Aromatic Chemistry Flashcards

1
Q

What is benzene’s molecular formula

A

C6H6

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2
Q

Explain benzene structure

A

Six carbon in a hexagonal ring ,with one hydrogen bonded to it

Each C atom is bonded to two other C atoms and one H atom by single covalent σ- bonds

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3
Q

Describe the shape of benzene

A

It is planar
Hexagonal
C-C bonds are equal in length

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4
Q

Describe the nitration reaction of benzene

A

Reagents:concentrated nitric acid
Catalyst:sulfuric acid
Mechanisms:electrophilic substitution
Electrophile:NO2

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5
Q

What is the overall equation for the formation of the electrophile

A

HNO3 + 2H2SO4 —>NO2+ +2H2SO4- + H3O+

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6
Q

What is the by product of the nitration reaction

A

H+

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7
Q

What is the functional group change in friedel crafts acylation

A

Benzene - phenylketone

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8
Q

What are the reagents for friedels crafts acylation

A

Acyl chloride and aluminium chloride catalyst

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9
Q

What is the equation for the formation of the electrophile for friedel crafts

A

AlCl3 + CH3COCl —> [CH3CO]+ + [AlCl4]-

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10
Q

What is the bond angle in benzene

A

120

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11
Q

Describe the delocalisation of benzene ring

A

The six p electrons are delocalised in a ring structure above and below the plane of carbon atoms.

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12
Q

Why is there delocalised electrons

A

Each C atom is bonded to two other C atoms and one H atom by single covalent σ-bonds.

This leaves one unused electron on each C atom in a p orbital, perpendicular to the plane of the ring

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13
Q

How is a pi bond formed

A

Spare electrons in the p orbital overlap

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14
Q

Compare the stability of benzene with cyclohexa-1,3,5- triene

A

Benzene is more stable
Expected hydrogenation of cyclohexantriene is -360
Whilst benezene is -208
Less exothermic by 152 kj

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15
Q

Does cyclone a-1,3 diene have delocalisation

A

Yes it does

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16
Q

Describe delocalisation in cyclohex-1,3-diene

A

The pi binds close together and so overlap
Hydrogenation would be less negative

17
Q

In cyclohexa-1,4-diene is there delocalised

A

No because the pi electrons are too far apart and don’t overlap