The oxidation state of nitrogen atoms in N 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 ) a n d Z n a n d 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 (non-bonded) atom) − (number of valence electrons assigned to the atom in the molecule)

Question

Want to see the full answer?

Answer 1

Question

Chapter 24, Problem 24.55P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO2− 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 (non-bonded) atom) − (number of valence electrons assigned to the atom in the molecule)

(b)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO3− has to be assigned.

Concept introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NH2OH has to be assigned.

Concept introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in N2O4 has to be assigned.

Concept introduction:

Refer to part (a).

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Table 1.1 Stock Standard Solutions Preparation. The amounts shown should be dissolved in 100 mL. Millipore water. Calculate the corresponding anion concentrations based on the actual weights of the reagents. Anion Amount of reagent (g) Anion Concentration (mg/L) 0.1649 Reagent Chloride NaCl Fluoride NaF 0.2210 Bromide NaBr 0.1288 Nitrate NaNO3 0.1371 Nitrite NaNO2 0.1500 Phosphate KH2PO4 0.1433 Sulfate K2SO4 0.1814

Draw the structure of the pound in the provided CO as a 300-1200 37(2), 11 ( 110, and 2.5 (20

Please help me with # 4 and 5. Thanks in advance!

Answer 2

Question

Chapter 24, Problem 24.55P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO2− 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 (non-bonded) atom) − (number of valence electrons assigned to the atom in the molecule)

(b)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO3− has to be assigned.

Concept introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NH2OH has to be assigned.

Concept introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in N2O4 has to be assigned.

Concept introduction:

Refer to part (a).

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 24, Problem 24.55P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO2− 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 (non-bonded) atom) − (number of valence electrons assigned to the atom in the molecule)

(b)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO3− has to be assigned.

Concept introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NH2OH has to be assigned.

Concept introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in N2O4 has to be assigned.

Concept introduction:

Refer to part (a).

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 24, Problem 24.55P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO2− 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 (non-bonded) atom) − (number of valence electrons assigned to the atom in the molecule)

(b)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO3− has to be assigned.

Concept introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NH2OH has to be assigned.

Concept introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in N2O4 has to be assigned.

Concept introduction:

Refer to part (a).

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 24, Problem 24.55P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO2− 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 (non-bonded) atom) − (number of valence electrons assigned to the atom in the molecule)

(b)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO3− has to be assigned.

Concept introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NH2OH has to be assigned.

Concept introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in N2O4 has to be assigned.

Concept introduction:

Refer to part (a).

Answer 6

Chapter 24, Problem 24.55P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO2− 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 (non-bonded) atom) − (number of valence electrons assigned to the atom in the molecule)

Answer 7

Chapter 24, Problem 24.55P

(a)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO2− 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 (non-bonded) atom) − (number of valence electrons assigned to the atom in the molecule)

Answer 8

(b)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO3− has to be assigned.

Concept introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NO3− has to be assigned.

Concept introduction:

Refer to part (a).

Answer 10

(c)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NH2OH has to be assigned.

Concept introduction:

Refer to part (a).

Answer 11

(c)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in NH2OH has to be assigned.

Concept introduction:

Refer to part (a).

Answer 12

(d)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in N2O4 has to be assigned.

Concept introduction:

Refer to part (a).

Answer 13

(d)

Interpretation Introduction

Interpretation:

The oxidation state of nitrogen atoms in N2O4 has to be assigned.

Concept introduction:

Refer to part (a).

Answer 14

Expert Solution & Answer

Answer 15

Expert Solution & Answer

Answer 16

Want to see the full answer?

Check out a sample textbook solution

See solution

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 nitrogen atoms in NO3− has to be assigned.

Concept introduction:

Refer to part (a).

Interpretation:

The oxidation state of nitrogen atoms in NH2OH has to be assigned.

Concept introduction:

Refer to part (a).

Interpretation:

The oxidation state of nitrogen atoms in N2O4 has to be assigned.

Concept introduction:

Refer to part (a).

Want to see the full answer?

Chapter 24 Solutions

Videos

Interpretation: The oxidation state of nitrogen atoms in NO3− has to be assigned. Concept introduction: Refer to part (a).

Interpretation: The oxidation state of nitrogen atoms in NH2OH has to be assigned. Concept introduction: Refer to part (a).

Interpretation: The oxidation state of nitrogen atoms in N2O4 has to be assigned. Concept introduction: Refer to part (a).

Want to see the full answer?

Chapter 24 Solutions

Interpretation:

The oxidation state of nitrogen atoms in NO3− has to be assigned.

Concept introduction:

Refer to part (a).

Interpretation:

The oxidation state of nitrogen atoms in NH2OH has to be assigned.

Concept introduction:

Refer to part (a).

Interpretation:

The oxidation state of nitrogen atoms in N2O4 has to be assigned.

Concept introduction:

Refer to part (a).