We aren't provided any data in the exam, we just need to find the increasing order of resonance energy per ring through logical guesswork. The logic for napthalene having lower resonance energy per ring is what I'm looking forBorek said:You can always try to divide molar resonance energy by the number of rings.
Resonance energy per ring is a measure of the stability of a molecule due to its delocalized electrons. It is the difference in energy between the actual energy of the molecule and the energy that would be expected if all the atoms were connected by single bonds.
Resonance energy per ring is calculated by subtracting the actual energy of the molecule from the expected energy based on single bonds. This difference is then divided by the number of rings in the molecule to give the resonance energy per ring.
The significance of resonance energy in these molecules is that it contributes to their overall stability. The presence of delocalized electrons in the rings allows for a more stable distribution of charge, making the molecules less reactive and more thermodynamically favorable.
Yes, there are differences in resonance energy per ring between these molecules. Benzene has a resonance energy per ring of 36 kcal/mol, naphthalene has 41 kcal/mol, and anthracene has 45 kcal/mol. This is due to the increasing number of rings and delocalized electrons in each molecule.
The resonance energy per ring contributes to the physical properties of benzene, naphthalene, and anthracene by making them more stable and less reactive. This stability also affects their melting and boiling points, as well as their solubility in different solvents.