Chapter 15, Problem 59APP

(a)

Interpretation Introduction

Interpretation:

To assign the oxidation number for each of the elements present in ${\text{Co}}_{\text{2}}{\text{O}}_{\text{3}}$ .

Concept Introduction :

Oxidation number or oxidation state of an atom in a molecule is the positive or the negative charge that an atom would have possessed if the compound would have been ionic. There are many rules for assigning the oxidation state to the given atom in a molecule. Some of them are:

1. The oxidation states of Group 1 elements are taken to be +1.
2. The oxidation states of Group 2 elements are taken to be +2.
3. The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
4. Oxidation state of halogens is taken to be -1 usually.
5. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
6. Any element when present in its elemental form has zero oxidation state.
7. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).
8. The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
9. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion.

(b)

Interpretation Introduction

Interpretation:

To assign the oxidation number for each of the elements present in ${\text{KMnO}}_{\text{4}}$ .

Concept Introduction :

Oxidation number or oxidation state of an atom in a molecule is the positive or the negative charge that an atom would have possessed if the compound would have been ionic. There are many rules for assigning the oxidation state to the given atom in a molecule. Some of them are :

1. The oxidation states of Group 1 elements are taken to be +1.
2. The oxidation states of Group 2 elements are taken to be +2.
3. The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
4. Oxidation state of halogens is taken to be -1 usually.
5. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
6. Any element when present in its elemental form has zero oxidation state.
7. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).
8. The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
9. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

(c)

Interpretation Introduction

Interpretation:

To assign the oxidation number for each of the elements present in ${\text{SbCl}}_{\text{5}}$ .

Concept Introduction :

Oxidation number or oxidation state of an atom in a molecule is the positive or the negative charge that an atom would have possessed if the compound would have been ionic. There are many rules for assigning the oxidation state to the given atom in a molecule. Some of them are:

1. The oxidation states of Group 1 elements are taken to be +1.
2. The oxidation state of Group 2 elements are taken to be +2.
3. The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
4. Oxidation state of halogens is taken to be -1 usually.
5. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
6. Any element when present in its elemental form has zero oxidation state.
7. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).
8. The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
9. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

(d)

Interpretation Introduction

Interpretation:

To assign the oxidation number for each of the elements present in ${\text{ClO}}_{\text{3}}{}^{\text{-}}$ .

Concept Introduction :

Oxidation number or oxidation state of an atom in a molecule is the positive or the negative charge that an atom would have possessed if the compound would have been ionic. There are many rules for assigning the oxidation state to the given atom in a molecule. Some of them are:

1. The oxidation states of Group 1 elements are taken to be +1.
2. The oxidation states of Group 2 elements are taken to be +2.
3. The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
4. Oxidation state of halogens is taken to be -1 usually.
5. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
6. Any element when present in its elemental form has zero oxidation state.
7. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).
8. The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
9. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

(e)

Interpretation Introduction

Interpretation:

To assign the oxidation number for each of the elements present in ${\text{PO}}_{\text{4}}{}^{3-}$ .

Concept Introduction :

Oxidation number or oxidation state of an atom in a molecule is the positive or the negative charge that an atom would have possessed if the compound would have been ionic. There are many rules for assigning the oxidation state to the given atom in a molecule. Some of them are:

1. The oxidation states of Group 1 elements are taken to be +1.
2. The oxidation states of Group 2 elements are taken to be +2.
3. The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
4. Oxidation state of halogens is taken to be -1 usually.
5. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
6. Any element when present in its elemental form has zero oxidation state.
7. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).
8. The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
9. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion