Chapter 9, Problem 9.85P

(a)

Interpretation Introduction

Interpretation:

Whether it is easier to remove an electron from a gaseous silver atom or from the surface of solid silver is to be determined.

Concept introduction:

The ionization energy is the amount of energy required to remove the most loosely bound valence electrons from an isolated neutral gaseous atom. It is represented by $\text{IE}$.

Its value varies with the ease of removal of the outermost valence electron. If the outermost electron is removed very easily then the value of ionization energy is very small. If the electron is removed with quite a difficulty then the value of ionization energy will be very high $\text{IE}$

When the first electron is removed from a neutral, isolated gaseous atom then the ionization energy is known as the first ionization energy. Similarly, when the second electron is removed from the positively charged cation the ionization energy is called the second ionization energy and so on.

(b)

Interpretation Introduction

Interpretation:

The reason for the easy removal of an electron from the surface of solid silver than a gaseous silver atom in terms of the electron-sea model of metallic bonding is to be determined.

Concept introduction:

Metallic bonds are formed between metals. A metallic bond is formed between positively charged ions in a sea of delocalized electrons. The electrons in metals are delocalized over the entire metal.

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.