Chapter 12, Problem 39E

Interpretation Introduction

(a)

Interpretation:

The electron dot formula and structural formula of ${\text{IO}}^{-}$ is to be drawn.

Concept introduction:

An electron dot formula is a way of representing the molecular structure in which electrons are represented by a dot. Structural formula is a way in which atoms are linked together through a solid line. This solid line represents the covalent bond. An electron dot structure is known as Lewis structure. Electron dot structure indicates the valence electrons of an atom which are involved in bonding.

Answer to Problem 39E

Electron dot structure of ${\text{IO}}^{-}$ is shown below.

The structural formula of ${\text{IO}}^{-}$ is shown below.

Explanation of Solution

In molecule ${\text{IO}}^{-}$ iodine and oxygen are present as the bonding atoms. Iodine has $7$ valence electrons and oxygen has $6$ valence electrons. Negative charge is present on the molecule indicates that one electron is gained by the any atom of the molecule. Total number of electron pairs is calculated by adding the valence electrons and the negative charge present on the molecule. So, number of electrons is $(6+7+1)$ which is $14$. This shows that total electrons must be $14$. Iodine is a halogen atom. Therefore, total electrons present in bond pair is $2$. Rest of the electrons are present as the lone pairs on iodine and oxygen atom. An electron dot structure and structural formula of ${\text{IO}}^{-}$ is shown below in Figure 1 and 2 respectively.

Figure 1

Figure 2

Solid line, in Figure 2, between the iodine and oxygen atom is the covalent bond which is made up of two electrons. This bond is formed by sharing of electrons between the atoms present in that bond.

Conclusion

An electron dot structure and structural formula of ${\text{IO}}^{-}$ is shown above in Figure 1 and Figure 2.

Interpretation Introduction

(b)

Interpretation:

The electron dot formula and structural formula of ${\text{IO}}_2^{-}$ is to be drawn.

Concept introduction:

An electron dot formula is a way of representing the molecular structure in which electrons are represented by a dot. Structural formula is a way in which atoms are linked together through a solid line. This solid line represents the covalent bond. An electron dot structure is known as Lewis structure. Electron dot structure indicates the valence electrons of an atom which are involved in bonding.

Answer to Problem 39E

Electron dot structure of ${\text{IO}}_2^{-}$ is shown below.

The structural formula of ${\text{IO}}_2^{-}$ is shown below.

Explanation of Solution

In molecule ${\text{IO}}_2^{-}$, iodine is the central atom and and oxygen is present as the surrounding atoms. Iodine has $7$ valence electrons and oxygen has $6$ valence electrons. Negative charge is present on the molecule indicates that one electron is gained by the atom of the molecule. Total number of electron pairs is calculated by adding the valence electrons and the negative charge present on the molecule. So, number of electrons is $(6+6+7+1)$ which is $20$. This shows that total electrons must be $20$ or $10$ pair of electrons. Iodine is a halogen. Therefore, total electrons present in each bond pair is $2$. Rest of the electrons are present as the lone pair on iodine and oxygen atoms. An electron dot structure and structural formula of ${\text{IO}}_2^{-}$ is shown below in Figure 3 and 4 respectively.

Figure 3

Figure 4

Each solid line, in Figure 4, between the iodine and oxygen atom is the covalent bond which is made up of two electrons. This bond is formed by sharing of electrons between the central atom iodine and the surrounding oxygen atom.

Conclusion

An electron dot structure and structural formula of ${\text{IO}}_2^{-}$ is shown above in Figure 3 and Figure 4.

Interpretation Introduction

(c)

Interpretation:

The electron dot formula and structural formula of ${\text{IO}}_3^{-}$ is to be drawn.

Concept introduction:

An electron dot formula is a way of representing the molecular structure in which electrons are represented by a dot. Structural formula is a way in which atoms are linked together through a solid line. This solid line represents the covalent bond. An electron dot structure is known as Lewis structure. Electron dot structure indicates the valence electrons of an atom which are involved in bonding.

Answer to Problem 39E

Electron dot structure of ${\text{IO}}_3^{-}$ is shown below.

The structural formula of ${\text{IO}}_3^{-}$ is shown below.

Explanation of Solution

In molecule ${\text{IO}}_3^{-}$, iodine is the central atom and and oxygen is present as the surrounding atoms. Iodine has $7$ valence electrons and oxygen has $6$ valence electrons. Negative charge is present on the molecule indicates that one electron is gained by the atom of the molecule. Total number of electron pairs is calculated by adding the valence electrons and the negative charge present on the molecule. So, number of electrons is $(6+6+6+7+1)$ which is $26$. This shows that total electrons must be $26$ or $13$ pair of electrons. Iodine is a halogen. Therefore, total electrons present in each bond pair is $2$. Rest of the electrons are present as the lone pair on iodine and oxygen atoms. An electron dot structure and structural formula of ${\text{IO}}_3^{-}$ is shown below in Figure 5 and 6 respectively.

Figure 5

Figure 6

Each solid line, in Figure 6, between the iodine and oxygen atom is the covalent bond which is made up of two electrons. This bond is formed by sharing of electrons between the central atom iodine and the surrounding oxygen atom.

Conclusion

An electron dot structure and structural formula of ${\text{IO}}_3^{-}$ is shown above in Figure 5 and Figure 6.

Interpretation Introduction

(d)

Interpretation:

The electron dot formula and structural formula of ${\text{IO}}_4^{-}$ is to be drawn.

Concept introduction:

An electron dot formula is a way of representing the molecular structure in which electrons are represented by a dot. Structural formula is a way in which atoms are linked together through a solid line. This solid line represents the covalent bond. An electron dot structure is known as Lewis structure. Electron dot structure indicates the valence electrons of an atom which are involved in bonding.

Answer to Problem 39E

Electron dot structure of ${\text{IO}}_4^{-}$ is shown below.

The structural formula of ${\text{IO}}_4^{-}$ is shown below.

Explanation of Solution

In molecule ${\text{IO}}_4^{-}$, iodine is the central atom and and oxygen is present as the surrounding atoms. Iodine has $7$ valence electrons and oxygen has $6$ valence electrons. Negative charge is present on the molecule indicates that one electron is gained by the atom of the molecule. Total number of electron pairs is calculated by adding the valence electrons and the negative charge present on the molecule. So, number of electrons is $(6+6+6+6+7+1)$ which is $32$. This shows that total electrons must be $32$ or $16$ pair of electrons. Iodine is a halogen. Therefore, total electrons present in each bond pair is $2$. Rest of the electrons are present as the lone pair on iodine and oxygen atoms. An electron dot structure and structural formula of ${\text{IO}}_4^{-}$ is shown below in Figure 7 and 8 respectively.

Figure 7

Figure 8

Each solid line, in Figure 8, between the iodine and oxygen atom is the covalent bond which is made up of two electrons. This bond is formed by sharing of electrons between the central atom iodine and the surrounding oxygen atoms.

Conclusion

An electron dot structure and structural formula of ${\text{IO}}_4^{-}$ is shown above in Figure 7 and Figure 8.