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A2 Chemistry 1 > 1.10 Aromatic Chemistry > Flashcards

1.10 Aromatic Chemistry Flashcards

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1
Q

Who proposed the first structure for benzene?

A

Kekulé

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2
Q

Describe Kekulé’s structure for benzene

A

three C=C and three C-C bonds

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3
Q

give evidence the Kekulé structure was incorrect

A
  • X ray studies revealed all 6 of he carbon-carbon bond lengths in benzene are the same length (0.139nm), and intermediate between C-C (0.153nm) and C=C (0.134nm)
  • Energy required to hydrogenate 1 mole benzene should be 3 times the energy required to hydrogenate 1 mole of cyclohexene to cyclohexane. If so, the energy change should be -360kJmol-1, however it is actually -208kJmol-1. The extra energy is the stability that is conferred by the π-system of electrons.
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4
Q

Describe the structure of benzene

A
  • Consists of six carbon atoms in a hexagonal planar ring arrangement (each carbon is bonded in a trigonal planar arrangement with a 120º bond angle)
  • Each carbon is bonded to two other carbons and a hydrogen. As carbon has 4 electrons in its outer shell, each carbon has an unbounded p orbital electron.
  • The p orbitals containing the free electrons can overlap to form a π-delocalised system of electrons above and below the plane of the main ring.
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5
Q

what is the name for C6H5OH?

A

phenol

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6
Q

what is the name for C6H5CH3?

A

methylbenzene/tolune

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7
Q

what is the name for C6H5NH2?

A

phenylamine

aniline

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8
Q

what is the name for C6H5I?

A

iodobenzene

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9
Q

what is the name for C6H5Br?

A

bromobenzene

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10
Q

what is the name for C6H5COOH?

A

benzoic acid

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11
Q

describe the reactivity of benzene

A
  • Arenes are very stable due to the stability of the delocalised π system of electrons in the six membered rings. Therefore it doesn’t undergo addition reactions easily, so the majority of reactions involve substitution to ensure the delocalised π system remains intact.
  • Benzene attracts electrophiles due to the region of high electron density above and below the plane of carbon atoms.
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12
Q

describe the mechanism for electrophilic addition of bromine to cyclohexene

A
  • electrons move from double bond in cyclohexene to bromine atom in the bromine molecule. Electrons move to the other bromine atom
  • intermediate carbocation of the double bond going, one bromine bonded to the cyclohexene, and carbon 2 being positive, with electrons from bromine anion moving to carbon 2
  • final molecule formed - 1,2-dibromocyclohexane
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13
Q

Describe the conditions required for the monohalogenation of benzene

A

Takes place in the presence of a halogen carrier catalyst - such as iron or aluminium chlorides or bromides (FeCl3, FeBr3, AlCl3, AlBr3)

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14
Q

why is a halogen carrier catalyst used for monohalogenation of benzene?

A

Halogen carriers make the halogen strongly electrophilic - cause heterolytic fission of the X-X bond, electrophilic X+ then attacks the ring.

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15
Q

What are Lewis acids and why are they used as halogen carriers in benzene reactions?

A

the metal doesn’t have full octet and therefore has a vacant orbital to attract electrons to (eg. FeBr3, AlCl3, metallic iron (forms FeBr3 in presence of bromine))

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16
Q

Give the mechanism and equation for the generation of the electrophile in the monobromination of benzene

A

electrons in bromine molecule move to one bromine atom, and then to the aluminium in the AlBr3 halogen carrier
Cr2 + AlBr3 -> Br+ + AlBr4-

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17
Q

describe the mechanism for the monobromination of benzene

A
  • electrons move from the pi bond system in benzene to the Br+ electrophile
  • carbocation intermediate where the pi bond is broken, the molecule is positively charged, and hydrogen and bromine are bonded to the same carbon. The electrons in the hydrogen move into the pi system
  • hydrogen leaves as a H+ ion, and bromobenzene is formed as the pi bond system is reformed.
18
Q

Give the mechanism and equation for the regeneration of the catalyst in the monobromination of benzene

A

electrons in AlBr4- move to H+, bromine molecule breaks off and forms a coordinate bond with the hydrogen
AlBr4- + H+ -> AlBr3 + HBr

19
Q

describe the appearance of nitrobenzene

A

a yellowish oily liquid

20
Q

describe the uses for nitrobenzene

A

the starting material for a variety of substances including dyes and explosives

21
Q

name the electrophile ion used in the nitration of benzene and how it is formed

A

NO2+ - nitronium ion

obtained from nitrating mixture of concentrated sulfuric and concentrated nitric acid

22
Q

describe the conditions necessary for the nitration of benzene, and why they are necessary

A

Temperature must be kept below 10ºC to prevent di- and tri-substituted nitrobenzene rings, which are explosive compounds

23
Q

give the equation for the generation of the electrophile in nitration of benzene

A

2H2SO4 + HNO3 _> NO2+ + H3O+ + 2HSO4-

24
Q

Describe the mechanism involved in the nitration of benzene

A
  • Nitronium ion is attracted to the high electron density of the π system in the benzene ring, substituting one of the H atoms in electrophilic substitution.
  • electrons in pi system move to NO2+
  • carbocation intermediate where H and NO2 are bonded to the same carbon, pi bond system is broken, and molecule is positive. electrons in H move into pi bond system
  • H breaks off as H+ and nitrobenzene is formed as the pi bond system is restored
25
Q

give the equation for the regeneration of the catalyst in the nitration of benzene

A

HSO4- + H+ -> H2SO4

26
Q

Give some reactions that benzene can undergo

A
  • monohalogenation
  • nitration
  • monoalkylation
  • monoacylation
27
Q

what is the other name for monoalkylation and monoacylation of benzene?

A

Friedel-Crafts alkylation/acylation

28
Q

Describe how the electrophile for monoalkylation of benzene is generated

A
  • AlCl3 is used to polarise the C-Cl bond in a chloroalkane (RCl), so that it undergoes heterolytic fission to form an alkyl cation electrophile (R+)
  • bond in RCl breaks, Cl bonds to AlCl3 via a coordinate bond, forming R+ and AlCl4-
29
Q

give the general equation for generation of an electrophile for monoalkylation of benzene

A

RCl + AlCl3 -> R+ + AlCl4-

30
Q

describe the mechanism involved in the monoalkylation of benzene

A
  • electrons in pi system of benzene are attracted to R+ cation
  • carbocation intermediate where H and R and bonded t the same carbon, pi bond system is broken and molecule is positively charged. electrons in hydrogen move into pi bond system
  • alkylbenzene (eg toluene) formed as hydrogen leaves as H+ and pi bond system is restored
31
Q

give the equation for regeneration of the catalyst in the monoalkylation of benzene

A

AlCl4- + H+ -> AlCl3 + HCl

32
Q

Describe how the electrophile is generated in monoacylation of benzene

A

AlCl3 is used to polarise the C-Cl bond in an acyl chloride (RCOCl), so that it undergoes heterolytic fission to form an acyl cation (acylium) electrophile (RCO+)

Cl breaks off from RCOCl, bonds to AlCl3 via a coordinate bond, forming RCO+ electrophile and AlCl4-

33
Q

why are acyl and alkyl cations good electrophiles?

A

they will form a coordinate bond by accepting an electron pair

34
Q

give the equation for the generation of the electrophile for the monoacylation of benzene

A

RCOCl + AlCl3 -> RCO+ + AlCl4-

35
Q

describe the mechanism for the monoacylation of benzene

A
  • electrons move from pi system in benzene to RCO+ electrophile
  • carbocation intermediate where H and RCO are bonded to the same carbon. pi bond system is broken and molecule is positive. hydrogen electrons move to the pi system
  • phenylketone (eg phenylethanone) is formed as hydrogen leaves as H+ and pi bond system is restored
36
Q

give the equation for the regeneration of the catalyst for the monoacylation of benzene

A

AlCl4- + H+ -> AlCl3 + HCl

37
Q

what is the physical appearance of methyl 3-nitrobenzoate?

A

cream solid

38
Q

give the practical technique for the preparation of methyl 3-nitrobenzoate

A
  1. Dissolve methyl benzoate in conc sulfuric acid. Cool the solution in ice
  2. Prepare nitrating mixture by adding conc sulfuric acid to conc nitric acid, and cool the mixture in ice
  3. Add the nitrating mixture drop by drop to the solution of methyl benzoate, stirring with a thermometer and keeping the temperature below 10ºC
  4. When the addition is complete, allow the mixture to stand at room temperature for 15 minutes
  5. Pour the reaction mixture onto crushed ice and stir until all the ice has melted, and crystalline methyl 3-nitrobenzoate is formed
  6. Filter the crystals using Buchner filtration, wash with cold water, recrystallise form ethanol, filter off and dry
39
Q

give the equation for the generation of the nitronium ion

A

2H2SO4 + HNO3 -> 2HSO4- + NO2+ + H3O+

40
Q

give the overall equation for the nitration of methyl benzoate

A

C6H5COOCH3 + HNO3 –H2SO4-> C6H4(NO2)(COOCH3) + H2O

A2 Chemistry 1 (10 decks)

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