Chapter 12, Problem 52E

A monatomic ion with a $2-$ charge has the electron configuration $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$. (a) What neutral noble gas atom has the same electron configuration? (b) What is the monatomic ion with $2-$ charge that has this configuration reaction? (c) Write the symbol of an ion with a $1+$ charge that is isoelectronic with the species in (a) and (b).

Interpretation Introduction

(a)

Interpretation:

The noble gas atom having electron configuration, $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$, is to be stated.

Concept introduction:

Electronic configuration is the ground state distribution of electrons among the orbital of species. Electronic configuration of an atom defines many chemical properties of an atom.

The number of electrons present in the highest occupied energy level is known as valence electrons.

Answer to Problem 52E

The noble gas atom having electron configuration, $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$, is krypton $\left(\text{Kr}\right)$.

Explanation of Solution

The electron configuration of noble gas atom is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$. Therefore, the total number of electron in noble gas atom is $36$. Total number of electron represents the atomic number of an atom. The atomic number of noble gas atom is $36$. Therefore, the noble gas atom having electron configuration, $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$, is krypton $\left(\text{Kr}\right)$.

Conclusion

The noble gas atom having electron configuration, $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$, is krypton $\left(\text{Kr}\right)$.

Interpretation Introduction

(b)

Interpretation:

The monatomic ion with $2-$ charge having electron configuration, $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$, is to be stated.

Concept introduction:

Electronic configuration is the ground state distribution of electrons among the orbital of species. Electronic configuration of an atom defines many chemical properties of an atom.

The number of electrons present in the highest occupied energy level is known as valence electrons.

Answer to Problem 52E

The monatomic ion with $2-$ charge having electron configuration, $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$, is selenide ion $\left({\text{Se}}^{2-}\right)$.

Explanation of Solution

The electron configuration of monatomic ion with $2-$ charge is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$. Therefore, the total number of electron in monatomic ion with $2-$ charge is $36$. The total number of electron in neutral atom is $\text{Z}=36-2=34$. Total number of electron represents the atomic number of an atom. Therefore, the neutral atom having atomic number $34$ is selenium $\left(\text{Se}\right)$. The monatomic ion with $2-$ charge is selenide ion $\left({\text{Se}}^{2-}\right)$.

Conclusion

The monatomic ion with $2-$ charge having electron configuration, $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$, is selenide ion $\left({\text{Se}}^{2-}\right)$.

Interpretation Introduction

(c)

Interpretation:

An ion with a $1+$ charge that is isoelectronic with the krypton $\left(\text{Kr}\right)$ and selenide ion $\left({\text{Se}}^{2-}\right)$, is to be stated.

Concept introduction:

Electronic configuration is the ground state distribution of electrons among the orbital of species. Electronic configuration of an atom defines many chemical properties of an atom.

The number of electrons present in the highest occupied energy level is known as valence electrons.

Answer to Problem 52E

An ion with a $1+$ charge that is isoelectronic with the krypton $\left(\text{Kr}\right)$ and selenide ion $\left({\text{Se}}^{2-}\right)$, is rubidium ion $\left({\text{Rb}}^{+}\right)$.

Explanation of Solution

Total number of electron in krypton $\left(\text{Kr}\right)$ and selenide ion is $36$. Therefore, the total number of electron in ion with a $1+$ charge is $36$. The total number of electron in neutral atom is $\text{Z}=36+1=37$. Total number of electron represents the atomic number of an atom. Therefore the neutral atom having atomic number $37$ is rubidium $\left(\text{Rb}\right)$. The ion with a $1+$ charge is rubidium ion $\left({\text{Rb}}^{+}\right)$.

Conclusion

An ion with a $1+$ charge that is isoelectronic with the krypton $\left(\text{Kr}\right)$ and selenide ion $\left({\text{Se}}^{2-}\right)$, is rubidium ion $\left({\text{Rb}}^{+}\right)$.