Chapter 10, Problem 10.93SP

(a)

Interpretation Introduction

Interpretation: In the pair of $\text{H}$ and ${\text{H}}_2$, the one with the higher first ionization energy have to be found and explained.

Concept Introduction:

Ionization energy is the energy required to remove an electron from an isolated gaseous atom or ion.

The first or initial ionization energy is the energy required to remove one mole of electron from the one of an isolated gaseous atom or ion.

Trends of ionization energy:

It is well known that bonding molecular orbitals have lower energy than the atomic orbitals whereas anti-bonding molecular orbitals have higher energy than the atomic orbitals. So the electrons in the bonding molecular orbitals will be more stabilized than that in the anti-bonding molecular orbitals. Thus the first ionization energy will be higher for removing one mole of electron from the bonding molecular orbital and it will be lower for removing one mole of electron from the anti-bonding molecular orbital.

(b)

Interpretation Introduction

Interpretation: In the pair of $\text{N}$ and ${\text{N}}_2$, the one with the higher first ionization energy have to be found out and explained.

Concept Introduction:

Ionization energy is the energy required to remove an electron from an isolated gaseous atom or ion.

The first or initial ionization energy is the energy required to remove one mole of electron from the one of an isolated gaseous atom or ion.

Trends of ionization energy:

It is well known that bonding molecular orbitals have lower energy than the atomic orbitals whereas anti-bonding molecular orbitals have higher energy than the atomic orbitals. So the electrons in the bonding molecular orbitals will be more stabilized than that in the anti-bonding molecular orbitals. Thus the first ionization energy will be higher for removing one mole of electron from the bonding molecular orbital and it will be lower for removing one mole of electron from the anti-bonding molecular orbital.

(c)

Interpretation Introduction

Interpretation: In the pair of $\text{O}$ and ${\text{O}}_2$, the one with the higher first ionization energy have to be found out and explained.

Concept Introduction:

Ionization energy is the energy required to remove an electron from an isolated gaseous atom or ion.

The first or initial ionization energy is the energy required to remove one mole of electron from the one of an isolated gaseous atom or ion.

Trends of ionization energy:

It is well known that bonding molecular orbitals have lower energy than the atomic orbitals whereas anti-bonding molecular orbitals have higher energy than the atomic orbitals. So the electrons in the bonding molecular orbitals will be more stabilized than that in the anti-bonding molecular orbitals. Thus the first ionization energy will be higher for removing one mole of electron from the bonding molecular orbital and it will be lower for removing one mole of electron from the anti-bonding molecular orbital.

(d)

Interpretation Introduction

Interpretation: In the pair of $\text{F}$ and ${\text{F}}_2$, the one with the higher first ionization energy have to be found out and explained.

Concept Introduction:

Ionization energy is the energy required to remove an electron from an isolated gaseous atom or ion.

The first or initial ionization energy is the energy required to remove one mole of electron from the one of an isolated gaseous atom or ion.

Trends of ionization energy:

It is well known that bonding molecular orbitals have lower energy than the atomic orbitals whereas anti-bonding molecular orbitals have higher energy than the atomic orbitals. So the electrons in the bonding molecular orbitals will be more stabilized than that in the anti-bonding molecular orbitals. Thus the first ionization energy will be higher for removing one mole of electron from the bonding molecular orbital and it will be lower for removing one mole of electron from the anti-bonding molecular orbital.