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CH 3 COCH 3 (acetone) is a common laboratory solvent that is often used in nail polish remover. Its Lewis structure and space-filling molecular image are shown here: Acetone is a polar molecule; the oxygen end has a slightly negative charge (oxygen is more electronegative), whereas the carbon and hydrogen end has a slightly positive charge. In liquid acetone, the molecules are attracted to each other via these polar ends-the positive end of one molecule is attracted to the negative end of its neighbor-and therefore align as shown here: Draw a Lewis structure and space-filling molecular image for CH 2 Cl 2 (dichloromethane), another common laboratory solvent. Is the molecule polar? Which end of the molecule has a slightly negative charge? Which end has a slightly positive charge? Draw several space-filling molecular images of CH 2 Cl 2 showing how they align in liquid dichloromethane.

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Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692

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Section
BuyFindarrow_forward

Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 5, Problem 46E
Textbook Problem
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CH 3 COCH 3 (acetone) is a common laboratory solvent that is often used in nail polish remover. Its Lewis structure and space-filling molecular image are shown here:

Chapter 5, Problem 46E, CH3COCH3 (acetone) is a common laboratory solvent that is often used in nail polish remover. Its , example  1

Acetone is a polar molecule; the oxygen end has a slightly negative charge (oxygen is more electronegative), whereas the carbon and hydrogen end has a slightly positive charge. In liquid acetone, the molecules are attracted to each other via these polar ends-the positive end of one molecule is attracted to the negative end of its neighbor-and therefore align as shown here:

Chapter 5, Problem 46E, CH3COCH3 (acetone) is a common laboratory solvent that is often used in nail polish remover. Its , example  2

Draw a Lewis structure and space-filling molecular image for CH 2 Cl 2 (dichloromethane), another common laboratory solvent. Is the molecule polar? Which end of the molecule has a slightly negative charge? Which end has a slightly positive charge? Draw several space-filling molecular images of CH 2 Cl 2 showing how they align in liquid dichloromethane.

Interpretation Introduction

Interpretation:

The space-filling molecular images and the Lewis structure of CH2Cl2 are to be represented.

Concept Introduction:

 The Lewis dot symbols contain dots, which give information about valence electrons.

 The Lewis dot symbols show both bonds and lone pairs as dots.

 The Lewis structures show bonds as lines and lone pairs as dots.

Explanation of Solution

The number of valence electrons in CH2Cl2 is calculated as follows:

=(C atoms)+2(H atom)+2(Cl atom)=4+2+14=20

Now, only eight electrons are required in bond formation to complete the octet of carbon, hydrogen, and chlorine. So, the number of remaining electrons is twelve and there are three lone pairs present on each chlorine atom.

Hence, the Lewis structure of CH2Cl2 is as follows:

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Chemistry In Focus
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