Organic chemistry: Arenes
- Created by: Gemma
- Created on: 07-01-14 09:19
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- Arenes
- Phenol
- Contains a hydroxyl, -OH group
- Reactions
- undergoes similar substituion reactions to benzene
- Why more reactive than benzene?
- Because of the -OH group. It directs incoming groups to particular positions around the ring
- Oxygen form the OH has two pairs of non-bonding electrons
- One pair is drawn to delocalised pi electron system
- Ring better at attracting electrophiles so reactions occur more easily
- One pair is drawn to delocalised pi electron system
- Substituion reactions
- With bromine water
- multi-electrophilic substituion occurs immediately, Bromine water is decolourised
- product= white ppt of 2,4,6-tribroophenol (smells antiseptic)
- multi-electrophilic substituion occurs immediately, Bromine water is decolourised
- With dil Nitric acids
- white ppt of 2,4,6-trinitrophenol
- multi-electrophilic substituion
- Does not need conc sulphuric acid to assist (unlike benzene)
- With bromine water
- Phenol
- Benzene
- Arenes
- Phenol
- Contains a hydroxyl, -OH group
- Reactions
- undergoes similar substituion reactions to benzene
- Why more reactive than benzene?
- Because of the -OH group. It directs incoming groups to particular positions around the ring
- Oxygen form the OH has two pairs of non-bonding electrons
- One pair is drawn to delocalised pi electron system
- Ring better at attracting electrophiles so reactions occur more easily
- One pair is drawn to delocalised pi electron system
- Substituion reactions
- With bromine water
- multi-electrophilic substituion occurs immediately, Bromine water is decolourised
- product= white ppt of 2,4,6-tribroophenol (smells antiseptic)
- multi-electrophilic substituion occurs immediately, Bromine water is decolourised
- With dil Nitric acids
- white ppt of 2,4,6-trinitrophenol
- multi-electrophilic substituion
- Does not need conc sulphuric acid to assist (unlike benzene)
- With bromine water
- Phenol
- Kekule
- six-membered carbon ring with alternate double and single bonds between carbon atoms
- Evidence against kekule
- double bonds would show a tendency to undergo addition reactions- They do not occur easily! Most are substituion reactions
- Thermochemical evidence-Theoretical value of enthalpy change= +252KJmol-1. Actual= 49KJmol-1= Benzene is more energetically stable than kekule model
- New model
- Each bond is between a double and a single bond
- Evidence for new model
- Enthalpy value very close to observed value
- enthalpy for hydrogenation of kekule benzene would be 3x-120KJmol-1. Actual is -208KJmol-1. Suggests an addition reaction with hydrogen is not occuring across a normal double bond.
- X-ray diffraction used to measure bond length
- A C-C bond length is 0.154nm. A C=C bond length is 0.133nm.
- Bond length= 0.139- Shows there is only one bond length in benzene- inbetween a single and a double bond
- Supported by the electron density map of benzene
- All bond angles= 120
- Evidence for new model
- Each bond is between a double and a single bond
- Arrangement of electrons
- Each carbon atom forms a single sigma bond with each of the two carbon atoms joined to it
- Planar hexagonal ring
- Each carbon has one p orbital containing a single electron that fuse to form a ring above and below the sigma bonded skeleton
- The electrons are free to move around the ring (delocalised) which causes all the C-C bonds to be identical in benzene and makes it stable
- Each carbon atom forms a single sigma bond with each of the two carbon atoms joined to it
- Reactions
- Combustion
- 6C6H6 (l) + 15O2 (g) --> 12CO2 (g) + 6H2O (l)
- Needs plenty of oxygen
- 6C6H6 (l) + 15O2 (g) --> 12CO2 (g) + 6H2O (l)
- substitutuion Reactions
- Involve attack on the ring by electrophiles
- Reaction of benzene with fuming sulphuric acid
- Sulfonation
- Room temp with conc sulphuric acid that contains extra sulfur trioxide as an effective electrophile
- Reversible reaction
- Used in the manufacture of soapless detergents
- SO3HC6H5
- Sulfonation
- With halogens
- In the dark- doesn't react without catalyst (Ironbromide, FeBr3)
- Catalyst is a hydrogen carrier. The bezene and hydrogen carrier are refluxed together
- Bromobenzene is formed
- Iron (III) polarises the bromine which didn't have a charge
- Catalyst is a hydrogen carrier. The bezene and hydrogen carrier are refluxed together
- In the dark- doesn't react without catalyst (Ironbromide, FeBr3)
- Nitation
- doesn't react with conc nitric acid but with a mixture of conc HNO3 and conc H2SO4
- Product= nitrobenzene
- temp below 55 degrees C
- If temp is higher- multiple substitution occurs resulting in a mixture of products
- doesn't react with conc nitric acid but with a mixture of conc HNO3 and conc H2SO4
- Alkylation
- Refluxing benzene with a halogenoalkane in the presence of AlCl3 (halogen carrier catalyst)
- AlCl3 polarises the halogenoalkane molecule promoting the fomration of an electrophilic alkyl cation which is attracted to the ring
- Refluxing benzene with a halogenoalkane in the presence of AlCl3 (halogen carrier catalyst)
- Acylation
- refluxed with acyl chloride
- Forms a ketone which can be reduced to a secondary alcohol
- Combustion
- Arenes
- Properties
- Freezes as 6 degrees C
- Benzene
- Kekule
- six-membered carbon ring with alternate double and single bonds between carbon atoms
- Evidence against kekule
- double bonds would show a tendency to undergo addition reactions- They do not occur easily! Most are substituion reactions
- Thermochemical evidence-Theoretical value of enthalpy change= +252KJmol-1. Actual= 49KJmol-1= Benzene is more energetically stable than kekule model
- New model
- Each bond is between a double and a single bond
- Evidence for new model
- Enthalpy value very close to observed value
- enthalpy for hydrogenation of kekule benzene would be 3x-120KJmol-1. Actual is -208KJmol-1. Suggests an addition reaction with hydrogen is not occuring across a normal double bond.
- X-ray diffraction used to measure bond length
- A C-C bond length is 0.154nm. A C=C bond length is 0.133nm.
- Bond length= 0.139- Shows there is only one bond length in benzene- inbetween a single and a double bond
- Supported by the electron density map of benzene
- All bond angles= 120
- Evidence for new model
- Each bond is between a double and a single bond
- Arrangement of electrons
- Each carbon atom forms a single sigma bond with each of the two carbon atoms joined to it
- Planar hexagonal ring
- Each carbon has one p orbital containing a single electron that fuse to form a ring above and below the sigma bonded skeleton
- The electrons are free to move around the ring (delocalised) which causes all the C-C bonds to be identical in benzene and makes it stable
- Each carbon atom forms a single sigma bond with each of the two carbon atoms joined to it
- Reactions
- Combustion
- 6C6H6 (l) + 15O2 (g) --> 12CO2 (g) + 6H2O (l)
- Needs plenty of oxygen
- 6C6H6 (l) + 15O2 (g) --> 12CO2 (g) + 6H2O (l)
- substitutuion Reactions
- Involve attack on the ring by electrophiles
- Reaction of benzene with fuming sulphuric acid
- Sulfonation
- Room temp with conc sulphuric acid that contains extra sulfur trioxide as an effective electrophile
- Reversible reaction
- Used in the manufacture of soapless detergents
- SO3HC6H5
- Sulfonation
- With halogens
- In the dark- doesn't react without catalyst (Ironbromide, FeBr3)
- Catalyst is a hydrogen carrier. The bezene and hydrogen carrier are refluxed together
- Bromobenzene is formed
- Iron (III) polarises the bromine which didn't have a charge
- Catalyst is a hydrogen carrier. The bezene and hydrogen carrier are refluxed together
- In the dark- doesn't react without catalyst (Ironbromide, FeBr3)
- Nitation
- doesn't react with conc nitric acid but with a mixture of conc HNO3 and conc H2SO4
- Product= nitrobenzene
- temp below 55 degrees C
- If temp is higher- multiple substitution occurs resulting in a mixture of products
- doesn't react with conc nitric acid but with a mixture of conc HNO3 and conc H2SO4
- Alkylation
- Refluxing benzene with a halogenoalkane in the presence of AlCl3 (halogen carrier catalyst)
- AlCl3 polarises the halogenoalkane molecule promoting the fomration of an electrophilic alkyl cation which is attracted to the ring
- Refluxing benzene with a halogenoalkane in the presence of AlCl3 (halogen carrier catalyst)
- Acylation
- refluxed with acyl chloride
- Forms a ketone which can be reduced to a secondary alcohol
- Combustion
- Kekule
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