The oxidation number of the metal atom in the given compound should be represented by using Roman numeral Concept introduction: The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number. Rules for assigning oxidation number 1. The oxidation number of the atom of an uncombined element is zero. 2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species. 3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1. 4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in O F 2 where it is +2.

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Answer 1

Question

Chapter 5.6, Problem 5.10P

(a)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(b)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(c)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(d)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(e)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

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Answer 2

Question

Chapter 5.6, Problem 5.10P

(a)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(b)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(c)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(d)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(e)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

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Answer 3

Question

Chapter 5.6, Problem 5.10P

(a)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(b)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(c)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(d)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(e)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

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Answer 4

Question

Chapter 5.6, Problem 5.10P

(a)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(b)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(c)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(d)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(e)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

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Answer 5

Chapter 5.6, Problem 5.10P

(a)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(b)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(c)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(d)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

(e)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

Answer 6

Chapter 5.6, Problem 5.10P

(a)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

Answer 7

Chapter 5.6, Problem 5.10P

(a)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

Answer 12

(d)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

Answer 13

(d)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1) The oxidation number of the atom of an uncombined element is zero.

2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

Answer 14

(e)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

Answer 15

(e)

Interpretation Introduction

Interpretation:

The oxidation number of the metal atom in the given compound should be represented by Using Roman numeral

Concept introduction:

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Rules for assigning oxidation number

1. The oxidation number of the atom of an uncombined element is zero.

2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.

3. Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.

4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in OF2 where it is +2.

Answer 16

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Answer 17

Expert Solution & Answer

Answer 18

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Answer 19

Ch. 5.2 - Ozone (O3) is formed in the earths upper...Ch. 5.2 - Balance the following equations:...Ch. 5.2 - Prob. 5.3KCP Ch. 5.3 - Many kidney stones are formed by precipitation of...Ch. 5.3 - Prob. 5.2CIAP Ch. 5.3 - Predict the solubility of the following compounds:...Ch. 5.3 - Prob. 5.5P Ch. 5.4 - Write and balance equations for the following...Ch. 5.5 - Prob. 5.7P Ch. 5.5 - Prob. 5.8P

Solution Summary: The author explains that the oxidation number of the metal atom in the given compound should be represented by using Roman numeral Concept introduction.

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