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 [Ar]3 d 3 .

Question

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Answer 1

Question

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 $[Ar]3d3$ .

(a)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (a) is $Cr3+$

Explanation of Solution

Electronic configuration of $Ar$ is,

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]3d3$

$Cr3+ = [Ar]3d3$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Cr3+$ .

(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 $[Ar]$ .

(b)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (b) is $Sc3+$

Explanation of Solution

Electronic configuration of $Ar$

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]$

$Sc3+ = [Ar]$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Sc3+$ .

(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 $[Kr]4d6$ .

(c)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (c) is $Rh3+$

Explanation of Solution

Electronic configuration of $Kr$ is,

$1s22s22p63s23p64s23d104p6$

The electronic configuration of $Kr$ is found using the total number of electrons present in the atom. The total number of electrons present in $Kr$ is 36. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Kr$ is found as $1s22s22p63s23p64s23d104p6$ .

Ion with net charge as +3 with electronic configuration $[Kr]4d6$ ,

$Rh3+ = [Kr]4d6$

Krypton is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p6$ . 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 $[Kr]4d6$ to be $Rh3+$ .

(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 $[Xe]4f145d6$ .

(d)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (d) is $Ir3+$

Explanation of Solution

Electronic configuration of $Xe$ is,

$1s22s22p63s23p64s23d104p65s24d105p6$

The electronic configuration of $Xe$ is found using the total number of electrons present in the atom. The total number of electrons present in $Xe$ is 54. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Xe$ is found as $1s22s22p63s23p64s23d104p65s24d105p6$ .

Ion with net charge as +3 with electronic configuration $[Xe]4f145d6$

$Ir3+ = [Xe]4f145d6$

Xenon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p65s24d105p6$ . 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 $[Xe]4f145d6$ to be $Ir3+$ .

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Answer 2

Question

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 $[Ar]3d3$ .

(a)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (a) is $Cr3+$

Explanation of Solution

Electronic configuration of $Ar$ is,

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]3d3$

$Cr3+ = [Ar]3d3$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Cr3+$ .

(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 $[Ar]$ .

(b)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (b) is $Sc3+$

Explanation of Solution

Electronic configuration of $Ar$

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]$

$Sc3+ = [Ar]$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Sc3+$ .

(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 $[Kr]4d6$ .

(c)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (c) is $Rh3+$

Explanation of Solution

Electronic configuration of $Kr$ is,

$1s22s22p63s23p64s23d104p6$

The electronic configuration of $Kr$ is found using the total number of electrons present in the atom. The total number of electrons present in $Kr$ is 36. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Kr$ is found as $1s22s22p63s23p64s23d104p6$ .

Ion with net charge as +3 with electronic configuration $[Kr]4d6$ ,

$Rh3+ = [Kr]4d6$

Krypton is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p6$ . 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 $[Kr]4d6$ to be $Rh3+$ .

(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 $[Xe]4f145d6$ .

(d)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (d) is $Ir3+$

Explanation of Solution

Electronic configuration of $Xe$ is,

$1s22s22p63s23p64s23d104p65s24d105p6$

The electronic configuration of $Xe$ is found using the total number of electrons present in the atom. The total number of electrons present in $Xe$ is 54. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Xe$ is found as $1s22s22p63s23p64s23d104p65s24d105p6$ .

Ion with net charge as +3 with electronic configuration $[Xe]4f145d6$

$Ir3+ = [Xe]4f145d6$

Xenon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p65s24d105p6$ . 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 $[Xe]4f145d6$ to be $Ir3+$ .

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Answer 3

Question

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 $[Ar]3d3$ .

(a)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (a) is $Cr3+$

Explanation of Solution

Electronic configuration of $Ar$ is,

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]3d3$

$Cr3+ = [Ar]3d3$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Cr3+$ .

(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 $[Ar]$ .

(b)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (b) is $Sc3+$

Explanation of Solution

Electronic configuration of $Ar$

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]$

$Sc3+ = [Ar]$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Sc3+$ .

(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 $[Kr]4d6$ .

(c)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (c) is $Rh3+$

Explanation of Solution

Electronic configuration of $Kr$ is,

$1s22s22p63s23p64s23d104p6$

The electronic configuration of $Kr$ is found using the total number of electrons present in the atom. The total number of electrons present in $Kr$ is 36. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Kr$ is found as $1s22s22p63s23p64s23d104p6$ .

Ion with net charge as +3 with electronic configuration $[Kr]4d6$ ,

$Rh3+ = [Kr]4d6$

Krypton is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p6$ . 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 $[Kr]4d6$ to be $Rh3+$ .

(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 $[Xe]4f145d6$ .

(d)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (d) is $Ir3+$

Explanation of Solution

Electronic configuration of $Xe$ is,

$1s22s22p63s23p64s23d104p65s24d105p6$

The electronic configuration of $Xe$ is found using the total number of electrons present in the atom. The total number of electrons present in $Xe$ is 54. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Xe$ is found as $1s22s22p63s23p64s23d104p65s24d105p6$ .

Ion with net charge as +3 with electronic configuration $[Xe]4f145d6$

$Ir3+ = [Xe]4f145d6$

Xenon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p65s24d105p6$ . 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 $[Xe]4f145d6$ to be $Ir3+$ .

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Answer 4

Question

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 $[Ar]3d3$ .

(a)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (a) is $Cr3+$

Explanation of Solution

Electronic configuration of $Ar$ is,

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]3d3$

$Cr3+ = [Ar]3d3$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Cr3+$ .

(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 $[Ar]$ .

(b)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (b) is $Sc3+$

Explanation of Solution

Electronic configuration of $Ar$

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]$

$Sc3+ = [Ar]$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Sc3+$ .

(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 $[Kr]4d6$ .

(c)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (c) is $Rh3+$

Explanation of Solution

Electronic configuration of $Kr$ is,

$1s22s22p63s23p64s23d104p6$

The electronic configuration of $Kr$ is found using the total number of electrons present in the atom. The total number of electrons present in $Kr$ is 36. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Kr$ is found as $1s22s22p63s23p64s23d104p6$ .

Ion with net charge as +3 with electronic configuration $[Kr]4d6$ ,

$Rh3+ = [Kr]4d6$

Krypton is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p6$ . 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 $[Kr]4d6$ to be $Rh3+$ .

(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 $[Xe]4f145d6$ .

(d)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (d) is $Ir3+$

Explanation of Solution

Electronic configuration of $Xe$ is,

$1s22s22p63s23p64s23d104p65s24d105p6$

The electronic configuration of $Xe$ is found using the total number of electrons present in the atom. The total number of electrons present in $Xe$ is 54. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Xe$ is found as $1s22s22p63s23p64s23d104p65s24d105p6$ .

Ion with net charge as +3 with electronic configuration $[Xe]4f145d6$

$Ir3+ = [Xe]4f145d6$

Xenon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p65s24d105p6$ . 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 $[Xe]4f145d6$ to be $Ir3+$ .

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Answer 5

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 $[Ar]3d3$ .

(a)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (a) is $Cr3+$

Explanation of Solution

Electronic configuration of $Ar$ is,

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]3d3$

$Cr3+ = [Ar]3d3$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Cr3+$ .

(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 $[Ar]$ .

(b)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (b) is $Sc3+$

Explanation of Solution

Electronic configuration of $Ar$

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]$

$Sc3+ = [Ar]$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Sc3+$ .

(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 $[Kr]4d6$ .

(c)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (c) is $Rh3+$

Explanation of Solution

Electronic configuration of $Kr$ is,

$1s22s22p63s23p64s23d104p6$

The electronic configuration of $Kr$ is found using the total number of electrons present in the atom. The total number of electrons present in $Kr$ is 36. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Kr$ is found as $1s22s22p63s23p64s23d104p6$ .

Ion with net charge as +3 with electronic configuration $[Kr]4d6$ ,

$Rh3+ = [Kr]4d6$

Krypton is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p6$ . 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 $[Kr]4d6$ to be $Rh3+$ .

(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 $[Xe]4f145d6$ .

(d)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (d) is $Ir3+$

Explanation of Solution

Electronic configuration of $Xe$ is,

$1s22s22p63s23p64s23d104p65s24d105p6$

The electronic configuration of $Xe$ is found using the total number of electrons present in the atom. The total number of electrons present in $Xe$ is 54. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Xe$ is found as $1s22s22p63s23p64s23d104p65s24d105p6$ .

Ion with net charge as +3 with electronic configuration $[Xe]4f145d6$

$Ir3+ = [Xe]4f145d6$

Xenon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p65s24d105p6$ . 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 $[Xe]4f145d6$ to be $Ir3+$ .

Answer 6

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 $[Ar]3d3$ .

(a)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (a) is $Cr3+$

Explanation of Solution

Electronic configuration of $Ar$ is,

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]3d3$

$Cr3+ = [Ar]3d3$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Cr3+$ .

Answer 7

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 $[Ar]3d3$ .

Answer 8

(a)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (a) is $Cr3+$

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Electronic configuration of $Ar$ is,

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]3d3$

$Cr3+ = [Ar]3d3$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Cr3+$ .

Answer 13

(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 $[Ar]$ .

(b)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (b) is $Sc3+$

Explanation of Solution

Electronic configuration of $Ar$

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]$

$Sc3+ = [Ar]$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Sc3+$ .

Answer 14

(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 $[Ar]$ .

Answer 15

(b)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (b) is $Sc3+$

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

Electronic configuration of $Ar$

$1s22s22p63s23p6$

The electronic configuration of $Ar$ is found using the total number of electrons present in the atom. The total number of electrons present in $Ar$ is 18. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Ar$ is found as $1s22s22p63s23p6$ .

Ion with net charge as +3 with electronic configuration $[Ar]$

$Sc3+ = [Ar]$

Argon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p6$ . 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 $[Ar]$ to be $Sc3+$ .

Answer 20

(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 $[Kr]4d6$ .

(c)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (c) is $Rh3+$

Explanation of Solution

Electronic configuration of $Kr$ is,

$1s22s22p63s23p64s23d104p6$

The electronic configuration of $Kr$ is found using the total number of electrons present in the atom. The total number of electrons present in $Kr$ is 36. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Kr$ is found as $1s22s22p63s23p64s23d104p6$ .

Ion with net charge as +3 with electronic configuration $[Kr]4d6$ ,

$Rh3+ = [Kr]4d6$

Krypton is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p6$ . 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 $[Kr]4d6$ to be $Rh3+$ .

Answer 21

(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 $[Kr]4d6$ .

Answer 22

(c)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (c) is $Rh3+$

Answer 23

(c)

Expert Solution

Answer 24

(c)

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

Electronic configuration of $Kr$ is,

$1s22s22p63s23p64s23d104p6$

The electronic configuration of $Kr$ is found using the total number of electrons present in the atom. The total number of electrons present in $Kr$ is 36. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Kr$ is found as $1s22s22p63s23p64s23d104p6$ .

Ion with net charge as +3 with electronic configuration $[Kr]4d6$ ,

$Rh3+ = [Kr]4d6$

Krypton is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p6$ . 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 $[Kr]4d6$ to be $Rh3+$ .

Answer 27

(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 $[Xe]4f145d6$ .

(d)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (d) is $Ir3+$

Explanation of Solution

Electronic configuration of $Xe$ is,

$1s22s22p63s23p64s23d104p65s24d105p6$

The electronic configuration of $Xe$ is found using the total number of electrons present in the atom. The total number of electrons present in $Xe$ is 54. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Xe$ is found as $1s22s22p63s23p64s23d104p65s24d105p6$ .

Ion with net charge as +3 with electronic configuration $[Xe]4f145d6$

$Ir3+ = [Xe]4f145d6$

Xenon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p65s24d105p6$ . 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 $[Xe]4f145d6$ to be $Ir3+$ .

Answer 28

(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 $[Xe]4f145d6$ .

Answer 29

(d)

Expert Solution

Answer to Problem 4.75QP

Answer

The ion with a net charge of +3 for (d) is $Ir3+$

Answer 30

(d)

Expert Solution

Answer 31

(d)

Expert Solution

Answer 32

Expert Solution

Answer 33

Explanation of Solution

Electronic configuration of $Xe$ is,

$1s22s22p63s23p64s23d104p65s24d105p6$

The electronic configuration of $Xe$ is found using the total number of electrons present in the atom. The total number of electrons present in $Xe$ is 54. According to Pauli Exclusion Principle and Hund’s rule, the electronic configuration of $Xe$ is found as $1s22s22p63s23p64s23d104p65s24d105p6$ .

Ion with net charge as +3 with electronic configuration $[Xe]4f145d6$

$Ir3+ = [Xe]4f145d6$

Xenon is a noble gas and has a complete octet electronic configuration as $1s22s22p63s23p64s23d104p65s24d105p6$ . 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 $[Xe]4f145d6$ to be $Ir3+$ .

Answer 34

Ch. 4.1 - Prob. 4.1WE Ch. 4.1 - Prob. 1PPA Ch. 4.1 - Prob. 1PPB Ch. 4.1 - Prob. 1PPC Ch. 4.1 - Prob. 4.1.1SR Ch. 4.1 - Prob. 4.1.2SR Ch. 4.1 - Prob. 4.1.3SR Ch. 4.2 - Prob. 4.2WE Ch. 4.2 - Without using a periodic table, give the...Ch. 4.2 - Identify the elements represented by (a)...

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Answer to Problem 4.75QP

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Answer to Problem 4.75QP

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Answer to Problem 4.75QP

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Answer to Problem 4.75QP

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