   Chapter 8, Problem 69GQ

Chapter
Section
Textbook Problem

Compare the F—Cl—F angles in CIF2+ and ClF2−. Using Lewis structures, determine the approximate bond angle in each ion. Which ion has the greater bond angle?

Interpretation Introduction

Interpretation: The FClF angles in ClF2+andClF2 has to be compared using its Lewis structures and the ion which has the greater bond angle has to be determined.

Concept Introduction:

Electron-dot structure: It is a diagram in which dots are placed around the chemical symbol of an element to show its valence electrons. It is also called as lewis dot diagrams.

• In VSEPR, the geometry of the molecule is explained based on minimizing electrostatic repulsion between the molecules’ valence electrons around a central atom
• Bond angle is the angle between two bonds of a molecule and it is determined based on the electron-domain geometry.

[Bond angles: tetrahedral = 109.5o, trigonal planar = 120o, T-shape = 90o]

Electron geometry is the shape of a molecule predicted by considering both bond electron pairs and lone pair of electrons.

Molecular geometry is the shape of a molecule predicted by considering only bond pair of electrons

Explanation

Consider the ClF+2ion.

The total number of valence electrons is found to be 211=20

The 16 electrons getting after reducing two electrons for each bond from the total valence electron are distributed on atoms to complete the octet.

Thus the electron dot structure of the compound is given below:

By considering the both bond pair electron and lone pair of electron, the F-Cl-F bond has the tetrahedral electron-pair geometry. Thus the bond angle will be approximately 109°

Consider the ClF2ion.

The total number of valence electrons is found to be 21+1=22

The 18 electrons getting after reducing two electrons for each bond from the total valence electron are distributed on atoms to complete the octet

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