Chemistry
Chemistry
4th Edition
ISBN: 9780078021527
Author: Julia Burdge
Publisher: McGraw-Hill Education
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Chapter 8, Problem 46QP
Interpretation Introduction

Interpretation:

The Lewis structures of the given molecules and ions are to be represented.

Concept Introduction:

In Lewis dot symbol, for each element, dots are mentioned around the symbol of an atom.

In Lewis dot symbol, valence electrons are represented by dots.

Dots are placed above and below as well as to the left and right of symbol.

Number of dots is important in Lewis dot symbol but not the order in which the dots are placed around the symbol.

In writing symbol pairing is not done until absolutely necessary.

For metals, the number of dots represents the number of electrons that are lost when the atom forms a cation.

For second period non metals, the number of unpaired dots is the number of bonds the atom can form.

Atomic ions can also be represented by dot symbols, by simply adding (for anions) and subtracting (for cations) the appropriate number of dots from Lewis dot symbol.

Lewis structure is the representation of bonding and non-bonding electron pairs present in the outermost shell of all atoms present in the molecule.

The number of bonds formed by an atom in the molecule is determined by the valence electron pairs.

Expert Solution & Answer
Check Mark

Answer to Problem 46QP

Solution:

(a)

Chemistry, Chapter 8, Problem 46QP , additional homework tip  1

(b)

Chemistry, Chapter 8, Problem 46QP , additional homework tip  2

(c)

Chemistry, Chapter 8, Problem 46QP , additional homework tip  3

(d)

Chemistry, Chapter 8, Problem 46QP , additional homework tip  4

(e)

Chemistry, Chapter 8, Problem 46QP , additional homework tip  5

(f)

Chemistry, Chapter 8, Problem 46QP , additional homework tip  6

Explanation of Solution

a) NCl3

The electronic configuration of nitrogen and chlorine in NCl3 is as:

N=1s22s22p3Cl=1s22s22p63s23p5

The nitrogen atom contains three valence electrons in its 2p subshell and the chlorine atom contains five valence electrons in its 3p subshell. Therefore, nitrogen has a tendency to donate three electrons and chlorine has a tendency to accept one electron, to complete their outermost shell. Therefore, the Lewis structure of NCl3 contains three NCl bonds and one lone pair on the nitrogen atom.

The Lewis structure of NCl3 is as follows:

Chemistry, Chapter 8, Problem 46QP , additional homework tip  7

b) OCS

The electronic configuration of oxygen, carbon, and sulfur in OCS is as:

O=1s22s22p4C=1s22s22p2S=1s22s22p63s23p4

Oxygen and sulfur atoms contain two valence electrons in their 2p and 3p subshells, respectively and the carbon atom contains four valence electrons in its 2s and 2p subshells. Therefore, carbon has a tendency to donate four electrons, and oxygen and sulfur have a tendency to accept two electrons, to complete their outermost shell. Therefore, the Lewis structure of OCS contains one oxygen-carbon double bond, one carbon-sulfur double bond, and two lone pairs on oxygen and sulfur atoms.

The Lewis structure of OCS is as follows:

Chemistry, Chapter 8, Problem 46QP , additional homework tip  8

c) H2O2

The electronic configuration of oxygen and hydrogen in H2O2 is as:

O=1s22s22p4H=1s1

The oxygen atom contains four valence electrons in its 2p and 3p subshell and the hydrogen atom contains one valence electron in its 1s subshell. Therefore, hydrogen has a tendency to donate one electron and oxygen has a tendency to accept two electrons, to complete their outermost shell. Therefore, the Lewis structure of H2O2 contains two oxygen-hydrogen bonds, one oxygen-oxygen bond, and two lone pairs on oxygen atoms.

The Lewis structure of H2O2 is as follows:

Chemistry, Chapter 8, Problem 46QP , additional homework tip  9

d) CH3COO

The electronic configuration of oxygen, carbon, and hydrogen in CH3COO is as:

O=1s22s22p4C=1s22s22p2H=1s1

The carbon atom has a tendency to form four bonds because of the presence of four valence electrons in its outermost shell, hydrogen has a tendency to form one bond because of the presence of one electron in its outermost shell, and oxygen has a tendency to form two bonds due to the presence of two electrons in its outermost shell.

The Lewis structure of CH3COO is as follows:

Chemistry, Chapter 8, Problem 46QP , additional homework tip  10

e) CN

The electronic configuration of nitrogen and carbon in CN is as:

N=1s22s22p3C=1s22s22p2

Cyanide ion is composed of one triple bond of carbon and nitrogen atom. This species contains one lone pair on both carbon and nitrogen atoms.

The Lewis structure of CN is as follows:

Chemistry, Chapter 8, Problem 46QP , additional homework tip  11

f) CH3CH2NH3+

The electronic configuration of carbon, nitrogen, and hydrogen in CH3CH2NH3+ is as:

N=1s22s22p3C=1s22s22p2H=1s1

Carbon atom has a tendency to form four bonds because of the presence of four valence electrons in its outermost shell, hydrogen has a tendency to form one bond because of the presence of one electron in its outermost shell, and nitrogen has tendency to form four bonds due to the presence of three electrons in its 2p subshell and one lone pair in 2s subshell.

The Lewis structure of CH3CH2NH3+ is as follows:

Chemistry, Chapter 8, Problem 46QP , additional homework tip  12

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Chapter 8 Solutions

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