The oxidation state of oxygen atom in H O 2 has to be assigned. Concept introduction: Rules for assigning oxidation state are given below. 1. Free elements have an oxidation state of 0. 2. The sum of the oxidation states of all the atoms in a species and net charge on the species must be equal. 3. The alkali metal atoms ( L i , N a , K , R b , a n d C s ) in compounds have an oxidation state of + 1 . 4. Fluorine atoms have an oxidation state of − 1 . 5. The alkaline-earth atoms ( B e , M g , C a , S r , B a , a n d R a ) and Z n and C d in compounds are always assigned an oxidation state of + 2. 6. Hydrogen atoms have an oxidation state of + 1 7. Oxygen atom have and oxidation state of − 2. 8. The above seven rules is used to find out the oxidation states in many of the cases. But in some cases these rules are not sufficient. In such cases Lewis formulas can be used to determine oxidation states. The oxidation states can be assigned by the following steps: a. Lewis formula for the molecule or ion should be written. b. The bonded electron should be assigned to the atom which has more electronegativity than the other and if the electronegativity is same then electron has to be divided among them. c. The total number of valence electrons assigned to each atom in the previous step has to be added. d. The oxidation state of each main-group element in the molecule can be determined by using the following formula. Oxidation state = (number of valance electrons in the free (nonbonded) atom) − (number of valence electrons assigned to the atom in the molecule)

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Answer 1

Question

Chapter 24, Problem 24.2P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in HO2 has to be assigned.

Concept introduction:

Rules for assigning oxidation state are given below.

1. Free elements have an oxidation state of 0.

2. The sum of the oxidation states of all the atoms in a species and net charge on the species must be equal.

3. The alkali metal atoms (Li, Na, K, Rb, and Cs) in compounds have an oxidation state of +1.

4. Fluorine atoms have an oxidation state of −1.

5. The alkaline-earth atoms (Be, Mg, Ca, Sr, Ba, and Ra) and Zn and Cd in compounds are always assigned an oxidation state of +2.

6. Hydrogen atoms have an oxidation state of +1

7. Oxygen atom have and oxidation state of −2.

8. The above seven rules is used to find out the oxidation states in many of the cases. But in some cases these rules are not sufficient. In such cases Lewis formulas can be used to determine oxidation states. The oxidation states can be assigned by the following steps:

a. Lewis formula for the molecule or ion should be written.

b. The bonded electron should be assigned to the atom which has more electronegativity than the other and if the electronegativity is same then electron has to be divided among them.

c. The total number of valence electrons assigned to each atom in the previous step has to be added.

d. The oxidation state of each main-group element in the molecule can be determined by using the following formula.

Oxidation state = (number of valance electrons in the free (nonbonded) atom) − (number of valence electrons assigned to the atom in the molecule)

(b)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in S2O82− [O3S−O−O−SO3]2− has to be assigned.

Concept introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in O3− has to be assigned.

Concept introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in H3COOCH3 has to be assigned.

Concept introduction:

Refer to part (a).

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3. Predict the major product and give a mechanism for the following reactions: (CH3)3COH/H₂SO4 a) b) NC CH₂O c) LOCH, (CH3)3COH/H2SO4 H,SO -OH

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Answer 2

Question

Chapter 24, Problem 24.2P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in HO2 has to be assigned.

Concept introduction:

Rules for assigning oxidation state are given below.

1. Free elements have an oxidation state of 0.

2. The sum of the oxidation states of all the atoms in a species and net charge on the species must be equal.

3. The alkali metal atoms (Li, Na, K, Rb, and Cs) in compounds have an oxidation state of +1.

4. Fluorine atoms have an oxidation state of −1.

5. The alkaline-earth atoms (Be, Mg, Ca, Sr, Ba, and Ra) and Zn and Cd in compounds are always assigned an oxidation state of +2.

6. Hydrogen atoms have an oxidation state of +1

7. Oxygen atom have and oxidation state of −2.

8. The above seven rules is used to find out the oxidation states in many of the cases. But in some cases these rules are not sufficient. In such cases Lewis formulas can be used to determine oxidation states. The oxidation states can be assigned by the following steps:

a. Lewis formula for the molecule or ion should be written.

b. The bonded electron should be assigned to the atom which has more electronegativity than the other and if the electronegativity is same then electron has to be divided among them.

c. The total number of valence electrons assigned to each atom in the previous step has to be added.

d. The oxidation state of each main-group element in the molecule can be determined by using the following formula.

Oxidation state = (number of valance electrons in the free (nonbonded) atom) − (number of valence electrons assigned to the atom in the molecule)

(b)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in S2O82− [O3S−O−O−SO3]2− has to be assigned.

Concept introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in O3− has to be assigned.

Concept introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in H3COOCH3 has to be assigned.

Concept introduction:

Refer to part (a).

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Answer 3

Question

Chapter 24, Problem 24.2P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in HO2 has to be assigned.

Concept introduction:

Rules for assigning oxidation state are given below.

1. Free elements have an oxidation state of 0.

2. The sum of the oxidation states of all the atoms in a species and net charge on the species must be equal.

3. The alkali metal atoms (Li, Na, K, Rb, and Cs) in compounds have an oxidation state of +1.

4. Fluorine atoms have an oxidation state of −1.

5. The alkaline-earth atoms (Be, Mg, Ca, Sr, Ba, and Ra) and Zn and Cd in compounds are always assigned an oxidation state of +2.

6. Hydrogen atoms have an oxidation state of +1

7. Oxygen atom have and oxidation state of −2.

8. The above seven rules is used to find out the oxidation states in many of the cases. But in some cases these rules are not sufficient. In such cases Lewis formulas can be used to determine oxidation states. The oxidation states can be assigned by the following steps:

a. Lewis formula for the molecule or ion should be written.

b. The bonded electron should be assigned to the atom which has more electronegativity than the other and if the electronegativity is same then electron has to be divided among them.

c. The total number of valence electrons assigned to each atom in the previous step has to be added.

d. The oxidation state of each main-group element in the molecule can be determined by using the following formula.

Oxidation state = (number of valance electrons in the free (nonbonded) atom) − (number of valence electrons assigned to the atom in the molecule)

(b)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in S2O82− [O3S−O−O−SO3]2− has to be assigned.

Concept introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in O3− has to be assigned.

Concept introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in H3COOCH3 has to be assigned.

Concept introduction:

Refer to part (a).

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Answer 4

Question

Chapter 24, Problem 24.2P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in HO2 has to be assigned.

Concept introduction:

Rules for assigning oxidation state are given below.

1. Free elements have an oxidation state of 0.

2. The sum of the oxidation states of all the atoms in a species and net charge on the species must be equal.

3. The alkali metal atoms (Li, Na, K, Rb, and Cs) in compounds have an oxidation state of +1.

4. Fluorine atoms have an oxidation state of −1.

5. The alkaline-earth atoms (Be, Mg, Ca, Sr, Ba, and Ra) and Zn and Cd in compounds are always assigned an oxidation state of +2.

6. Hydrogen atoms have an oxidation state of +1

7. Oxygen atom have and oxidation state of −2.

8. The above seven rules is used to find out the oxidation states in many of the cases. But in some cases these rules are not sufficient. In such cases Lewis formulas can be used to determine oxidation states. The oxidation states can be assigned by the following steps:

a. Lewis formula for the molecule or ion should be written.

b. The bonded electron should be assigned to the atom which has more electronegativity than the other and if the electronegativity is same then electron has to be divided among them.

c. The total number of valence electrons assigned to each atom in the previous step has to be added.

d. The oxidation state of each main-group element in the molecule can be determined by using the following formula.

Oxidation state = (number of valance electrons in the free (nonbonded) atom) − (number of valence electrons assigned to the atom in the molecule)

(b)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in S2O82− [O3S−O−O−SO3]2− has to be assigned.

Concept introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in O3− has to be assigned.

Concept introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in H3COOCH3 has to be assigned.

Concept introduction:

Refer to part (a).

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Answer 5

Chapter 24, Problem 24.2P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in HO2 has to be assigned.

Concept introduction:

Rules for assigning oxidation state are given below.

1. Free elements have an oxidation state of 0.

2. The sum of the oxidation states of all the atoms in a species and net charge on the species must be equal.

3. The alkali metal atoms (Li, Na, K, Rb, and Cs) in compounds have an oxidation state of +1.

4. Fluorine atoms have an oxidation state of −1.

5. The alkaline-earth atoms (Be, Mg, Ca, Sr, Ba, and Ra) and Zn and Cd in compounds are always assigned an oxidation state of +2.

6. Hydrogen atoms have an oxidation state of +1

7. Oxygen atom have and oxidation state of −2.

8. The above seven rules is used to find out the oxidation states in many of the cases. But in some cases these rules are not sufficient. In such cases Lewis formulas can be used to determine oxidation states. The oxidation states can be assigned by the following steps:

a. Lewis formula for the molecule or ion should be written.

b. The bonded electron should be assigned to the atom which has more electronegativity than the other and if the electronegativity is same then electron has to be divided among them.

c. The total number of valence electrons assigned to each atom in the previous step has to be added.

d. The oxidation state of each main-group element in the molecule can be determined by using the following formula.

Oxidation state = (number of valance electrons in the free (nonbonded) atom) − (number of valence electrons assigned to the atom in the molecule)

(b)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in S2O82− [O3S−O−O−SO3]2− has to be assigned.

Concept introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in O3− has to be assigned.

Concept introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in H3COOCH3 has to be assigned.

Concept introduction:

Refer to part (a).

Answer 6

Chapter 24, Problem 24.2P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in HO2 has to be assigned.

Concept introduction:

Rules for assigning oxidation state are given below.

1. Free elements have an oxidation state of 0.

2. The sum of the oxidation states of all the atoms in a species and net charge on the species must be equal.

3. The alkali metal atoms (Li, Na, K, Rb, and Cs) in compounds have an oxidation state of +1.

4. Fluorine atoms have an oxidation state of −1.

5. The alkaline-earth atoms (Be, Mg, Ca, Sr, Ba, and Ra) and Zn and Cd in compounds are always assigned an oxidation state of +2.

6. Hydrogen atoms have an oxidation state of +1

7. Oxygen atom have and oxidation state of −2.

8. The above seven rules is used to find out the oxidation states in many of the cases. But in some cases these rules are not sufficient. In such cases Lewis formulas can be used to determine oxidation states. The oxidation states can be assigned by the following steps:

a. Lewis formula for the molecule or ion should be written.

b. The bonded electron should be assigned to the atom which has more electronegativity than the other and if the electronegativity is same then electron has to be divided among them.

c. The total number of valence electrons assigned to each atom in the previous step has to be added.

d. The oxidation state of each main-group element in the molecule can be determined by using the following formula.

Oxidation state = (number of valance electrons in the free (nonbonded) atom) − (number of valence electrons assigned to the atom in the molecule)

Answer 7

Chapter 24, Problem 24.2P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in HO2 has to be assigned.

Concept introduction:

Rules for assigning oxidation state are given below.

1. Free elements have an oxidation state of 0.

2. The sum of the oxidation states of all the atoms in a species and net charge on the species must be equal.

3. The alkali metal atoms (Li, Na, K, Rb, and Cs) in compounds have an oxidation state of +1.

4. Fluorine atoms have an oxidation state of −1.

5. The alkaline-earth atoms (Be, Mg, Ca, Sr, Ba, and Ra) and Zn and Cd in compounds are always assigned an oxidation state of +2.

6. Hydrogen atoms have an oxidation state of +1

7. Oxygen atom have and oxidation state of −2.

8. The above seven rules is used to find out the oxidation states in many of the cases. But in some cases these rules are not sufficient. In such cases Lewis formulas can be used to determine oxidation states. The oxidation states can be assigned by the following steps:

a. Lewis formula for the molecule or ion should be written.

b. The bonded electron should be assigned to the atom which has more electronegativity than the other and if the electronegativity is same then electron has to be divided among them.

c. The total number of valence electrons assigned to each atom in the previous step has to be added.

d. The oxidation state of each main-group element in the molecule can be determined by using the following formula.

Oxidation state = (number of valance electrons in the free (nonbonded) atom) − (number of valence electrons assigned to the atom in the molecule)

Answer 8

(b)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in S2O82− [O3S−O−O−SO3]2− has to be assigned.

Concept introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in S2O82− [O3S−O−O−SO3]2− has to be assigned.

Concept introduction:

Refer to part (a).

Answer 10

(c)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in O3− has to be assigned.

Concept introduction:

Refer to part (a).

Answer 11

(c)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in O3− has to be assigned.

Concept introduction:

Refer to part (a).

Answer 12

(d)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in H3COOCH3 has to be assigned.

Concept introduction:

Refer to part (a).

Answer 13

(d)

Interpretation Introduction

Interpretation:

The oxidation state of oxygen atom in H3COOCH3 has to be assigned.

Concept introduction:

Refer to part (a).

Answer 14

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Answer 15

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Answer 16

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Answer 17

Ch. 24 - Prob. 24.1P Ch. 24 - Prob. 24.2P Ch. 24 - Prob. 24.3P Ch. 24 - Prob. 24.4P Ch. 24 - Prob. 24.5P Ch. 24 - Prob. 24.6P Ch. 24 - Prob. 24.7P Ch. 24 - Prob. 24.8P Ch. 24 - Prob. 24.9P Ch. 24 - Prob. 24.10P

Videos

Interpretation:

The oxidation state of oxygen atom in S2O82− [O3S−O−O−SO3]2− has to be assigned.

Concept introduction:

Refer to part (a).

Interpretation:

The oxidation state of oxygen atom in O3− has to be assigned.

Concept introduction:

Refer to part (a).

Interpretation:

The oxidation state of oxygen atom in H3COOCH3 has to be assigned.

Concept introduction:

Refer to part (a).

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Chapter 24 Solutions

Videos

Interpretation: The oxidation state of oxygen atom in S2O82− [O3S−O−O−SO3]2− has to be assigned. Concept introduction: Refer to part (a).

Interpretation: The oxidation state of oxygen atom in O3− has to be assigned. Concept introduction: Refer to part (a).

Interpretation: The oxidation state of oxygen atom in H3COOCH3 has to be assigned. Concept introduction: Refer to part (a).

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Chapter 24 Solutions

Interpretation:

The oxidation state of oxygen atom in S2O82− [O3S−O−O−SO3]2− has to be assigned.

Concept introduction:

Refer to part (a).

Interpretation:

The oxidation state of oxygen atom in O3− has to be assigned.

Concept introduction:

Refer to part (a).

Interpretation:

The oxidation state of oxygen atom in H3COOCH3 has to be assigned.

Concept introduction:

Refer to part (a).