   Chapter 20, Problem 6QAP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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# Draw the Lewis structures for carbon dioxide and carbon monoxide.

Interpretation Introduction

Interpretation:

Lewis structure for the carbon dioxide and carbon monoxide should be drawn.

Concept Introduction:

• Lewis structures are the diagrams that show the bonding between the atoms of the molecules and existing lone pairs of electrons.
• Bonding electrons are those electrons which are shared between the atoms resulting in the formation of bond.
• Non-bonding electrons are the valence electrons of the atom which are not shared with another atom.
Explanation

For carbon dioxide:

1. Calculate the total number of valence electrons in molecule CO2 :.
2. Total number of valence electrons = valence electrons of C + 2(valence electrons of O)

=4+2(6)=16 e

3. Arrange the atoms in such a way that the least electronegative atom is at the center. Then put the valence electrons around them such that each atom contributes at least 1 electron to single bond and the octet rule for each atom is followed.
4. To complete the octet the formation of double bond takes place between carbon and oxygen. So, the electrons involved in the bond formation are 8 that is 2 from each bond (2 double bond). The rest number of electrons are present as lone pair on oxygen atoms, the number of lone pair of electrons = Total number of valence electrons − Total number of electrons involved in bond formation. the number of lone pair of electrons = 16 − 8 = 8 electrons.
5. Thus, as C is the least electronegative, it would be the central atom and on arranging all the valence electrons, we get the Lewis structure of CO2 as:.

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