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Chapter 14: Problem 79

Which of these is a Lewis acid? A Lewis base? (a) \(\mathrm{NH}_{3}\) (b) \(\mathrm{BeCl}_{2}\) (c) \(\mathrm{BCl}_{3}\)

Short Answer

Expert verified
\(\mathrm{NH}_{3}\) is a Lewis base; \(\mathrm{BeCl}_{2}\) and \(\mathrm{BCl}_{3}\) are Lewis acids.

Step by step solution

01

Identify Lewis Acid and Lewis Base

A Lewis acid is a substance that can accept a pair of electrons, while a Lewis base is a substance that can donate a pair of electrons. We will analyze each compound to determine which category they fall into.
02

Analyze \\(\mathrm{NH}_{3}\\)

The molecule \(\mathrm{NH}_{3}\) (ammonia) has a lone pair of electrons on the nitrogen atom, which it can donate to an acceptor. Hence, \(\mathrm{NH}_{3}\) is a Lewis base.
03

Analyze \\(\mathrm{BeCl}_{2}\\)

\(\mathrm{BeCl}_{2}\), or beryllium chloride, has beryllium in a \(sp\) hybridization state and is electron-deficient, which allows it to accept a pair of electrons. Therefore, it acts as a Lewis acid.
04

Analyze \\(\mathrm{BCl}_{3}\\)

The molecule \(\mathrm{BCl}_{3}\) (boron trichloride) is also electron-deficient due to the boron atom lacking a complete octet, making it capable of accepting an electron pair. Therefore, \(\mathrm{BCl}_{3}\) is a Lewis acid.

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Key Concepts

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

Electron Pair Acceptor
In chemistry, an electron pair acceptor is often referred to as a Lewis acid. These substances can accept an electron pair from another substance.
A classic example of a Lewis acid is a molecule that is electron-deficient. This deficiency allows it to attract and accept an electron pair from a donor.
  • For instance, beryllium chloride (\( \mathrm{BeCl}_{2} \)) acts as a Lewis acid because the beryllium atom is surrounded by only four electrons, which is less than a full octet.
  • Similarly, boron trichloride (\( \mathrm{BCl}_{3} \)) also functions as a Lewis acid. The boron atom in \( \mathrm{BCl}_{3} \) is also electron-deficient, motivating it to accept additional electrons to achieve stability.
When you encounter a molecule that seems lacking in a complete electron shell, this is usually a good sign that you have found an electron pair acceptor or a Lewis acid.
Electron Pair Donor
In contrast to an electron pair acceptor, an electron pair donor is called a Lewis base. It has electrons that it can donate to another molecule, often filling the deficiency present in a Lewis acid.
These electron pairs, typically found as lone pairs on atoms, are key to their identification as donors.
  • Take ammonia, \(\mathrm{NH}_{3}\), for example. The nitrogen atom in ammonia has a lone pair of electrons.
  • This lone pair is readily available to be donated to a Lewis acid, which makes \(\mathrm{NH}_{3}\) a strong Lewis base.
Whenever you see a molecule with lone pairs, you are likely looking at a potential Lewis base. These lone pairs can interact with Lewis acids to form coordinate covalent bonds, completing the acid's electron requirements.
Molecular Analysis
Molecular analysis is the thorough examination of a compound's structure to determine its potential to act as a Lewis acid or base. By understanding the arrangement of electrons, you can predict how a molecule might behave in different chemical reactions.
This process involves:
  • Looking at electron configurations to identify instances of electron deficiency or surplus.
  • Checking for lone pairs that signify potential for electron donation.
  • Identifying hybridization states that signal a molecule's ability to accept electrons.
With this analysis:
  • \(\mathrm{NH}_{3}\), with its lone pairs, is identified as a Lewis base.
  • Beryllium chloride, \(\mathrm{BeCl}_{2}\), and boron trichloride, \(\mathrm{BCl}_{3}\), lacking full electron shells, are recognized as Lewis acids.
Paying attention to these factors allows for a deeper understanding of chemical interactions and how different substances will react with one another.

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Most popular questions from this chapter

Write a chemical equation to describe the proton transfer that occurs when each of these bases is added to water. (a) \(\mathrm{HSO}_{4}^{-}\) (b) \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) (c) I (d) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)

Explain in your own words what \(100 \%\) ionization means.

Calculate the \(\mathrm{pH}\) of a solution that is \(0.025-\mathrm{M}\) in \(\mathrm{NaOH}\). Calculate the pOH of this solution.

When a 0.1-M aqueous ammonia solution is tested with a conductivity apparatus ( \(\in\) Sec. \(3-3 b\) ), the bulb glows dimly. When a 0.1-M hydrochloric acid solution is tested, the bulb glows brightly. As water is added to each of the solutions, predict whether the bulb glows brighter, stops glowing, or stays the same. Explain your reasoning.

Write the ionization equation for a weak acid and the equation for its conjugate base reaction with water. Show that adding these two equations gives the autoionization equation for water.
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