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Summary A Level Chemistry- Organic- Aromatic Chemistry- Bonding £3.49
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  7. Unit 3.3.10 - Aromatic chemistry

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Summary A Level Chemistry- Organic- Aromatic Chemistry- Bonding
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Master A Level Chemistry's aromatic chemistry with exam-style summary notes. Covers benzenes and essential Q&A. Boost understanding and confidence in aromatic compounds and reactions. Simplify revision and strengthen knowledge with concise notes

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  • June 16, 2023
  • 6
  • 2020/2021
  • Summary

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Bonding
3.3.10.1:

The nature of the bonding in a benzene ring, limited to planar structure and bond
length intermediate between single and double

Delocalisation of p electrons makes benzene more stable than the theoretical
molecule cyclohexa-1,3,5-triene

Students should be able to:

use thermochemical evidence from enthalpies of hydrogenation to account for
this extra stability

explain why substitution reactions occur in preference to addition reactions



What is benzene’s formula and structure?

C6H6




What is another name for arenes? Why did this come about?

Aromatic compounds, as first found in sweet-smelling dyes

Dangers of benzene? (why it is not used in schools)

It is a carcinogen

What is the shape of benzene?




Bonding 1

, Flat, regular hexagon

Bond angle = 120*

Describe the bonding in benzene

there are sigma bonds between each C-C bond

this creates a planar shape with bond angle of 120* with the hydrogens




there are also pi-bonds due to the delocalised electrons in the delocalised pi-
system, making benzene stable

What happens to the 4th electron in the p orbital of each C atom in benzene?

It delocalises to form rings of electron density above & below the hexagon,
forming rings of delocalised electron density above/below the hexagon

forms a delocalised pi system

What is the effect on benzene’s stability of the rings of electron density?

Makes benzene very stable



Bonding 2

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