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I remember Lavelle discussing this, but I can't seem to recall why this is the case.
Bond enthalpies are averages of many bonds.
And I think the bond enthalpies are values under standard conditions, which might not always be the case.
Only diatomic molecules have accurate bond enthalpy measurements, all other molecules' bond enthalpies are taken as averages
While formation enthalpies are very precise, bond enthalpies are calculated as the average of many bonds. Even if you take the bond C-H, there are many different ways it can be formed into in different molecules.
Bond enthalpies are composed of multiple averages and therefore are an overall average. Whereas other values nad methods such as enthalpy of formation are much more accurate.
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