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Chapter 15: Problem 7

Define an acid and a base according to the Lewis concept. Give a chemical equation to illustrate.

Short Answer

Expert verified
A Lewis acid accepts an electron pair, while a Lewis base donates an electron pair. Example: \(\text{NH}_3 + \text{BF}_3 \rightarrow \text{F}_3\text{B-NH}_3\) where \(\text{NH}_3\) is the base and \(\text{BF}_3\) is the acid.

Step by step solution

01

Understand the Lewis Definition

According to the Lewis concept, an acid is defined as a substance that can accept an electron pair. A base, on the other hand, is a substance that can donate an electron pair. This definition broadens the scope of what can be considered acids and bases beyond those that release hydrogen or hydroxide ions.
02

Choose an Example

One classic example of a Lewis acid-base reaction is the reaction between ammonia (\(\text{NH}_3\)) and boron trifluoride (\(\text{BF}_3\)). Ammonia is the Lewis base because it donates an electron pair, while boron trifluoride is the Lewis acid because it accepts that electron pair.
03

Write the Chemical Equation

The Lewis acid-base reaction can be represented by the following chemical equation:\[\text{NH}_3 + \text{BF}_3 \rightarrow \text{F}_3\text{B-NH}_3\]In this equation, ammonia (\(\text{NH}_3\)) donates an electron pair to boron trifluoride (\(\text{BF}_3\)), forming a complex.
04

Interpret the Reaction

In the reaction, the nitrogen of ammonia donates a lone pair of electrons to the boron atom in boron trifluoride. The formation of the \(\text{F}_3\text{B-NH}_3\) complex illustrates how the electron pair is shared, demonstrating the Lewis acid-base interaction.

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Key Concepts

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

Electron Pair Donor
In the Lewis acid-base theory, an important term to understand is the electron pair donor. This is the role played by the Lewis base in a reaction. A Lewis base is a substance that can donate a pair of electrons. Imagine an element with excess electrons looking for a reaction partner. This is essentially the behavior of the electron pair donor.
For example, consider ammonia ( H_3 ext{NH ext{NH}_3} ). It's a classic example of a Lewis base. Ammonia has a lone pair of electrons on its nitrogen atom, making it very eager to share this pair with other chemical species looking for electrons.
When ammonia encounters a Lewis acid, it readily donates that lone electron pair. This plays a crucial part in forming a new bond in the molecular structure of the resulting compound.
Electron Pair Acceptor
On the flip side of the Lewis definition, we have the electron pair acceptor, which is the characteristic role of a Lewis acid. A Lewis acid is a species that can accept a pair of electrons.
This definition expands the traditional view of acids to include any species that can ac-capture electrons. A perfect example of this is boron trifluoride ( F_3 ext{BF ext{BF}_3} ).
Boron trifluoride lacks a complete octet around the boron, which makes it very receptive to accepting electron pairs from Lewis bases. This electron-pair accepting behavior is fundamental in forming new adv ionic or covalent bonds during a chemical reaction.
Lewis Acid
Lewis acids broaden our understanding of what makes a compound an acid, beyond the traditional notion of hydrogen ion donors. A Lewis acid is defined by its ability to accept an electron pair. Let's consider BF_3 ext{BF}_3 as an example again.
It acts as a Lewis acid because it seeks to complete its boron atom's octet by accepting an electron pair. Most Lewis acids are central atoms in compounds with unfilled valence shells.
The reactivity of these compounds in forming bonds by electron acceptance is what classifies them as acids in the Lewis sense, enabling many reactions that wouldn't fit under the traditional definition of acids.
Lewis Base
A Lewis base is defined by its capability to donate an electron pair. This expands the traditional base definition beyond substances that produce OH鈦� ions in water.
Ammonia, H_3 ext{NH ext{NH}_3}, demonstrates this broader definition beautifully. It acts as a Lewis base because it possesses a lone pair of electrons, making it ready to share and form a bond with a Lewis acid.
This interaction is essential for forming new compounds and illustrates the flexibility and breadth of the Lewis acid-base theory. Bases can now be viewed as potential electron pair donors, enhancing our understanding of basicity in chemical reactions.

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Most popular questions from this chapter

You make a solution by dissolving \(0.0010\) mol of \(\mathrm{HCl}\) in enough water to make \(1.0 \mathrm{~L}\) of solution. a. Write the chemical equation for the reaction of \(\mathrm{HCl}(a q)\) and water. b. Without performing calculations, give a rough estimate of the \(\mathrm{pH}\) of the \(\mathrm{HCl}\) solution. Justify your answer. c. Calculate the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration and the \(\mathrm{pH}\) of the solution. d. Is there any concentration of the base \(\mathrm{OH}^{-}\) present in this solution of \(\mathrm{HCl}(a q) ?\) If so, where did it come from? e. If you increase the OH \(^{-}\) concentration of the solution by adding \(\mathrm{NaOH}\), does the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration change? If you think it does, explain why this change occurs and whether the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration increases or decreases. f. If you were to measure the \(\mathrm{pH}\) of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g. Explain how two different volumes of your original \(\mathrm{HCl}\) solution can have the same \(\mathrm{pH}\) yet contain different moles of \(\mathrm{H}_{3} \mathrm{O}^{+}\) h. If \(1.0 \mathrm{~L}\) of pure water were added to the \(\mathrm{HCl}\) solution, would this have any impact on the \(\mathrm{pH}\) ? Explain.

You want to make up \(3.00 \mathrm{~L}\) of aqueous hydrochloric acid, \(\mathrm{HCl}(a q)\), that has a \(\mathrm{pH}\) of \(2.00 .\) How many grams of concentrated hydrochloric acid will you need? Concentrated hydrochloric acid contains \(37.2\) mass percent of \(\mathrm{HCl}\).

A detergent solution has a pH of \(11.63\) at \(25^{\circ} \mathrm{C}\). What is the hydroxide-ion concentration?

Aluminum chloride, \(\mathrm{AlCl}_{3}\), reacts with trimethylamine, \(\mathrm{N}\left(\mathrm{CH}_{3}\right)_{3} .\) What would you guess to be the product of this reaction? Explain why you think so. Describe the reaction in terms of one of the acid-base concepts. Write an appropriate equation to go with this description. Which substance is the acid according to this acid-base concept? Explain.

The dihydrogen phosphate ion has the ability to act as an acid in the presence of a base and as a base in the presence of an acid. What is this property called? Illustrate this behavior with water by writing Br酶nsted-Lowry acid- base reactions. Also illustrate this property by selecting a common acid and base to react with the dihydrogen phosphate ion.
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