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Chemistry

9th Edition
Steven S. Zumdahl
Publisher: Cengage Learning
ISBN: 9781133611097

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BuyFindarrow_forward

Chemistry

9th Edition
Steven S. Zumdahl
Publisher: Cengage Learning
ISBN: 9781133611097
Chapter 9, Problem 92CP
Textbook Problem
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As compared with CO and O2, CS and S2 are very unstable molecules. Give an explanation based on the relative abilities of the sulfur and oxygen atoms to form π bonds.

Interpretation Introduction

Interpretation:

The given molecules CS and S2 is very unstable compared to other two given molecules namely CO and O2 hence using the phi bond forming ability of O and S the reason for their stability should be explained.

Concept Introduction:

Hybridization: The mixing of atomic orbitals gives the equal number of molecular orbitals.

Lewis structures: Diagrams that tell the bonding between atoms in a molecule and the lone pairs of electrons in the molecule.

Add dots for anions and remove dots for cations.  The total number of dots indicates the valence electron of an atom.

VSEPR: Valence shell electron pair repulsion theory is method to predict the geometry of the molecule from the number of electron pairs surrounding the central atom. Idea is that repulsion between electron pairs occurs and increases the separation between the terminal groups or atoms.

To Explain: The stability of CS and S2 molecules using phi bond forming ability of O and S .

Explanation of Solution

  • Comparison between MO of O2 and S2 :

MO of S2 ,

From the above Molecular diagram of oxygen and disulfur , the energy gap between the bonding and anti-bonding in the oxygen is less than the sulfur because oxygen is more electronegative than sulfur reduces the energy gap of the sub-shell in the oxygen. Since, the π - π* splitting is much larger in O2 t

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Chapter 9 Solutions

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