Chapter 9, Problem 9.4P

(a)

Interpretation Introduction

Interpretation:

The more metallic element among $\text{Na}$ and $\text{Cs}$ is to be determined.

Concept introduction:

The metallic character is characterized by the tendency of metals to lose their outermost valence shell electrons. Greater the ease of electron removal, higher will be the electropositivity of the corresponding elements and vice versa.

The metallic character is characterized by the tendency of metals to lose their outermost valence shell electrons.

Down the group, the number of shells increases with the increase in the atomic number and the outermost valence electrons becomes farther from the nucleus and therefore can be removed easily. So the metallic character increases from top to bottom in a group.

Along the period, the electrons are added in the same outer shell and the effective nuclear charge increases due to which the electrons are attracted to the nucleus by strong electrostatic forces of attraction. Therefore the removal of the electron becomes difficult which results in the decrease of metallic character in a period.

(b)

Interpretation Introduction

Interpretation:

The more metallic element among $\text{Mg}$ and $\text{Rb}$ is to be determined.

Concept introduction:

The metallic character is characterized by the tendency of metals to lose their outermost valence shell electrons. Greater the ease of electron removal, higher will be the electropositivity of the corresponding elements and vice versa.

The metallic character is characterized by the tendency of metals to lose their outermost valence shell electrons.

Down the group, the number of shells increases with the increase in the atomic number and the outermost valence electrons becomes farther from the nucleus and therefore can be removed easily. So the metallic character increases from top to bottom in a group.

Along the period, the electrons are added in the same outer shell and the effective nuclear charge increases due to which the electrons are attracted to the nucleus by strong electrostatic forces of attraction. Therefore the removal of the electron becomes difficult which results in the decrease of metallic character in a period.

(c)

Interpretation Introduction

Interpretation:

The more metallic element among $\text{As}$ and $\text{N}$ is to be determined.

Concept introduction:

The metallic character is characterized by the tendency of metals to lose their outermost valence shell electrons. Greater the ease of electron removal, higher will be the electropositivity of the corresponding elements and vice versa.

The metallic character is characterized by the tendency of metals to lose their outermost valence shell electrons.

Down the group, the number of shells increases with the increase in the atomic number and the outermost valence electrons becomes farther from the nucleus and therefore can be removed easily. So the metallic character increases from top to bottom in a group.

Along the period, the electrons are added in the same outer shell and the effective nuclear charge increases due to which the electrons are attracted to the nucleus by strong electrostatic forces of attraction. Therefore the removal of the electron becomes difficult which results in the decrease of metallic character in a period.