Chemistry, Books a la Carte Edition and Modified Mastering Chemistry with Pearson eText & ValuePack Access Card (7th Edition)

7th Edition

ISBN: 9780134172514

Author: John E. McMurry

Publisher: PEARSON

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Textbook Question

Chapter 9, Problem 9.150MP

The reaction S 8 ( g ) → 4 S 2 ( g ) has Δ H ° = +237 kJ

(a) The S₈ molecule has eight sulfur atoms arranged in a ring. What is the hybridization and geometry around each sulfur atom in S₈?

(b) The average S-S bond dissociation energy is 225 kJ/mol. Using the value of Δ H ° given above, what is the S=S double bond energy in S₂(g)?

(c) Assuming that the bonding in S₂ is similar to the bonding in O₂, give a molecular orbital description of the bonding in S₂. Is S₂ likely to be paramagnetic or diamagnetic?

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

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Chapter 9, Problem 9.149CP

Chapter 9, Problem 9.151MP

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