Chapter 8, Problem 8.30QP

(a)

Interpretation Introduction

Interpretation: To write the name of the ion with +3 charge having an electronic configuration of $\left[Ar\right]3d^3$.

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

• Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atoms that is, no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number ${\text{(m}}_{\text{l}}\text{)}$ or same spin magnetic quantum numbers ${\text{(m}}_{\text{s}}\text{)}$
• Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
• Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Cation is formed when one or more electrons get removed from the outermost subshell of an atom.

Answer to Problem 8.30QP

The name of the ion with +3 charge having an electronic configuration of $\left[Ar\right]3d^3$ is $C{r}^{3+}$

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the (n-1)d orbitals and are filled first.

The given electronic configuration is $\left[Ar\right]3d^3$ so the number of electrons of the given ion is 21

The ion has +3 charge which indicates that three electrons are removed from the outermost subshell of the element. The atom has an atomic number 24 and thus the element is $Cr$

Therefore,

The name of the ion with +3 charge having an electronic configuration of $\left[Ar\right]3d^3$ is $C{r}^{3+}$

(b)

Interpretation Introduction

Interpretation: To write the name of the ion with +3 charge having an electronic configuration of $\left[Ar\right]$.

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

• Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atoms that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number ${\text{(m}}_{\text{l}}\text{)}$ or same spin magnetic quantum numbers ${\text{(m}}_{\text{s}}\text{)}$
• Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
• Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Cation is formed when one or more electrons get removed from the outermost subshell of an atom.

Answer to Problem 8.30QP

The name of the ion with +3 charge having an electronic configuration of $\left[Ar\right]3d^3$ is $S{c}^{3+}$

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first.

The given electronic configuration is $\left[Ar\right]$ so the number of electrons of the given ion is 18

The ion has +3 charge which indicates that three electrons are removed from the outermost subshell of the element. The atom has an atomic number 21 and thus the element is $Sc$

Therefore,

The name of the ion with +3 charge having an electronic configuration of $\left[Ar\right]$ is $S{c}^{3+}$

(c)

Interpretation Introduction

Interpretation: To write the name of the ion with +3 charge having an electronic configuration of $\left[Kr\right]4d^6$.

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

• Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atoms that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number ${\text{(m}}_{\text{l}}\text{)}$ or same spin magnetic quantum numbers ${\text{(m}}_{\text{s}}\text{)}$
• Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
• Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Cation is formed when one or more electrons get removed from the outermost subshell of an atom.

Answer to Problem 8.30QP

The name of the ion with +3 charge having an electronic configuration of $\left[Kr\right]4d^6$ is $R{h}^{3+}$

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first.

The given electronic configuration is $\left[Kr\right]4d^6$ so the number of electrons of the given ion is 42

The ion has +3 charge which indicates that three electrons are removed from the outermost subshell of the element. The atom has an atomic number 45 and thus the element is $Rh$

Therefore,

The name of the ion with +3 charge having an electronic configuration of $\left[Kr\right]4d^6$ is $R{h}^{3+}$

(d)

Interpretation Introduction

Interpretation: To write the name of the ion with +3 charge having an electronic configuration of $\left[Kr\right]4f^{14}5d^6$.

Concept Introduction:

Electron configuration is the distribution of electrons in the atomic orbitals. It gives an idea about the shape and energy of electrons in an atom.

There are 3 rules to decide the electronic configuration of an atom. They are,

• Pauli Exclusion Principle: No two electrons should not have same four quantum numbers in an atoms that is, it no two electrons should have same principal quantum number (n), same orbital angular momentum quantum number (l), the same magnetic quantum number ${\text{(m}}_{\text{l}}\text{)}$ or same spin magnetic quantum numbers ${\text{(m}}_{\text{s}}\text{)}$
• Aufbau Principle: In an atom, electrons fill according to the increasing energy of the orbital.
• Hund's Rule: The orbital having maximum number of electrons with same spin in separate orbitals is the most stable arrangement in an orbital.

Cation is formed when one or more electrons get removed from the outermost subshell of an atom.

Answer to Problem 8.30QP

The name of the ion with +3 charge having an electronic configuration of $\left[Kr\right]4f^{14}5d^6$ is $I{r}^{3+}$

Explanation of Solution

The orbitals are filled according to Pauli Exclusion Principle, Aufbau Principle and Hund's Rule. The maximum number of electrons that can be accommodating in each orbital is 2.

Since the ns orbitals have lower energy comparing to the np orbitals and ns orbital is filled first.

The given electronic configuration is $\left[Kr\right]4d^6$ so the number of electrons of the given ion is 74

The ion has +3 charge which indicates that three electrons are removed from the outermost subshell of the element. The atom has an atomic number 77 and thus the element is $Ir$

Therefore,

The name of the ion with +3 charge having an electronic configuration of $\left[Kr\right]4f^{14}5d^6$ is $I{r}^{3+}$