Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 14: Problem 137

Would you expect \(\mathrm{Fe}^{3+}\) or \(\mathrm{Fe}^{2+}\) to be the stronger Lewis acid? Explain.

Short Answer

Expert verified
We can conclude that \(\mathrm{Fe^{3+}}\) is the stronger Lewis acid compared to \(\mathrm{Fe^{2+}}\). This is because both ions have a similar size, but \(\mathrm{Fe^{3+}}\) has a higher positive charge (+3) than \(\mathrm{Fe^{2+}}\) (+2). As a result, \(\mathrm{Fe^{3+}}\) is more attracted to negatively charged electron pairs, making it a better electron-pair acceptor and thus a stronger Lewis acid.

Step by step solution

01

Understand the concept of a Lewis acid

A Lewis acid is a substance that can accept an electron pair to form a covalent bond. In other words, a Lewis acid is an electron-pair acceptor.
02

Analyze the charge of both ions

In this case, we are comparing the acid strength of Fe³⁺ and Fe²⁺. The Fe³⁺ ion has a charge of +3, while the Fe²⁺ ion has a charge of +2. The higher the positive charge, the more the ion is attracted to negatively charged electron pairs. This means that the higher the positive charge of an ion, the stronger the Lewis acid.
03

Analyze the size of both ions

The size of the ion is another factor that affects the Lewis acid strength. When comparing ions with the same charge, smaller ions are more attracted to electron pairs than larger ions, making them stronger Lewis acids. In this case, both ions have the same element (iron) and are therefore similar in size.
04

Draw a conclusion based on charge and size

Since both Fe³⁺ and Fe²⁺ ions have a similar size, and Fe³⁺ has a higher positive charge than Fe²⁺, we can conclude that Fe³⁺ is the stronger Lewis acid. The higher positive charge results in a stronger attraction to electron pairs, making it a better electron-pair acceptor.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Making use of the assumptions we ordinarily make in calculating the pH of an aqueous solution of a weak acid, calculate the \(\mathrm{pH}\) of a \(1.0 \times 10^{-6} M\) solution of hypobromous acid \(\left(\mathrm{HBrO}, K_{\mathrm{a}}=\right.\) \(\left.2 \times 10^{-9}\right) .\) What is wrong with your answer? Why is it wrong? Without trying to solve the problem, tell what has to be included to solve the problem correctly.

One mole of a weak acid HA was dissolved in \(2.0 \mathrm{~L}\) of solution. After the system had come to equilibrium, the concentration of HA was found to be \(0.45 M .\) Calculate \(K_{\mathrm{a}}\) for HA.

Calculate the \(\mathrm{pH}\) of a \(2.0 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) solution.

For the following, mix equal volumes of one solution from Group I with one solution from Group II to achieve the indicated \(\mathrm{pH}\). Calculate the \(\mathrm{pH}\) of each solution. Group I: \(0.20 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}, 0.20 \mathrm{MHCl}, 0.20 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{Cl}, 0.20\) \(M\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{3} \mathrm{NHCl}\) Group II: \(0.20 \mathrm{M} \mathrm{KOI}, 0.20 \mathrm{M} \mathrm{NaCN}, 0.20 \mathrm{M} \mathrm{KOCl}, 0.20 \mathrm{M}\) \(\mathrm{NaNO}_{2}\) a. the solution with the lowest \(\mathrm{pH}\) b. the solution with the highest \(\mathrm{pH}\) c. the solution with the \(\mathrm{pH}\) closest to \(7.00\)

Calculate \(\left[\mathrm{OH}^{-}\right]\) in a solution obtained by adding \(0.0100 \mathrm{~mol}\) solid \(\mathrm{NaOH}\) to \(1.00 \mathrm{~L}\) of \(15.0 \mathrm{M} \mathrm{NH}_{3}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free