   # Given that the ionization energy of F 2 − is 290 kJ/mol, do the following: a. Calculate the bond energy of F 2 − . You will need to look up the bond energy of F2 and ionization energy of F − . b. Explain the difference in bond energy between F 2 − and F 2 using MO theory. ### Chemistry: An Atoms First Approach

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

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 4, Problem 122CP
Textbook Problem
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## Given that the ionization energy of F2− is 290 kJ/mol, do the following:a. Calculate the bond energy of F2−. You will need to look up the bond energy of F2 and ionization energy of F−.b. Explain the difference in bond energy between F2− and F2 using MO theory.

(a)

Interpretation Introduction

Interpretation: The ionization energy of the F2 ion has been given. The various satted questions are to be answered using this given value.

Concept introduction: Bond energy is defined as the amount of energy required to break a chemical bond. It can be determined by the addition of the ionization energy, bond dissociation energy and the electron affinity values.

The bond order is calculated by difference between the anti-bonding electrons and the bonding electrons by two. This can be stated as,

Bondorder=[(Electronsinbondingorbitals)(Electronsinanti-bondingorbitals)]2

To determine: The bond energy of F2.

### Explanation of Solution

Given

Ionization energy of F2=290kJ

F2F2+1eΔE1=290kJ/mol

The bond dissociation energy of the F2 molecule is 154kJ.

F2(g)F(g)+F(g)ΔE2=154kJ/mol

The formation of the F ions is,

F(g)+eF

(b)

Interpretation Introduction

To determine: The difference between the bond energy between F2 ion and the F2 molecule, on the basis of the molecular orbital theory.

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