Oxidation of Alcohols (Oxford AQA International A Level Chemistry)

Revision Note

Philippa Platt

Written by: Philippa Platt

Reviewed by: Stewart Hird

Classification of Alcohols

  • Alcohols are compounds that contain at least one hydroxy (-OH) group

  • The general formula of alcohols is CnH2n+1OH

  • They can be classed as primary, secondary and tertiary

Primary alcohols

  • A primary alcohol contains a carbon atom, bonded to the -OH group, which is attached to one other carbon atom (or alkyl group)

A diagram to show a secondary alcohol
In a primary alcohol, the O-H group is bonded to a carbon atom which is bonded to one other carbon atom in the chain

Secondary alcohols

  • A secondary alcohol contains a carbon atom, bonded to the -OH group, that is attached to two other carbon atoms (or alkyl groups)

A diagram to show a secondary alcohol
In a secondary alcohol, the O-H group is bonded to a carbon atom which is bonded to two other carbon atoms in the chain

Tertiary alcohols

  • A tertiary alcohol contains a carbon atom, bonded to the -OH group, that is attached to three other carbon atoms (or alkyl groups)

A diagram to show a tertiary alcohol
In a tertiary alcohol, the O-H group is bonded to a carbon atom that is bonded to three other carbon atoms

Oxidation of Alcohols

  • Primary alcohols can be oxidised to form aldehydes which can undergo further oxidation to form carboxylic acids

  • Secondary alcohols can be oxidised to form ketones only

  • Tertiary alcohols do not undergo oxidation

  • The oxidising agent of alcohols is acidified potassium dichromate(VI), K2Cr2O7 

  • The colour change is from orange to green

    • For potassium dichromate(VI) to act as an oxidising agent, it itself needs to be reduced

    • This reduction requires hydrogen (H+) ions which are provided by an acid, typically sulfuric acid

    • When alcohols are oxidised, the orange dichromate ions (Cr2O72-) are reduced to green Cr3+ ions

Primary alcohols

Oxidation of primary alcohols

oxidation

Formation of a carboxylic acid (using ethanol)

  • This reaction is performed using reflux apparatus

  • A primary alcohol, such as ethanol, is added to the oxidising agent and warmed

CH3CH3OH (l) + 2[O] → CH3COOH (g) + H2O (l)

Heating under Reflux
Ethanol and ethanal vapour condense and drip back into the reaction flask until it is all oxidised. Ethanoic acid can then be distilled off

Formation of an aldehyde (using ethanol)

  • This reaction is performed using distillation apparatus

  • A primary alcohol, such as ethanol, is added to the oxidising agent and warmed

  • The aldehyde product has a lower boiling point than the alcohol reactant so it can be distilled off as soon as it forms 

CH3CH2OH (l) + [O] → CH3CHO (g) + H2O (l)

distillation-with-addition
If the aldehyde is not distilled off, further refluxing with excess oxidising agent will oxidise it to a carboxylic acid

Secondary alcohols

Oxidation of Secondary Alcohols

Hydroxy Compounds Oxidation of Secondary Alcohols, downloadable AS & A Level Chemistry revision notes
  • Secondary alcohols, such as propan-2-ol, are oxidised to ketones

  • Since ketones cannot be further oxidised, the ketone product does not need to be distilled off straight away after it has been formed

CH3CH(OH)CH3 (l) + [O] → CH3COCH3 (g) + H2O (l)

Tertiary alcohols

  • Tertiary alcohols do not undergo oxidation

    • This is because there must be a hydrogen on the functional group carbon, which breaks off to form water

    • There are only C-C bonds on the functional group carbon in a tertiary alcohol

Distinguishing Between Aldehydes and Ketones

  • Aldehydes can be oxidised further to carboxylic acids

  • Ketones can not be oxidised

  • This difference allows us to use chemical tests to distinguish between aldehydes and ketones

Fehling’s solution

  • Fehling’s solution is an alkaline solution containing copper(II) ions which act as the oxidising agent

  • When warmed with an aldehyde, the aldehyde is oxidised to a carboxylic acid and the Cu2+ ions are reduced to Cu+ ions 

Cu2+ + e- → Cu+

  • The clear blue solution turns opaque due to the formation of a red precipitate of copper(I) oxide

  • Ketones cannot be oxidised and therefore give a negative test when warmed with Fehling’s solution

Carbonyl Compounds Fehlings Solution,
The positive test for an aldehyde is a brick-red precipitate

Tollens’ reagent

  • Tollens' reagent is an aqueous alkaline solution of silver nitrate in excess ammonia solution

    • Tollens' reagent is also called ammoniacal silver nitrate solution

  • When warmed with an aldehyde, the aldehyde is oxidised to a carboxylic acid and the Agions are reduced to Ag atoms

Ag+ + e- → Ag

  • The Ag atoms form a silver ‘mirror’ on the inside of the tube

  • Ketones cannot be oxidised and therefore give a negative test when warmed with Tollens’ reagent

Carbonyl Compounds Tollens Reagent,
The positive test for an aldehyde is the formation of a silver mirror

Examiner Tips and Tricks

Make sure you can write equations using [O] to represent the oxidising agent in these reactions. The equation must still be balanced!

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Philippa Platt

Author: Philippa Platt

Expertise: Chemistry

Philippa has worked as a GCSE and A level chemistry teacher and tutor for over thirteen years. She studied chemistry and sport science at Loughborough University graduating in 2007 having also completed her PGCE in science. Throughout her time as a teacher she was incharge of a boarding house for five years and coached many teams in a variety of sports. When not producing resources with the chemistry team, Philippa enjoys being active outside with her young family and is a very keen gardener

Stewart Hird

Author: Stewart Hird

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Topic Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.