Chapter 5, Problem 5.64CP

(a)

Interpretation Introduction

Interpretation:

The oxidation number for transition metals in the given set of compounds should be calculated.

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. 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 for transition metals in the given set of compounds should be calculated.

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. 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.