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Chapter 6: Problem 13

Discuss Lewis concept of acids and bases.

Short Answer

Expert verified
The Lewis concept of acids and bases is an extension of the traditional definition of acids and bases. It defines a Lewis acid as a species that can accept an electron pair and a Lewis base as a species that can donate an electron pair. This concept includes a wider range of substances that can act as acids or bases. It is useful in explaining a broad range of chemical reactions, including those that do not involve protons, by focusing on the movement of electron pairs.

Step by step solution

01

Define Lewis Acids and Lewis Bases

A Lewis acid is a species that can accept an electron pair, whereas a Lewis base is a species that can donate an electron pair. This concept is much broader than the traditional definition of acids and bases and includes more substances that can act as acids or bases. Except hydrogen ions, other positively charged ions, or cations, can also act as Lewis acids, such as Fe3+ and Al3+. At the same time, molecules with at least one lone pair of electrons can behave as Lewis bases, such as NH3 and H2O.
02

Discuss typical examples of Lewis acid-base reactions

Consider the reaction between NH3 (ammonia) and BF3 (boron trifluoride): \[ BF3 + NH3 \rightarrow F3B:NH3 \] Here, the ammonia (NH3) donates a lone pair of electrons to the boron in boron trifluoride (BF3), forming a dative covalent bond (also called a coordinate bond). Therefore, according to the Lewis concept, BF3 acts as an acid and NH3 acts as a base in this reaction.
03

Discuss the importance of Lewis concept

The Lewis concept is particularly useful because it extends our ability to talk about reactions, beyond just protons and hydroxide ions, by focusing on the movement of electron pairs. This makes the concept widely applicable to a broad range of chemical reactions, including those that do not involve protons at all.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Lewis acids
In chemistry, Lewis acids are species that have the capability to accept an electron pair. This is a broader concept than traditional acids, which are usually defined by their ability to donate protons. Lewis acids often include metal cations like \( Fe^{3+} \) and \( Al^{3+} \), which have vacant orbitals to accommodate extra electrons.
  • Not limited to protons, which allows for a wider range of chemical interactions.
  • Includes substances with incomplete octets, such as \( BF_3 \) (boron trifluoride) and \( AlCl_3 \) (aluminum chloride).
The flexibility of the Lewis definition makes it highly applicable in coordination chemistry and catalytic processes.
Lewis bases
Conversely, Lewis bases are species capable of donating an electron pair. These typically feature atoms with lone pairs of electrons that are not engaged in bonding. Typical examples include ammonia \( NH_3 \) and water \( H_2O \), both of which have lone pairs available for donation.
Unlike the traditional Br酶nsted-Lowry bases that accept protons, Lewis bases provide a perspective that centers around electron pair dynamics.
  • Substances with lone pairs, such as halides, can act as Lewis bases.
  • Able to interact with a broader range of species, not just acids involving hydrogen ions.
This gives Lewis bases a crucial role in various chemical reactions, particularly in forming complex ions.
Dative covalent bond
A dative covalent bond, also known as a coordinate bond, forms when a Lewis base donates a pair of electrons to a Lewis acid. This shared electron pair creates a stable bond between the two species. An illustrative example is the reaction between ammonia \( NH_3 \) and boron trifluoride \( BF_3 \):
\[ BF_3 + NH_3 \rightarrow F_3B:NH_3 \] Here, the lone pair from \( NH_3 \) (ammonia) creates a bond with \( BF_3 \) (boron trifluoride), a classic scenario where a dative bond is formed.
This bond type is essential in many coordination compounds and complexes.
Chemical reactions
Chemical reactions under the Lewis acid-base theory encompass interactions where electron pairs are transferred. Unlike other acid-base theories focusing solely on protons, Lewis's concept is especially meaningful in understanding reactions that involve metals and nonmetals.
It simplifies our understanding of how different molecules and ions can react by centering on electron pairs. This viewpoint reveals a broader scope of reactions, such as those found in organometallic chemistry and inorganic reactions involving transition metals.
Electron pair donor and acceptor
The essence of the Lewis acid-base theory lies in its ability to classify species based on their electron pair interactions. A Lewis acid is an electron pair acceptor, while a Lewis base is an electron pair donor.
  • This focus on electron movement expands the traditional view of acids and bases by including a variety of species.
  • Compounds with incomplete electron shells (electron-deficient) typically act as electron pair acceptors.
  • Molecules with available lone pairs often serve as donors, facilitating wide-ranging reactions.
Consequently, this framework enhances our ability to predict and understand a vast array of chemical processes.

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Most popular questions from this chapter

Discuss Bronsted-Lowry concept of acids and bases. What are its uses?

What do you mean by auto-ionisation? Illustrate your answer with the help of suitable examples.

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