(a) Interpretation: The electron dot formula and structural formula of 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.

Question

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Answer 1

Question

Chapter 12, Problem 39E

Interpretation Introduction

(a)

Interpretation:

The electron dot formula and structural formula of 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO− is shown below.

The structural formula of IO− is shown below.

Explanation of Solution

In molecule 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 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 IO− is shown above in Figure 1 and Figure 2.

Interpretation Introduction

(b)

Interpretation:

The electron dot formula and structural formula of IO2− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO2− is shown below.

The structural formula of IO2− is shown below.

Explanation of Solution

In molecule IO2−, 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 IO2− 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 IO2− is shown above in Figure 3 and Figure 4.

Interpretation Introduction

(c)

Interpretation:

The electron dot formula and structural formula of IO3− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 9

The structural formula of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 10

Explanation of Solution

In molecule IO3−, 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 IO3− is shown below in Figure 5 and 6 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 11

Figure 5

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 12

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 IO3− is shown above in Figure 5 and Figure 6.

Interpretation Introduction

(d)

Interpretation:

The electron dot formula and structural formula of IO4− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 13

The structural formula of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 14

Explanation of Solution

In molecule IO4−, 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 IO4− is shown below in Figure 7 and 8 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 15

Figure 7

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 16

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 IO4− is shown above in Figure 7 and Figure 8.

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Answer 2

Question

Chapter 12, Problem 39E

Interpretation Introduction

(a)

Interpretation:

The electron dot formula and structural formula of 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO− is shown below.

The structural formula of IO− is shown below.

Explanation of Solution

In molecule 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 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 IO− is shown above in Figure 1 and Figure 2.

Interpretation Introduction

(b)

Interpretation:

The electron dot formula and structural formula of IO2− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO2− is shown below.

The structural formula of IO2− is shown below.

Explanation of Solution

In molecule IO2−, 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 IO2− 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 IO2− is shown above in Figure 3 and Figure 4.

Interpretation Introduction

(c)

Interpretation:

The electron dot formula and structural formula of IO3− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 9

The structural formula of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 10

Explanation of Solution

In molecule IO3−, 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 IO3− is shown below in Figure 5 and 6 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 11

Figure 5

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 12

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 IO3− is shown above in Figure 5 and Figure 6.

Interpretation Introduction

(d)

Interpretation:

The electron dot formula and structural formula of IO4− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 13

The structural formula of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 14

Explanation of Solution

In molecule IO4−, 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 IO4− is shown below in Figure 7 and 8 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 15

Figure 7

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 16

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 IO4− is shown above in Figure 7 and Figure 8.

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Answer 3

Question

Chapter 12, Problem 39E

Interpretation Introduction

(a)

Interpretation:

The electron dot formula and structural formula of 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO− is shown below.

The structural formula of IO− is shown below.

Explanation of Solution

In molecule 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 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 IO− is shown above in Figure 1 and Figure 2.

Interpretation Introduction

(b)

Interpretation:

The electron dot formula and structural formula of IO2− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO2− is shown below.

The structural formula of IO2− is shown below.

Explanation of Solution

In molecule IO2−, 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 IO2− 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 IO2− is shown above in Figure 3 and Figure 4.

Interpretation Introduction

(c)

Interpretation:

The electron dot formula and structural formula of IO3− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 9

The structural formula of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 10

Explanation of Solution

In molecule IO3−, 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 IO3− is shown below in Figure 5 and 6 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 11

Figure 5

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 12

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 IO3− is shown above in Figure 5 and Figure 6.

Interpretation Introduction

(d)

Interpretation:

The electron dot formula and structural formula of IO4− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 13

The structural formula of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 14

Explanation of Solution

In molecule IO4−, 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 IO4− is shown below in Figure 7 and 8 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 15

Figure 7

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 16

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 IO4− is shown above in Figure 7 and Figure 8.

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Answer 4

Question

Chapter 12, Problem 39E

Interpretation Introduction

(a)

Interpretation:

The electron dot formula and structural formula of 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO− is shown below.

The structural formula of IO− is shown below.

Explanation of Solution

In molecule 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 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 IO− is shown above in Figure 1 and Figure 2.

Interpretation Introduction

(b)

Interpretation:

The electron dot formula and structural formula of IO2− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO2− is shown below.

The structural formula of IO2− is shown below.

Explanation of Solution

In molecule IO2−, 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 IO2− 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 IO2− is shown above in Figure 3 and Figure 4.

Interpretation Introduction

(c)

Interpretation:

The electron dot formula and structural formula of IO3− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 9

The structural formula of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 10

Explanation of Solution

In molecule IO3−, 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 IO3− is shown below in Figure 5 and 6 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 11

Figure 5

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 12

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 IO3− is shown above in Figure 5 and Figure 6.

Interpretation Introduction

(d)

Interpretation:

The electron dot formula and structural formula of IO4− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 13

The structural formula of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 14

Explanation of Solution

In molecule IO4−, 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 IO4− is shown below in Figure 7 and 8 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 15

Figure 7

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 16

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 IO4− is shown above in Figure 7 and Figure 8.

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Answer 5

Chapter 12, Problem 39E

Interpretation Introduction

(a)

Interpretation:

The electron dot formula and structural formula of 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO− is shown below.

The structural formula of IO− is shown below.

Explanation of Solution

In molecule 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 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 IO− is shown above in Figure 1 and Figure 2.

Interpretation Introduction

(b)

Interpretation:

The electron dot formula and structural formula of IO2− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO2− is shown below.

The structural formula of IO2− is shown below.

Explanation of Solution

In molecule IO2−, 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 IO2− 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 IO2− is shown above in Figure 3 and Figure 4.

Interpretation Introduction

(c)

Interpretation:

The electron dot formula and structural formula of IO3− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 9

The structural formula of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 10

Explanation of Solution

In molecule IO3−, 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 IO3− is shown below in Figure 5 and 6 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 11

Figure 5

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 12

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 IO3− is shown above in Figure 5 and Figure 6.

Interpretation Introduction

(d)

Interpretation:

The electron dot formula and structural formula of IO4− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 13

The structural formula of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 14

Explanation of Solution

In molecule IO4−, 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 IO4− is shown below in Figure 7 and 8 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 15

Figure 7

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 16

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 IO4− is shown above in Figure 7 and Figure 8.

Answer 6

Chapter 12, Problem 39E

Interpretation Introduction

(a)

Interpretation:

The electron dot formula and structural formula of 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO− is shown below.

The structural formula of IO− is shown below.

Explanation of Solution

In molecule 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 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 IO− is shown above in Figure 1 and Figure 2.

Answer 7

Chapter 12, Problem 39E

Interpretation Introduction

(a)

Interpretation:

The electron dot formula and structural formula of 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 8

Expert Solution

Answer to Problem 39E

Electron dot structure of IO− is shown below.

The structural formula of IO− is shown below.

Answer 9

Expert Solution

Answer 10

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

In molecule 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 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.

Answer 13

Conclusion

An electron dot structure and structural formula of IO− is shown above in Figure 1 and Figure 2.

Answer 14

Interpretation Introduction

(b)

Interpretation:

The electron dot formula and structural formula of IO2− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO2− is shown below.

The structural formula of IO2− is shown below.

Explanation of Solution

In molecule IO2−, 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 IO2− 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 IO2− is shown above in Figure 3 and Figure 4.

Answer 15

Interpretation Introduction

(b)

Interpretation:

The electron dot formula and structural formula of IO2− 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 16

Expert Solution

Answer to Problem 39E

Electron dot structure of IO2− is shown below.

The structural formula of IO2− is shown below.

Answer 17

Expert Solution

Answer 18

Expert Solution

Answer 19

Expert Solution

Answer 20

Explanation of Solution

In molecule IO2−, 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 IO2− 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.

Answer 21

Conclusion

An electron dot structure and structural formula of IO2− is shown above in Figure 3 and Figure 4.

Answer 22

Interpretation Introduction

(c)

Interpretation:

The electron dot formula and structural formula of IO3− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 9

The structural formula of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 10

Explanation of Solution

In molecule IO3−, 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 IO3− is shown below in Figure 5 and 6 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 11

Figure 5

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 12

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 IO3− is shown above in Figure 5 and Figure 6.

Answer 23

Interpretation Introduction

(c)

Interpretation:

The electron dot formula and structural formula of IO3− 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 24

Expert Solution

Answer to Problem 39E

Electron dot structure of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 9

The structural formula of IO3− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 10

Answer 25

Expert Solution

Answer 26

Expert Solution

Answer 27

Expert Solution

Answer 28

Explanation of Solution

In molecule IO3−, 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 IO3− is shown below in Figure 5 and 6 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 11

Figure 5

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 12

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.

Answer 29

Conclusion

An electron dot structure and structural formula of IO3− is shown above in Figure 5 and Figure 6.

Answer 30

Interpretation Introduction

(d)

Interpretation:

The electron dot formula and structural formula of IO4− 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.

Expert Solution

Answer to Problem 39E

Electron dot structure of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 13

The structural formula of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 14

Explanation of Solution

In molecule IO4−, 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 IO4− is shown below in Figure 7 and 8 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 15

Figure 7

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 16

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 IO4− is shown above in Figure 7 and Figure 8.

Answer 31

Interpretation Introduction

(d)

Interpretation:

The electron dot formula and structural formula of IO4− 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 32

Expert Solution

Answer to Problem 39E

Electron dot structure of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 13

The structural formula of IO4− is shown below.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 14

Answer 33

Expert Solution

Answer 34

Expert Solution

Answer 35

Expert Solution

Answer 36

Explanation of Solution

In molecule IO4−, 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 IO4− is shown below in Figure 7 and 8 respectively.

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 15

Figure 7

INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN, Chapter 12, Problem 39E , additional homework tip 16

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.