Chapter 8, Problem 8.56P

(a)

Interpretation Introduction

Interpretation:

The order of decreasing ${\text{IE}}_1$ of $\text{Na}$, $\text{Li}$, $\text{K}$ is to be arranged.

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 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 difficulty then the value of ionization energy will be very high.

When the first electron is removed from a neutral, isolated gaseous atom then the ionization energy is known as the first ionization energy $\left({\text{IE}}_1\right)$. Similarly when the second electron is removed from the positively charged cation the ionization energy is called the second ionization energy $\left({\text{IE}}_2\right)$ and so on.

(b)

Interpretation Introduction

Interpretation:

The order of decreasing ${\text{IE}}_1$ of $\text{Be}$, $\text{F}$, $\text{C}$ is to be arranged.

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 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 difficulty then the value of ionization energy will be very high.

When the first electron is removed from a neutral, isolated gaseous atom then the ionization energy is known as the first ionization energy $\left({\text{IE}}_1\right)$. Similarly when the second electron is removed from the positively charged cation the ionization energy is called the second ionization energy $\left({\text{IE}}_2\right)$ and so on.

(c)

Interpretation Introduction

Interpretation:

The order of decreasing ${\text{IE}}_1$ of $\text{Cl}$, $\text{Ar}$, $\text{Na}$ is to be arranged.

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 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 difficulty then the value of ionization energy will be very high.

When the first electron is removed from a neutral, isolated gaseous atom then the ionization energy is known as the first ionization energy $\left({\text{IE}}_1\right)$. Similarly when the second electron is removed from the positively charged cation the ionization energy is called the second ionization energy $\left({\text{IE}}_2\right)$ and so on.

(d)

Interpretation Introduction

Interpretation:

The order of decreasing ${\text{IE}}_1$ of $\text{Cl}$, $\text{Br}$, $\text{Se}$ is to be arranged.

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 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 difficulty then the value of ionization energy will be very high.

When the first electron is removed from a neutral, isolated gaseous atom then the ionization energy is known as the first ionization energy $\left({\text{IE}}_1\right)$. Similarly when the second electron is removed from the positively charged cation the ionization energy is called the second ionization energy $\left({\text{IE}}_2\right)$ and so on.