Chapter 20, Problem 67E

(a)

Interpretation Introduction

Interpretation: The ion or molecule, having iodine as the central atom, that is isoelectronic with each of the given compounds is to be stated.

Concept introduction: Two compounds are said to be isoelectronic if they contains same number of valence electrons.

Total number of valence electrons in a compound is equal to the sum of valence electrons present in each atom of that compound.

To determine: The ion or molecule, having iodine as the central atom, that is isoelectronic with each of the given compounds.

Explanation of Solution

The compound ${\text{XeO}}_{\text{4}}$ and ${\text{IO}}_{\text{4}}{}^{-}$ ion are isoelectronic.

The molecule xenon tetroxide $\left({\text{XeO}}_{\text{4}}\right)$ is made of four oxygen $\left(\text{O}\right)$ atoms and single xenon $\left(\text{Xe}\right)$ atom. The number of valence electrons in xenon is $8$ whereas the number of valence electrons in oxygen atom is $6$. Hence, the total number of valence electrons is,

$\begin{array}{c}\text{Xe}\text{+}4\text{O}\text{=}\left(8\text{+}4\times 6\right){\text{e}}^{-}\\ \text{=}32{\text{e}}^{-}\end{array}$

An ion ${\text{IO}}_{\text{4}}{}^{-}$ is made of four oxygen atoms and single iodine atom. This ion also contains a negative charge. The number of valence electrons in iodine $\left(\text{I}\right)$ is $7$. Hence, the total number of valence electrons is,

$\begin{array}{c}\text{I}\text{+}4\text{O}+1{\text{e}}^{-}\text{=}\left(7\text{+}4\times 6+1\right){\text{e}}^{-}\\ \text{=}32{\text{e}}^{-}\end{array}$

Since ${\text{XeO}}_{\text{4}}$ and ${\text{IO}}_{\text{4}}{}^{-}$ contains same number of valence electrons. Hence, these are isoelectronic compounds.

(b)

Interpretation Introduction

Interpretation: The ion or molecule, having iodine as the central atom, that is isoelectronic with each of the given compounds is to be stated.

Concept introduction: Two compounds are said to be isoelectronic if they contains same number of valence electrons.

Total number of valence electrons in a compound is equal to the sum of valence electrons present in each atom of that compound.

To determine: The ion or molecule, having iodine as the central atom, that is isoelectronic with each of the given compounds.

Explanation of Solution

The compound ${\text{XeO}}_{\text{3}}$ and ${\text{IO}}_{\text{3}}{}^{-}$ ion are isoelectronic.

The molecule xenon tetroxide $\left({\text{XeO}}_{\text{3}}\right)$ is made of three oxygen atoms and single xenon atom. The number of valence electrons in xenon is $8$ whereas the number of valence electrons in oxygen atom is $6$. Hence, the total number of valence electrons is,

$\begin{array}{c}\text{Xe}\text{+}3\text{O}\text{=}\left(8\text{+}3\times 6\right){\text{e}}^{-}\\ \text{=}26{\text{e}}^{-}\end{array}$

An ion ${\text{IO}}_{\text{3}}{}^{-}$ is made of three oxygen atoms and single iodine atom. This ion also contains a negative charge. The number of valence electrons in iodine is $7$. Hence, the total number of valence electrons is,

$\begin{array}{c}\text{I}\text{+}3\text{O}+1{\text{e}}^{-}\text{=}\left(7\text{+}3\times 6+1\right){\text{e}}^{-}\\ \text{=}26{\text{e}}^{-}\end{array}$

Since ${\text{XeO}}_{\text{3}}$ and ${\text{IO}}_{\text{3}}{}^{-}$ contains same number of valence electrons. Hence, these are isoelectronic compounds.

(c)

Interpretation Introduction

Interpretation: The ion or molecule, having iodine as the central atom, that is isoelectronic with each of the given compounds is to be stated.

Concept introduction: Two compounds are said to be isoelectronic if they contains same number of valence electrons.

Total number of valence electrons in a compound is equal to the sum of valence electrons present in each atom of that compound.

To determine: The ion or molecule, having iodine as the central atom, that is isoelectronic with each of the given compounds.

Explanation of Solution

The compound ${\text{XeF}}_{\text{2}}$ and ${\text{IF}}_{\text{2}}{}^{-}$ ion are isoelectronic.

The molecule xenon difluoride $\left({\text{XeF}}_{\text{2}}\right)$ is made of two fluorine $\left(\text{F}\right)$ atoms and single xenon atom. The number of valence electrons in xenon is $8$ whereas the number of valence electrons in fluorine atom is $7$. Hence, the total number of valence electrons is,

$\begin{array}{c}\text{Xe}\text{+}2\text{F}\text{=}\left(8\text{+}2\times 7\right){\text{e}}^{-}\\ \text{=}22{\text{e}}^{-}\end{array}$

An ion ${\text{IF}}_{\text{2}}{}^{-}$ is made of two fluorine atoms and single iodine atom. This ion also contains a negative charge. The number of valence electrons in iodine is $7$. Hence, the total number of valence electrons is,

$\begin{array}{c}\text{I}\text{+}2\text{F}+1{\text{e}}^{-}\text{=}\left(7\text{+}2\times 7+1\right){\text{e}}^{-}\\ \text{=}22{\text{e}}^{-}\end{array}$

Since ${\text{XeF}}_{\text{2}}$ and ${\text{IF}}_{\text{2}}{}^{-}$ contains same number of valence electrons. Hence, these are isoelectronic compounds.

(d)

Interpretation Introduction

Interpretation: The ion or molecule, having iodine as the central atom, that is isoelectronic with each of the given compounds is to be stated.

Concept introduction: Two compounds are said to be isoelectronic if they contains same number of valence electrons.

Total number of valence electrons in a compound is equal to the sum of valence electrons present in each atom of that compound.

To determine: An ion or molecule in which iodine is the central atom and that is isoelectronic with xenon tetrafluoride.

Explanation of Solution

The compound ${\text{XeF}}_{\text{4}}$ and ${\text{IF}}_{\text{4}}{}^{-}$ ion are isoelectronic.

The molecule xenon tetrafluoride $\left({\text{XeF}}_{\text{4}}\right)$ is made of four fluorine $\left(\text{F}\right)$ atoms and single xenon atom. The number of valence electrons in xenon is $8$ whereas the number of valence electrons in fluorine atom is $7$. Hence, the total number of valence electrons is,

$\begin{array}{c}\text{Xe}\text{+}4\text{F}\text{=}\left(8\text{+}4\times 7\right){\text{e}}^{-}\\ \text{=}36{\text{e}}^{-}\end{array}$

An ion ${\text{IF}}_{\text{4}}{}^{-}$ is made of four fluorine atoms and single iodine atom. This ion also contains a negative charge. The number of valence electrons in iodine is $7$. Hence, the total number of valence electrons is,

$\begin{array}{c}\text{I}\text{+}4\text{F}+1{\text{e}}^{-}\text{=}\left(7\text{+}4\times 7+1\right){\text{e}}^{-}\\ \text{=}36{\text{e}}^{-}\end{array}$

Since ${\text{XeF}}_{\text{4}}$ and ${\text{IF}}_{\text{4}}{}^{-}$ contains same number of valence electrons. Hence, these are isoelectronic compounds.

(e)

Interpretation Introduction

Interpretation: The ion or molecule, having iodine as the central atom, that is isoelectronic with each of the given compounds is to be stated.

Concept introduction: Two compounds are said to be isoelectronic if they contains same number of valence electrons.

Total number of valence electrons in a compound is equal to the sum of valence electrons present in each atom of that compound.

To determine: An ion or molecule in which iodine is the central atom and that is isoelectronic with xenon hexafluoride.

Explanation of Solution

The compound ${\text{XeF}}_{\text{6}}$ and ${\text{IF}}_{\text{6}}{}^{-}$ ion are isoelectronic.

The molecule xenon hexafluoride $\left({\text{XeF}}_{\text{6}}\right)$ is made of six fluorine $\left(\text{F}\right)$ atoms and single xenon atom. The number of valence electrons in xenon is $8$ whereas the number of valence electrons in fluorine atom is $7$. Hence, the total number of valence electrons is,

$\begin{array}{c}\text{Xe}\text{+}6\text{F}\text{=}\left(8\text{+}6\times 7\right){\text{e}}^{-}\\ \text{=}50{\text{e}}^{-}\end{array}$

An ion ${\text{IF}}_{\text{6}}{}^{-}$ is made of six fluorine atoms and single iodine atom. This ion also contains a negative charge. The number of valence electrons in iodine is $7$. Hence, the total number of valence electrons is,

$\begin{array}{c}\text{I}\text{+}6\text{F}+1{\text{e}}^{-}\text{=}\left(7\text{+}6\times 7+1\right){\text{e}}^{-}\\ \text{=}50{\text{e}}^{-}\end{array}$

Since ${\text{XeF}}_{\text{6}}$ and ${\text{IF}}_{\text{6}}{}^{-}$ contains same number of valence electrons. Hence, these are isoelectronic compounds.