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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 4, Problem 33E
Textbook Problem
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Write Lewis structures and predict the molecular structures of the following. (See Exercises 25 and 26.)

a. OCl2, KrF2, BeH2, SO2

b. SO3, NF3, TF3

c. CF4 SeF4, KrF4

d. IF5, AsF5

Which of these compounds are polar?

(I-a)

Interpretation Introduction

Interpretation: The Lewis structures for the given molecules are to be drawn and

whether they are polar or non-polar is to predicted.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis structure of the given molecules and their molecular structure.

Explanation of Solution

Explanation

There are six valence electrons on oxygen and seven valence electrons on each chlorine atom. Two chlorine atoms and one oxygen atoms are present in the molecule, therefore the total number of valence electrons is 6+2×7=20 . There are two lone pairs of electrons on oxygen atom and three lone pairs on each chlorine atom. Oxygen is bonded to two chlorine atoms by sigma bond. Due to repulsion between the lone pairs, the shape of the molecule is bent and the bond angle is less than 109.5ο .

The Lewis structure of OCl2 is,

Figure 1

There are eight valence electrons on krypton and seven valence electrons on each fluorine atom. Therefore, the total number of valence electrons is 8+2×7=22 . There are three lone pairs of electrons on krypton atom and three lone pairs on each fluorine atom. Krypton is bonded to two fluorine atoms by sigma bond. Since the geometry of the molecule is linear, therefore the bond angle is equals to 180ο .

The Lewis structure of KrF2 is,

(I-b)

Interpretation Introduction

Interpretation: The Lewis structures for the given molecules are to be drawn and weather they are polar or non-polar is to predicted.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis structure of the given molecules and their molecular structure.

(I-c)

Interpretation Introduction

Interpretation: The Lewis structures for the given molecules are to be drawn and weather they are polar or non-polar is to predicted.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis structure of the given molecules and their molecular structure.

(I-d)

Interpretation Introduction

Interpretation: The Lewis structures for the given molecules are to be drawn and weather they are polar or non-polar is to predicted.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The Lewis structure of the given molecules and their molecular structure.

(II)

Interpretation Introduction

Interpretation: The Lewis structures for the given molecules are to be drawn and weather they are polar or non-polar is to predicted.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The molecules which are polar.

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Chapter 4 Solutions

Chemistry: An Atoms First Approach
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