Structure and Bonding - Aromatic Chemistry

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What type of hybridization is observed in the carbon atoms of a benzene molecule?

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sp hybridised

sp³ hybridised

d²sp³ hybridised

sp² hybridised

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Benzene's structure can be accurately represented by a single Lewis structure.

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True

False

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Which statement best describes the electron configuration in benzene?

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The π-electrons are localized between individual carbon atoms.

The π-electrons are delocalized over all six carbon atoms.

Benzene has alternating single and triple bonds in its stable form.

The π-electrons are free and do not contribute to benzene’s stability.

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Fill in the Blank.
The resonance in benzene leads to ____________________ bond lengths between carbon atoms, which are shorter than single bonds but longer than double bonds.

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Why does benzene undergo electrophilic aromatic substitution reactions rather than addition reactions under normal conditions?

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Because benzene is fully saturated and cannot accommodate more hydrogen atoms.

Because the addition reactions would disrupt the delocalized π-electron system, reducing the molecule's stability.

Because benzene lacks π-electrons necessary for addition reactions.

Because the carbon-carbon bonds in benzene are too strong to be broken by electrophiles.

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What is the role of the delocalized π-electrons in the stability of benzene?

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They increase the reactivity of benzene with nucleophiles.

They reduce the overall energy of the molecule, making it more stable.

They are responsible for the high polarity of benzene.

They decrease the melting point of benzene.

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