Chapter 9, Problem 9.47QE

(a)

Interpretation Introduction

Interpretation:

The atom that has greater electronegativity among $\text{Br}$ and $\text{I}$ has to be determined.

Concept Introduction:

Electronegativity is defined as ability of an atom to attract the shared electrons in a chemical bond. Electronegativity of atoms relates to many properties, such as ionization energy. Elements with low ionization energies have low electronegativity, and elements with high ionization energies have high electronegativity.

Electronegativity is measured by the relative scale. All elements are compared with the most electronegative element that is as fluorine has an electronegativity value of 4.0. The trend of electronegativity in the group and period is as follows:

1. Group: Electronegativity decreases from top to bottom within a group due to the larger atomic size. The larger distance between the nucleus and the valence electron shell, the lesser the attraction atom has for electrons or protons.

2. Period: Electronegativity increases from left to right across a period. This is due to an increase in nuclear charge. Alkali metals have the lowest electronegativity.

(b)

Interpretation Introduction

Interpretation:

The atom that has greater electronegativity among $\text{S}$ and $\text{Cl}$ has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The atom that has greater electronegativity among $\text{N}$ and $\text{C}$ has to be determined.

Concept Introduction:

Refer to part (a).