G.N. Lewis

Definition

G.N. Lewis was a renowned American chemist who developed the Lewis definition of acids and bases, which expanded upon the earlier Brønsted-Lowry definition. The Lewis definition provides a more general framework for understanding acid-base reactions by focusing on the transfer of electron pairs rather than just protons.

5 Must Know Facts For Your Next Test

1. The Lewis definition of acids and bases is based on the concept of electron-pair donation and acceptance, rather than just the transfer of protons.
2. According to the Lewis definition, an acid is a species that can accept a pair of electrons, while a base is a species that can donate a pair of electrons.
3. The Lewis definition is more general than the Brønsted-Lowry definition, as it can be applied to a wider range of chemical reactions, including those that do not involve the transfer of protons.
4. The Lewis definition is particularly useful in understanding the behavior of metal ions and complex ions in acid-base reactions, which are not easily explained by the Brønsted-Lowry definition.
5. The Lewis definition has been widely adopted in modern chemistry and is an essential concept for understanding the nature of acid-base reactions and the properties of chemical species.

Review Questions

• Explain how the Lewis definition of acids and bases differs from the Brønsted-Lowry definition.
  • The key difference between the Lewis and Brønsted-Lowry definitions of acids and bases is the focus on the transfer of electron pairs rather than just protons. The Brønsted-Lowry definition defines acids as proton donors and bases as proton acceptors, while the Lewis definition defines acids as electron pair acceptors and bases as electron pair donors. This allows the Lewis definition to be applied to a wider range of chemical reactions, including those that do not involve the transfer of protons, such as the formation of coordination complexes.
• Describe the role of electron-pair sharing in the Lewis definition of acid-base reactions.
  • In the Lewis definition, acid-base reactions are characterized by the sharing of an electron pair between the acid (electron pair acceptor) and the base (electron pair donor). This electron-pair sharing results in the formation of a new bond, which stabilizes both the acid and the base. The ability of a species to accept or donate an electron pair is the key factor in determining whether it is a Lewis acid or a Lewis base, rather than its ability to donate or accept protons as in the Brønsted-Lowry definition.
• Analyze the advantages of the Lewis definition of acids and bases over the Brønsted-Lowry definition, particularly in the context of understanding the behavior of metal ions and complex ions.
  • The Lewis definition of acids and bases is more general and versatile than the Brønsted-Lowry definition, as it can be applied to a wider range of chemical reactions, including those involving metal ions and complex ions. The Brønsted-Lowry definition is limited to the transfer of protons, which can be insufficient to explain the behavior of species that do not readily donate or accept protons. In contrast, the Lewis definition focuses on the transfer of electron pairs, which allows for a better understanding of the reactivity and properties of metal ions and complex ions, which often participate in acid-base reactions through the formation of coordination complexes. This makes the Lewis definition a more powerful and comprehensive tool for analyzing and predicting the behavior of a diverse range of chemical species in acid-base reactions.

Related terms

Lewis Acid: A Lewis acid is a species that can accept a pair of electrons, forming a new bond and increasing its electron pair count.

Lewis Base: A Lewis base is a species that can donate a pair of electrons, forming a new bond and decreasing its electron pair count.

Electron-Pair Sharing: The process by which Lewis acids and bases form a new bond through the sharing of an electron pair, resulting in the stabilization of both species.