(a) Interpretation: The oxidation state of oxygen in each oxide and the oxidation state of the other element should be determined. Concept introduction: Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding. When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides. All the oxygen in oxides are in − 2 oxidation state.

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Answer 1

Question

Chapter 22, Problem 22.24CP

Interpretation Introduction

(a)

Interpretation:

The oxidation state of oxygen in each oxide and the oxidation state of the other element should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

All the oxygen in oxides are in −2 oxidation state.

Interpretation Introduction

(b)

Interpretation:

Each oxide should be identified as ionic or covalent.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

Interpretation Introduction

(c)

Interpretation:

Each oxide should be identified as acidic or basic

Concept introduction:

Oxides can be categorized as basic, acidic or amphoteric. Basic oxides are ionic and are formed by metals on the left side of the periodic table. Acidic oxides are covalent and are formed by nonmetals on the right side of the periodic table.

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (1) and (2) should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

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Answer 2

Question

Chapter 22, Problem 22.24CP

Interpretation Introduction

(a)

Interpretation:

The oxidation state of oxygen in each oxide and the oxidation state of the other element should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

All the oxygen in oxides are in −2 oxidation state.

Interpretation Introduction

(b)

Interpretation:

Each oxide should be identified as ionic or covalent.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

Interpretation Introduction

(c)

Interpretation:

Each oxide should be identified as acidic or basic

Concept introduction:

Oxides can be categorized as basic, acidic or amphoteric. Basic oxides are ionic and are formed by metals on the left side of the periodic table. Acidic oxides are covalent and are formed by nonmetals on the right side of the periodic table.

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (1) and (2) should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

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Answer 3

Question

Chapter 22, Problem 22.24CP

Interpretation Introduction

(a)

Interpretation:

The oxidation state of oxygen in each oxide and the oxidation state of the other element should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

All the oxygen in oxides are in −2 oxidation state.

Interpretation Introduction

(b)

Interpretation:

Each oxide should be identified as ionic or covalent.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

Interpretation Introduction

(c)

Interpretation:

Each oxide should be identified as acidic or basic

Concept introduction:

Oxides can be categorized as basic, acidic or amphoteric. Basic oxides are ionic and are formed by metals on the left side of the periodic table. Acidic oxides are covalent and are formed by nonmetals on the right side of the periodic table.

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (1) and (2) should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

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Answer 4

Question

Chapter 22, Problem 22.24CP

Interpretation Introduction

(a)

Interpretation:

The oxidation state of oxygen in each oxide and the oxidation state of the other element should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

All the oxygen in oxides are in −2 oxidation state.

Interpretation Introduction

(b)

Interpretation:

Each oxide should be identified as ionic or covalent.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

Interpretation Introduction

(c)

Interpretation:

Each oxide should be identified as acidic or basic

Concept introduction:

Oxides can be categorized as basic, acidic or amphoteric. Basic oxides are ionic and are formed by metals on the left side of the periodic table. Acidic oxides are covalent and are formed by nonmetals on the right side of the periodic table.

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (1) and (2) should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

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Answer 5

Chapter 22, Problem 22.24CP

Interpretation Introduction

(a)

Interpretation:

The oxidation state of oxygen in each oxide and the oxidation state of the other element should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

All the oxygen in oxides are in −2 oxidation state.

Interpretation Introduction

(b)

Interpretation:

Each oxide should be identified as ionic or covalent.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

Interpretation Introduction

(c)

Interpretation:

Each oxide should be identified as acidic or basic

Concept introduction:

Oxides can be categorized as basic, acidic or amphoteric. Basic oxides are ionic and are formed by metals on the left side of the periodic table. Acidic oxides are covalent and are formed by nonmetals on the right side of the periodic table.

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (1) and (2) should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

Answer 6

Chapter 22, Problem 22.24CP

Interpretation Introduction

(a)

Interpretation:

The oxidation state of oxygen in each oxide and the oxidation state of the other element should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

All the oxygen in oxides are in −2 oxidation state.

Answer 7

Chapter 22, Problem 22.24CP

Interpretation Introduction

(a)

Interpretation:

The oxidation state of oxygen in each oxide and the oxidation state of the other element should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

All the oxygen in oxides are in −2 oxidation state.

Answer 8

Interpretation Introduction

(b)

Interpretation:

Each oxide should be identified as ionic or covalent.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

Answer 9

Interpretation Introduction

(b)

Interpretation:

Each oxide should be identified as ionic or covalent.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

Answer 10

Interpretation Introduction

(c)

Interpretation:

Each oxide should be identified as acidic or basic

Concept introduction:

Oxides can be categorized as basic, acidic or amphoteric. Basic oxides are ionic and are formed by metals on the left side of the periodic table. Acidic oxides are covalent and are formed by nonmetals on the right side of the periodic table.

Answer 11

Interpretation Introduction

(c)

Interpretation:

Each oxide should be identified as acidic or basic

Concept introduction:

Oxides can be categorized as basic, acidic or amphoteric. Basic oxides are ionic and are formed by metals on the left side of the periodic table. Acidic oxides are covalent and are formed by nonmetals on the right side of the periodic table.

Answer 12

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (1) and (2) should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

Answer 13

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (1) and (2) should be determined.

Concept introduction:

Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.

When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.

Answer 14

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Answer 16

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Answer 17

Ch. 22 - Which element has more nonmetallic character:Cl or...Ch. 22 - Prob. 22.2A Ch. 22 - Prob. 22.3P Ch. 22 - Prob. 22.4A Ch. 22 - Prob. 22.5P Ch. 22 - Look at the location of elements A, B, C, and Din...Ch. 22 - What are the formula and charge of the silicate...Ch. 22 - Suggest a plausible structure for the silicate...Ch. 22 - Prob. 22.9P Ch. 22 - Write balanced net ionic equations for the...

Solution Summary: The author explains that oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electron through covalent bonding.

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Chapter 22 Solutions