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Chemistry In Focus

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

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BuyFindarrow_forward

Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 5, Problem 36E
Textbook Problem
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Determine whether each molecule is polar:

a . CH 3 OH b . CH 2 Cl 2 c . N 2 H 2 d . CF 4

Interpretation Introduction

Interpretation:

The molecular polarity for the given molecules, is to be determined.

Concept Introduction:

A polar bond is formed between the elements with different electronegativities. Due to uneven electron distribution, there is a charge separation that results in a dipole. Non-polar molecules do not have a charge separation.

If a molecule has polar bonds, it may or may not be polar, depending on the molecular geometry. Determine the geometry of the molecule using VSEPR theory and then determine whether the polar bonds are adding together, giving polarity to a molecule, or do they negate each other.

Explanation of Solution

a) The given molecule is CH3OH.

The Lewis structure of CH3OH is as follows:

The carbon atom is in the centre surrounded by three hydrogen atoms and one OH group. The carbon atom has different groups around it. Oxygen makes the bond polar. The molecule is unsymmetrical. Its electronic geometry is tetrahedral with respect to the carbon atoms but the molecule is a little bent at oxygen and due to which dipoles do not cancel each other. Hence, CH3OH is a polar molecule.

b) The given molecule is CH2Cl2.

The Lewis structure of CH2Cl2 is as follows:

The carbon atom is in the centre surrounded by two chlorine atoms and two hydrogen atoms.

There are four electron groups around the carbon and there is no lone pair. Therefore, the molecule is tetrahedral. Carbon-chlorine bonds are polar.

Hence, CH2Cl2 is a polar molecule

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Chapter 5 Solutions

Chemistry In Focus
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