Chapter 8, Problem 8.27QP

(a)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of lithium ion $L{i}^{+}$ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of 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 atom 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 8.27QP

The electronic configuration of $L{i}^{+}$ is ${\text{1s}}^{\text{2}}$

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 atomic number of $Li$ is 3 and the electronic configuration is ${\text{1s}}^{\text{2}}{\text{2s}}^1$

For $L{i}^{+}$, one electron is removed from the outermost subshell. Hence, the number of electrons becomes 2

Therefore,

The electronic configuration of $L{i}^{+}$ is given as:

  ${\text{1s}}^{\text{2}}$

(b)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of $H^{-}$ ions has to be written.

Concept Introduction:

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

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

Answer to Problem 8.27QP

The electronic configuration of $H^{-}$ is ${\text{1s}}^{\text{2}}$

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 $\text{ns}$ orbitals have lower energy comparing to the np orbitals and ns orbital is filled first. The ns orbitals have lower energy comparing to the $\left(\text{n-1}\right)\text{d}$ orbitals and are filled first.

The atomic number of $H$ is 1 and the electronic configuration is ${\text{1s}}^1$

For $H^{-}$, one electron is added to the outermost subshell. Hence, the number of electrons becomes 2

Therefore,

The electronic configuration of $H^{-}$ is given as:

  ${\text{H}}^{\text{-}}--\to {\text{1s}}^{\text{2}}$

(b)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of $N^{3-}$ has to be written.

Concept Introduction:

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

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

Answer to Problem 8.27QP

The electronic configuration of $N^{3-}$ is ${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^6$

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 atomic number of $N$ is 7 and the electronic configuration is ${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{\text{3}}$

For $N^{3-}$, three electrons are added to the outermost subshell. Hence, the number of electrons becomes 10

Therefore,

The electronic configuration of $N^{3-}$ is given as:

  ${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^6$

(d)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of $F^{-}$ has to be written.

Concept Introduction:

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

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

Answer to Problem 8.27QP

The electronic configuration of $F^{-}$ is ${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^5$

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 atomic number of $F$ is 9 and the electronic configuration is ${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^5$

For $F^{-}$, one electron is added to the outermost subshell. Hence, the number of electrons becomes 10

Therefore,

The electronic configuration of $F^{-}$ is given as:

  ${\text{F}}^{\text{-}}\text{---}\to {\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^6$

(e)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of $S^{2-}$ ion has to be written.

Concept Introduction:

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

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

Answer to Problem 8.27QP

The electronic configuration of $S^{2-}$ is ${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{\text{6}}{\text{3s}}^{\text{2}}{\text{3p}}^6$

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 atomic number of $S$ is 16 and the electronic configuration is ${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{\text{6}}{\text{3s}}^{\text{2}}{\text{3p}}^{\text{4}}$

For $S^{2-}$, three electrons are added to the outermost subshell. Hence, the number of electrons becomes 18

Therefore,

The electronic configuration of $S^{2-}$ is given as:

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

(f)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of $A{l}^{3+}$ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of 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 atom 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 8.27QP

The electronic configuration of $A{l}^{3+}$ is ${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{\text{6}}$

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 atomic number of $Al$ is 13 and the electronic configuration is ${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{\text{6}}{\text{3s}}^{\text{2}}{\text{3p}}^{\text{1}}$

For $A{l}^{3+}$, three electrons are removed from the outermost subshell. Hence, the number of electrons becomes 10

Therefore,

The electronic configuration of $A{l}^{3+}$ is given as:

  ${\text{Al}}^{\text{3+}}\text{----}\to {\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^{\text{6}}$

(g)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of $S{e}^{2-}$ has to be written.

Concept Introduction:

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

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

Answer to Problem 8.27QP

The electronic configuration of $S{e}^{2-}$ is $\left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^6$

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 atomic number of $Se$ is 34 and the electronic configuration is $\left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^{\text{4}}$

For $S{e}^{2-}$, three electrons are added to the outermost subshell. Hence, the number of electrons becomes 36

Therefore,

The electronic configuration of $S{e}^{2-}$ is given as:

  $\left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^6$

(h)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of $B{r}^{-}$ has to be written.

Concept Introduction:

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

Anion is formed when one or more electrons get added to the outermost subshell of an atom.

Answer to Problem 8.27QP

The electronic configuration of $B{r}^{-}$ is $\left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^6$

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 atomic number of $Br$ is 35 and the electronic configuration is $\left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^5$

For $B{r}^{-}$, one electron is added to the outermost subshell. Hence, the number of electrons becomes 36

Therefore,

The electronic configuration of $B{r}^{-}$ is given as:

  ${\text{Br}}^{\text{-}}---\left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^6$

(i)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of $R{b}^{+}$ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of 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 atom 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 8.27QP

The electronic configuration of $R{b}^{+}$ is $\left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^6$

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 atomic number of $Rb$ is 37 and the electronic configuration is $\left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^{\text{6}}{\text{5s}}^{\text{1}}$

For $R{b}^{+}$, one electron is removed from the outermost subshell. Hence, the number of electrons becomes 36

Therefore,

The electronic configuration of $R{b}^{+}$ is given as:

  ${\text{Rb}}^{\text{+}}---\to \left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^6$

(j)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of $S{r}^{2+}$ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of 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 atom 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 8.27QP

The electronic configuration of $S{r}^{2+}$ is $\left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^6$

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 atomic number of $Sr$ is 38 and the electronic configuration is $\left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^{\text{6}}{\text{5s}}^2$

For $S{r}^{2+}$, two electrons are removed from the outermost subshell. Hence, the number of electrons becomes 36

Therefore,

The electronic configuration of $S{r}^{2+}$ is given as:

  ${\text{Sr}}^{\text{2+}}--\to \left[\text{Ar}\right]{\text{4s}}^{\text{2}}{\text{3d}}^{\text{10}}{\text{4p}}^6$

(k)

Interpretation Introduction

Interpretation:

Ground–state electronic configuration of $S{n}^{2+}$ has to be written.

Concept Introduction:

Electron configuration is the distribution of electrons in atomic orbitals. It gives an idea about the shape and energy of 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 atom 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 8.27QP

The electronic configuration of $S{n}^{2+}$ is $\left[\text{Kr}\right]{\text{5s}}^{\text{2}}{\text{4d}}^{\text{10}}$

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 atomic number of $Sn$ is 50 and the electronic configuration is $\left[\text{Kr}\right]{\text{5s}}^{\text{2}}{\text{4d}}^{\text{10}}{\text{4p}}^2$

For $S{n}^{2+}$, two electrons are removed from the outermost subshell. Hence, the number of electrons becomes 48

Therefore,

The electronic configuration of $S{n}^{2+}$ is given as:

  $\left[\text{Kr}\right]{\text{5s}}^{\text{2}}{\text{4d}}^{\text{10}}$