Chapter 3, Problem 3.29E

Interpretation Introduction

(a)

Interpretation:

The symbol and name for an element that contains one unpaired $5p$ electron is to be predicted.

Concept introduction:

The elements in a modern periodic table are arranged in increasing order of their atomic number. In the modern periodic table, the horizontal rows are known as periods and vertical columns are known as groups. There are $7$ periods and $18$ groups in modern periodic table.

Answer to Problem 3.29E

The name of an element that contains one unpaired $5p$ electron is indium and its symbol is $\text{In}$ respectively.

Explanation of Solution

Electronic configuration tells about the arrangement of the electrons in each subshell and orbit of an atom.

The electronic configuration for an element that contains one unpaired $5p$ electron would be $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^1$. Thus, the total number of electrons is $49$. The number of electrons corresponds to the atomic number of an element. Therefore, the atomic number of an element is $49$ that is indium. The symbol used for indium is $\text{In}$.

Conclusion

The name of the element that contains one unpaired $5p$ electron is indium and its symbol is $\text{In}$ respectively.

Interpretation Introduction

(b)

Interpretation:

The symbol and name for an element that contains a half-filled $5s$ electron is to be predicted.

Concept introduction:

The elements in a modern periodic table are arranged in increasing order of their atomic number. In the modern periodic table, the horizontal rows are known as periods and vertical columns are known as groups. There are $7$ periods and $18$ groups in modern periodic table.

Answer to Problem 3.29E

The name of an element that contains a half-filled $5s$ electron is rubidium and its symbol is $\text{Rb}$ respectively.

Explanation of Solution

Electronic configuration tells about the arrangement of the electrons in each subshell and orbit of an atom.

The electronic configuration for an element that contains a half-filled $5s$ electron would be $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^1$. Thus, the total number of electrons is $37$. The number of electrons corresponds to the atomic number of an element. Therefore, the atomic number of an element is $37$ that is rubidium. The symbol used for rubidium is $\text{Rb}$

Conclusion

The name of an element that contains a half-filled $5s$ electron is rubidium and its symbol is $\text{Rb}$ respectively.

Interpretation Introduction

(c)

Interpretation:

The symbol and name for an element that contains half-filled $6p$ electrons is to be predicted.

Concept introduction:

The elements in a modern periodic table are arranged in increasing order of their atomic number. In the modern periodic table, the horizontal rows are known as periods and vertical columns are known as groups. There are $7$ periods and $18$ groups in modern periodic table.

Answer to Problem 3.29E

The name of an element that contains half-filled $6p$ electrons is bismuth and its symbol is $\text{Bi}$ respectively.

Explanation of Solution

Electronic configuration tells about the arrangement of the electrons in each subshell and orbit of an atom.

The electronic configuration for an element that contains a half-filled $6p$ electrons would be $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^3$. The $4s$ and $5s$ orbitals are filled first because the energy of $4s$ and $5s$ orbital is lower than the $3d$ and $4d$. Thus, the total number of electrons is $83$. The number of electrons corresponds to the atomic number of an element. Therefore, the atomic number of an element is $83$ that is bismuth. The symbol used for bismuth is $\text{Bi}$.

Conclusion

The name of an element that contains half-filled $6p$ electrons is bismuth and its symbol is $\text{Bi}$ respectively.

Interpretation Introduction

(d)

Interpretation:

The symbol and name for an element in which last electron completes the $4d$ subshell is to be predicted.

Concept introduction:

The elements in a modern periodic table are arranged in increasing order of their atomic number. In the modern periodic table, the horizontal rows are known as periods and vertical columns are known as groups. There are $7$ periods and $18$ groups in modern periodic table.

Answer to Problem 3.29E

The name of an element in which the last electron completes the $4d$ subshell is palladium and its symbol is $\text{Pd}$ respectively.

Explanation of Solution

Electronic configuration tells about the arrangement of the electrons in each subshell and orbit of an atom.

The electronic configuration for an element in which the last electron completes the $4d$ subshell would be $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}$. The $4s$ and $5s$ orbitals are filled first because the energy of $4s$ and $5s$ orbital is lower than the $3d$ and $4d$. Thus, the total number of electrons is $46$. The number of electrons corresponds to the atomic number of an element. Therefore, the atomic number of an element is $46$ that is palladium. The symbol used for palladium is $\text{Pd}$.

Conclusion

The name of an element in which the last electron completes the $4d$ subshell is palladium and its symbol is $\text{Pd}$ respectively.

Interpretation Introduction

(e)

Interpretation:

The symbol and name for the element in which the last electron half fills the $4f$ subshell is to be predicted.

Concept introduction:

The elements in a modern periodic table are arranged in increasing order of their atomic number. In the modern periodic table, the horizontal rows are known as periods and vertical columns are known as groups. There are $7$ periods and $18$ groups in modern periodic table.

Answer to Problem 3.29E

The name of an element in which the last electron half fills the $4f$ subshell is europium. The symbol used for europium is $\text{Eu}$.

Explanation of Solution

Electronic configuration tells about the arrangement of the electrons in each subshell and orbit of an atom.

The electronic configuration for an element in which the last electron half fills the $4f$ subshell would be $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^7$. The $4s$ and $5s$ orbitals are filled first because the energy of $4s$ and $5s$ orbital is lower than the $3d$ and $4d$. Thus, the total number of electrons is $63$. The number of electrons corresponds to the atomic number of an element. Therefore, the atomic number of an element is $63$ that is palladium. The symbol used for europium is $\text{Eu}$.

Conclusion

The name of an element in which the last electron half fills the $4f$ subshell is europium. The symbol used for europium is $\text{Eu}$.