Calorimetric and infrared study of methyl iodide and some monosubstituted butyl halides. Does methyl iodide form hydrogen bonds as a proton donor?

Borisover, Mikhail; Stolov, Andrei A.; Baitalov, Felix D.; Морозов, А. И.; Solomonov, Boris N.

doi:10.1016/0040-6031(96)02908-5

Cited by 11 publications

(3 citation statements)

References 18 publications

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“…The detailed technique for the determination of the solution enthalpies can be found elsewhere. 12,90 The volume of the calorimetric cell was 100 ml. The final solute concentration did not exceed 0.03 mol l À1 .…”

Section: Methodsmentioning

confidence: 99%

A new method for the extraction of specific interaction enthalpy from the enthalpy of solvation

Solomonov¹,

Novikov²,

Varfolomeev³

et al. 2004

J of Physical Organic Chem

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A new, simple method for the extraction of specific interaction enthalpy from the enthalpy of solvation is proposed. It is based on empirical but very general relationships describing the non-specific solvation enthalpy. The specific interaction enthalpy is calculated from the solution enthalpies in the solvent under consideration, cyclohexane and tetrachloromethane. The solution enthalpy of at least one linear alkane in the solvent must also be available. The solution enthalpies of a 'model compound' or homomorph are not required. This method is applicable not only for proton-donor solutes but also for acceptor solutes such as iodine. It can be used also for solvents associated by hydrogen bonding (e.g. alcohols). The enthalpies of specific interaction for 280 solute-solvent systems were calculated. Solution enthalpy data were mainly obtained from the literature and partially measured by the authors. The results were compared with literature data on complexation enthalpy.

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Section: Methodsmentioning

confidence: 99%

A new method for the extraction of specific interaction enthalpy from the enthalpy of solvation

Solomonov¹,

Novikov²,

Varfolomeev³

et al. 2004

J of Physical Organic Chem

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“…The technique for the determination of these values was described in more detail earlier. 24,25 Concentrations of solutes did not exceed 0.01 M for alcohols and 0.02 M for others. The absence of a concentration dependence of the heat effects was used as a criterion for infinite dilution conditions.…”

Section: Calorimetrymentioning

confidence: 93%

A new method for the determination of cooperative hydrogen bonding enthalpy of proton acceptors with associated species of alcohols

Solomonov

Varfolomeev

Novikov

2006

J of Physical Organic Chem

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A calorimetric method for the determination of cooperative hydrogen bonding (HB) enthalpy of proton acceptors (B) with associated species of alcohols is proposed. The average enthalpy of cooperative HB of pyridine with associated species of alcohols was found to be À19.8 AE 0.6 kJ mol À1 for all alcohols investigated. This value exceeds the enthalpy of HB in the complex ROH . . . NC 5 H 5 (the average for all alcohols is À15.8 AE 0.2 kJ mol À1 ) by 20-30%. Cooperativity factors (A b , A Ox ) of hydrogen bonds for (ROH) 2 . . . NC 5 H 5 complexes were determined using the IR-spectroscopic method. The average values for the alcohols under consideration were found to be A b ¼ 1.41 AE 0.04 and A Ox ¼ 1.54 AE 0.05. On the basis of IR-spectroscopic and calorimetric data, the enthalpy of cooperative interactions of pyridine with the dimer (ROH) 2 was estimated. This value for all the alcohols studied is, on average, À20.9 AE 0.1 kJ mol À1 .

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“…The technique for the determination of the heat effects was described in more detail earlier. 23,38 The volume of the calorimetric cell was 100 ml. The final solute concentration did not exceed 0.03 mol 1…”

Section: Methodsmentioning

confidence: 99%

Solvent effects on infrared spectroscopic and calorimetric characteristics of aliphatic ketones in binary solvent mixtures

Novikov

Stolov

Gorbatchuk

et al. 1998

J. Phys. Org. Chem.

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Solution enthalpies of n-hexane, acetone, butan-2-one and octan-2-one in a series of tetrachloromethane-acetonitrile mixtures and the carbonyl stretching absorption frequencies in the IR spectra of these ketones were determined. It was found that over the whole range of concentrations (varying from neat tetrachloromethane up to neat acetonitrile) the solvation enthalpy of these compounds can be obtained additively from the contributions of the alkyl and carbonyl fragments. The solvent effect on the solvation enthalpy of the carbonyl group was found to be satisfactorily correlated with the corresponding IR frequency shifts of the C=O group. It was also found that the sensitivities of the carbonyl IR frequencies to the solvent composition are different for various ketones. From both IR and calorimetric data, the preferential solvation parameters were evaluated. The differences between the IR spectroscopic and calorimetric data are discussed.

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Calorimetric and infrared study of methyl iodide and some monosubstituted butyl halides. Does methyl iodide form hydrogen bonds as a proton donor?

Cited by 11 publications

References 18 publications

A new method for the extraction of specific interaction enthalpy from the enthalpy of solvation

A new method for the extraction of specific interaction enthalpy from the enthalpy of solvation

A new method for the determination of cooperative hydrogen bonding enthalpy of proton acceptors with associated species of alcohols

Solvent effects on infrared spectroscopic and calorimetric characteristics of aliphatic ketones in binary solvent mixtures

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