Alcohols Knockhardy

AN INTRODUCTION TOAN INTRODUCTION TO

THE CHEMISTRYTHE CHEMISTRYOF ALCOHOLSOF ALCOHOLS

KNOCKHARDY PUBLISHINGKNOCKHARDY PUBLISHING2008 2008

SPECIFICATIONSSPECIFICATIONS

INTRODUCTION

This Powerpoint show is one of several produced to help students understand selected topics at AS and A2 level Chemistry. It is based on the requirements of the AQA and OCR specifications but is suitable for other examination boards.

Individual students may use the material at home for revision purposes or it may be used for classroom teaching.

Accompanying notes on this, and the full range of AS and A2 topics, are available from the KNOCKHARDY SCIENCE WEBSITE at...

www.knockhardy.org.uk/sci.htm

Navigation is achieved by...

either clicking on the grey arrows at the foot of each page

or using the left and right arrow keys on the keyboard

KNOCKHARDY PUBLISHINGKNOCKHARDY PUBLISHING

THE CHEMISTRY OF ALCOHOLSTHE CHEMISTRY OF ALCOHOLS

CONTENTS• Structure of alcohols

• Nomenclature

• Isomerism

• Physical properties

• Chemical properties of alcohols

• Identification using infra-red spectroscopy

• Industrial preparation and uses of ethanol

• Revision check list


Before you start it would be helpful to…

• Recall the definition of a covalent bond

• Recall the difference types of physical bonding

• Be able to balance simple equations

• Be able to write out structures for simple organic molecules

• Understand the IUPAC nomenclature rules for simple organic compounds

• Recall the chemical properties of alkanes and alkenes


CLASSIFICATION OF ALCOHOLSCLASSIFICATION OF ALCOHOLS

Aliphatic • general formula CnH2n+1OH - provided there are no rings • the OH replaces an H in a basic hydrocarbon skeleton



Aromatic • in aromatic alcohols (or phenols) the OH is attached directly to the ring • an OH on a side chain of a ring behaves as a typical aliphatic alcohol

The first two compounds are classified as aromatic alcohols (phenols) because the OH group is attached directly to the ring.



Aromatic • in aromatic alcohols (or phenols) the OH is attached directly to the ring • an OH on a side chain of a ring behaves as a typical aliphatic alcohol

The first two compounds are classified as aromatic alcohols (phenols) because the OH group is attached directly to the ring.

Structuraldifferences • alcohols are classified according to the environment of the OH group

• chemical behaviour, eg oxidation, often depends on the structural type

PRIMARY 1° SECONDARY 2° TERTIARY 3°

Alcohols are named according to standard IUPAC rules

• select the longest chain of C atoms containing the O-H group;

• remove the e and add ol after the basic name

• number the chain starting from the end nearer the O-H group

• the number is placed after the an and before the ol ... e.g butan-2-ol

• as in alkanes, prefix with alkyl substituents

• side chain positions are based on the number allocated to the O-H group

e.g. CH3 - CH(CH3) - CH2 - CH2 - CH(OH) - CH3 is called 5-methylhexan-2-ol

NAMING ALCOHOLSNAMING ALCOHOLS

STRUCTURAL ISOMERISM IN ALCOHOLSSTRUCTURAL ISOMERISM IN ALCOHOLS

Different structures are possible due to...

A Different positions for the OH group andB Branching of the carbon chain

butan-1-ol butan-2-ol

2-methylpropan-1-ol2-methylpropan-2-ol

BOILING POINTS OF ALCOHOLSBOILING POINTS OF ALCOHOLS

Increases with molecular size due to increased van der Waals’ forces.

Alcohols have higher boiling points thansimilar molecular mass alkanes

This is due to the added presence ofinter-molecular hydrogen bonding.More energy is required to separate the molecules.

Mr bp / °Cpropane C3H8 44 -42 just van der Waals’ forcesethanol C2H5OH 46 +78 van der Waals’ forces + hydrogen bonding

BOILING POINTS OF ALCOHOLSBOILING POINTS OF ALCOHOLS

Increases with molecular size due to increased van der Waals’ forces.

Alcohols have higher boiling points thansimilar molecular mass alkanes

This is due to the added presence ofinter-molecular hydrogen bonding.More energy is required to separate the molecules.

Mr bp / °C

propane C3H8 44 -42 just van der Waals’ forcesethanol C2H5OH 46 +78 van der Waals’ forces + hydrogen bonding

Boiling point is higher for “straight” chain isomers.

bp / °Cbutan-1-ol CH3CH2CH2CH2OH 118butan-2-ol CH3CH2CH(OH)CH3 1002-methylpropan-2-ol (CH3)3COH 83

Greater branching = lower inter-molecular forces

SOLVENT PROPERTIES OF ALCOHOLSSOLVENT PROPERTIES OF ALCOHOLS

SolubilityLow molecular mass alcohols are miscible with waterDue to hydrogen bonding between the two moleculesHeavier alcohols are less miscible

Solventproperties Alcohols are themselves very good solvents

They dissolve a large number of organic molecules

Show the relevant lone pair(s) when drawing hydrogen bonding

CHEMICAL PROPERTIES OF ALCOHOLSCHEMICAL PROPERTIES OF ALCOHOLS

The OXYGEN ATOM HAS TWO LONE PAIRS; this makes alcohols...

BASES Lewis bases are lone pair donors Bronsted-Lowry bases are proton acceptors

The alcohol uses one of its lone pairs to form a co-ordinate bond

NUCLEOPHILES Alcohols can use the lone pair to attack electron deficient centres

ELIMINATION OF WATER (DEHYDRATION)ELIMINATION OF WATER (DEHYDRATION)

Reagent/catalyst conc. sulphuric acid (H2SO4) or conc. phosphoric acid (H3PO4)

Conditions reflux at 180°CProduct alkeneEquation e.g. C2H5OH(l) ——> CH2 = CH2(g) + H2O(l)Mechanism

Step 1 protonation of the alcohol using a lone pair on oxygenStep 2 loss of a water molecule to generate a carbocationStep 3 loss of a proton (H+) to give the alkene

AlternativeMethod Pass vapour over a heated alumina (aluminium oxide) catalyst

ELIMINATION OF WATER (DEHYDRATION)ELIMINATION OF WATER (DEHYDRATION)

MECHANISM

Step 1 protonation of the alcohol using a lone pair on oxygenStep 2 loss of a water molecule to generate a carbocationStep 3 loss of a proton (H+) to give the alkene

Note 1 There must be an H on a carbon atom adjacent the carbon with the OH

Note 2 Alcohols with the OH in the middle of a chaincan have two ways of losing water.

In Step 3 of the mechanism, a proton can be lostfrom either side of the carbocation. This gives amixture of alkenes from unsymmetrical alcohols...

OXIDATION OF ALCOHOLSOXIDATION OF ALCOHOLSAll alcohols can be oxidised depending on the conditions

Oxidation is used to differentiate between primary, secondary and tertiary alcoholsThe usual reagent is acidified potassium dichromate(VI)

Primary Easily oxidised to aldehydes and then to carboxylic acids.

Secondary Easily oxidised to ketones

Tertiary Not oxidised under normal conditions.They do break down with very vigorous oxidation

PRIMARY 1° SECONDARY 2° TERTIARY 3°

OXIDATION OF PRIMARY ALCOHOLSOXIDATION OF PRIMARY ALCOHOLSPrimary alcohols are easily oxidised to aldehydes

e.g. CH3CH2OH(l) + [O] ——> CH3CHO(l) + H2O(l) ethanol ethanal

it is essential to distil off the aldehyde before it gets oxidised to the acid

CH3CHO(l) + [O] ——> CH3COOH(l) ethanal ethanoic acid

OXIDATION OF PRIMARY ALCOHOLSOXIDATION OF PRIMARY ALCOHOLSPrimary alcohols are easily oxidised to aldehydes

e.g. CH3CH2OH(l) + [O] ——> CH3CHO(l) + H2O(l) ethanol ethanal

it is essential to distil off the aldehyde before it gets oxidised to the acid

CH3CHO(l) + [O] ——> CH3COOH(l) ethanal ethanoic acid

Practical details• the alcohol is dripped into a warm solution of acidified K2Cr2O7

• aldehydes have low boiling points - no hydrogen bonding - they distil off immediately• if it didn’t distil off it would be oxidised to the equivalent carboxylic acid• to oxidise an alcohol straight to the acid, reflux the mixture

compound formula intermolecular bonding boiling point ETHANOL C2H5OH HYDROGEN BONDING 78°C

ETHANAL CH3CHO DIPOLE-DIPOLE 23°C

ETHANOIC ACID CH3COOH HYDROGEN BONDING 118°C

OXIDATION OF PRIMARY ALCOHOLSOXIDATION OF PRIMARY ALCOHOLSControlling the products

e.g. CH3CH2OH(l) + [O] ——> CH3CHO(l) + H2O(l)

then CH3CHO(l) + [O] ——> CH3COOH(l)

Aldehyde has a lower boiling point so distils off before being oxidised further

OXIDATION TO ALDEHYDESDISTILLATION

OXIDATION TO CARBOXYLIC ACIDSREFLUX

Aldehyde condenses back into the mixture and gets oxidised to the acid

OXIDATION OF SECONDARY ALCOHOLSOXIDATION OF SECONDARY ALCOHOLSSecondary alcohols are easily oxidised to ketones

e.g. CH3CHOHCH3(l) + [O] ——> CH3COCH3(l) + H2O(l) propan-2-ol propanone

The alcohol is refluxed with acidified K2Cr2O7. However, on prolonged treatment with a powerful oxidising agent they can be further oxidised to a mixture of acids with fewer carbon atoms than the original alcohol.

OXIDATION OF SECONDARY ALCOHOLSOXIDATION OF SECONDARY ALCOHOLSSecondary alcohols are easily oxidised to ketones

e.g. CH3CHOHCH3(l) + [O] ——> CH3COCH3(l) + H2O(l) propan-2-ol propanone

The alcohol is refluxed with acidified K2Cr2O7. However, on prolonged treatment with a powerful oxidising agent they can be further oxidised to a mixture of acids with fewer carbon atoms than the original alcohol.

OXIDATION OF TERTIARY ALCOHOLSOXIDATION OF TERTIARY ALCOHOLSTertiary alcohols are resistant to normal oxidation

OXIDATION OF ALCOHOLSOXIDATION OF ALCOHOLSWhy 1° and 2° alcohols are easily oxidised and 3° alcohols are not

For oxidation to take place easily you must have two hydrogen atoms on adjacent C and O atoms.



H H

R C O + [O] R C O + H2O

H H

1°



H H

R C O + [O] R C O + H2O

H H H H

R C O + [O] R C O + H2O

R R

1°

2°



H H

R C O + [O] R C O + H2O

H H H H

R C O + [O] R C O + H2O

R R

This is possible in 1° and 2° alcohols but not in 3° alcohols.

1°

2°



H H

R C O + [O] R C O + H2O

H H H H

R C O + [O] R C O + H2O

R R

R H

R C O + [O]

R

This is possible in 1° and 2° alcohols but not in 3° alcohols.

1°

2°

3°

ESTERIFICATION OF ALCOHOLSESTERIFICATION OF ALCOHOLS

Reagent(s) carboxylic acid + strong acid catalyst (e.g conc. H2SO4 )Conditions refluxProduct esterEquation e.g. CH3CH2OH(l) + CH3COOH(l) CH3COOC2H5(l) + H2O(l)

ethanol ethanoic acid ethyl ethanoate

Notes Concentrated H2SO4 is a dehydrating agent - it removes watercausing the equilibrium to move to the right and increases the yield

ESTERIFICATION OF ALCOHOLSESTERIFICATION OF ALCOHOLS

Reagent(s) carboxylic acid + strong acid catalyst (e.g conc. H2SO4 )Conditions refluxProduct esterEquation e.g. CH3CH2OH(l) + CH3COOH(l) CH3COOC2H5(l) + H2O(l)

ethanol ethanoic acid ethyl ethanoate

Notes Concentrated H2SO4 is a dehydrating agent - it removes watercausing the equilibrium to move to the right and increases the yield

Uses of esters Esters are fairly unreactive but that doesn’t make them uselessUsed as flavourings

Naming esters Named from the alcohol and carboxylic acid which made them...

CH3OH + CH3COOH CH3COOCH3 + H2O

from ethanoic acid CH3COOCH3 from methanol

METHYL ETHANOATE

OTHER REACTIONS OF ALCOHOLSOTHER REACTIONS OF ALCOHOLS

OXYGEN Alcohols make useful fuelsC2H5OH(l) + 3O2(g) ———> 2CO2(g) + 3H2O(l)

Advantages have high enthalpies of combustion do not contain sulphur so there is less pollution can be obtained from renewable resources

OTHER REACTIONS OF ALCOHOLSOTHER REACTIONS OF ALCOHOLS

OXYGEN Alcohols make useful fuelsC2H5OH(l) + 3O2(g) ———> 2CO2(g) + 3H2O(l)

Advantages have high enthalpies of combustion do not contain sulphur so there is less pollution can be obtained from renewable resources

SODIUMConditions room temperatureProduct sodium alkoxide and hydrogenEquation 2CH3CH2OH(l) + 2Na(s) ——> 2CH3CH2O¯ Na + + H2(g)

sodium ethoxide

Notes alcohols are organic chemistry’s equivalent of waterwater reacts with sodium to produce hydrogen and so do alcoholsthe reaction is slower with alcohols than with water.

Alkoxides are white, ionic crystalline solids e.g. CH3CH2O¯ Na+

BROMINATION OF ALCOHOLSBROMINATION OF ALCOHOLS

Reagent(s) conc. hydrobromic acid HBr(aq) orsodium (or potassium) bromide and concentrated sulphuric acid

Conditions refluxProduct haloalkaneEquation C2H5OH(l) + conc. HBr(aq) ———> C2H5Br(l) + H2O(l)

Mechanism The mechanism starts off similar to that involving dehydration(protonation of the alcohol and loss of water) but the carbocation(carbonium ion) is attacked by a nucleophilic bromide ion in step 3

Step 1 protonation of the alcohol using a lone pair on oxygenStep 2 loss of a water molecule to generate a carbocation (carbonium ion)Step 3 a bromide ion behaves as a nucleophile and attacks the carbocation

INFRA-RED SPECTROSCOPYINFRA-RED SPECTROSCOPY

Chemical bonds vibrate at different frequencies. When infra red (IR) radiation is passed through a liquid sample of an organic molecule, some frequencies are absorbed. These correspond to the frequencies of the vibrating bonds.

Most spectra are very complex due to the large number of bonds present and each molecule produces a unique spectrum. However the presence of certain absorptions can be used to identify functional groups.

BOND COMPOUND ABSORBANCE RANGE

O-H alcohols broad 3200 cm-1 to 3600 cm-1

O-H carboxylic acids medium to broad 2500 cm-1 to 3500 cm-1

C=O ketones, aldehydes strong and sharp 1600 cm-1 to 1750 cm-1

esters and acids

INFRA-RED SPECTROSCOPYINFRA-RED SPECTROSCOPY

IDENTIFYING ALCOHOLS USING INFRA RED SPECTROSCOPY

Differentiation Compound O-H C=OALCOHOL YES NOALDEHYDE / KETONE NO YESCARBOXYLIC ACID YES YESESTER NO YES

ALCOHOL ALDEHYDE CARBOXYLIC ACID PROPAN-1-OL PROPANAL PROPANOIC ACID O-H absorption C=O absorption O-H + C=O absorption

INDUSTRIAL PREPARATION OF ALCOHOLSINDUSTRIAL PREPARATION OF ALCOHOLS

FERMENTATION

Reagent(s) GLUCOSE - produced by the hydrolysis of starch

Conditions yeastwarm, but no higher than 37°C

Equation C6H12O6 ——> 2 C2H5OH + 2 CO2


FERMENTATION

Reagent(s) GLUCOSE - produced by the hydrolysis of starch

Conditions yeastwarm, but no higher than 37°C

Equation C6H12O6 ——> 2 C2H5OH + 2 CO2

Advantages LOW ENERGY PROCESSUSES RENEWABLE RESOURCES - PLANT MATERIALSIMPLE EQUIPMENT

Disadvantages SLOWPRODUCES IMPURE ETHANOLBATCH PROCESS


HYDRATION OF ETHENE

Reagent(s) ETHENE - from cracking of fractions from distilled crude oil

Conditions catalyst - phosphoric acid high temperature and pressure

Equation C2H4 + H2O ——> C2H5OH


HYDRATION OF ETHENE

Reagent(s) ETHENE - from cracking of fractions from distilled crude oil

Conditions catalyst - phosphoric acid high temperature and pressure

Equation C2H4 + H2O ——> C2H5OH

Advantages FASTPURE ETHANOL PRODUCEDCONTINUOUS PROCESS

Disadvantages HIGH ENERGY PROCESSEXPENSIVE PLANT REQUIREDUSES NON-RENEWABLE FOSSIL FUELS TO MAKE ETHENE

Uses of ethanol ALCOHOLIC DRINKSSOLVENT - industrial alcohol / methylated spiritsFUEL - petrol substitute in countries with limited oil reserves

USES OF ALCOHOLSUSES OF ALCOHOLS

ETHANOLDRINKSSOLVENT industrial alcohol / methylated spirits (methanol is added)FUEL used as a petrol substitute in countries with limited oil reserves

METHANOL

PETROL ADDITIVE improves combustion properties of unleaded petrolSOLVENTRAW MATERIAL used as a feedstock for important industrial processesFUEL

Health warning Methanol is highly toxic

LABORATORY PREPARATION OF ALCOHOLSLABORATORY PREPARATION OF ALCOHOLS

from haloalkanes - reflux with aqueous sodium or potassium hydroxide

from aldehydes - reduction with sodium tetrahydridoborate(III) - NaBH4

from alkenes - acid catalysed hydration using concentrated sulphuric acid

Details of the reactions may be found in other sections.

REVISION CHECKREVISION CHECKWhat should you be able to do?

Recall and explain the physical properties of alcohols

Recall the different structural types of alcohols

Recall the Lewis base properties of alcohols

Recall and explain the chemical reactions of alcohols

Write balanced equations representing any reactions in the section

Understand how oxidation is affected by structure

Recall how conditions and apparatus influence the products of oxidation

Explain how infrared spectroscopy can be used to differentiate between functional groups

CAN YOU DO ALL OF THESE? CAN YOU DO ALL OF THESE? YES YES NONO

You need to go over the You need to go over the relevant topic(s) againrelevant topic(s) again

Click on the button toClick on the button toreturn to the menureturn to the menu

WELL DONE!WELL DONE!Try some past paper questionsTry some past paper questions

© 2009 JONATHAN HOPTON & KNOCKHARDY PUBLISHING© 2009 JONATHAN HOPTON & KNOCKHARDY PUBLISHING

THE ENDTHE END

AN INTRODUCTION TOAN INTRODUCTION TO

THE CHEMISTRYTHE CHEMISTRYOF ALCOHOLSOF ALCOHOLS

Alcohols Knockhardy

Documents

Transcript of Alcohols Knockhardy