Question 8.77

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Question 8.77

Postby Josephine_Tang_1N » Mon Jan 30, 2017 12:21 am

For this problem, it can be calculated that the energy of the unhybridized carbon bonds = 2880 kJ while the hybridized bonds = 3108 kJ.

Why is the higher energy more stable in this case? Even with consideration that these bonds are the ones formed (therefore negative), the absolute energy is higher which contradicts the idea that lower energy is more stable.

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Re: Question 8.77

Postby Chem_Mod » Mon Jan 30, 2017 11:32 pm

The resonance structure of benzene is generally more stable and less reactive because it has a much higher overall bond enthalpy.

You can think of it more like the energy to break a bond. The more energy it takes to break the bond, the more stable it is. i.e you will need to spend more energy in order to break it to get it to react with another molecule.

Return to “Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)”

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