Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 8: Problem 120

Two different compounds have the formula \(\mathrm{XeF}_{2} \mathrm{Cl}_{2} .\) Write Lewis structures for these two compounds, and describe how measurement of dipole moments might be used to distinguish between them.

Short Answer

Expert verified
The two possible arrangements for \(\mathrm{XeF}_{2} \mathrm{Cl}_{2}\) have different shapes and dipole moments. Arrangement 1: \(\mathrm{Xe}( \mathrm{F})( \mathrm{F})( \mathrm{Cl})( \mathrm{Cl})\) is asymmetrical and has nonzero dipole moment, while arrangement 2: \(\mathrm{Xe}( \mathrm{F})( \mathrm{Cl})( \mathrm{F})( \mathrm{Cl})\) is symmetrical and has a zero dipole moment. By measuring the dipole moment, we can distinguish between the two compounds - a nonzero value indicates arrangement 1, while a zero value indicates arrangement 2.

Step by step solution

01

Identify possible arrangements of atoms for the given formula

Since we are given the formula \(\mathrm{XeF}_{2} \mathrm{Cl}_{2}\), we can predict two possible arrangements for the molecule: 1. Xe in the center, with two F atoms and two Cl atoms attached to it: \(\mathrm{Xe}( \mathrm{F})( \mathrm{F})( \mathrm{Cl})( \mathrm{Cl})\) 2. Xe in the center, with one F and one Cl atom on one side and one F and one Cl atom on the other side: \(\mathrm{Xe}( \mathrm{F})( \mathrm{Cl})( \mathrm{F})( \mathrm{Cl})\)
02

Draw the Lewis structures for the two possible arrangements

For both possible arrangements, draw the Lewis structures by following these steps: 1. Identify the valence electrons for each atom 2. Connect the atoms with single bonds and complete the octets with electron pairs 3. Check if the octet rule is followed For arrangement 1: 1. Xe - 8 valence electrons, F - 7 valence electrons, Cl - 7 valence electrons 2. Xe - F - F - Cl - Cl with single bonds and complete the octets with electron pairs 3. Octet rule is followed For arrangement 2: 1. Xe - 8 valence electrons, F - 7 valence electrons, Cl - 7 valence electrons 2. Xe - F - Cl - F - Cl with single bonds and complete the octets with electron pairs 3. Octet rule is followed
03

Determine the dipole moments of both arrangements

In order to determine the dipole moments of both arrangements, first identify the electronegativity difference between Xe, F, and Cl. - Xe: 2.6 - F: 3.98 - Cl: 3.16 Now, we can calculate the difference in electronegativities for the bonds: - Xe-F: 1.38 - Xe-Cl: 0.56 For arrangement 1: Since F and Cl are not identical, the structure is asymmetrical. Therefore, there will be a net dipole moment present. For arrangement 2: The molecule is symmetrical; hence, individual bond dipole moments will cancel each other out. Therefore, there will be no net dipole moment present for this arrangement.
04

Use the dipole moment measurements to distinguish the two compounds

Based on the results obtained in step 3, we can use the dipole moment measurements to distinguish between these two compounds. For both arrangements: 1. If the dipole moment measurement is nonzero, the compound corresponds to arrangement 1 - an asymmetrical structure with a net dipole moment present. 2. If the dipole moment measurement is zero, the compound corresponds to arrangement 2 - a symmetrical structure with no net dipole moment present.

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

Write Lewis structures and predict the molecular structures of the following. (See Exercises 105 and 106 .) a. \(\mathrm{OCl}_{2}, \mathrm{KrF}_{2}, \mathrm{BeH}_{2}, \mathrm{SO}_{2}\) b. \(\mathrm{SO}_{3}, \mathrm{NF}_{3}, \mathrm{IF}_{3}\) c. \(\mathrm{CF}_{4}, \mathrm{SeF}_{4}, \mathrm{KrF}_{4}\) d. \(\mathrm{IF}_{5}, \mathrm{AsF}_{5}\) Which of these compounds are polar?

The most common type of exception to the octet rule are compounds or ions with central atoms having more than eight electrons around them. \(\mathrm{PF}_{5}, \mathrm{SF}_{4}, \mathrm{ClF}_{3}\) and \(\mathrm{Br}_{3}^{-}\) are examples of this type of exception. Draw the Lewis structure for these compounds on ions. Which elements, when they have to, can have more than eight electrons around them? How is this rationalized?

Would you expect the electronegativity of titanium to be the same in the species \(\mathrm{Ti}, \mathrm{Ti}^{2+}, \mathrm{Ti}^{3+}\), and \(\mathrm{Ti}^{4+} ?\) Explain.

When comparing the size of different ions, the general radii trend discussed in Chapter 7 is usually not very useful. What do you concentrate on when comparing sizes of ions to each other or when comparing the size of an ion to its neutral atom?

The alkali metal ions are very important for the proper functioning of biologic systems, such as nerves and muscles, and \(\mathrm{Na}^{+}\) and \(\mathrm{K}^{+}\) ions are present in all body cells and fluids. In human blood plasma, the concentrations are $$ \left[\mathrm{Na}^{+}\right] \approx 0.15 M \text { and }\left[\mathrm{K}^{+}\right] \approx 0.005 M $$ For the fluids inside the cells, the concentrations are reversed: $$ \left[\mathrm{Na}^{+}\right] \approx 0.005 M \text { and }\left[\mathrm{K}^{+}\right] \approx 0.16 M $$ Since the concentrations are so different inside and outside the cells, an elaborate mechanism is needed to transport \(\mathrm{Na}^{+}\) and \(\mathrm{K}^{+}\) ions through the cell membranes. What are the ground-state electron configurations for \(\mathrm{Na}^{+}\) and \(\mathrm{K}^{+}\) ? Which ion is smaller in size? Counterions also must be present in blood plasma and inside intracellular fluid. Assume the counterion present to balance the positive charge of \(\mathrm{Na}^{+}\) and \(\mathrm{K}^{+}\) is \(\mathrm{Cl}^{-}\). What is the ground-state electron configuration for \(\mathrm{Cl}^{-}\) ? Rank these three ions in order of increasing size.
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Analysis

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