Abstract:The accuracy of experimental data on enthalpies of formation and vaporization of aliphatic amines (primary, secondary, and tertiary amines, di-, tri-, and tetramines, and cycloalkylamines) was assessed by theoretical calculations. The gas-phase enthalpies of formation were calculated using the Gaussian 4 (G4) method combined with isodesmic reactions. Three amines, CH 3 NH 2 , CH 3 NHCH 3 , and (CH 3 ) 3 N, were used as the main reference species in the isodesmic reactions; their experimental enthalpies of form… Show more
“…Unless explicitly said to the contrary, the recent literature study [41] will likewise always be used as the source of information for the enthalpy of formation of acyclic amines. In particular, we accept their recommended value of −76 kJ/mol for the enthalpy of formation of diethylamine.…”
Section: Resultsmentioning
confidence: 99%
“…For the tertiary N-methylaziridine, the secondary 2-methylaziridine, and the primary cyclopropylamine, the enthalpies of formation are 120, 89 and 77 kJ/mol, respectively. [39,41] As a general rule, we find the isomerization transformation [Eq (21)] of isostructural tertiary to secondary to primary amines is exothermic, of increasingly N-alkylated to C-alkylated amines, by ca. 20 kJ/mol.…”
Section: Hcnc ! Ccnh (21)mentioning
confidence: 99%
“…The simplest example is that of 2butylamine, CH 3 CH(NH 2 )CH 2 CH 3 , and 2-methyl-n-propylamine, CH 3 CH(CH 3 )CH 2 NH 2 , both isostructural with 2-methylbutane. With the recommended enthalpies of formation of these two primary amines from [41] of À 105 and À 98 kJ/mol, the difference is 7 kJ/mol. Let us take a consensus ofÀ 101 kJ/mol for the enthalpy of formation of the primary amine to be compared with 2-methylbutane.…”
Small ring nitrogen heterocycles, azabicyclobutanes and azirines, were investigated by computational methods in order to address the discrepancy between their regioisomers 1‐ and 2‐azabicyclobutane and 1H‐ and 2H‐azirines. Both 1‐azabicyclobutane and 2H‐azirine are well known synthetic starting points to larger nitrogen heterocycles whereas 2‐azabicyclobutane and 1H‐azirine and their derivatives have yet to be reported as isolable compounds. Calculated parameters such as structure, base strength (proton affinities), NICS values and enthalpies of formation from which strain energies are derived are reported. The destabilization of the less stable regioisomers is attributed to homoantiaromaticity in 2‐azabicyclobutane and antiaromaticity in 1H‐azirine. Two stereoisomers exist for 2‐azabicyclobutane with the endo‐ stereoisomer being more stable. This phenomenon is indicative of the hydrogen bond acceptor properties of the neighboring cyclpropane and the π‐bond character of the central bond in 2‐azabicyclobutane.
“…Unless explicitly said to the contrary, the recent literature study [41] will likewise always be used as the source of information for the enthalpy of formation of acyclic amines. In particular, we accept their recommended value of −76 kJ/mol for the enthalpy of formation of diethylamine.…”
Section: Resultsmentioning
confidence: 99%
“…For the tertiary N-methylaziridine, the secondary 2-methylaziridine, and the primary cyclopropylamine, the enthalpies of formation are 120, 89 and 77 kJ/mol, respectively. [39,41] As a general rule, we find the isomerization transformation [Eq (21)] of isostructural tertiary to secondary to primary amines is exothermic, of increasingly N-alkylated to C-alkylated amines, by ca. 20 kJ/mol.…”
Section: Hcnc ! Ccnh (21)mentioning
confidence: 99%
“…The simplest example is that of 2butylamine, CH 3 CH(NH 2 )CH 2 CH 3 , and 2-methyl-n-propylamine, CH 3 CH(CH 3 )CH 2 NH 2 , both isostructural with 2-methylbutane. With the recommended enthalpies of formation of these two primary amines from [41] of À 105 and À 98 kJ/mol, the difference is 7 kJ/mol. Let us take a consensus ofÀ 101 kJ/mol for the enthalpy of formation of the primary amine to be compared with 2-methylbutane.…”
Small ring nitrogen heterocycles, azabicyclobutanes and azirines, were investigated by computational methods in order to address the discrepancy between their regioisomers 1‐ and 2‐azabicyclobutane and 1H‐ and 2H‐azirines. Both 1‐azabicyclobutane and 2H‐azirine are well known synthetic starting points to larger nitrogen heterocycles whereas 2‐azabicyclobutane and 1H‐azirine and their derivatives have yet to be reported as isolable compounds. Calculated parameters such as structure, base strength (proton affinities), NICS values and enthalpies of formation from which strain energies are derived are reported. The destabilization of the less stable regioisomers is attributed to homoantiaromaticity in 2‐azabicyclobutane and antiaromaticity in 1H‐azirine. Two stereoisomers exist for 2‐azabicyclobutane with the endo‐ stereoisomer being more stable. This phenomenon is indicative of the hydrogen bond acceptor properties of the neighboring cyclpropane and the π‐bond character of the central bond in 2‐azabicyclobutane.
Liquid organic hydrogen carriers can store hydrogen in a safe and dense form through covalent bonds. Hydrogen uptake and release are realized by catalytic hydrogenation and dehydrogenation, respectively. Indoles have been demonstrated to be interesting candidates for this task. The enthalpy of reaction is a crucial parameter in this regard as it determines not only the heat demand for hydrogen release, but also the reaction equilibrium at given conditions. In this work, a combination of experimental measurements, quantum chemical methods and a group-additivity approach has been applied to obtain a consistent dataset on the enthalpies of formation of different methylated indole derivatives and their hydrogenated counterparts. The results show a namable influence of the number and position of methyl groups on the enthalpy of reaction. The enthalpy of reaction of the overall hydrogenation reaction varies in the range of up to 18.2 kJ·mol−1 (corresponding to 4.6 kJ·mol(H2)−1). The widest range of enthalpy of reaction data for different methyl indoles has been observed for the last step (hydrogenation for the last double bond in the five-membered ring). Here a difference of up to 7.3 kJ·mol(H2)−1 between the highest and the lowest value was found.
“…show that the proposed DLPNO−CCSD(T)-based atom equivalents methodology is more efficient than the G4 method. In our previous studies of amines, amino acids, hydrazines, azides, ureas, nitro compounds, and phenols (see Reference [26] and references therein) it was shown that the G4 method, especially combined with isodesmic reactions, can give reliable theoretical estimates of the gas-phase enthalpies of formation. At the same time, for polycyclic adamantane T A B L E 1 Experimental and theoretical enthalpies of formation (kJ/mol) of adamantane and molecules of norbornadiene cycle we could not get a good agreement with the experiment either for atomization or isodesmic reaction.…”
The DLPNO‐CCSD(T1)/CBS method combined with simple reactions containing small reference species leads to an improvement in the accuracy of theoretically evaluated enthalpies of formation of medium‐sized polyalicyclic hydrocarbons when compared with the widely used composite approach. The efficiency of the DLPNO‐CCSD(T1)/CBS method is most vividly demonstrated by comparing with the results of G4 calculations for adamantane. The most important factor in choosing appropriate working reaction is the same number of species on both sides of the equation. Among these reactions, the reactions with small enthalpy change usually provide a better cancellation of errors. The DLPNO‐CCSD(T1)/CBS method was used to calculate the enthalpies of formation of compounds belonging to the norbornadiene cycle (norbornadiene, quadricyclane, norbornene, nortricyclane, and norbornane). The most reliable experimental enthalpies of formation are recommended for these compounds by comparing calculated values with conflicting experimental data.
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