alcohol chemistry of -oh 5/12/2015dr seemal jelani1
TRANSCRIPT
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ALCOHOL
Chemistry of -OH
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Alcohols
Butan - 1, 4 - diol
Butan- 1- ol
Propan- 2- ol
Propan- 1- ol
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These all have the formula C4H9OH
butan-1-ol butan-2-ol
2-methylpropan-1-ol2-methylpropan-2-ol
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Bond angles in alcohol groups
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Solubility in water
The alcohol groups form hydrogen bonding which makes the short chain molecules soluble in water.
The solubility in water decreases as the chain length increases.
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Low-mass alcohols are soluble in water (because they hydrogen bond with water).
As the hydrocarbon chain lengthens, the solubility decreases.
Ethanol Propan-1-ol Butan-1-ol
This photo shows ethanol, propan-1-ol and butan-1-ol in water. The first two are completely miscible in water, while butan-1-ol is not miscible in water.
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Boiling Points of Alcohols
Increases with molecular size due to increased instantaneous dipoles
• Alcohols have higher boiling points than similar molecular mass alkanes
•This is due to the added presence of inter-molecular hydrogen bonding
• More energy is required to separate the molecules
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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
Structuraldifferences • Alcohols are classified according to the environment of
the OH group
• Chemical behaviour, e.g oxidation, often depends on the
structural type
NB. Aliphatic - straight chain molecule (not a ring / cyclic)
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PRIMARY 1° SECONDARY 2° TERTIARY 3°
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Luca’s Reagent
• Solution of anhydrous zinc chloride in concentrated hydrochloric acid
• This solution is used to classify alcohols of low molecular weight.
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Distinguishing alcohols
Lucas reagent can be used to distinguish between low mass primary, secondary and tertiary alcohols.
Lucas reagent contains anhydrous zinc chloride dissolved in concentrated hydrochloric acid. It contains a very high concentration of chloride ions and the Zn2+ ion acts as a catalyst.
Take 1–2 mL of Lucas reagent in a dry test tube, add a few drops of the alcohol and shake. If there is no reaction, place the test tube in a beaker of boiling water for a few minutes.
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Distinguishing alcohols - Lucas test
Primary alcohol - remain unchanged
tertiary alcohol - turns cloudy immediately
Secondary alcohol - will turn cloudy but takes a bit of time
Lucas reagent = conc. HCl and ZnCl2
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Tertiary alcohols turn cloudy immediately.
Once heated, the secondary alcohol quickly turned cloudy.
The primary alcohol tube is unchanged.
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OXIDATION OF PRIMARY ALCOHOLSOXIDATION OF PRIMARY ALCOHOLS
Primary 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
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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 oxidize 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
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Oxidising a primary alcohol to an aldehyde
Full oxidation is not wanted:
use dilute acid and less dichromate. The reaction mixture is heated gently,
ethanal vapourises (21°C) as soon as it is formed and distils over. This stops it being oxidised further to ethanoic acid.
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Apparatus for the oxidation of ethanol to ethanoic acid
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Oxidising a primary alcohol to a carboxylic acid
reflux Distil to separate
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Oxidising a secondary alcohol to a ketone
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Oxidation of alcohols
Primary and secondary alcohols are oxidised by acidified potassium dichromate.
A beaker of hot water speeds up the reaction.
There is no reaction with tertiary alcohols.
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Oxidation of alcohols
Primary alcohols
tertiary alcohol
Secondary alcohol
aldehydes
Carboxylic acid
Don’t oxidise
Ketones
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Formation of ethanol by fermentation
Conditions yeastwarm, but no higher than 37°C (optimum temp. for
yeast)
Advantages LOW ENERGY PROCESSUSES RENEWABLE RESOURCES - PLANT MATERIALSIMPLE EQUIPMENT
Disadvantages SLOWPRODUCES IMPURE ETHANOL - will need distilling to purifyBATCH PROCESS
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Formation of haloalkane
Ethanol and PCl5
C2H5OH(l) + PCl5(s) C2H5Cl(g) + POCl3(l) + HCl(g)fumes
solid
Ethanol and SOCl2
C2H5OH(l) + SOCl2(l) C2H5Cl(g) + SO2(g) + HCl(g)
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Phosphoryl chloride
Thionyl chloride
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Formation of ethanol from ethene
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
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Dehydration of alcohols
Reagent: concentrated sulphuric acid
or passing the alcohol over aluminium oxide
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Reaction with sodium
The reaction is similar to the reaction of alkali metals with water, but less vigorous.
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Esterification
Catalyst: concentrated H2SO4 (dehydrating agent - it removes water causing the equilibrium to move to the right and increases the yield
Conditions: reflux
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Uses of esters Esters are fairly unreactive but that doesn’t make them useless
Used 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
Esters
Ethanoate Methyl
Methyl Ethanoate
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