The Mechanisms of Electrophilic Addition Reactions (HL) (DP IB Chemistry): Revision Note

Philippa Platt

Written by: Philippa Platt

Reviewed by: Richard Boole

Updated on

The mechanisms of electrophilic addition reactions

Electrophilic addition

  • Electrophilic addition is a reaction in which an electrophile (or Lewis acid) adds across the C=C double bond of an alkene

  • The C=C bond is an area of high electron density

    • This makes it susceptible to attack by electrophiles

  • The π bond in the double bond breaks, forming:

    • A single C–C bond

    • Two new σ-bonds from each carbon atom

  • Electrophilic addition reactions include the addition of:

    • Hydrogen, H2 (g) - catalytic hydrogenation

    • Steam, H2O (g) - hydration of alkenes

    • Hydrogen halides, HX - formation of halogenoalkanes

    • Halogens, X2 - formation of dihalogenoalkanes

Four chemical reactions of alkenes: hydrogenation to alkane, steam to alcohol, hydrogen halides to halogenoalkane, halogens to dihalogenoalkane.
Overview of the main alkene electrophilic addition reactions

Examiner Tips and Tricks

The IB Chemistry Guide states that you need to be able to describe and explain the electrophilic addition mechanisms for symmetrical alkenes with:

  • Halogens

  • Water

  • Hydrogen halides

Hydrogenation is assumed prior knowledge, no mechanism is required.

Addition of steam (H2O)

  • Water is a weak electrophile

  • Water does not readily react with alkenes without a strong acid catalyst

    • H3O+ acts as the electrophile

  • The electrophilic addition of water occurs in two steps:

    • Step 1

      • The π electrons in the C=C attack a proton from H3O+

      • Heterolytic fission occurs and a carbocation is formed

    • Step 2

      • Water donates a lone pair of electrons to the carbocation 

      • This forms a protonated alcohol (oxonium ion)

      • An equilibrium is established between the protonated alcohol and the alcohol

      • This regenerates the H3O+ catalyst

Electrophilic addition of H2O mechanism

Chemical reaction mechanism of ethene with water in two steps: slow addition forming a carbocation, followed by fast hydration, yielding ethanol.
The electrophilic addition of water is catalysed by strong acid

Addition of hydrogen halides (HX)

  • Hydrogen halides such as HBr are permanently polar

    • This is due to the electronegativity difference between H and the halogen

  • In a hydrogen bromide molecule, the bromine atom has a stronger pull on the electrons in the H-Br bond

  • This causes:

    • The Br atom to have a partial negative charge

    • The H atom to have a partial positive charge

H-Br bond diagram. H is δ+, electrophile, less electronegative. Br is δ-, attracts electrons, more electronegative. Arrows indicate electron flow.
HBr is a polar molecule due to electronegativity
  • The electrophilic addition of hydrogen halides occurs in two steps:

    • Step 1

      • The π electrons in the C=C attack the δ⁺ hydrogen atom in HBr

      • Heterolytic fission occurs forming a carbocation intermediate and a bromide ion

    • Step 2

      • The bromide ion donates a lone pair of electrons to the carbocation

      • This forms the halogenoalkane product

Diagram illustrating electrophilic addition of HBr to ethene forming bromomethane, showing electron movement and formation of primary carbocation.
Electrophilic addition reaction of HBr and ethene to form bromoethane 

Examiner Tips and Tricks

  • For electrophilic addition mechanisms, the curly arrows must:

    • Be double-headed to show the movement of an electron pair

    • Start from a lone pair or a region of high electron density (e.g. a C=C bond)

    • Point towards a δ⁺ atom (electrophile) or a positive charge (e.g. carbocation)

  • Examiners often comment on incorrect or careless use of curly arrows in organic mechanisms

    • Arrows must be positioned and directed precisely

Addition of halogens (X2)

  • Halogen molecules like Br2 are non-polar

  • They become polarised when they approach the high electron density of a C=C bond

    • This induces a temporary dipole in the Br–Br bond

    • One Br atom becomes slightly δ⁺ and the other δ⁻

Diagram showing a non-polar bromine molecule with an induced dipole by a carbon-carbon double bond, indicating areas of high electron density.
Br₂ is a non-polar molecule, but it becomes polarised when it approaches the high electron density of a C=C bond
  • The electrophilic addition of bromine occurs in two steps:

    • Step 1

      • The π electrons in the C=C attack the δ⁺ bromine atom in Br2

      • Heterolytic fission occurs forming a brominated carbocation intermediate and a bromide ion

    • Step 2

      • The bromide ion donates a lone pair of electrons to the carbocation

      • This forms the 1,2-dibromoalkane product

Diagram showing the reaction of ethene with bromine forming a primary carbocation intermediate and resulting in dibromoethane.
Electrophilic addition reaction of bromine and ethene to form 1,2-dibromoethane 

Examiner Tips and Tricks

  • The electrophilic addition mechanisms for halogens and hydrogen halides are similar

  • The key difference is that:

    • Hydrogen halides are permanently polar

    • Halogens are non-polar and rely on temporary induced dipoles

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Philippa Platt

Author: Philippa Platt

Expertise: Chemistry Content Creator

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

Richard Boole

Reviewer: Richard Boole

Expertise: Chemistry Content Creator

Richard has taught Chemistry for over 15 years as well as working as a science tutor, examiner, content creator and author. He wasn’t the greatest at exams and only discovered how to revise in his final year at university. That knowledge made him want to help students learn how to revise, challenge them to think about what they actually know and hopefully succeed; so here he is, happily, at SME.

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