In chemistry, bond energy (BE) is one measure of the strength of a chemical bond. It is sometimes called the mean bond, bond enthalpy, average bond enthalpy, or bond strength.[1][2][3] IUPAC defines bond energy as the average value of the gas-phase bond-dissociation energy (usually at a temperature of 298.15 K) for all bonds of the same type within the same chemical species.[1]
The bond dissociation energy (enthalpy)[4] is also referred to as bond disruption energy, bond energy, bond strength, or binding energy (abbreviation: BDE, BE, or D). It is defined as the standard enthalpy change of the following fission: R—X → R + X. The BDE, denoted by Dº(R—X), is usually derived by the thermochemical equation,
This equation tells us that the BDE for a given bond is equal to the energy of the individual components that make up the bond when they are free and unbonded minus the energy of the components when they are bonded together. These energies are given by the enthalpy of formation ΔHfº of the components in each state.
The enthalpy of formation of a large number of atoms, free radicals, ions, clusters and compounds is available from the websites of NIST, NASA, CODATA, and IUPAC. Most authors use the BDE values at 298.15 K.[5]
For example, the carbon–hydrogen bond energy in methane BE(C–H) is the enthalpy change (∆H) of breaking one molecule of methane into a carbon atom and four hydrogen radicals, divided by four. The exact value for a certain pair of bonded elements varies somewhat depending on the specific molecule, so tabulated bond energies are generally averages from a number of selected typical chemical species containing that type of bond.[6]
^ abTreptow, Richard S. (1995). "Bond Energies and Enthalpies: An Often Neglected Difference". Journal of Chemical Education. 72 (6): 497. doi:10.1021/ed072p497.
^Christian, Jerry D. (1973-03-01). "Strength of Chemical Bonds". Journal of Chemical Education. 50 (3): 176. doi:10.1021/ed050p176. hdl:2060/19980004003. ISSN 0021-9584.
^March, Jerry (1985), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure, 3rd edition, New York: Wiley, ISBN 9780471854722, OCLC 642506595
^Haynes, William (2016–2017). CRC Handbook of Chemistry and Physics, 97th Edition (CRC Handbook of Chemistry & Physics) 97th Edition (97th ed.). CRC Press; 97 edition. ISBN 978-1498754286.
^Luo, Yu-Ran and Jin-Pei Cheng "Bond Dissociation Energies". In Lide, David R. (ed) 2017, CRC Handbook of Chemistry and Physics, 97th edition (2016–2017). Boca Raton: Taylor & Francis Group. 9-73.
^IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "Bond energy (mean bond energy)". doi:10.1351/goldbook.B00701
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