Difference between revisions of "Homolytic Bond Dissociation Energies"
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Homolytic bond dissociation energies or just bond dissociation energies (BDE) is a measure of a particular bond strength. BDE are also referred to as bond enthalpies. | Homolytic bond dissociation energies or just bond dissociation energies (BDE) is a measure of a particular bond strength. BDE are also referred to as bond enthalpies. | ||
| + | ==Example== | ||
For example, the BDE for the C-C bond in | For example, the BDE for the C-C bond in | ||
:H<sub>3</sub>C-CH<sub>3</sub> --> H<sub>3</sub>C• + •CH<sub>3</sub> | :H<sub>3</sub>C-CH<sub>3</sub> --> H<sub>3</sub>C• + •CH<sub>3</sub> | ||
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can be determined using the calculated enthalpies of formation (ΔH<sub>f</sub>) using the following method: | can be determined using the calculated enthalpies of formation (ΔH<sub>f</sub>) using the following method: | ||
| + | ===HF/6-31(G)d=== | ||
Using WebMO/Gaussian to calculate the ΔH<sub>f</sub>(H<sub>3</sub>C-CH<sub>3</sub>), returns the following: | Using WebMO/Gaussian to calculate the ΔH<sub>f</sub>(H<sub>3</sub>C-CH<sub>3</sub>), returns the following: | ||
:[[File:Screen Shot 2021-04-07 at 8.13.05 AM.png|400px]] | :[[File:Screen Shot 2021-04-07 at 8.13.05 AM.png|400px]] | ||
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As can bee seen in this table (shown in all Gen Chem textbooks), the "average bond enthalpy" for a C-C bond is 348 kJ/mol. | As can bee seen in this table (shown in all Gen Chem textbooks), the "average bond enthalpy" for a C-C bond is 348 kJ/mol. | ||
[[File:TB08_004.gif|400px]] | [[File:TB08_004.gif|400px]] | ||
| + | |||
| + | ===B3LYP/6-311+G(2d,p)=== | ||
| + | Using a more accurate computational approach, B3LYP/6-311+G(2d,p): | ||
| + | :- B3LYP Energy -39.8561207613 Hartree | ||
| + | :- B3LYP Energy -79.8583705307 Hartree | ||
| + | ::ΔH<sub>rxn</sub> = 0.14613 Hartree = 384 kJ/mol | ||
| + | |||
| + | |||
| + | ===GGG=== | ||
| + | |||
| + | ===FFF=== | ||
Latest revision as of 15:45, 7 April 2021
Homolytic bond dissociation energies or just bond dissociation energies (BDE) is a measure of a particular bond strength. BDE are also referred to as bond enthalpies.
Example
For example, the BDE for the C-C bond in
- H3C-CH3 --> H3C• + •CH3
can be determined using the calculated enthalpies of formation (ΔHf) using the following method:
HF/6-31(G)d
Using WebMO/Gaussian to calculate the ΔHf(H3C-CH3), returns the following:
The RHF (Restricted HF) energy, ie. ΔHf(H3C-CH3) is reported in units of Hartree, -79.2287548119 Hartree
Using WebMO/Gaussian to calculate the ΔHf(CH3•), returns the following:
The RHF (Restricted HF) energy, ie ΔHf(CH3•) is reported in units of Hartree, -39.5589916118 Hartree
- ΔHrxn = ΔHf(Products) - ΔHf(Reactants)
- ΔHrxn = 2*ΔHf(CH3•) - Hf(H3C-CH3)
- ΔHrxn = 2*-39.5589916118 - (-79.2287548119)
- ΔHrxn = 0.110771588 Hartree = 290.830826448 kJ/mol
- According to Engel, 2nd, Chapter 15, table 15.2, the actual value is 406 kJ/mol)
As can bee seen in this table (shown in all Gen Chem textbooks), the "average bond enthalpy" for a C-C bond is 348 kJ/mol.
B3LYP/6-311+G(2d,p)
Using a more accurate computational approach, B3LYP/6-311+G(2d,p):
- - B3LYP Energy -39.8561207613 Hartree
- - B3LYP Energy -79.8583705307 Hartree
- ΔHrxn = 0.14613 Hartree = 384 kJ/mol