So bond energy is the same bond enthalpy, which means the amount of energy needed to break the bond. Based on this definition, you would need to put in more energy to break the bonds of cyclohexane than cyclopropane due to the increased stability of cyclohexane, correct?

 

From a combustion rxn, which would yield more energy: cyclopropane or cyclohexane? I would think cyclopropane due to the high ring strain within the molecule.

 

 

Yes and yes.

Yes and yes seems a good reply

 

Here's a link to (Google books) a table that has the actual heat of combustion per CH₂ of cyclopropane, cyclohexane, as well as a few more rings.