Chapter 8, Problem 8.21P

(a)

Interpretation Introduction

Interpretation:

The full set of possible quantum numbers for the outermost electron in $\text{Rb}$ atom is to be determined.

Concept introduction:

The electrons in the outermost occupied shell that determine the chemical properties of the elements are called the outermost electrons.

The quantum numbers provide complete information about the electron. There are four quantum numbers as follows:

1. The principal quantum number and it is represented by n. It tells about the shell to which the electron belongs.

2. The azimuthal quantum number and it is represented by l. It tells about the subshell of the electrons.

3. The magnetic quantum number and it is represented by $m_l$. It tells about the orbitals present in the subshell. The value of $m_l$ ranges from $l$ to $-l$ including 0.

4. The spin quantum number and it is represented by $m_s$. It tells about the spin of the electron and its value can either be $+\frac{\text{1}}{\text{2}}$ or $-\frac{\text{1}}{\text{2}}$.

(b)

Interpretation Introduction

Interpretation:

The full set of possible quantum numbers for the electron gained when an ${\text{S}}^{-}$ ion becomes an ${\text{S}}^2{}^{-}$ ion is to be determined.

Concept introduction:

The quantum numbers provide complete information about the electron. There are four quantum numbers as follows:

1. The principal quantum number and it is represented by n. It tells about the shell to which the electron belongs.

2. The azimuthal quantum number and it is represented by l. It tells about the subshell of the electrons.

3. The magnetic quantum number and it is represented by $m_l$. It tells about the orbitals present in the subshell. The value of $m_l$ ranges from $l$ to $-l$ including 0.

4. The spin quantum number and it is represented by $m_s$. It tells about the spin of the electron and its value can either be $+\frac{\text{1}}{\text{2}}$ or $-\frac{\text{1}}{\text{2}}$.

(c)

Interpretation Introduction

Interpretation:

The full set of possible quantum numbers for the electron lost when an $\text{Ag}$ atom ionizes is to be determined.

Concept introduction:

The quantum numbers provide complete information about the electron. There are four quantum numbers as follows:

1. The principal quantum number and it is represented by n. It tells about the shell to which the electron belongs.

2. The azimuthal quantum number and it is represented by l. It tells about the subshell of the electrons.

3. The magnetic quantum number and it is represented by $m_l$. It tells about the orbitals present in the subshell. The value of $m_l$ ranges from $l$ to $-l$ including 0.

4. The spin quantum number and it is represented by $m_s$. It tells about the spin of the electron and its value can either be $+\frac{\text{1}}{\text{2}}$ or $-\frac{\text{1}}{\text{2}}$.

(d)

Interpretation Introduction

Interpretation:

The full set of possible quantum numbers for the electron gained when an ${\text{F}}^{-}$ ion is formed from $\text{F}$ atom is to be determined.

Concept introduction:

The quantum numbers provide complete information about the electron. There are four quantum numbers as follows:

1. The principal quantum number and it is represented by n. It tells about the shell to which the electron belongs.

2. The azimuthal quantum number and it is represented by l. It tells about the subshell of the electrons.

3. The magnetic quantum number and it is represented by $m_l$. It tells about the orbitals present in the subshell. The value of $m_l$ ranges from $l$ to $-l$ including 0.

4. The spin quantum number and it is represented by $m_s$. It tells about the spin of the electron and its value can either be $+\frac{\text{1}}{\text{2}}$ or $-\frac{\text{1}}{\text{2}}$.