Chapter 3, Problem 3.118MP

(a)

Interpretation Introduction

Interpretation:

The electronic configuration of ${\text{Fe}}^{\text{2+}}\text{and}{\text{Fe}}^{\text{3+}}$ ions have to be given.

(b)

Interpretation Introduction

Interpretation:

The quantum numbers n and l values of outermost electron of ${\text{Fe}}^{\text{2+}}\text{and}{\text{Fe}}^{\text{3+}}$ ions have to be identified.

(c)

Interpretation Introduction

Interpretation:

The highest probable wavelength of light that can ionize iron if the third ionization energy is $\text{+2952 kJ/mol}$ has to be calculated.

Concept introduction:

Ionization energy:

In a gaseous state isolated neutral atom, the amount of energy required to eject an electron from outermost shell is known as ionization energy. Ionization energy increases from left to right across periods due to increase of effective nuclear charge. Ionization energy decreases down the group due to addition of electrons enters into new orbital which is far from nucleus.

(d)

Interpretation Introduction

Interpretation:

The third ionization energy of ruthenium and iron has to be compared.

Concept introduction:

Ionization energy:

In a gaseous state isolated neutral atom, the amount of energy required to eject an electron from outermost shell is known as ionization energy. Ionization energy increases from left to right across periods due to increase of effective nuclear charge. Ionization energy decreases down the group due to addition of electrons enters into new orbital which is far from nucleus.