Aromatic Hydrocarbons: Videos & Practice Problems

Determine whether the ion given below is aromatic, antiaromatic, or nonaromatic. If the ion is aromatic/antiaromatic, calculate the n in the Hückel's/Breslow's rule. If it is nonaromatic, justify your answer using the rules of aromaticity.

Specify whether the ion below is aromatic, nonaromatic, or antiaromatic. If the ion is aromatic/antiaromatic, determine the value of n in Hückel's/Breslow's rule. If the ion is nonaromatic, explain your answer using the rules of aromaticity.

Using the rules of aromaticity, classify the given ion below as aromatic, antiaromatic, or nonaromatic. If classified as aromatic/antiaromatic, determine the value of n in Hückel's/Breslow's rule. If classified as nonaromatic, provide an explanation.

Is the anion below nonaromatic, antiaromatic, or aromatic? If it is aromatic, what is its n in Hückel's rule? If not, explain the aromaticity rule it breaks.

Determine if the cation below is aromatic, antiaromatic, or nonaromatic. If it is aromatic, determine its n in Hückel's rule. If not, explain how it breaks the aromaticity rule.

Is the given molecule antiaromatic, aromatic, or nonaromatic? If it is aromatic, what is its n in Hückel's rule? If not, why does it break the aromaticity rule?

Which of these are aromatic structures?

Which of these are aromatic structures?

Identify each of the compounds shown below as nonaromatic, antiaromatic, or aromatic. Provide a brief explanation for your answer.

In the given ion pair, determine which is more stable.

Categorize each of the given species as aromatic, antiaromatic, or nonaromatic. For those classified as aromatic or antiaromatic, specify the number of delocalized π electrons in the cyclic system.

Classify each of the following species as aromatic, antiaromatic, or nonaromatic. For those classified as aromatic or antiaromatic, specify the number of delocalized π electrons in the cyclic system.

Among the three given compounds, one exhibits significantly greater stability compared to the others. Categorize each of these molecules as aromatic, antiaromatic, or nonaromatic.

The following pair of ions are given. Determine which is more stable.

We are given the following ion pair. Determine which is more stable.

When we are given the following pair of molecules, determine which is more stable.

The structure of p-triphenyl is illustrated below.

(i) Is it acceptable to classify p-triphenyl as a fused polynuclear aromatic hydrocarbon?

(ii) Count the number of pi electrons in p-triphenyl. How does this number compare to naphthalene's?

Shown below is the structure of p-triphenyl.

(i) If the heat of hydrogenation for p-triphenyl is 630 kJ/mol, and the heat of hydrogenation for an isolated alkene is 120 kJ/mol, determine the resonance energy of p-triphenyl.
(ii) Compare the resonance energy of p-triphenyl with that of three benzene rings and with that of naphthalene. Explain the difference in the resonance energies of p-triphenyl and naphthalene.
(The resonance energy of benzene and naphthalene is 150 kJ/mol and 252 kJ/mol, respectively.)

The compounds listed below are not aromatic compounds. Provide the reaction needed to transform them into aromatic compounds.

Identify whether the following compounds exhibit aromatic characteristics or not. If the compound is aromatic, explain why it is aromatic.