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Get Full Access to Chemistry: The Central Science - 14 Edition - Chapter 8 - Problem 8.7
Get Full Access to Chemistry: The Central Science - 14 Edition - Chapter 8 - Problem 8.7

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# ?The partial Lewis structure that follows is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and th

ISBN: 9780134414232 1274

## Solution for problem 8.7 Chapter 8

Chemistry: The Central Science | 14th Edition

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Problem 8.7

The partial Lewis structure that follows is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and there are no unshared electron pairs in the molecule. The carbon—carbon bonds are labeled 1, 2, and 3.

(a) How many hydrogen atoms are in the molecule?

(b) Rank the carbon–carbon bonds in order of increasing bond length.

(c) Which carbon—carbon bond is the strongest one? [Sections 8.3 and 8.8]

$$C \stackrel{1}{=} \mathrm{C} \stackrel{2}{-} \mathrm{C} \stackrel{3}{=} \mathrm{C}$$

Text Transcription:

C \stackrel 1= C \stackrel 2 - C \stackrel 3 =C

Step-by-Step Solution:

Step 1 of 5) The instantaneous distribution of the electrons, however, can be different from the average distribution. If we could freeze the motion of the electrons at any given instant, both electrons could be on one side of the nucleus. At just that instant, the atom has an instantaneous dipole moment as shown in Figure 11.4(b). The motions of electrons in one atom influence the motions of electrons in its neighbors. The instantaneous dipole on one atom can induce an instantaneous dipole on an adjacent atom, causing the atoms to be attracted to each other as shown in Figure 11.4(c). This attractive interaction is called the dispersion force (also called London dispersion forces or induced dipole–induced dipole interactions). It is significant only when molecules are very close together. The strength of the dispersion force depends on the ease with which the charge distribution in a molecule can be distorted to induce an instantaneous dipole. The ease with which the charge distribution is distorted is called the molecule’s polarizability. We can think of the polarizability of a molecule as a measure of the “squashiness” of its electron cloud: The greater the polarizability, the more easily the electron cloud can be distorted to give an instantaneous dipole. Therefore, more polarizable molecules have larger dispersion forces.

Step 2 of 2

##### ISBN: 9780134414232

Since the solution to 8.7 from 8 chapter was answered, more than 209 students have viewed the full step-by-step answer. Chemistry: The Central Science was written by and is associated to the ISBN: 9780134414232. The answer to “?The partial Lewis structure that follows is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and there are no unshared electron pairs in the molecule. The carbon—carbon bonds are labeled 1, 2, and 3. (a) How many hydrogen atoms are in the molecule? (b) Rank the carbon–carbon bonds in order of increasing bond length. (c) Which carbon—carbon bond is the strongest one? [Sections 8.3 and 8.8]$$C \stackrel{1}{=} \mathrm{C} \stackrel{2}{-} \mathrm{C} \stackrel{3}{=} \mathrm{C}$$Text Transcription:C \stackrel 1= C \stackrel 2 - C \stackrel 3 =C” is broken down into a number of easy to follow steps, and 91 words. This full solution covers the following key subjects: . This expansive textbook survival guide covers 29 chapters, and 2820 solutions. The full step-by-step solution to problem: 8.7 from chapter: 8 was answered by , our top Chemistry solution expert on 10/03/18, 06:29PM. This textbook survival guide was created for the textbook: Chemistry: The Central Science, edition: 14.

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?The partial Lewis structure that follows is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and th