Chapter 5, Problem 38A

(a)

Interpretation Introduction

Interpretation: The maximum number of electrons present in the 2s sublevels needs to be determined.

Concept Introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. For any given shell, the number of subshells can be calculated as $2l+1$ . Here, l is an azimuthal quantum number. In each subshell maximum of two electrons (opposite spin) can be occupied. Thus, the maximum number of electrons in a subshell can be calculated using the following formula:

  $\begin{array}{c}X=2\left(2l+1\right)\\ =4l+2\end{array}$

Here, l is an azimuthal quantum number.

Answer to Problem 38A

2

Explanation of Solution

The given orbital is 2s. For s orbital, the value of the azimuthal quantum number is 0. Thus, the maximum number of electrons present in it can be calculated as follows:

  $\begin{array}{l}{X}_{2s}=4l+2\\ =4\left(0\right)+2\\ =2\end{array}$

Therefore, the maximum number of electrons present in the 2s sublevel is 2.

(b)

Interpretation Introduction

Interpretation: The maximum number of electrons present in the 4s sublevels needs to be determined.

Concept Introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. For any given shell, the number of subshells can be calculated as $2l+1$ here, l is an azimuthal quantum number. In each subshell maximum of two electrons (opposite spin) can be occupied. Thus, the maximum number of electrons in a subshell can be calculated using the following formula:

  $\begin{array}{c}X=2\left(2l+1\right)\\ =4l+2\end{array}$

Here, l is an azimuthal quantum number.

Answer to Problem 38A

2

Explanation of Solution

The given orbital is 4s. For s orbital, the value of an azimuthal quantum number is 0. Thus, the maximum number of electrons present in it can be calculated as follows:

  $\begin{array}{l}{X}_{4s}=4l+2\\ =4\left(0\right)+2\\ =2\end{array}$

Therefore, the maximum number of electrons present in the 4s sublevel is 2.

(c)

Interpretation Introduction

Interpretation: The maximum number of electrons present in the 4p sublevels needs to be determined.

Concept Introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. For any given shell, the number of subshells can be calculated as $2l+1$ . Here, l is an azimuthal quantum number. In each subshell maximum of two electrons (opposite spin) can be occupied. Thus, the maximum number of electrons in a subshell can be calculated using the following formula:

  $\begin{array}{c}X=2\left(2l+1\right)\\ =4l+2\end{array}$

Here, l is an azimuthal quantum number.

Answer to Problem 38A

6

Explanation of Solution

The given orbital is 4p. For p orbital, the value of an azimuthal quantum number is 1. Thus, the maximum number of electrons present in it can be calculated as follows:

  $\begin{array}{l}{X}_{4p}=4l+2\\ =4\left(1\right)+2\\ =6\end{array}$

Therefore, the maximum number of electrons present in the 4p sublevel is 6.

(d)

Interpretation Introduction

Interpretation: The maximum number of electrons present in the 4f sublevels needs to be determined.

Concept Introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. For any given shell, the number of subshells can be calculated as $2l+1$ . Here, l is an azimuthal quantum number. In each subshell maximum of two electrons (opposite spin) can be occupied. Thus, the maximum number of electrons in a subshell can be calculated using the following formula:

  $\begin{array}{c}X=2\left(2l+1\right)\\ =4l+2\end{array}$

Here, l is an azimuthal quantum number.

Answer to Problem 38A

14

Explanation of Solution

The given orbital is 4f. For f orbital, the value of an azimuthal quantum number is 3. Thus, the maximum number of electrons present in it can be calculated as follows:

  $\begin{array}{l}{X}_{4f}=4l+2\\ =4\left(3\right)+2\\ =12+2\\ =14\end{array}$

Therefore, the maximum number of electrons present in the 4f sublevel is 14.

(e)

Interpretation Introduction

Interpretation: The maximum number of electrons present in the 3p sublevels needs to be determined.

Concept Introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. For any given shell, the number of subshells can be calculated as $2l+1$ . Here, l is an azimuthal quantum number. In each subshell maximum of two electrons (opposite spin) can be occupied. Thus, the maximum number of electrons in a subshell can be calculated using the following formula:

  $\begin{array}{c}X=2\left(2l+1\right)\\ =4l+2\end{array}$

Here, l is an azimuthal quantum number.

Answer to Problem 38A

6

Explanation of Solution

The given orbital is 3p. For p orbital, the value of an azimuthal quantum number is 1. Thus, the maximum number of electrons present in it can be calculated as follows:

  $\begin{array}{l}{X}_{3p}=4l+2\\ =4\left(1\right)+2\\ =6\end{array}$

Therefore, the maximum number of electrons present in the 3p sublevel is 6.

(f)

Interpretation Introduction

Interpretation: The maximum number of electrons present in the 3d sublevels needs to be determined.

Concept Introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. For any given shell, the number of subshells can be calculated as $2l+1$ . Here, l is an azimuthal quantum number. In each subshell maximum of two electrons (opposite spin) can be occupied. Thus, the maximum number of electrons in a subshell can be calculated using the following formula:

  $\begin{array}{c}X=2\left(2l+1\right)\\ =4l+2\end{array}$

Here, l is an azimuthal quantum number.

Answer to Problem 38A

10

Explanation of Solution

The given orbital is 3d. For d orbital, the value of an azimuthal quantum number is 2. Thus, the maximum number of electrons present in it can be calculated as follows:

  $\begin{array}{l}{X}_{3d}=4l+2\\ =4\left(2\right)+2\\ =10\end{array}$

Therefore, the maximum number of electrons present in the 3d sublevel is 10.

(g)

Interpretation Introduction

Interpretation: The maximum number of electrons present in the 5s sublevels needs to be determined.

Concept Introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. For any given shell, the number of subshells can be calculated as $2l+1$ . Here, l is an azimuthal quantum number. In each subshell maximum of two electrons (opposite spin) can be occupied. Thus, the maximum number of electrons in a subshell can be calculated using the following formula:

  $\begin{array}{c}X=2\left(2l+1\right)\\ =4l+2\end{array}$

Here, l is an azimuthal quantum number.

Answer to Problem 38A

2

Explanation of Solution

The given orbital is 5s. For s orbital, the value of an azimuthal quantum number is 0. Thus, the maximum number of electrons present in it can be calculated as follows:

  $\begin{array}{l}{X}_{5s}=4l+2\\ =4\left(0\right)+2\\ =2\end{array}$

Therefore, the maximum number of electrons present in the 5s sublevel is 2.

(h)

Interpretation Introduction

Interpretation: The maximum number of electrons present in the 5p sublevels needs to be determined.

Concept Introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. For any given shell, the number of subshells can be calculated as $2l+1$ . Here, l is an azimuthal quantum number. In each subshell maximum of two electrons (opposite spin) can be occupied. Thus, the maximum number of electrons in a subshell can be calculated using the following formula:

  $\begin{array}{c}X=2\left(2l+1\right)\\ =4l+2\end{array}$

Here, l is an azimuthal quantum number.

Answer to Problem 38A

6

Explanation of Solution

The given orbital is 5p. For p orbital, the value of an azimuthal quantum number is 1. Thus, the maximum number of electrons present in it can be calculated as follows:

  $\begin{array}{l}{X}_{5p}=4l+2\\ =4\left(1\right)+2\\ =6\end{array}$

Therefore, the maximum number of electrons present in the 5p sublevel is 6.