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Benzene Chemistry Summary - Unit A2 1 - Periodic Trends and Further Organic, Physical and Inorganic Chemistry $5.97
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Benzene Chemistry Summary - Unit A2 1 - Periodic Trends and Further Organic, Physical and Inorganic Chemistry

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  • Course
  • Unit A2 1 - Periodic Trends and Further Organic, Physical and Inorganic Chemistry
  • Institution
  • CCEA

Summary of benzene's shape, bonding, delocalisation, hydrogenation, reaction with bromine water vs alkenes, bond angles and more shown in an organised and logical 2-page explanation.

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Document information

  • July 1, 2024
  • 2
  • 2022/2023
  • Summary

Subjects

  • aromatic chemistry
  • ccea chemistry
  • a level chemistry
  • benzene chemistry
  • benzene
  • electrophile
  • hydrogenation
  • delocalisation

Written for

  • A/AS Level
  • CCEA
  • Chemistry
  • Unit A2 1 - Periodic Trends and Further Organic, Physical and Inorganic Chemistry
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Benzene is a colourless, sweet smelling liquid at room temp.
It is highly flammable. p-orbitals combine
It is carcinogenic.
Shape = hexagonal C C
It is a component of crude oil. planar
Bond angle = 120°
Benzene has the formula C6H 6 C C
It consists of 6 carbons in a hexagonal, planar ring.
Each carbon is bonded to 1 hydrogen.
C C
Each carbon forms 3 covalent bonds, leaving 1 electron that is not
bonded.
This electron is in a p-orbital.
=6 These p-orbitals overlap to form a π delocalised system of electrons above
delocalised and below the plane of the hexagonal ring. This gives benzene its stability.
elctrons All carbon-carbon bond lengths are
Delocalisation def: intermediate in length between that of a
The π electrons are spread over several atoms. BENZENE single C-C and a double C=C.


The delocalisation of π electrons gives benzene greater than expected stability.
Alkenes readily undergo addition reactions whereas benzene doesn’t.
Electrophile - An ion or molecule that
Alkene Benzene Alkenes readily undergo electrophilic attacks regions of high electron density.
Add bromine Electrophilic No reaction addition reactions where Br2 and H2 act
water addition (Remains as electrophiles.
Orange to orange).
colourless

Hydrogenation H adds across Does not easily However, since benzene has a lower electron density because the
double bond - undergo electrons are delocalised they require a more powerful electrophile.
nickel addition This is why benzene will instead undergo electrophilic
catalyst reactions substitution reactions.

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