Define the terms bond enthalpy and mean bond enthalpy.Use examples to illustrate the difference between the two quantities.

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Define the terms bond enthalpy and mean bond enthalpy.
Use examples to illustrate the difference between the two quantities.

Expert Solution
Step 1

The bond enthalpy of a chemical bond can be defined as the total amount of energy required to break 1 mole of that chemical bond. For example, the bond enthalpy of the oxygen-hydrogen single bond is equal to 463 kJ/mol. This implies that a total of 463 kilojoules of energy is required to break 1 mole of hydrogen-oxygen single bonds.

Step 2

To express the strength of a single, specific bond in a molecule, the quantity ‘mean bond enthalpy’ or ‘average bond enthalpy’ can be used. The mean bond energy of a chemical bond (in a molecule) can be determined by calculating the average value of all the bond dissociation energies of that type of bond in the molecule.

If a molecule has several bonds, bond enthalpy is calculated for each bond and the average value has been considered. For example, methane (CH4) has four C-H bonds, and the average bond energy is +1652 kJ and +415.5kJ per mole of the bond.

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