(a) Interpretation: The oxidation number for each of the elements present in NO 2 is to be determined. 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: The oxidation state of Group 1 elements is taken to be +1. The oxidation states of Group 2 elements are taken to be +2. The oxidation state of oxygen is always -2 in most of the compounds except peroxides. Oxidation state of halogens is taken to be -1 usually. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals. Any element when present in its elemental form has zero oxidation state. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F 2 ). The sum of oxidation states of all the atoms present in a given molecule is equal to zero. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

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Answer 1

Question

Chapter 4, Problem 4.108SP

Interpretation Introduction

(a)

Interpretation:

The oxidation number for each of the elements present in NO₂ is to be determined.

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:

The oxidation state of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements are taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(b)

Interpretation:

The oxidation number for each of the elements present in SO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(c)

Interpretation:

The oxidation number for each of the elements present in COCl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(d)

Interpretation:

The oxidation number for each of the elements present in CH₂Cl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(e)

Interpretation:

The oxidation number for each of the elements present in KClO₃ is to be determined.

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:

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(f)

Interpretation:

The oxidation number for each of the elements present in HNO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

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Answer 2

Question

Chapter 4, Problem 4.108SP

Interpretation Introduction

(a)

Interpretation:

The oxidation number for each of the elements present in NO₂ is to be determined.

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:

The oxidation state of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements are taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(b)

Interpretation:

The oxidation number for each of the elements present in SO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(c)

Interpretation:

The oxidation number for each of the elements present in COCl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(d)

Interpretation:

The oxidation number for each of the elements present in CH₂Cl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(e)

Interpretation:

The oxidation number for each of the elements present in KClO₃ is to be determined.

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:

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(f)

Interpretation:

The oxidation number for each of the elements present in HNO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

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Answer 3

Question

Chapter 4, Problem 4.108SP

Interpretation Introduction

(a)

Interpretation:

The oxidation number for each of the elements present in NO₂ is to be determined.

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:

The oxidation state of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements are taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(b)

Interpretation:

The oxidation number for each of the elements present in SO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(c)

Interpretation:

The oxidation number for each of the elements present in COCl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(d)

Interpretation:

The oxidation number for each of the elements present in CH₂Cl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(e)

Interpretation:

The oxidation number for each of the elements present in KClO₃ is to be determined.

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:

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(f)

Interpretation:

The oxidation number for each of the elements present in HNO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

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Answer 4

Question

Chapter 4, Problem 4.108SP

Interpretation Introduction

(a)

Interpretation:

The oxidation number for each of the elements present in NO₂ is to be determined.

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:

The oxidation state of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements are taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(b)

Interpretation:

The oxidation number for each of the elements present in SO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(c)

Interpretation:

The oxidation number for each of the elements present in COCl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(d)

Interpretation:

The oxidation number for each of the elements present in CH₂Cl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(e)

Interpretation:

The oxidation number for each of the elements present in KClO₃ is to be determined.

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:

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(f)

Interpretation:

The oxidation number for each of the elements present in HNO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

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Answer 5

Chapter 4, Problem 4.108SP

Interpretation Introduction

(a)

Interpretation:

The oxidation number for each of the elements present in NO₂ is to be determined.

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:

The oxidation state of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements are taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(b)

Interpretation:

The oxidation number for each of the elements present in SO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(c)

Interpretation:

The oxidation number for each of the elements present in COCl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(d)

Interpretation:

The oxidation number for each of the elements present in CH₂Cl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(e)

Interpretation:

The oxidation number for each of the elements present in KClO₃ is to be determined.

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:

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(f)

Interpretation:

The oxidation number for each of the elements present in HNO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 6

Chapter 4, Problem 4.108SP

Interpretation Introduction

(a)

Interpretation:

The oxidation number for each of the elements present in NO₂ is to be determined.

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:

The oxidation state of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements are taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 7

Chapter 4, Problem 4.108SP

Interpretation Introduction

(a)

Interpretation:

The oxidation number for each of the elements present in NO₂ is to be determined.

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:

The oxidation state of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements are taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 8

Interpretation Introduction

(b)

Interpretation:

The oxidation number for each of the elements present in SO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 9

Interpretation Introduction

(b)

Interpretation:

The oxidation number for each of the elements present in SO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 10

Interpretation Introduction

(c)

Interpretation:

The oxidation number for each of the elements present in COCl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 11

Interpretation Introduction

(c)

Interpretation:

The oxidation number for each of the elements present in COCl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 12

Interpretation Introduction

(d)

Interpretation:

The oxidation number for each of the elements present in CH₂Cl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 13

Interpretation Introduction

(d)

Interpretation:

The oxidation number for each of the elements present in CH₂Cl₂ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 14

Interpretation Introduction

(e)

Interpretation:

The oxidation number for each of the elements present in KClO₃ is to be determined.

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:

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 15

Interpretation Introduction

(e)

Interpretation:

The oxidation number for each of the elements present in KClO₃ is to be determined.

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:

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 16

Interpretation Introduction

(f)

Interpretation:

The oxidation number for each of the elements present in HNO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 17

Interpretation Introduction

(f)

Interpretation:

The oxidation number for each of the elements present in HNO₃ is to be determined.

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 :

The oxidation states of Group 1 elements is taken to be +1.

The oxidation states of Group 2 elements is taken to be +2.

The oxidation state of oxygen is always -2 in most of the compounds except peroxides.

Oxidation state of halogens is taken to be -1 usually.

The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.

Any element when present in its elemental form has zero oxidation state.

The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F₂).

The sum of oxidation states of all the atoms present in a given molecule is equal to zero.

In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Answer 18

Expert Solution & Answer

Answer 19

Expert Solution & Answer

Answer 20

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Answer 21

Ch. 4 - Prob. 4.1P Ch. 4 - Prob. 4.2A Ch. 4 - How many moles of solute are present in 125 mLof...Ch. 4 - Prob. 4.4A Ch. 4 - Prob. 4.5P Ch. 4 - APPLY 4.7 Sulfuric acid is normally purchased at a...Ch. 4 - Prob. 4.7P Ch. 4 - Conceptual APPLY 4.9 Three different substances,...Ch. 4 - Write ne ionic equations for the following...Ch. 4 - Prob. 4.10A

Solution Summary: The author explains the rules for assigning the oxidation state to an atom in a molecule.

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