   Chapter 8.10, Problem 3.3ACP

Chapter
Section
Textbook Problem

Calculate the electronegativity of sulfur atoms using ionization energy and electron attachment enthalpy values (Appendix F). Compare the value with the one in Figure 8.11.

Interpretation Introduction

Interpretation: The electronegativity of sulphur atoms should be calculated using ionization energy and electron attachment enthalpy values which should be compared with the electronegativity value of given atom.

Concept Introduction:

Electronegativity: It is defined as the capacity of the atom to abstract the pair of electrons towards itself results to have high negative charge.

Polar molecule: The molecule consists of atoms bonded with different electronegativity. Dipole moment is used to measure the polarity of the molecule.

Polarity of a molecule is measured in term of dipole moment.

Dipole moment for a polar molecule is non-zero and for a non-polar molecule dipole moment is zero.

Bond dissociation enthalpy: Bond energy or more correctly the bond dissociation enthalpy is the enthalpy change when breaking a bond in a molecule with the reactant and products in the gas phase. The process of breaking bonds in a molecule is always endothermic, so ΔrH for bond breaking is always positive.

Explanation

The electronegativity of sulphur atom using ionization energy and electron attachment enthalpy values was determined by using the following equation.

XA = 1.97×10-3(IE - ΔEAH)+ 0.19

XS = 1.97×10-3(IE-ΔEAH)+0

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