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Chapter 16: Problem 71

What is the essential structural feature of all Br酶nstedLowry bases?

Short Answer

Expert verified
The essential structural feature of all Br酶nsted-Lowry bases is the presence of a lone pair of electrons on a highly electronegative atom, such as oxygen or nitrogen, which allows the base to attract and bond with a proton (H+ ion).

Step by step solution

01

Definition of Br酶nsted-Lowry Acid-Base Theory

The Br酶nsted-Lowry acid-base theory is a definition of acids and bases that characterizes them based on their ability to donate or accept protons (H+ ions). In this theory, an acid is a substance that donates a proton, and a base is a substance that accepts a proton.
02

Understanding Br酶nsted-Lowry Bases

According to the Br酶nsted-Lowry acid-base theory, a base is a substance that has the ability to accept a proton (H+ ion). This means that a Br酶nsted-Lowry base must have a part of its structure that can attract or bond with a proton.
03

Essential Structural Feature of Br酶nsted-Lowry Bases

The essential structural feature of all Br酶nsted-Lowry bases is the presence of a lone pair of electrons that can form a bond with a proton (H+ ion). This lone pair of electrons, typically present on a highly electronegative atom such as oxygen or nitrogen, allows the base to attract and bond with a proton, thereby accepting it.

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Key Concepts

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

Proton Acceptor
In the context of the Br酶nsted-Lowry acid-base theory, a fundamental property of a base is its ability to act as a proton acceptor. A proton, represented as an H鈦� ion, is simply a hydrogen atom that has lost its electron, leaving it with just a single proton in its nucleus. When a base accepts a proton, it forms a covalent bond with this H鈦� ion. Understanding this role as a proton acceptor is crucial to identifying substances that can act as bases in chemical reactions. By accepting protons, bases help to neutralize acids, which are proton donors.
Lone Pair of Electrons
One of the key features that allow Br酶nsted-Lowry bases to accept protons is the presence of a lone pair of electrons. Lone pairs are unshared pairs of electrons that are not involved in bonding. These electrons are often found on non-metal atoms within a molecule. Because they are not bonded, these lone pairs are available to form new bonds, such as when a base accepts a proton. This interaction is critical because the lone pair electrons are used to form a covalent bond with the proton, effectively integrating the proton into the molecular structure of the base.
Electronegative Atoms
Electronegative atoms like nitrogen and oxygen are central to the behavior of Br酶nsted-Lowry bases. These atoms tend to attract electrons strongly, contributing to the availability of a lone pair of electrons. For instance:
  • Oxygen in water (H鈧侽) or the hydroxide ion (OH鈦�)
  • Nitrogen in ammonia (NH鈧�) or amines
The high electronegativity of these atoms enhances their ability to hold onto lone pairs and thus accept protons. This characteristic is why many common bases include such atoms鈥攖hey make excellent proton acceptors due to their strong electron holding capabilities.
Br酶nsted-Lowry Theory
The Br酶nsted-Lowry theory is a broader perspective on acids and bases, focusing primarily on the transfer of protons. Unlike earlier definitions that were limited to substances dissolved in water, this theory does not restrict the acids and bases to aqueous solutions. It offers a more universal understanding of chemical reactions beyond the simple aqueous environment. In this view, acid-base reactions are understood as proton transfer processes, where one substance donates and another substance accepts a proton. This theory expands the range of identifiable acids and bases in chemistry, making it an essential concept for understanding a variety of chemical interactions.

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Most popular questions from this chapter

Write the chemical equation and the \(K_{b}\) expression for the reaction of each of the following bases with water: (a) propylamine, \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{NH}_{2}\); (b) monohydrogen phosphate ion, \(\mathrm{HPO}_{4}{ }^{2-} ;\) (c) benzoate ion, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2}^{-}\)

(a) What does the term autoionization mean? (b) Explain why pure water is a poor conductor of electricity. (c) You are told that an aqueous solution is acidic. What does this statement mean?

By what factor does \(\left[\mathrm{H}^{+}\right]\) change for a pH change of (a) \(2.00\) units, (b) \(0.50\) units?

(a) What is a strong base? (b) A solution is labeled \(0.035 \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}\). What is \(\left[\mathrm{OH}^{-}\right]\) for the solution? (c) Is the following statement true or false? Because \(\mathrm{Mg}(\mathrm{OH})_{2}\) is not very soluble, it cannot be a strong base. Explain.

The acid-dissociation constant for hypochlorous acid \((\mathrm{HClO})\) is \(3.0 \times 10^{-8} .\) Calculate the concentrations of \(\mathrm{H}_{3} \mathrm{O}^{+}, \mathrm{ClO}^{-}\), and \(\mathrm{HClO}\) at equilibrium if the initial concentration of \(\mathrm{HClO}\) is \(0.0090 \mathrm{M}\).
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