Module 6.1 - Aromatic Compounds, Carbonyls and Acids Flashcards

1
Q

What is benzene?

A
  • naturally occurring aromatic hydrocarbon. Stable ring structure with delocalised electrons
  • C6H6 (empirical formula: CH)
  • liquid at room temperature
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2
Q

Give one use of benzene.

A

Key ingredient in gasoline (which increases efficiency of car engine)

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3
Q

Describe Kekulé’s model of benzene.

A
  • 6 membered ring with alternating double and single bonds
  • discovered when one group was added to benzene, only one isomer was ever made but when 2 groups were added there were 3 isomers
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4
Q

What were the experimental evidence that didn’t support Kekulé’s model of benzene?

A
  • benzene is resistant to addition reactions (unlike alkenes) (Kekulé tried to explain this saying double and single bonds alternate in very fast equilibrium)
  • enthalpy of hydrogenation of benzene shows it’s more stable than predicted (can calculate enthalpy change of hydrogenation of cyclo-1,3,5-hexatriene, Kekulé model, but actual value is -208kJmol-1, 152kJmol-1 more energetically stable than predicted)
  • all 6 carbon bonds in benzene are the same length (C-C bond length: 0.147nm, C=C bond length: 0.135nm, benzene: 0.140nm, Kekulé should have 3 longer and 3 shorter bond lengths, disproving Kekulé’s model)
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5
Q

Describe the delocalised structure of benzene.

A
  • bezene has a delocalised structure, explaining all 3 pieces of evidence disproving Kekulé’s model
  • each of the 6 C atoms donates one e- from p orbital
  • e- combine to form a ring of e- above and below the plane of the molecule
  • e- said to be delocalised as able to move freely within ring and don’t belong to a single atom meaning all bonds in the ring are identical
  • enthalpy of hydrogenation is 152kJmol-1 more stable than expected w Kekulé as more energy needed to disrupt delocalisation so benzene is v stable and resistant to addition reactions
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6
Q

What is a substitution reaction?

A

Where a group or atom is exchanged for another group or atom in a chemical reaction

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7
Q

What is a benzene derivative?

A

A benzene ring that has undergone a substitution reaction

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8
Q

What is the prefix when a nitro functional group is substituted onto a molecule?

A

nitro-

functional group: -NO2

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9
Q

Name this molecule.

A

phenylethene

Aromatic ring isn’t main functional group so aromatic ring is a phenyl group as H atom removed. Alkene group used for addition polymerisation in this molecules

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10
Q

Describe the general mechanism for the electrophilic substitution on a benzene molecule.

A
  1. Electrons above and below plane of atoms in benzene ring attract electrophile
  2. Electrophile accepts a pair of π electrons from delocalised ring and makes a covalent bond. This is the slowest, rate determining step
  3. Reactive intermediate is formed where the delocalised electrons have been disrupted
  4. Unstable intermediate releases a H+ ion and the stable product has formed (v fast step)
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11
Q

Describe the nitration of benzene.

A
  • electrophilic substitution reaction (H atom exchanged for a nitro group (-NO2)
  • reagent: conc nitric acid, catalyst: conc sulfuric acid
  • C6H6 + HNO3 –> C6H5NO2 + H2O
  • initially, conc nitric acid and conc sulfuric acid mixed in a flask held in an ice bath. Benzene then added and reflux condenser set up, keeping mixture at 50°C to prevent further substitution occurring
  • sulfuric acid needed to generate NO2+ electrophile from nitric acid. Sulfuric acid is regenerated after nitration so is catalyst
  • HNO3 + H2SO4 –> NO2+ + HSO4- + H2O
  • regeneration of catalyst: H+ + HSO4- –> H2SO4
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12
Q

Describe the halogenation of benzene.

A
  • halogen carrier needed as ring too stable to react directly w halogens
  • halogen carriers:
  • chlorination: AlCl3/FeCl3/Fe (Fe forms iron halide in situ)
  • bromination: AlCl3/FeCl3/Fe (Fe forms iron halide in situ)
  • halogen carrier used to generate positive halogen ion
  • e.g. Br2 + FeBr3 –> Br+ + FeBr4- (creates positive bromine ion to act as an electrophile. It’s generated in situ. Can then attack benzene ring)
  • halogen carrier is catalyst and gets regenerated at end of halogenation as H+ from benzene ring forms HBr:

FeBr4- + H+ –> HBr + FeBr3

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13
Q

Compare how bezene reacts with bromine water compared to cyclohexene. What does this show?

A
  • cyclohexene: π bonds break in an addition reaction
  • bezene: no addition reaction even though electrons in benzene are delocalised in π system so benzene must have a lower electron density between carbon atoms than an alkene
  • when non polar molecules e.g. bromine approach ring there’s not enough electron density between C atoms to induce dipole and start a reaction (also the case when attempting to substitute alkyl halides like haloalkanes). Using a halogen carrier means a stronger electrophile can be generated and alkylation can occur
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14
Q

What is a Friedel Crafts reaction?

A

A substitution reaction where hydrogen is exchanged for an alkyl or acyl chain. C-H bond broken and C-C bond formed

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15
Q

Describe the alkylation of benzene.

A
  • haloalkanes e.g. chloromethane mixed w halogen carrier e.g. AlCl3
  • anhydrous
  • halogen carrier = catalyst and gets regenerated (Lewis acid also used as catalyst)
  • reactive carbocation is made which undergoes electrophilic substitution within benzene ring
  • multiple substitutions likely so mixture of products made. Products may be separated by fractional distillation or chromatography
  • actual yield of substituted product can be improved by adding excess benzene
  • mixture of products caused as each successive substitution makes delocalised π electrons more nucleophilic so more susceptible to electrophilic attack. Increase in reactivity due to alkyl chain donating electrons to aromatic ring
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16
Q

Describe the acylation of benzene.

A
  • acyl chloride: RCOCl (very reactive)
  • can be used in Friedel-Crafts reaction as halogen carrier to substitute a H atom
  • anhydrous
  • as carbonyl group withdraws electrons from aromatic ring, a less reactive ketone is made, so only one substitution can occur
  • reaction mixture at 60°C for 30 minutes under reflux for reaction to occur
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17
Q

What is phenol?

A

Class of aromatic compounds where a hydroxyl group is directly attached to the aromatic ring

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18
Q

What is the difference between a phenol derivative and an aromatic alcohol?

A
  • phenol: hydroxyl group attached directly to aromatic ring
  • aromatic alcohol: hydroxyl group attached to alkyl chain attached to aromatic ring
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19
Q

Describe the acidity of phenol.

A

-weak acid that partially dissociates in water

C6H5OH + H2O ⇌ H3O+ + C6H5O-

-acid as reacts w strong bases e.g. NaOH but only weak acid as doesn’t react w carbonates. Phenol won’t react w weak bases e.g Na2CO3

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20
Q

Describe the reaction of phenol with strong bases.

A

-forms salt and water

C6H5OH + NaOH → C6H5O-Na+ + H2O

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21
Q

How does the reactivity of phenol compare to that of benzene?

A
  • phenol more reactive than benzene
  • p orbital electrons from oxygen of hydroxyl group adding to delocalised electrons of aromatic ring so π system of aromatic ring becomes more nucleophilic
  • increase in electron density allows aromatic ring in phenol to be mroe susceptible to electrophilic attack as can induce dipole in no polar molecules
  • e.g. can induce dipole in bromine to react w it
22
Q

What is a directing effect?

A

How a functional group directly attached to an aromatic ring affects which carbon atoms are more likely to undergo substitution

23
Q

Describe the bromination of phenol.

A

-undergoes a triple substitution reaction w bromine water at room temp

C6H5OH + 3Br2 –> C6H2Br3OH + 3HBr

-resulting product is a white ppt of 2,4,6-tribromophenol (smells of antiseptic)

24
Q

Describe the nitration of phenol.

A
  • dilute HNO3 to undergo single substitution at room tempt
  • forms a mixture of 2-nitrophenol and 4-nitrophenol

C6H5OH + HNO3 –> C6H4(NO2)OH + H2O

  • doesn’t require a H2SO4 catalyst
  • when conc HNO3 used a triple substitution occurs, forming 2,4,6-trinitrophenol
25
Q

How does a hydroxyl group (and other electron donating groups) on an aromatic ring affect the position of substitution?

A
  • additional electrons in π system
  • reactions mainly occur on 2 and 4 positions on ring (2- and 4-directing effect)
  • hydroxyl group activates these carbon atoms so their rate of substitutions is faster than other positions
  • effect more pronounced when NH2 group attached to aromatic ring
26
Q

How does a nitro group (and other electron withdrawing) on an aromatic ring affect the position of substitution?

A
  • 3-directing effect
  • nitro groups withdraw electrons from π system making rate of substitution highest on 3rd C atom
27
Q

What is a nucleophile?

A

A species attracted to an electron deficient part of a molecule where it donates a pair of electrons to make a new covalent bond

28
Q

What is the ionic equation of the oxidation of ethanal to ethanoic acid?

A

3CH3CHO(l) + Cr2O72-(aq) + 8H+(aq) –> 2CH3COOH(aq) + 2Cr3+(aq) + 4H2O(l)

29
Q

Describe the general nucelophilic addition reactions to carbonyls.

A
  • carbonyls have a dipole over C=O functional group so susceptible to nucleophilic attack on δ+ C atom
  • nucleophile donates lone pair of electrons to electron deficient carbon
  • simultaneously, π bond in C=O breaks forming a reactive intermediate
  • extra electron pair quickly donated to neighbouring hydrogen to form an alcohol group and the stable product
30
Q

Describe the reduction of carbonyls by sodium tetrahybridoborate(III).

A
  • NaBH4 is a reducing agent. Made of BH4- ion, a source of hydride ions, H-
  • hydride ion involved in electrophilic addition and reduction of carbonyls to alcohols
  • CH3COC3H7 + 2[H] –> CH3CH(OH)C3H7
  • hydride ion attacks δ+ C atom and forms a bond, intermediate forms that reacts with an ethanol/water molecule, to form an organic product (alcohol)
31
Q

Desccribe the reaction between hydrogen cyanide and carbonyls.

A

-HCN: weak acid that partially ionises in solution, forming a cyanide nucleophile with negative charge on carbon atom

HCN + H2O ⇌ CN- + H3O+

  • other sources of CN- include NaCN
  • cyanide ion can’t react directly w carbonyl compound but when reaction is acidified the carbonyl group becomes more reactive as polarity of C=O bond increases
  • allows additional H atoms to be added, forming a hydroxynitrile (used in many industrial processes)
32
Q

Describe the reaction between 2,4-dinitrophenylhydrazine and aldehydes/ketones as a test for the carbonyl functional group of aldehydes/ketones only.

A
  • Brady’s reagent: mixture of methanol, sulfuric acid and 2,4-DNP
  • when added to aldehyde/ketone a yellow/orange ppt of 2,4-dinitrophenylhydrazone derivative is seen
  • no ppt observed w carboxylic acid or ester even though they have C=O
33
Q

How would you identify the specific aldehyde/ketone after using Brady’s reagent to discover you have an aldehyde/ketone?

A
  • 2,4-dinitrophenylhydrazone derivative ppt can be collected by filtration and purified using recrystallisation
  • once dried, accurate melting point or pure product can be measured through experiment
  • aldehyde/ketone identified by comparing melting point of 2,4-dinitrophenylhydrazone derivative ppt w a database
34
Q

When working out the specific aldehyde/ketone, why is the melting point of the 2,4-dinitrophenylhydrazone derivative precipitate used rather than the aldehyde/ketone?

A
  • experimentally different for different ketones as have v similar mp
  • ketones of similar chain length have similar bp so difficult to distinguish between
  • 2,4-dinitrophenylhydrazone derivatives have v different mp and bps
35
Q

How do you make Tollens’ reagent and how do you use it to test whether you have an aldehyde/ketone?

A

Making:

  1. NaOH solution added to AgNO3 solution until brown ppt formed
  2. Dilute NH3 added drop wise until brown ppt redissolves
  • used to distinguish between an aldehyde/ketone
  • it’s a weak oxidising agent and can react w carbonyl functional group in aldehyde but not ketone
  • when Tollens’ added to ketone, no reaction as ketones can’t be oxidised further
  • when added to aldehyde a silver mirror is observed as redox reaction occurs between Tollens’ and aldehyde tro form carboxylic acid
  • Ag+(aq) + e- → Ag(s)
  • silver metal precipitated out appearing as silver mirror effect on inside of reaction vessel
36
Q

Describe the solubility (physical property) of carboxylic acids.

A
  • small carboxylic acids are v soluble in polar solvent e.g. water as H bonds can form between carboxylic acid functional group and water
  • as hydrocarbon chain length increases, solubility decreases as only polar COOH functional group can form H bonds w water so as molecule becomes non polar the solubility decreases
37
Q

Describe the partial ionisation of carboxylic acids.

A
  • weak acid so only partially ionise to release H+ into solution from carboxylic acid group
  • forms carboxylate ion

(-lone pair of electrons from O of H2O to H causing fission of COOH O-H bond)

-reactions of carboxylic acids happen at slower rate w a strong acid as pH is higher so conc of H+(aq) will be lower

38
Q

Describe the reaction between carboxylic acids and metals.

A
  • reactive w metals above H in the reactivity series
  • form H2 and a metal salt
  • name of salt generated from acid
    e. g.

sodium + ethanoic acid → sodium ethanoate + hydrogen

2Na + 2CH2COOH → 2CH3COONa + H2

39
Q

Describe the reaction between carboxylic acids and metal oxides.

A
  • metal oxides classified as bases as react w acids
  • forms metal salt and water
    e. g.

magnesium oxide + methanoic acid → magnesium methanoate + water

MgO(s) + HCOOH(aq) → (HCOO)2Mg(aq) + H2O(l)

40
Q

Describe the reaction between carboxylic acids and metal hydroxides.

A
  • group 1 metal hydroxides are soluble bases that release OH-(aq)
  • form water and metal salt
    e. g.

potassium hydroxide + propanoic acid → potassium propanoate + water

KOH(aq) + CH3CH2COOH(aq) → CH3CH2COOK(aq) + H2O(l)

41
Q

Describe the reaction between carboxylic acids and metal carbonates.

A
  • metal carbonates are bases
  • form water, carbon dioxide and a metal salt
    e. g.

sodium carbonate + methanoic acid → sodium methanoate + carbon dioxide + water

Na2CO3(s) + 2HCOOH(aq) → 2HCOONa(aq) + CO2(g) + H2O(l)

-group 1 metals can also form metal hydrogencarbonates where carbonic acid only had 1 proton exchanged to form metal hydrogencarbonate (MHCO3 where M is group 1 metal). Acids react with metal hydrogencarbonates forming salt, water and carbon dioxide

42
Q

Name this ester.

A

propyl butanoate

43
Q

Describe esterification from carboxylic acids and alcohols.

A
  • alcohol and carboxylic acid heated gently in presence of H2SO4 catalyst
  • reversible reaction and has a slow rate of reaction
  • ester separated from reaction mixture by distillation as it’s volatile w lowest bp of the chemicals. Separation has to happen quickly to prevent reverse reaction occurring
  • for larger esters: reaction mixture needs to be heated under reflux until equilibrium is established. Ester can be separated using fractional distillation
  • this method of ester prep not suitable for phenols/its derivatives as reaction rate is so low
44
Q

Describe esterification from an acid anhydride and an alcohol.

A
  • acid anhydride: acid derivative more reative than a similar carboxylic acid, made from removal of water from 2 carboxylic acid molecules
  • acid anhydrides react w alcohols, including phenol/its derivatives making an ester
  • not reversible so higher yield than carboxylic acid
  • rate of reaction still slow but can be increased by gently warming the reaction mixture
45
Q

Describe the hydrolysis of esters in acidic conditions.

A
  • refluxed w a catalyst of hot aqueous acids e.g. dilute H2SO4 or dilute HCl as source of H+(aq)
  • ester reversibly decomposes to an alcohol and carboxylic acid
46
Q

Describe the hydrolysis of esters in alkaline conditions.

A
  • alkaline chemicals: bases that can dissolve in water
  • ester refluxed w hot aqueous alkali e.g. KOH(aq)/NaOH(aq)
  • decomposes to carboxylate salt and an alcohol
  • not reversible
  • alkaline hydrolysis of esters used to make soaps so it’s also called saponification
47
Q

Name this acyl chloride.

A

butanoyl chloride

48
Q

How can you prepare an acyl chloride?

A
  • OH group on carboxylic acid must be substituted for chlorine atom
  • SOCl2 (thionyl chloride), liquid at room temp and reacts readily w carboxylic acids to form acyl chlorides
  • SO2 and hydrogen chloride gases made
  • acyl chloride separated from mixture by distillation
    e. g.

CH3COOH + SOCl2 → CH3COCl + SO2 + HCl

49
Q

How can acyl chlorides be used to make esters?

A
  • react w alcohols
  • not reversible so has a higher yield than w carboxylic acid
    e. g.

CH3COCl + CH3CH2OH → CH3COOCH2CH3 + HCl

-can be used to make esters from phenols but reaction is violent and produces corrosive fumes of HCl

50
Q

How can acyl chlorides be used to make carboxylic acids?

A
  • small acyl chlorides (e.g. ethanoyl chloride) is added to water, quickly hydrolyses to produce a carboxylic acid
  • v exothermic reaction and misty fumes of HCl given off

CH3COCl + H2O → CH3COOH + HCl

51
Q

How can acyl chlorides be used to make primary amides?

A
  • primary amides made when acyl chlorides react w ammonia
  • ethanamide: ethanoyl chloride added to conc ammonia solution. Quickly produces a mixture of solid ammonium chloride and ethanamide observed as white smoke
  • some of the products remain in a colourless solution

CH3COCl + 2NH3 → CH3CONH2 + NH4Cl

52
Q

How can acyl chlorides be used to make secondary amides?

A
  • formed when acyl chlorides react w primary amides
  • N has 1 H directly bonded to it
  • N also has 2 organic groups attached (often called an N-substituted amide)
  • white solid compound of N-ethylethanamide can be made from ethanoyl chloride and cold conc solution of ethylamine

CH3COCl + CH3CH2NH2 → CH3CONHCH2CH3 + HCl