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Get Full Access to Atkins' Physical Chemistry - 11 Edition - Chapter 14a - Problem P14a.9
Get Full Access to Atkins' Physical Chemistry - 11 Edition - Chapter 14a - Problem P14a.9

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ISBN: 9780198769866 2042

## Solution for problem P14A.9 Chapter 14A

Atkins' Physical Chemistry | 11th Edition

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Atkins' Physical Chemistry | 11th Edition

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Problem P14A.9

In his classic book Polar molecules, Debye reports some early measurements of the polarizability of ammonia. From the selection below, determine the dipole moment and the polarizability volume of the molecule.

$$\begin{array}{lcccccc} T / \mathrm{K} & 292.2 & 309.0 & 333.0 & 387.0 & 413.0 & 446.0 \\ P_{\mathrm{m}} /\left(\mathrm{cm}^{3} \mathrm{~mol}^{-1}\right) & 57.57 & 55.01 & 51.22 & 44.99 & 42.51 & 39.59 \end{array}$$

The refractive index of ammonia at 273K and 100 kPa is 1.000 379 (for yellow sodium light). Calculate the molar polarization of the gas at this temperature. Combine the value calculated with the static molar polarization at 292.2K and deduce from this information alone the molecular dipole moment.

Text Transcription:

T/K

P_m/(cm^3 mol^-1)

Step-by-Step Solution:
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Predicting bond polarity Chemical bonds are usually polar whenever the two atoms involved have different electronegativities, because the more electronegative atom will tend to pull the shared valence electrons in the bond toward it. Since electrons have a negative charge, that will give the more electronegative atom a slight negative charge. The other atom will get a slight positive charge, because it will no longer have enough electrons to fully cancel the positive charge of its nucleus. • The higher the electronegativity, the more negative the element (when comparing bond polarity) Note: The polarity is only noticeable in practice when the difference in electronegativities between atoms is greater than about 0.50. Your instructor may want you to label bonds between atoms with electronegativities that differ by less than 0.50 as nonpolar. Identifying common chemical groups in a Lewis structure A chemical group is a part of a molecule. It's important to get to know the the common chemical groups, because a very large number of molecules are made of the same chemical groups shuffled around in different ways. If you think of atoms as "letters" and molecules as "sentences" made from those letters, then chemical groups are like the "words" that make up the sentences. Here are the chemical groups you'll need to recognize to be able to solve this problem: The lines that go nowhere, on the left or right side of each group, show you where each group is bonded to the rest of

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##### ISBN: 9780198769866

This textbook survival guide was created for the textbook: Atkins' Physical Chemistry, edition: 11. Atkins' Physical Chemistry was written by Aimee Notetaker and is associated to the ISBN: 9780198769866. This full solution covers the following key subjects: . This expansive textbook survival guide covers 327 chapters, and 1120 solutions. Since the solution to P14A.9 from 14A chapter was answered, more than 201 students have viewed the full step-by-step answer. The full step-by-step solution to problem: P14A.9 from chapter: 14A was answered by Aimee Notetaker, our top Chemistry solution expert on 04/25/22, 03:45PM. The answer to “?In his classic book Polar molecules, Debye reports some early measurements of the polarizability of ammonia. From the selection below, determine the dipole moment and the polarizability volume of the molecule.$$\begin{array}{lcccccc}T / \mathrm{K} & 292.2 & 309.0 & 333.0 & 387.0 & 413.0 & 446.0 \\P_{\mathrm{m}} /\left(\mathrm{cm}^{3} \mathrm{~mol}^{-1}\right) & 57.57 & 55.01 & 51.22 & 44.99 & 42.51 & 39.59\end{array}$$The refractive index of ammonia at 273K and 100 kPa is 1.000 379 (for yellow sodium light). Calculate the molar polarization of the gas at this temperature. Combine the value calculated with the static molar polarization at 292.2K and deduce from this information alone the molecular dipole moment.Text Transcription:T/KP_m/(cm^3 mol^-1)” is broken down into a number of easy to follow steps, and 109 words.

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