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18 Cards in this Set
- Front
- Back
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Describe benzene |
- cyclic planar molecule with a formula of C6H6 - carbon has 4 valent electrons. each carbon is Bonded to 2 other carbons and 1 hydrogen. The final lone electron is in a p orbital which sticks out above and below planar ring - lone electrons in p orbitals combine to form a delocalised ring -due to delocalised structure all c-c bonds are the same length |
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What does kekulè’s structure look like |
Back (Definition) |
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What does the delocalised electron system benzene look like |
Back (Definition) |
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Explain why benzene is more stable than cyclohexane-1,3,5-triene |
More energy required to break bonds in benzene. More stable due to the delocalised electron structure |
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How to name benzenes |
Back (Definition) |
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What reaction do arena undergo |
Electrophilic substitution |
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Why are electrophiles attracted to benzene |
High electron density |
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What are the 2 benzene mechanisms |
Dreidel-crafts acylation Nitration reaction |
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What is friedel-crafts acylation |
Used to add acyl groups to the benzene ring |
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Some electrophiles are positive enough to react, what is added to make the electrophiles stronger |
Halogen carrier (AlCl3) |
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Show have the halogen carrier makes the acyl group (electrophile) stronger |
Back (Definition) |
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Show the friedel-crafts mechanism |
Back (Definition) |
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What’s the final product in this mechanism called |
Phenylketone |
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Why is friedel-crafts acylation used |
The stability of benzene can make is difficult to react |
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Why is nitrating benzene useful |
Allows us to make dyes and explosives |
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How do you form the powerful electrophile for this reaction |
Back (Definition) |
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Show the reaction with a nitronium ion and benzene |
Back (Definition) |
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What molecule does this form |
Nitrobenzene |
