Abstract:Prepared froni 4-(2,6,6-trimcthylcyclohex-l-cnyl) -but-3-yn-2-01 acetate by epoxidation followed by lithium aluminium hydridc reduction: NMR. (CDCI,) : 1.04(3H, s). 1.20(3H, s ) , 1.27(311, d, J = ~H z ) , 1.34(3H, s), 4,36(1H, q, ,I = 7 Hz), 5,46(1H, d x d , J = 7HZ, J' -5112) ppni; IR. (liq.): 3350, 1955 cm-l.Summary. The literature data on hcteropolar and homopolar 2-center bond dissociation energies in organic molecules in the gas phase and the corrcsponding heats of formation of radicals and ions havc bee… Show more
“…A comparison of the rate constants for the loss of NO 2 (fast) and NO (slower) 7,17 suggests, however, that formation of NO 2 by process (2) is unlikely. The reasoning is that since the dissociation energies of the C-N and C-O bonds of C 6 H 5 NO 2 and C 6 H 5 ONO, respectively, are similar (ca 70 kcal mol À1 ), 4,20 but the O-NO bond of C 6 H 5 NO is weak (17-24 kcal mol À1 ), 20,34 the rates of loss of NO 2 and NO would be expected to be similar if NO 2 came from the C 6 H 5 ONO isomer. As just noted, they have been found to be different.…”
The relative extents of loss of NO 2 and NO were determined by 70 eV electron ionization and tandem mass spectrometry using B/E linked scans to investigate metastable (unimolecular) and collision-induced dissociation processes for molecular ions formed by electron ionization of para-substituted nitrobenzene compounds. The substituents used (NO 2 , CHO, H, OCH 3 ) represent a wide range of electron donor-acceptor properties. Loss of NO 2 was favored by electron-withdrawing groups, while an electron-donor group favored loss of NO. Ion fragmentation mechanisms are consistent with the hypothesis that NO 2 to ONO (nitro to nitrite) isomerization precedes the loss of NO. Ring fragmentation (loss of CO) was observed only after all of the electron-withdrawing groups had dissociated. while the electron-donor group OCH 3 remained attached to the ring in the analogous CO elimination. These results are placed in the context of the thermolysis behavior of nitroaromatic explosives.
“…A comparison of the rate constants for the loss of NO 2 (fast) and NO (slower) 7,17 suggests, however, that formation of NO 2 by process (2) is unlikely. The reasoning is that since the dissociation energies of the C-N and C-O bonds of C 6 H 5 NO 2 and C 6 H 5 ONO, respectively, are similar (ca 70 kcal mol À1 ), 4,20 but the O-NO bond of C 6 H 5 NO is weak (17-24 kcal mol À1 ), 20,34 the rates of loss of NO 2 and NO would be expected to be similar if NO 2 came from the C 6 H 5 ONO isomer. As just noted, they have been found to be different.…”
The relative extents of loss of NO 2 and NO were determined by 70 eV electron ionization and tandem mass spectrometry using B/E linked scans to investigate metastable (unimolecular) and collision-induced dissociation processes for molecular ions formed by electron ionization of para-substituted nitrobenzene compounds. The substituents used (NO 2 , CHO, H, OCH 3 ) represent a wide range of electron donor-acceptor properties. Loss of NO 2 was favored by electron-withdrawing groups, while an electron-donor group favored loss of NO. Ion fragmentation mechanisms are consistent with the hypothesis that NO 2 to ONO (nitro to nitrite) isomerization precedes the loss of NO. Ring fragmentation (loss of CO) was observed only after all of the electron-withdrawing groups had dissociated. while the electron-donor group OCH 3 remained attached to the ring in the analogous CO elimination. These results are placed in the context of the thermolysis behavior of nitroaromatic explosives.
“…Heats of formation (± 0.5 kcal • mol 1 ) were obtained by the experimental determination of heats of combustion 25 -27 ) using either a stirred liquid calorimeter 25 ) or an aneroid microcalorimeter 26 ); heats of fusion and heat capacities were measured by differential scanning calorimetry (DSC), heats of vaporization 21. 25.…”
Section: Methodsmentioning
confidence: 99%
“…2 or 3 or in Eq. (1)(2)(3)(4)(5)(6)(7)(8)(9)(10)(11) in general. Ali is equal to or slightly than the corresponding bond dissociation energy (BDE) 6 "' 81 ) as pointed out earlier.…”
“…Accurate values of many parameters are required, such as the experimental electron affinity 27 ͑EA͒ of Cl and the experimental dissociation energy, 28 D 0 ͑C-Cl͒, in methyl chloride. The calculated DA cross section is also sensitive to the precise values of the vibrational energies of the neutral molecule.…”
Section: B Calculation Of Potential Curvesmentioning
The dissociative attachment ͑DA͒ cross section of hot CH 3 Cl has been measured in a crossed electron-molecule beam apparatus at temperatures up to 750 K and electron energies from 0-0.5 eV. The results are compared to cross sections computed using a mixed ab initio-semiempirical approach, treating CH 3 Cl as a quasidiatomic molecule. The theoretical treatment requires an anion potential curve in the stable region as a portion of the input data. Computations with three different basis sets show the results to be sensitive to the size of basis set from which the potential is determined. At high temperatures, the experimental DA cross sections are found to be in very good agreement with those derived from theory using the potential curve computed with the most flexible of the basis sets. At room temperature the theory suggests that the measured DA cross section is still limited by the presence of impurities.
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