Lewis Acids & Bases (HL) (DP IB Chemistry): Revision Note

Philippa Platt

Last updated

Lewis Acids & Bases

  • A more general definition of acids and bases was given by G.N. Lewis:

    • A Lewis acid is an lone pair acceptor

    • A Lewis base is an lone pair donor

  • This enabled a wider range of substances to be classed as acids or bases, beyond those that donate or accept protons

Lewis acid and base interactions

  • The interaction between a Lewis acid and base can be shown as:

A+ + :B- → A←:B

  • A coordinate covalent bond forms when the Lewis base donates a lone pair of electrons to the Lewis acid

  • Lewis theory is broader than Brønsted–Lowry theory because it includes reactions that do not involve proton transfer

  • Some species, such as OH- and NH3, act as both types of base:

    • As Lewis bases they donate a lone pair of electrons

    • As Brønsted–Lowry bases they accept a proton

Diagram to show how OH and ammonia act as Lewis bases

Hydroxide ion and ammonia acting as Lewis bases
The OH– ion and ammonia act as Lewis bases in both examples by donating a lone pair of electrons

Comparing Lewis and Brønsted–Lowry acid-base theory

  • Brønsted-Lowry acid is a species that can donate H+

  • For example, hydrogen chloride (HCl) is a Brønsted-Lowry acid as it can donate a H+ ion

HCl (aq) → H+ (aq) + Cl– (aq)

  • Lewis acids are any species that are able to accept a lone pair of electrons

    • This includes H⁺

  • This means Lewis theory covers a broader spectrum than Brønsted–Lowry acids

  • Brønsted-Lowry theory strictly defines acids as H+ donors only

    • Not all acid–base reactions involve proton transfer

    • This is where Lewis theory is more broadly applicable

  • A Brønsted-Lowry base is a species that can accept H+

    • For example, a hydroxide (OH) ion is a Brønsted-Lowry base as it can accept H+ to form water

H+ (aq) + OH- (aq) → H2O (l)

  • Lewis bases and Brønsted-Lowry bases are in the same group of chemicals because they both must have a lone pair of electrons 

    • Lewis bases donate a lone pair of electrons

    • Brønsted-Lowry bases accept a proton vis their lone pair of electrons

  • Examples of chemicals that can act as Lewis bases and Brønsted-Lowry bases include:

    • Hydroxide, OH-

    • Cyanide, CN-

    • Methylamine, CH3NH2

Hydroxide ion, cyanide ion, and methylamine molecule are shown with chemical structures and electron dot diagrams.
These species can act as both Lewis bases and Brønsted–Lowry bases
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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

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