Chapter 5.6, Problem 5.11P

(a)

Interpretation Introduction

Interpretation: The oxidation number of each element in the reactant and product in the given reaction has to be determined and so it should be identified that whether the reaction is redox or not.

Concept introduction:

• Oxidation-reduction reaction: Both the oxidation and reduction reaction occurs together in a chemical reaction. It is also known as redox reaction.
• The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.
• Oxidation: Losing electrons, increasing oxidation number.
• Reduction: Gaining electron, decreasing oxidation number.
• Rules for assigning oxidation number

1. 1. 1. The oxidation number of the atom of an uncombined element is zero.
   2. 2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.
   3. 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. 4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in $O{F}_2$ where it is +2.

(b)

Interpretation Introduction

Interpretation: The oxidation number of each element in the reactant and product in the given reaction has to be determined and so it should be identified that whether the reaction is redox or not.

Concept introduction:

• Oxidation-reduction reaction: Both the oxidation and reduction reaction occurs together in a chemical reaction. It is also known as redox reaction.
• The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.
• Oxidation: Losing electrons, increasing oxidation number.
• Reduction: Gaining electron, decreasing oxidation number.
• Rules for assigning oxidation number

1. 1. 1) The oxidation number of the atom of an uncombined element is zero.
   2. 2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.
   3. 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. 4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in $O{F}_2$ where it is +2.

(c)

Interpretation Introduction

Interpretation: The oxidation number of each element in the reactant and product in the given reaction has to be determined and so it should be identified that whether the reaction is redox or not.

Concept introduction:

• Oxidation-reduction reaction: Both the oxidation and reduction reaction occurs together in a chemical reaction. It is also known as redox reaction.
• The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.
• Oxidation: Losing electrons, increasing oxidation number.
• Reduction: Gaining electron, decreasing oxidation number.
• Rules for assigning oxidation number

1. 1. 1) The oxidation number of the atom of an uncombined element is zero.
   2. 2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.
   3. 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. 4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in $O{F}_2$ where it is +2.

(d)

Interpretation Introduction

Interpretation: The oxidation number of each element in the reactant and product in the given reaction has to be determined and so it should be identified that whether the reaction is redox or not.

Concept introduction:

• Oxidation-reduction reaction: Both the oxidation and reduction reaction occurs together in a chemical reaction. It is also known as redox reaction.
• The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.
• Oxidation: Losing electrons, increasing oxidation number.
• Reduction: Gaining electron, decreasing oxidation number.
• Rules for assigning oxidation number

1. 1. 1) The oxidation number of the atom of an uncombined element is zero.
   2. 2) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.
   3. 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. 4) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in $O{F}_2$ where it is +2.

(e)

Interpretation Introduction

Interpretation: The oxidation number of each element in the reactant and product in the given reaction has to be determined and so it should be identified that whether the reaction is redox or not.

Concept introduction:

• Oxidation-reduction reaction: Both the oxidation and reduction reaction occurs together in a chemical reaction. It is also known as redox reaction.
• The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.
• Oxidation: Losing electrons, increasing oxidation number.
• Reduction: Gaining electron, decreasing oxidation number.
• Rules for assigning oxidation number

1. 1. 1. The oxidation number of the atom of an uncombined element is zero.
   2. 2. The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.
   3. 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. 4. Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in $O{F}_2$ where it is +2.

(f)

Interpretation Introduction

Interpretation: The oxidation number of each element in the reactant and product in the given reaction has to be determined and so it should be identified that whether the reaction is redox or not.

Concept introduction:

• Oxidation-reduction reaction: Both the oxidation and reduction reaction occurs together in a chemical reaction. It is also known as redox reaction.
• The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.
• Oxidation: Losing electrons, increasing oxidation number.
• Reduction: Gaining electron, decreasing oxidation number.
• Rules for assigning oxidation number

1. 1. 5) The oxidation number of the atom of an uncombined element is zero.
   2. 6) The sum of the oxidation numbers of all atoms in a compound must equal to the total charge on the species.
   3. 7) Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1.
   4. 8) Oxygen has an oxidation number of -2, except in peroxides where it is -1 and in $O{F}_2$ where it is +2.