Heat Capacity and Bond Dissociation Energy Calculations of Some Fluorinated Ethanol’s and its Radicals: CH_3-xCH₂F_xOH, CH₃CH_2-xF_xOH

Hebah M. Abdel-Wahab, Joseph W. Bozzelli

Department of Chemistry and Environmental Science, New Jersey Institute of Technology, Newark, New Jersey, USA.

DOI: 10.4236/ojpc.2021.112002                

Abstract

Structures and thermochemical properties of these species were determined by the gaussian M-062x/6-31 + g (d, p) calculation enthalpies of formation for 19 fluorinated ethanol and some radicals were calculated with a popular Ab initio and density functional theory methods: The gaussian M-062x/6-31 + g (d, p) via several series of isodesmic reactions. Entropies (S298°K in Cal·Mol^-1 K^-1) were estimated using the M-062x/6-31 + g (d, p) computed frequencies and geometries. Contributions of entropy, S298°K, and heat capacities, Cp(T) due to vibration, translation, and external rotation of the molecules were calculated based on the vibration frequencies and structures obtained from the M-062x/6-31 + g (d, p) Density Functional Method. Potential barriers are calculated using M-062x/6-31 + g (d, p) density functional method and are used to calculate rotor contributions to entropy and heat capacity using integration over energy levels of rotational potential. Rotational barriers were determined and hindered internal rotational contributions for S298° - 1500°K, and Cp (T) were calculated using the rigid rotor harmonic oscillator approximation, with direct integration over energy levels of the intramolecular rotation potential energy curves. Thermochemical properties of fluorinated alcohols are needed for understanding their stability and reactions in the environment and in thermal process

Keywords

Thermo-Chemistry, Enthalpy, Fluorinated Ethanol’s, Thermochemical Properties

1. Introduction

Fluorinated hydrocarbons are used as refrigerants, in polymers, heat exchange fluids, and as solvents. They are present in the atmosphere, lithosphere, and hydrosphere. Because of their less adverse effects on the stratospheric ozone layer, they are used in place of greenhouse gases [1]. Fluorinated hydrocarbons exist as compounds ranging from pure to oxidized intermediates resulting from oxidation in the environment. In order to study their reactivity in biological systems, lifetimes, and in the environment, it’s critical to understand the chemical and thermodynamic properties of fluorocarbons and their breakdown intermediates.

The thermochemistry of fluorinated alcohols with one carbon atom was studied in the past and is in the literature [2]. In 2016, Hang Wang studied thermodynamic properties of fluorinated methanol using CBS-QB3, M06, M06-2X, WB97X, W1U, B3LYP, CBS-APNO and G4 Calculations. Small standard deviation suggests good error cancellation of work reactions and accuracy. M06-2x/6-31 + g (d, p) calculation had small values for standard deviations. It is an accurate method to calculate Enthalpy of fluorinated alcohols. It shows the second smallest standard deviation after CBS-QB3 method of calculation.

Halogenated compounds are highly stable, have low reactivity and are valued chemicals in industry [3]. Due to its widespread use and their persistence in the environment, they are of concern to the environment. In order to understand the oxidation and reduction reactions involving such molecules, their thermochemical properties must be studied [3].

1.1. Isodesmic and Isogyric Reaction

The enthalpy of formation of mono and di fluorinated ethanol’s and its radicals has been calculated using Gaussian M-062x/6-31 + g (d, p) method of calculation. In order to calculate the enthalpy of formation of fluorinated ethanols using this method, we use the calculated enthalpies of formation in work reactions along with reference species.

The number of each type of bond must be conserved in the isodesmic reactions in order to cancel any systematic error in the molecular orbital calculations using this method. Calculations of enthalpies of formation are allowed to accuracies close to experimental values by the careful choice of the isodesmic reactions [2]. Standard enthalpy of formation for the reference species used in the isodesmic work reactions along with their uncertainties is listed in Table 1. Taking 1-fluoroethanol as an example, two isodesmic reactions (Table 2) are selected to determine the Δ_fH^˚_(298˚K) of the target molecule, 1-fluoroethanol. Since the Δ_fH^˚_(298˚K) values of all species but 1-fluoroethanol in 1 - 2 (Table 2) are known, the Δ_fH^˚_(298˚K) of the target species 1-fluoroethanol is obtained from this data and the calculated Δ_rxnH^˚_(298˚K). Δ_fH^˚_(298˚K) calculated using two different reference molecules are within ±2 Kcal∙mol⁻¹.

1.2. Reference Species

Standard enthalpy of formation for the reference species used in the isodesmic work reactions along with their uncertainties is listed in Table 1. Table 2 provides one example on the method of Isodesmic Work Reactions used for the

Table 1. Reference Species in the Isodesmic Reactions Standard Enthalpy of Formation Values (kcal∙mol⁻¹) [4].

^aWang [2], ^bWang [4], ^cRuscic [5], ^dBurke [6], ^eChase [7], ^fLuo [8], ^gBodi [9], ^hPedley, ⁱATcT Tables [10], ^hCsontos [11]. ^jThe value we used in this study [4]

Table 2. Example for Enthalpy of Formation Calculations for 1-fluoroethanol using Isodesmic Reactions; using different reference molecules, Units in kcal∙mol⁻¹.

^aHartrees, kcal∙mol⁻¹; *SD Standard Deviation kcal∙mol⁻¹ Errors reported avg of sum of uncertainties in rxn’s reference species.

calculation of the Standard Enthalpy of Formation Δ_fH^˚_(298˚K) for the fluoroethanols.

1.3. Computational Method

Composite calculations and series of Isodesmic Reactions are used to calculate enthalpy of formation of fluorinated ethanols. All calculations are performed using the Gaussian 16 program. The DFT method M06-2x is used to initially analyze optimized structures, frequencies, thermo energies and internal rotors of the molecules studied. It’s a Global-hybrid meta-GGA density functional approximation, GGA, generalized gradient approximation, in which the density functional depends on the up and down spin densities and their reduced gradient, meta GGA, in which the functional also depends on the up and down spin kinetic energy densities, hybrid GGA, a combination of GGA with Hartree-Fock exchange, hybrid meta GGA, a combination of meta GGA with Hartree-Fock exchange [12]. All reported values are for standard state of 298 K and 1 atm. We continue the calculation of fluorinated alcohols in this study with this method, because the M-062x/6-31 + g (d, p) level of calculation have been applied to fluoro hydrocarbons 6 with small reported standard deviations values.

2. Results and Discussion

2.1. Entropy and Heat Capacity Values

Internal rotor contributions to calculated entropy and heat capacity at 298 - 1500 K were determined using the molecular mass of each molecule, number of optical isomers, symmetry of the molecule, electron degeneracy, moment of inertia, and vibrational frequencies values (Table3). The vibrational frequencies for the calculation of heat capacity and entropy at the M-062x/6-31 + g (d, p) level of calculation was scaled by a factor of 0.97 [13]. The moment of inertia values is shown in the Supplemental Information Tableprovided. To calculate the contributions of external rotor, vibration and transition to the calculated entropy and heat capacity, the “SMCPS” [14] program is used. It employs the rigid-rotor harmonic oscillator approximation using moment of inertia from optimized structure and frequencies. The “Rotator” [15] program by Lay et al. [16] is used to calculate internal rotor contributions from the corresponding internal rotor torsion frequencies. In this paper, a torsional potential curve presenting a ten-parameter Fourier series function is used to calculate the contribution of internal rotor. Parameters and detailed functions are shown in the Supplemental Information Tableprovided. Rotor [16] program is used to calculate thermodynamic functions from hindered rotations with arbitrary potentials.

Calculation of the Hamiltonian matrix of the internal rotor, and subsequent calculation of energy levels by direct diagonalization of the matrix are employed by this technique. Rotational barriers versus dihedral angle are presented as a potential curve. In this paper, the calculated torsional potential at discrete torsional angles.

$V\left(\Phi \right)=a_0+{\displaystyle \sum a_i\cos \left(i\Phi \right)}+{\displaystyle \sum b_j\cos \left(j\Phi \right)}i,j=1-10$ (1)

The coefficients $a_i$ and $b_j$ are calculated to present the maxima and minima of the torsional potentials with a possibility to shift from the extreme angular positions.

Table 3. Monofluoro and Difluoro-Ethanol’s Ideal Gas phase Entropy and Heat Capacity obtained using M-062x/6-31 + g (d, p) level of theory (Cal∙mol⁻¹∙K⁻¹).

Calculations of heat capacity and standard entropy based on benchmark database and the computational chemistry comparison for the M-062x/6-31 + g (d, p) calculation method, the vibrational frequencies were scaled by a factor of 0.987 [13]. Potential Energy profiles for mono and di fluorinated ethanol and their related radicals are listed in the Supplemental Information Tableprovided., the solid lines are the fit of Fourier series expansion, rotator contribution for barriers below 7 kcal∙mol⁻¹ were added to the SMCPS calculated entropy and heat capacity. Energies are in kcal∙mol⁻¹ (Table3).

2.2. Standard Enthalpy Values

Enthalpies of formation were determined from isodesmic work reactions from M-062x/6-31 + g (d, p) method of calculation. The standard enthalpy of formation for the reference species along with their uncertainties, which are used the isodesmic work reactions, Table 4, are listed in Table 1 in kcal∙mol⁻¹. The standard deviation was calculated [17] for all Enthalpies of formation values for all 19 fluorinated ethanol and is included in Table 4. Details of the method of

Table 4. Standard Enthalpy of Formation using isodesmic reactions: Monofluoro and Difluoro-Ethanols using the M06-2x/6-31 + g (d, p) Level of Theory. Errors reported as sum of avg uncertainty in rxn’s reference species.

Hartrees, kcal∙mole⁻¹ *SD Standard Deviation kcal∙mol⁻¹ Errors reported avg of sum of uncertainties in rxn’s reference species.

standard deviation [19] and example calculation(s) are shown in the Supplemental Information table provided. The bond dissociation energy (BDE’s) of Monofluoro and Difluoro-Ethanol’s are also calculated in Table 5 with a small percent error, ranging from 0.2 - 0.8 Kcal/mol. A small value for percent error indicates accurate calculated values for BDB of these molecules.

2.3. Bond Energies

*Supplemental Information

Supplemental Information is available, Cartesian Coordinates; Z-matrixes, vibration frequencies, moments of inertia, the method of standard deviation, Optimized Geometries, and C-C and C-O internal rotors potential energy profile for target fluorinated ethanol and their related radicals are included.

Table 5. Bond Dissociation Energy (BDE’s) of Monofluoro and Difluoro-Ethanol’s.

3. Conclusions

Thermodynamic properties of 19 mono and di-fluoro ethanols and their related radicals are calculated using the abinitio and Global-hybrid meta-GGA density function methods. Isodesmic work reactions are employed for cancellation of calculation errors. Multiple work reactions are utilized to calculate standard enthalpy of formation at the Gaussian M06-2X calculation level. Optimized geometries and frequencies are used to determine entropy and heat capacity with M06-2x/6-31 + g (d, p) level of calculation. Intermolecular torsion potential curves at the M-06-2x/6-31 + g (d, p) level of calculation are used to calculate hindered internal rotation contributions to heat capacity and entropy with a correction to the calculated heat capacity and entropy. The Thermochemical properties: Entropy, Heat Capacities at (298˚ - 1500˚K), Standard Enthalpy of formation (298K), and the C—F and C—H Bond Dissociation Energies (BDEs) for Mono and Difluorinated Ethanols and Radicals: CH_3−xCHF_xOH, CH₃CH_2-xF_xOH have been calculated. The C-H bond energies range from 102.2 to 107.2 Kcal∙mol⁻¹ on the methyl carbons, and from 97.3 to 105.2 Kcal∙mol⁻¹ on the secondary ethyl carbons. The calculated values for C-H bond energies for fluorinated methyl carbons are higher than those of the fluorinated ethyl carbons. Calculated values for the O-H bond energies for 2-fluoroethanol are higher than those of O-H bond energies for 1-fluoroethanol and an intermediate calculated value for O-H bond energies for 1,2-difluoroethanol. Introducing a fluorine atom to either methyl or ethyl carbon increases O-H bond energy [18].

Acknowledgements

We acknowledge the NJIT Advanced Research Computing Services for significant help in providing the computer calculation software.

Supplemental Information

Table S1. Cartesian Coordinates in Angstroms for target fluorinated ethanol and their related radical’s geometries at the m062x/6-31 + g (d, p) level of theory.

Table S2. Frequencies for target fluorinated ethanol and their related radicals at the m062x/6-31 + g (d, p) level of theory (cm⁻¹).

Table S3. Moment of inertia for target fluorinated ethanol and their related radicals at the m062x/6-31 + g (d, p) level of theory (GHZ).

Optimized Geometries for target fluorinated ethanol and their related radicals at the m062x/6-31 + g (d, p) level of theory

Figure S1. Optimized Geometry for CH2FCH2OH at the m062x/6-31 + g (d, p) level of theory.

Figure S2. Optimized Geometry for CH₃CHFOH at the m062x/6-31 + g (d, p) level of theory.

Figure S3. Optimized Geometry for C•HFCH₂OH at the m062x/6-31 + g (d, p) level of theory.

Figure S4. Optimized Geometry for CH₂FCH•OH at the m062x/6-31 + g (d, p) level of theory.

Figure S5. Optimized Geometry for CH₂FCH₂O• at the m062x/6-31 + g (d, p) level of theory.

Figure S6. Optimized Geometry for CH₂•CHFOH at the m062x/6-31 + g (d, p) level of theory.

Figure S7. Optimized Geometry for CH₃CF•OH at the m062x/6-31 + g (d, p) level of theory.

Figure S8. Optimized Geometry for CH₃CHFO• at the m062x/6-31 + g (d, p) level of theory.

Figure S9. Optimized Geometry for CH₂FCHFOH at the m062x/6-31 + g (d, p) level of theory.

Figure S10. Optimized Geometry for CF₂HCH₂OH at the m062x/6-31 + g (d, p) level of theory.

Figure S11. Optimized Geometry for CH₃CF₂OH at the m062x/6-31 + g (d, p) level of theory.

Figure S12. Optimized Geometry for C•HFCFHOH at the m062x/6-31 + g (d, p) level of theory.

Figure S13. Optimized Geometry for CH₂FC•FOH at the m062x/6-31 + g (d, p) level of theory.

Figure S14. Optimized Geometry for C•F₂CH₂OH at the m062x/6-31 + g (d, p) level of theory.

Figure S15. Optimized Geometry for CHF₂C•HOH at the m062x/6-31 + g (d, p) level of theory.

Figure S16. Optimized Geometry for CHF₂CH₂O• at the m062x/6-31 + g (d, p) level of theory.

Figure S17. Optimized Geometry for CH₂•CF₂OH at the m062x/6-31 + g (d, p) level of theory.

Figure S18. Optimized Geometry for CH₃CF₂O• at the m062x/6-31 + g (d, p) level of theory.

Figure S19. Potential energy profile of C-C and C-O internal rotors for CH₂FCH₂OH. The solid lines indicate Fourier series expansion.

Figure S20. Potential energy profile of C-C and C-O internal rotors for CH₃CHFOH. The solid lines indicate Fourier series expansion.

Figure S21. Potential energy profile of C-C and C-O internal rotors for C•HFCH₂OH. The solid lines indicate Fourier series expansion.

Figure S22. Potential energy profile of C-C and C-O internal rotors for CH₂FCH•OH. The solid lines indicate Fourier series expansion.

Figure S23. Potential energy profile of C-C and C-O internal rotors for CH₂FCH₂O•. The solid lines indicate Fourier series expansion.

Figure S24. Potential energy profile of C-C and C-O internal rotors for CH₂•CHFOH. The solid lines indicate Fourier series expansion.

Figure S25. Potential energy profile of C-C and C-O internal rotors for CH₃CF•OH.The solid lines indicate Fourier series expansion.

Figure S26. Potential energy profile of C-C and C-O internal rotors for CH₃CHFO•.The solid lines indicate Fourier series expansion.

Figure S27. Potential energy profile of C-C and C-O internal rotors for CH₂FCHFOH. The solid lines indicate Fourier series expansion.

Figure S28. Potential energy profile of C-C and C-O internal rotors for CF₂HCH₂OH. The solid lines indicate Fourier series expansion.

Figure S29. Potential energy profile of C-C and C-O internal rotors for CH₃CF₂OH. The solid lines indicate Fourier series expansion.

Figure S30. Potential energy profile of C-C and C-O internal rotors for CH₂FC•FOH. The solid lines indicate Fourier series expansion.

Figure S31. Potential energy profile of C-C and C-O internal rotors for C•HFCFHOH. The solid lines indicate Fourier series expansion.

Figure S32. Potential energy profile of C-C and C-O internal rotors for CH₂FCHFO•. The solid lines indicate Fourier series expansion.

Figure S33. Potential energy profile of C-C and C-O internal rotors for CHF₂C•HOH. The solid lines indicate Fourier series expansion.

Figure S34. Potential energy profile of C-C and C-O internal rotors for C•F₂CH₂OH. The solid lines indicate Fourier series expansion.

Figure S35. Potential energy profile of C-C and C-O internal rotors for CHF₂CH₂O•. The solid lines indicate Fourier series expansion.

Figure S36. Potential energy profile of C-C and C-O internal rotors for CH₂•CF₂OH. The solid lines indicate Fourier series expansion.

Figure S37. Potential energy profile of C-C and C-O internal rotors for CH₃CF₂O•. The solid lines indicate Fourier series expansion.

Table S4. The method of standard deviation and example calculation.

Conflicts of Interest

The authors declare no conflicts of interest regarding the publication of this paper.

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