The statement, “The Lewis structure of H 2 O is bent while that of CO 2 is a linear”, is to be explained. Concept introduction: According to VSEPR theory, the geometry of molecules is based on the force of repulsion between the electron pairs in the valence shell. The electron pairs minimize this repulsion by getting as far away from each other as possible. The number of bonding pairs and lone pairs of electrons determines the shape of the molecule. The order of force of repulsion between the various electron pairs is as follows: lone pair-lone pair > lone pair-bond pair > bond pair-bond pair.

Question

1.1 Define electronegativity and explain why electronegativity increases with atomic number within a period of the Periodic Table. 1.2 Describe the type of bonding that exists in F2 (g) molecule. How does this type of bonding differ from that found in the HF (g) molecule? 1.3 Define hydrogen bonding using examples. 1.4 PH3 and NH3 moleculea are the same shape but the molecules are non-polar and polar respectively. Explain why this is so. 1.5 Give an example of molecule that has a coordinate covalent bond. 1.6 Draw a Lewis structure for each of the following molecules of ions: a) HF3 b) CIO3-

Answer 1

Question

Chapter 5, Problem 4SC

Interpretation Introduction

Interpretation:

The statement, “The Lewis structure of H2O is bent while that of CO2 is a linear”, is to be explained.

Concept introduction:

According to VSEPR theory, the geometry of molecules is based on the force of repulsion between the electron pairs in the valence shell. The electron pairs minimize this repulsion by getting as far away from each other as possible.

The number of bonding pairs and lone pairs of electrons determines the shape of the molecule.

The order of force of repulsion between the various electron pairs is as follows:

lone pair-lone pair > lone pair-bond pair > bond pair-bond pair.

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