Chapter 4, Problem 4.75QP

(a)

Interpretation Introduction

Interpretation: Ions with a +3 net charge need to be identified for the given set of electronic configurations.

Concept Introduction:

• Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
• According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
• According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals is singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.
• When cation is formed it means the electrons are removed from the outermost orbital of atom.  If anion is formed means then the electrons are added to the atom in its outermost orbital.
• For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.

To identify: Ion with net charge of +1 with electronic configuration of $\text{[Ar]3}{d}^{\text{3}}$.

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (a) is ${\text{Cr}}^{\text{3+}}$

Explanation of Solution

Electronic configuration of $\text{Ar}$ is,

$1s^{2}2s^{2}2p^{6}3s^{2}3p^6$

The electronic configuration of $\text{Ar}$ is found using the total number of electrons present in the atom.  The total number of electrons present in $\text{Ar}$ is 18.  According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $\text{Ar}$ is found as $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.

Ion with net charge as +3 with electronic configuration $\text{[Ar]3}{d}^{\text{3}}$

${\text{Cr}}^{\text{3+}}{\text{ = [Ar]3d}}^{\text{3}}$

Argon is a noble gas and has a complete octet electronic configuration as $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.  If an ion has the same configuration with net charge as +3 and three electrons in “3d” orbital means, that three electrons are removed from the atom having total number of electrons as 24, namely chromium.  This in turn tells that the ion with the net charge of “+3” that has configuration as $\text{[Ar]}$ to be ${\text{Cr}}^{\text{3+}}$ .

(b)

Interpretation Introduction

Interpretation: Ions with a +3 net charge need to be identified for the given set of electronic configurations.

Concept Introduction:

• Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
• According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
• According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals is singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.
• When cation is formed it means the electrons are removed from the outermost orbital of atom.  If anion is formed means then the electrons are added to the atom in its outermost orbital.
• For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.

To identify: Ion with net charge of +3 with electronic configuration of $\text{[Ar]}$.

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (b) is ${\text{Sc}}^{\text{3+}}$

Explanation of Solution

Electronic configuration of $\text{Ar}$

$1s^{2}2s^{2}2p^{6}3s^{2}3p^6$

The electronic configuration of $\text{Ar}$ is found using the total number of electrons present in the atom.  The total number of electrons present in $\text{Ar}$ is 18.  According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $\text{Ar}$ is found as $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.

Ion with net charge as +3 with electronic configuration $\text{[Ar]}$

   ${\text{Sc}}^{\text{3}}{}^{\text{+}}\text{ = [Ar]}$

Argon is a noble gas and has a complete octet electronic configuration as $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.  If an ion has the same configuration with net charge as “+3” means the total number of electrons in the atom is 21, namely scandium.  This in turn tells that the ion with the net charge of “+3” that has configuration as $\text{[Ar]}$ to be ${\text{Sc}}^{\text{3+}}$.

(c)

Interpretation Introduction

Interpretation: Ions with a +3 net charge need to be identified for the given set of electronic configurations.

Concept Introduction:

• Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
• According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
• According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals is singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.
• When cation is formed it means the electrons are removed from the outermost orbital of atom.  If anion is formed means then the electrons are added to the atom in its outermost orbital.
• For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.

To identify: Ion with net charge of +3 with electronic configuration of $\text{[Kr]4}{d}^{\text{6}}$.

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (c) is ${\text{Rh}}^{\text{3+}}$

Explanation of Solution

Electronic configuration of $\text{Kr}$ is,

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$

The electronic configuration of $\text{Kr}$ is found using the total number of electrons present in the atom.  The total number of electrons present in $\text{Kr}$ is 36.  According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $\text{Kr}$ is found as $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$.

Ion with net charge as +3 with electronic configuration $\text{[Kr]4}{d}^{\text{6}}$,

${\text{Rh}}^{\text{3}}{}^{\text{+}}{\text{ = [Kr]4d}}^{\text{6}}$

Krypton is a noble gas and has a complete octet electronic configuration as $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$.  If an ion has the same configuration with net charge as “+3” and six electrons in its 4d orbital means the total number of electrons in the atom is 45, namely rhodium.  This in turn tells that the ion with the net charge of “+3” that has configuration as $\text{[Kr]4}{d}^{\text{6}}$ to be ${\text{Rh}}^{\text{3+}}$.

(d)

Interpretation Introduction

Interpretation: Ions with a +3 net charge need to be identified for the given set of electronic configurations.

Concept Introduction:

• Electronic configuration is the arrangement of the electrons of atoms in the orbital.  For atoms and ions the electronic configuration are written by using Pauli Exclusion Principle and Hund’s rule.
• According to Pauli Exclusion Principle, no two electrons having the same spin can occupy the same orbital.
• According to Hund’s rule, the orbital in the subshell is filled singly by one electron before the same orbital is doubly filled.  When the orbitals is singly filled, all the electrons have same spin.  In a doubly filled orbital, there are two electrons with opposite spin.
• When cation is formed it means the electrons are removed from the outermost orbital of atom.  If anion is formed means then the electrons are added to the atom in its outermost orbital.
• For simpler representation of ions or atoms, the electronic configuration of the completed octet noble gas configuration is considered and the remaining orbital alone is shown explicitly.

To identify: Ion with net charge of +3 with electronic configuration of $\text{[Xe]4}{f}^{\text{14}}5d^{\text{6}}$.

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (d) is ${\text{Ir}}^{\text{3+}}$

Explanation of Solution

Electronic configuration of $\text{Xe}$ is,

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^6$

The electronic configuration of $\text{Xe}$ is found using the total number of electrons present in the atom.  The total number of electrons present in $\text{Xe}$ is 54.  According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $\text{Xe}$ is found as $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^6$.

Ion with net charge as +3 with electronic configuration $\text{[Xe]4}{f}^{\text{14}}5d^{\text{6}}$

${\text{Ir}}^{\text{3}}{}^{\text{+}}{\text{ = [Xe]4f}}^{\text{14}}{\text{5d}}^{\text{6}}$

Xenon is a noble gas and has a complete octet electronic configuration as $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^6$.  If an ion has the same configuration with net charge as “+3” and six electrons in its 5d orbital along with fourteen electrons in 4f orbital means the total number of electrons in the atom is 77, namely iridium.  This in turn tells that the ion with the net charge of “+3” that has configuration as $\text{[Xe]4}{f}^{\text{14}}5d^{\text{6}}$ to be ${\text{Ir}}^{\text{3+}}$.