General chemistryLesson 1 of 1 in the course Equilibria of Other Reaction Classes

Lewis Acid–Base Reactions and Complex-Ion Equilibria

5 flashcards · 5 quiz questions · 5 match pairs · 5 fill-in sentences · English

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Summary

In 1923, G. N. Lewis proposed a broad way to describe acid–base reactions: acids accept electron pairs, while bases donate them. This definition includes familiar reactions involving hydrogen ions, as well as reactions where no proton is transferred.

A coordinate covalent bond, also called a dative bond, is a covalent bond in which both shared bonding electrons are supplied by one atom. After the bond forms, it behaves as a covalent bond; the term describes how the bond's electron pair was supplied.

All flashcards

What is a Lewis acid?
A species that accepts an electron pair to form a bond.
What is a Lewis base?
A species that donates an electron pair, commonly from a lone pair.
What is a coordinate covalent bond?
A covalent bond whose shared electron pair is supplied by one atom.
What is a Lewis acid–base adduct?
The product formed when a Lewis acid and base become bonded.
How are formation and dissociation constants related?
For a reaction and its reverse, the dissociation constant is the reciprocal of the formation constant.

Quiz questions

  1. Why can BF₃ act as a Lewis acid?Answer: Boron has an incomplete valence shell and can accept an electron pair.
  2. How does Lewis theory classify Brønsted–Lowry proton-transfer reactions?Answer: They are a subset of Lewis reactions, with H⁺ accepting an electron pair.
  3. For a complex-forming reaction and its reverse, how are KfK_f and KdK_d related?Answer: Kd=1/KfK_d = 1/K_f
  4. Why can adding ammonia promote the dissolution of AgCl in water?Answer: Ammonia complexes dissolved Ag⁺, lowering its free concentration and prompting more AgCl to dissolve.
  5. In the formation reaction Cu⁺ + 2 CN⁻ ⇌ Cu(CN)₂⁻, what power applies to [CN⁻] in the KfK_f expression?Answer: The cyanide concentration is raised to the second power.

Based on Chemistry 2e by Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson, PhD (OpenStax), licensed CC BY 4.0. Adapted into a summary, flashcards and quizzes.

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