Relative Rates of Nucleophilic Substitution (HL) (DP IB Chemistry): Revision Note

Philippa Platt

Written by: Philippa Platt

Reviewed by: Richard Boole

Updated on

Relative rates of nucelophilic substitution

  • Various factors affect the rate of nucleophilic substitution of a halogenoalkane:

    1. The nature of the nucleophile

    2. The halogen involved (leaving group)

    3. The structure (class) of the halogenoalkane

  • This is regardless of whether it is SN1 or SN2

1. The nature of the nucleophile

  • The strength of a nucleophile depends on how readily it can donate a lone pair of electrons to the δ⁺ carbon atom in a halogenoalkane

  • Two key factors influence this:

    • Charge: Negatively charged species are stronger nucleophiles than their neutral counterparts

      • For example, OH- is stronger than H2O

    • Electronegativity: When species have the same charge, the species with a lower electronegativity are stronger nucleophiles

      • For example, NH3 is stronger than H2O because nitrogen holds its lone pair less tightly than oxygen

  •  The effectiveness of nucleophiles is:

Strongest     CN- > OH- > NH3 > H2O     Weakest

2. The halogen involved (leaving group)

  • Substitution reactions involve breaking the carbon–halogen (C–X) bond

  • The weaker the bond, the faster the reaction

    • This is because less energy is required for the halogen to leave

  • This helps explain why different halogenoalkanes react at different rates

Relative bond energies of halogenoalkanes

  • The approximate bond energies for different carbon–halogen bonds are:

    • C–F: 492 kJ mol-1 (strongest bond)

    • C–Cl: 324 kJ mol-1

    • C–Br: 285 kJ mol-1

    • C–I: 228 kJ mol-1 (weakest bond)

  • The C–I bond is the weakest and requires the least energy to break

    • So, in substitution reactions this bond breaks heterolytically:

R3C-I + OH- → R3C-OH + I-

  • The C-F bond is the strongest and requires the most energy to break

    • So, fluoroalkanes are less likely to undergo substitution reactions

Halogenoalkane precipitate colours

  • When different halogenoalkanes undergo nucleophilic substitution, the halide ions released can be detected using aqueous silver nitrate

  • Each halide forms a characteristic precipitate, except fluoride:

    • Fluoride (F-) → no visible precipitate because silver fluoride is soluble in water

    • Chloride (Cl-) → white precipitate of silver chloride (AgCl)

    • Bromide (Br-) → cream precipitate of silver bromide (AgBr)

    • Iodide (I-) → yellow precipitate of silver iodide (AgI)

Three test tubes with blue liquid show white, cream, and yellow precipitates, labelled respectively, on a rack.
The white AgCl, cream AgBr and yellow AgI precipitates formed by the halide ions
  • The pale yellow silver iodide forms most quickly, indicating that

    • Iodide ions are released fastest

    • Iodoalkanes are the most reactive

  • No visible precipitate is formed with fluoroalkanes, indicating that:

    • Fluoride ions are not easily released

    • Fluoroalkanes are the least reactive

  • This confirms the relative reactivity of the halogenoalkanes:

Reactivity order of haloalkanes: Fluoroalkanes (least reactive) to Iodoalkanes (most reactive) shown with downward arrow.
The trend in reactivity of halogenoalkanes

3. The class of halogenoalkane

  • The classes of halogenoalkane are:

    • Primary

    • Secondary

    • Tertiary

Diagram illustrating primary, secondary, and tertiary halogenoalkanes with structures; X denotes a halogen.
The number of alkyl groups attached determines if the halogenoalkane is primary, secondary or tertiary
  • Primary halogenoalkanes undergo SN2 reactions

    • They do not form carbocations

    • Nucleophiles attack directly, displacing the halide in a single step

  • Secondary halogenoalkanes can undergo either SN1 or SN2 reactions

    • The preferred mechanism depends on:

      • The solvent

      • The temperature

      • The nucleophile involved

  • Tertiary halogenoalkanes undergo SN1 reactions

    • They form stable tertiary carbocations

Carbocation stability

  • The stability of a carbocation increases with the number of alkyl groups attached to the positively charged carbon

    • This is due to the positive inductive effect

    • This is where alkyl groups push electron density towards the positively charged carbon, reducing its charge density

  • Tertiary carbocations have three alkyl groups stabilising the charge, while primary ones have only one

  • This difference in stability influences how easily the carbocation forms, and the rate of reaction

Primary, secondary and tertiary carbocations

Diagram showing primary, secondary, and tertiary carbocations with increasing stability from left to right
The diagram shows the trend in the stability of primary, secondary and tertiary carbocations
  • This trend is relevant for SN1 reactions, which involve carbocation intermediates

    • Tertiary halogenoalkanes form the most stable carbocations and react fastest by the SN1 mechanism

    • Primary halogenoalkanes react by the SN2 mechanism and do not form carbocations, but are included here for comparison

  • In SN1 reactions, the formation of a carbocation depends on the class of halogenoalkane

    • Only tertiary halogenoalkanes form stable carbocations, making SN1 the preferred pathway

  • This directly influences the rate-determining step, which controls the overall rate of nucleophilic substitution

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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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