Textbook Problem

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For each of the bonds listed below, tell which atom is the more negatively charged.

1. (a) C—N
2. (b) C—H
3. (c) C—Br
4. (d) S—O

Interpretation Introduction

Interpretation: The more negatively charged atom in the given bond should be determined.

Concept Introduction:

Electronegativity: It is defined as the capacity of the atom to abstract the pair of electrons towards itself results to have high negative charge.

Explanation of Solution

$\text{C-N}$

Electronegative atoms are those which are closest to Fluorine atom since electronegativity follows the trend that it increases as we move from left to

Interpretation Introduction

Interpretation: The more negatively charged atom in the given bond should be determined.

Concept Introduction:

Electronegativity: It is defined as the capacity of the atom to abstract the pair of electrons towards itself results to have high negative charge.

Interpretation Introduction

Interpretation: The more negatively charged atom in the given bond should be determined.

Concept Introduction:

Electronegativity: It is defined as the capacity of the atom to abstract the pair of electrons towards itself results to have high negative charge.

Interpretation Introduction

Interpretation: The more negatively charged atom in the given bond should be determined.

Concept Introduction:

Electronegativity: It is defined as the capacity of the atom to abstract the pair of electrons towards itself results to have high negative charge.