Chapter 12, Problem 12.32E

Interpretation Introduction

(a)

Interpretation:

The possible ways by which the electrons in the outermost shell of $\text{Li}$ can occupy spin orbitals and satisfy Hund’s rule are to be stated.

Concept introduction:

According to the Aufbau principle, the electrons are firstly filled into the orbitals having lower energy. The electrons are filled in the orbitals as,

$\begin{array}{l}1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s<5f<6d<7p\end{array}$

Hund’s rule states that all the degenerate orbitals are firstly filled with one electron each and then paired. This rule favors unpaired electrons in the orbital.

Interpretation Introduction

(b)

Interpretation:

The possible ways by which the electrons in the outermost shell of $\text{C}$ can occupy spin orbitals and satisfy Hund’s rule are to be stated.

Concept introduction:

According to the Aufbau principle, the electrons are firstly filled into the orbitals having lower energy. The electrons are filled in the orbitals as,

$\begin{array}{l}1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s<5f<6d<7p\end{array}$

Hund’s rule states that all the degenerate orbitals are firstly filled with one electron each and then paired. This rule favors unpaired electrons in the orbital.

Interpretation Introduction

(c)

Interpretation:

The possible ways by which the electrons in the outermost shell of $\text{K}$ can occupy spin orbitals and satisfy Hund’s rule are to be stated.

Concept introduction:

According to the Aufbau principle, the electrons are firstly filled into the orbitals having lower energy. The electrons are filled in the orbitals as,

$\begin{array}{l}1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s<5f<6d<7p\end{array}$

Hund’s rule states that all the degenerate orbitals are firstly filled with one electron each and then paired. This rule favors unpaired electrons in the orbital.

Interpretation Introduction

(d)

Interpretation:

The possible ways by which the electrons in the outermost shell of $\text{Be}$ can occupy spin orbitals and satisfy Hund’s rule are to be stated.

Concept introduction:

According to the Aufbau principle, the electrons are firstly filled into the orbitals having lower energy. The electrons are filled in the orbitals as,

$\begin{array}{l}1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s<5f<6d<7p\end{array}$

Hund’s rule states that all the degenerate orbitals are firstly filled with one electron each and then paired. This rule favors unpaired electrons in the orbital.

Interpretation Introduction

(e)

Interpretation:

The possible ways by which the electrons in the outermost shell of $\text{U}$ can occupy spin orbitals and satisfy Hund’s rule are to be stated.

Concept introduction:

According to the Aufbau principle, the electrons are firstly filled into the orbitals having lower energy. The electrons are filled in the orbitals as,

$\begin{array}{l}1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s<5f<6d<7p\end{array}$

Hund’s rule states that all the degenerate orbitals are firstly filled with one electron each and then paired. This rule favors unpaired electrons in the orbital.