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Organic Chemistry Unit 14B £6.79
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Organic Chemistry Unit 14B
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Organic chemistry this assignment covers the criteria from a Pass to Distinction. This is in BTEC Applied Science level 3 - My assignment was awarded Distinction, evidence can be provided if required... Any queries please do not hesitate to contact :)

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  • June 21, 2022
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  • 2021/2022
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Unit 14 B: Benzene containing molecules- aromatic chemistry

PASS – structure and uses of benzene and its compounds

Explain what adding bromine water shows about the structure of benzene.

Benzene should react with bromine when added and if it does it is an alkene,
however, this does not happen as it is a colourless solution. Therefore,
concluding that it is not an alkene.

Explain what bond length data shows about the structure of benzene.

Benzene has a regular hexagon structure inferring that it has specialised bonds
meaning that if it had double and single bond it would be irregular.

Name the two scanning methods that were used to study benzene more
closely and what these scans showed about the structure of benzene.

X – ray crystallography showed that there are no standard single or double
carbon -carbon bonds, inferring that the bonds are all the same and is unique to
benzene.

Scanning Tunnelling Microscopy (STM) – The image illustrated that benzene has
an undistorted hexagonal shape and has a bond angle of 120o.


Explain what infrared spectroscopy shows about the structure of benzene.

Infrared spectroscopy portrays the bonds by their absorption. The is no
stretch in benzene which overall means that it does not have double bonds.

Explain what energy studies show about the structure of benzene.

Theoretical has a higher energy output compared to the experimental structure.
Therefore, Benzene is more stable than the double bond model, as it only gives
off a smaller amount of energy.

, Class notes, K. Kaur – 20/02/22

Using referenced images to help, explain the bonding in benzene including
sigma bonding and the pi ring structure.




Socratic.org. (n.d.) – 24/02/2022

Benzene uses carbon bonds which entail of 2s and 2p orbitals. The 1s and 2p
orbitals join to form three hybrid orbitals named sp2 hybrids and overall, have
equal energy.

Benzene has sp2 hybridisation and then has three sp2 hybrids per carbon atom,
which forms single bonds. The P orbitals are blended and merged to form a Pi
ring which overall, creates a high level of stability, and so it has an unreactive
structure.

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