Phenol Flashcards

1
Q

What is a phenol?

A

Contain a OH group bonded directly to a benzene ring

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2
Q

Bond angles and shapes in phenol

A

120 degrees in benzene ring (each carbon forms 3 bonds) so trigonal planar
104.5 degrees in O-H bond, oxygen has 2 lone pairs of electrons and forms 2 bonds so bent

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3
Q

Pi system in benzene ring of phenol

A

Each C atom is bonded to 2 C atoms and one H atom by
single covalent σ-bonds
Leaves one unused electron on each C atom in a p orbital, perpendicular to the plane of the ring.
The Six p electrons are delocalised in a ring structure above and below the plane of carbon atoms

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4
Q

What happens to lone pair of electrons in oxygen? (NOT DISSOCIATION)

A

Delocalised into the benzene ring due to overlap between:
pi bond perpendicular to plane in oxygen
ring of delocalised electrons in benzene
Above and below the plane of benzene

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5
Q

Why do phenols attract electrophiles more than benzene

A

Because lone pair of electrons in oxygen delocalised into pi system, this increases electron density above and below plan (higher electron density than benzene)
So attracts electron pair acceptors MORE

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6
Q

Why can phenols dissociate?

A

Because the lone pair of electrons on the oxygen atom are withdrawn into pi system due to overlap of p orbitals of oxygen atom with pi system
Which withdraws electron density in O-Hbond making it weaker and easier to break

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7
Q

What do phenols dissociate into?

A

Phenoxide anion
H+

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8
Q

Phenoxide anion

A

Benzene ring bonded to an oxygen anion because the O-H bond broke so electrons in this bonded was donated to oxygen atom
= -1 charged

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9
Q

How can phenols act as weak acids?

A

Because they dissociate so O-H bond breaks and the H+ ion can be donated
= acts as acid

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10
Q

What does the OH group do in phenol?

A

Activates the benzene ring

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11
Q

Does phenol require a halogen carrier catalyst to react with halogen?

A

No because unlike benzene, it has more attraction to electrophile

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12
Q

Is phenol soluble in water?

A

A small bit in cold water because despite having OH group that can form H bonds to water, non polar aromatic ring interferes with H bonding

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13
Q

Halogenation of phenol example

A

Phenol+ bromine water makes 2,4,6-tribromophenol

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14
Q

2,4,6-tribromophenol appearance

A

White precipitate that is insoluble in water

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15
Q

Observation for phenol+ bromine water

A

Forms a white precipitate + decolourises orange bromine water to colourless

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16
Q

Can halogenation of phenol happen with chlorine?

17
Q

Conditions for halogenation of phenol

A

At standard room temperature and pressure

18
Q

Why does phenol only require standard conditions + no catalyst needed for halogenation?

A

Because OH group activates the ring to attract electrophiles more strongly so hs a lower activation energy for reaction to occur

19
Q

Phenol + concentrated nitric acid products

A

2,4,6-trinitrophenol

20
Q

Can Phenol + concentrated nitric acid occur at standard conditions? WHy?

A

Yes because the OH group activates BENZENE RING to attract electrophiles (NO2+) more strongly

21
Q

Can phenol react with dilute nitric acid?

A

Yes to give 2-nitrophenol and 4-nitrophenol

22
Q

Why can phenol react with dilute nitric acid?

A

Because the OH group activates BENZENE RING to attract electrophiles (NO2+) more strongly

23
Q

Are phenols weaker acids than carboxylic acids?

24
Q

Can phenol react with hydroxide base?

A

Yes to give phenoxide salt (phenoxide anion- metal cation+)
And water

25
Q

Can phenol react with metal?

A

Yes to give phenoxide salt (phenoxide anion- metal cation+)
AND HYDROGEN GAS

26
Q

Is phenoxide salt soluble?

A

Yes more so than phenol so will dissolve on addition of hydroxide solution
Forms ion dipole interactions with water which is stronger than H bonds

27
Q

How to differentiate phenol from carboxylic acid

A

React with sodium carbonate:
Phenol does not react to give negative result
Carboxylic acid gives pos result by forming effervescence which when bubbled through lime water turns cloudy

28
Q

Can phenol react with a metal carbonate base?

A

No, not strong enough of an acid