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For all molecules that are not diatomic, their bond enthalpies are averages from the bonds in many different molecules. For example many molecules can have a C-H bond, and the bond enthalpies of each one is different.
Because they are not tailor-made to every type of bond in every molecule, they are an average of the energy required to break bonds across many different molecules. For example, the O-H bond in CCl3COOH is different than the O-H bond in CCH3COOH because we know that the Cl pulls electrons more than H and results in a weaker O-H bond. However, we use only one value for O-H bonds when referring to bond enthalpy. Examples such as this result in inaccuracies.
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