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Chapter 18: Problem 133

How do Lewis acids differ from Br贸nsted-Lowry acids? How are they similar? Do Lewis bases differ from BronstedLowry bases? Explain.

Short Answer

Expert verified
Lewis acids accept electron pairs; Br枚nsted-Lowry acids donate protons. Lewis bases donate electron pairs; Br枚nsted-Lowry bases accept protons.

Step by step solution

01

- Definition of Lewis Acids

A Lewis acid is defined as a substance that can accept a pair of electrons to form a covalent bond. This definition focuses on electron pair acceptance.
02

- Definition of Br枚nsted-Lowry Acids

A Br枚nsted-Lowry acid is defined as a substance that can donate a proton (H鈦� ion) to another substance. This focuses on proton donation.
03

- Comparison of Lewis Acids and Br枚nsted-Lowry Acids

Lewis acids and Br枚nsted-Lowry acids are similar in that they both participate in acid-base reactions. However, they differ in their mechanisms鈥擫ewis acids accept electron pairs, whereas Br枚nsted-Lowry acids donate protons.
04

- Definition of Lewis Bases

A Lewis base is defined as a substance that can donate a pair of electrons to form a covalent bond. This definition emphasizes electron pair donation.
05

- Definition of Br枚nsted-Lowry Bases

A Br枚nsted-Lowry base is defined as a substance that can accept a proton (H鈦� ion) from another substance. This focuses on proton acceptance.
06

- Comparison of Lewis Bases and Br枚nsted-Lowry Bases

Both Lewis bases and Br枚nsted-Lowry bases participate in acid-base reactions and are similar in that they accept entities (electrons or protons). However, Lewis bases donate electron pairs, whereas Br枚nsted-Lowry bases accept protons.

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Key Concepts

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

Lewis acids
Lewis acids are unique in their ability to accept electron pairs. They do not have to involve hydrogen ions (H鈦�) as Br枚nsted-Lowry acids do. Instead, any molecule or ion that can accept an electron pair to form a covalent bond qualifies as a Lewis acid.
Common examples include metal cations like Fe鲁鈦� and Al鲁鈦�, as well as molecules like BF鈧� and AlCl鈧�.
Their general mechanism is to facilitate reactions by accepting electron pairs from Lewis bases, which donate them.
Br枚nsted-Lowry acids
Br枚nsted-Lowry acids are defined by their ability to donate a proton (H鈦�) to another substance. This concept revolves around proton transfer reactions.
Unlike Lewis acids, which can accept any electron pair, Br枚nsted-Lowry acids are solely concerned with protons.
Classic examples of Br枚nsted-Lowry acids include substances like hydrochloric acid (HCl), sulfuric acid (H鈧係O鈧�), and acetic acid (CH鈧僀OOH). These acids lose a proton and thus transform into their conjugate bases when reacting.
Lewis bases
Lewis bases are substances that can donate a pair of electrons to form a covalent bond. Their primary role in reactions is to search for electron-acceptors like Lewis acids.
This characteristic makes substances like ammonia (NH鈧�), hydroxide ions (OH鈦�), and fluoride ions (F鈦�) typical examples of Lewis bases.
It's interesting to note that Lewis bases often align with Br枚nsted-Lowry bases, but the key defining feature remains their ability to donate electrons, not necessarily accept a proton.
Thus, Lewis bases are crucial in various chemical reactions, acting as a source of electron pair donating species.

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Most popular questions from this chapter

What is an amphiprotic species? Name one and write balanced equations that show why it is amphiprotic.

What is a conjugate acid-base pair? What is the relationship between the two members of the pair?

A strong acid has a weak bond to its acidic proton, whereas a weak acid has a strong bond to its acidic proton. Explain.

A solution of propanoic acid \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}\right),\) made by dissolving \(7.500 \mathrm{~g}\) in sufficient water to make \(100.0 \mathrm{~mL}\), has a freezing point of \(-1.890^{\circ} \mathrm{C}\). (a) Calculate the molarity of the solution. (b) Calculate the molarity of the propanoate ion. (Assume the molarity of the solution equals the molality.) (c) Calculate the percent dissociation of propanoic acid.

What does "weak" mean for acids? The \(K_{a}\) values of weak acids vary over more than 10 orders of magnitude. What do the acids have in common that makes them "weak"?
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