylene glycol, 2-cyanoethanol and 2-(N,N-diethylamino)ethanol decomposed and deactivated the catalyst.The other alcohols were studied from the point of kinetics of dehydrogenation, which was described by a Langmuir-Hinshelwood type rate equation (3), and of substituent effects on rate, which were correlated by Taft equation (1) with the slope ρ* = -1.46.The preparative value of catalytic dehydrogenation for obtaining substituted aldehydes was confirmed by prolonged runs and isolation of the aldehydic product by distillation using as the feeds 2-methoxyethanol and 2-(N,N-dimethylamino)ethanol, respectively.

1,5,7-TRISUBSTITUTED ISOQUINOLINE DERIVATIVES, PREPARATION THEREOF, AND USE THEREOF IN MEDICINES

The present disclosure relates to 1,5,7-trisubstituted isoquinoline derivatives, their preparation and pharmaceutical use. In particular, the present disclosure discloses a compound of formula (I) or a pharmaceutically acceptable salt, stereoisomer, solvate or prodrug thereof, and a preparation method and use thereof. The definitions of the groups in the formula can be found in the specification and claims.

Gas-Phase Reaction of Methyl n-Propyl Ether with OH, NO3, and Cl: Kinetics and Mechanism

Rate constants at room temperature (293 ± 2 K) and atmospheric pressure for the reaction of methyl n-propyl ether (MnPE), CH3OCH2CH2CH3, with OH and NO3 radicals and the Cl atom have been determined in a 100 L FEP-Teflon reaction chamber in conjunction with gas chromatography-flame ionization detector (GC-FID) as the detection technique. The obtained rate constants k (in units of cm3 molecule-1 s-1) are (9.91 ± 2.30) × 10-12, (1.67 ± 0.32) × 10-15, and (2.52 ± 0.14) × 10-10 for reactions with OH, NO3, and Cl, respectively. The products of these reactions were investigated by gas chromatography-mass spectrometry (GC-MS), and formation mechanisms are proposed for the observed reaction products. Atmospheric lifetimes of the studied ether, calculated from rate constants of the different reactions, reveal that the dominant loss process for MnPE is its reaction with OH, while in coastal areas and in the marine boundary layer, MnPE loss by Cl reaction is also important.