Resonance energy per ring in benzene, napthalene, anthracene

In summary, the resonance energy per ring increases in the order of benzene < napthalene < anthracene, with anthracene having the highest resonance energy per ring due to its greater stability. The resonance energy per ring can be determined by dividing the molar resonance energy by the number of rings. In the given scenario, napthalene may have a lower resonance energy per ring due to its structure and the logic behind this is yet to be determined through logical guesswork in the absence of provided data.
  • #1
Krushnaraj Pandya
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Homework Statement


Compare resonance energy per ring in benzene, napthalene and anthracene

Homework Equations


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The Attempt at a Solution


I know Resonance energy of benzene is 36 KCal/mol, I also know anthracene is the most stable followed by napthalene so their resonance energy is in the order anthracene>napthalene>benzene but how do I compare it per ring?
 
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  • #2
You can always try to divide molar resonance energy by the number of rings.
 
  • #3
Borek said:
You can always try to divide molar resonance energy by the number of rings.
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 for
 

1. What is resonance energy per ring?

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.

2. How is resonance energy per ring calculated?

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.

3. What is the significance of resonance energy in benzene, naphthalene, and anthracene?

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.

4. Are there differences in resonance energy per ring between benzene, naphthalene, and anthracene?

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.

5. How does the resonance energy per ring affect the physical properties of these molecules?

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.

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