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Chapter 16: Problem 123

All Br枚nsted acids are Lewis acids, but the reverse is not true. Give two examples of Lewis acids that are not Br枚nsted acids.

Short Answer

Expert verified
BF鈧� and AlCl鈧� are Lewis acids that are not Br枚nsted acids.

Step by step solution

01

Define Br枚nsted Acid

A Br枚nsted acid is a substance that can donate a proton (H鈦�) to another substance. Examples include hydrochloric acid (HCl) and sulfuric acid (H鈧係O鈧�).
02

Define Lewis Acid

A Lewis acid is a compound that can accept an electron pair from a Lewis base. It does not necessarily donate protons. Examples include boron trifluoride (BF鈧�) and aluminum chloride (AlCl鈧�).
03

Identify Lewis Acids that are not Br枚nsted Acids

Since Lewis acids accept electron pairs and are not required to donate protons, we can identify compounds like boron trifluoride (BF鈧�) and aluminum chloride (AlCl鈧�) as Lewis acids that do not have protons to donate, making them not Br枚nsted acids.

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Key Concepts

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

Br枚nsted acids
Br枚nsted acids are an essential concept in chemistry. They are defined by their ability to donate a proton, commonly known as a hydrogen ion (H鈦�), to another substance. This donation process is what primarily characterizes a Br枚nsted acid.

Classic examples of Br枚nsted acids include:
  • Hydrochloric acid (HCl)
  • Sulfuric acid (H鈧係O鈧�)
When a Br枚nsted acid donates a proton, it becomes its conjugate base. For instance, when HCl donates a proton, it turns into Cl鈦�, its conjugate base. This proton donation is a central part of acid-base reactions in chemistry, emphasizing the important role Br枚nsted acids play.
Proton donation
Proton donation is a fundamental process in which a Br枚nsted acid releases a proton, or H鈦� ion, to another molecule or ion. This process is integral to what defines a substance as a Br枚nsted acid.

During this donation:
  • The Br枚nsted acid loses a proton.
  • The accepting molecule or ion, termed the base, becomes a conjugate acid.
For example, in the reaction between hydrochloric acid (HCl) and water (H鈧侽), HCl donates a proton to water, forming the hydronium ion (H鈧僌鈦�) and chloride ion (Cl鈦�). Proton donation is crucial for facilitating many chemical reactions, including those in biological systems, like enzyme functions and metabolic pathways.
Electron pair acceptance
Electron pair acceptance is the hallmark of Lewis acids. A Lewis acid is any compound capable of accepting an electron pair from a donor, known as a Lewis base. This can occur without the need for proton donation, distinguishing Lewis acids from Br枚nsted acids.

Key points about Lewis acid electron pair acceptance:
  • Lewis acids are not defined by the presence or absence of protons.
  • They generally have empty orbitals, allowing them to accept electron pairs effectively.
This mechanism enables Lewis acids to participate in a wide range of chemical reactions, including the formation of complex compounds and catalytic cycles, demonstrating their versatility in the field of chemistry.
Boron trifluoride
Boron trifluoride (BF鈧�) is a classic example of a Lewis acid that does not qualify as a Br枚nsted acid. It does not donate protons but excels in accepting electron pairs due to the electron-deficient nature of boron.

Here's how boron trifluoride acts as a Lewis acid:
  • The boron atom in BF鈧� has an empty p-orbital.
  • It can accept an electron pair from a Lewis base, like ammonia (NH鈧�).
Due to its capacity to form coordinate bonds by accepting electron pairs, BF鈧� finds wide application in industrial processes, such as catalysis and the synthesis of various organic compounds, underscoring its importance beyond a standard acid-base interaction.
Aluminum chloride
Aluminum chloride (AlCl鈧�) is another prominent Lewis acid that is not a Br枚nsted acid. It is highly reactive due to its ability to accept electron pairs, rather than donating protons.

Understanding aluminum chloride:
  • AlCl鈧�, especially in its anhydrous form, has an electron-deficient aluminum atom.
  • This deficiency allows it to readily accept electrons, making it an efficient catalyst in many chemical reactions.
AlCl鈧� is extensively used in the Friedel-Crafts reactions, particularly in the synthesis of aromatic compounds. This utility showcases its role as a strong Lewis acid in facilitating complex chemical transformations, illustrating its widespread use in both industrial and laboratory settings.

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Most popular questions from this chapter

Calculate the \(\mathrm{pH}\) of a \(0.36 \mathrm{M} \mathrm{CH}_{3} \mathrm{COONa}\) solution. \(\left(K_{\mathrm{a}}\right.\) for acetic acid \(\left.=1.8 \times 10^{-5} .\right)\)

Predict the \(\mathrm{pH}(>7,<7,\) or \(\approx 7)\) of aqueous solutions containing the following salts: (a) \(\mathrm{KBr}\) (b) \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3},\) (c) \(\mathrm{BaCl}_{2}\) (d) \(\mathrm{Bi}\left(\mathrm{NO}_{3}\right)_{3}\).

Classify each of the following species as a Lewis acid or a Lewis base: (a) \(\mathrm{CO}_{2},(\mathrm{~b}) \mathrm{H}_{2} \mathrm{O},(\mathrm{c}) \mathrm{I}^{-},(\mathrm{d}) \mathrm{SO}_{2},(\mathrm{e}) \mathrm{NH}_{3},\) (f) \(\mathrm{OH}^{-},(\mathrm{g}) \mathrm{H}^{+},(\mathrm{h}) \mathrm{BCl}_{3}\)

What is the original molarity of a solution of formic acid \((\mathrm{HCOOH})\) whose \(\mathrm{pH}\) is 3.26 at \(25^{\circ} \mathrm{C} ?\left(K_{\mathrm{a}}\right.\) for $$ \text { formic acid } \left.=1.7 \times 10^{-4} .\right) $$

Predict the direction that predominates in this reaction: $$ \mathrm{F}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HF}(a q)+\mathrm{OH}^{-}(a q) $$
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