(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 22.25CP

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 molecular or a solid with an infinity extended three-dimensional structure

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:

The oxides which are likely to be a gas or a liquid and which are likely to be a high-melting solid should be determined.

Concept introduction:

Most of ionic oxides form crystal lattice structures. Lattice energies are very high, so, the bonds between atoms are difficult to break. So, ionic oxides have higher melting points. Most first row and second row nonmetal oxides have lower melting points, so, most of them exists as gas or liquid at room temperature.

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (2) and (3) 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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Students have asked these similar questions

The elements sodium, aluminum, and chlorine are in the same period. (a) Which has the greatest electronegativity? (b) Which of the atoms is smallest? (c) Which is the largest possible oxidation state for each of these elements? (d) Will the oxide of each element in the highest oxidation state (write its formula) be acidic, basic, or amphoteric?

(a) What are the common oxidation states of the halogens?(b) Give an explanation based on electron configuration for the range and values of the oxidation states of chlorine.(c) Why is fluorine an exception to the pattern of oxidation states found for the other group members?

Q.5(a) The alkali metals follow the noble gases in their atomic structure. What properties of these metals can be predicted from this information? (b) Arrange the carbonates of alkaline earth metals in order of thermal stability. (c) Explain the process involved in the manufacture of NaOH, Na2CO3 and NaHCO3. (d) Identify the element X in each of the following: (i) The oxide of XO2 has a high M.P., and is very abundant in nature. (ii) X forms three oxides: XO, XO2, X3O2. (iii) X forms compounds mainly in the +2 O.S., though some compounds in +4 state do exist. (iv) X occurs as several allotropes, including a molecular one. (e) Borazine reacts with three mole equivalents of HCl to give a material with chemical composition B3N3H9C13. (i) What is the structure of product? (ii) How does the isoelectronic benzene react with HCl? (f) Explain why bond length in NO (115 pm) is longer than that in nitrosonium ion (106 pm)?

Answer 2

Question

Chapter 22, Problem 22.25CP

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 molecular or a solid with an infinity extended three-dimensional structure

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:

The oxides which are likely to be a gas or a liquid and which are likely to be a high-melting solid should be determined.

Concept introduction:

Most of ionic oxides form crystal lattice structures. Lattice energies are very high, so, the bonds between atoms are difficult to break. So, ionic oxides have higher melting points. Most first row and second row nonmetal oxides have lower melting points, so, most of them exists as gas or liquid at room temperature.

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (2) and (3) 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 22.25CP

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 molecular or a solid with an infinity extended three-dimensional structure

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:

The oxides which are likely to be a gas or a liquid and which are likely to be a high-melting solid should be determined.

Concept introduction:

Most of ionic oxides form crystal lattice structures. Lattice energies are very high, so, the bonds between atoms are difficult to break. So, ionic oxides have higher melting points. Most first row and second row nonmetal oxides have lower melting points, so, most of them exists as gas or liquid at room temperature.

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (2) and (3) 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 22.25CP

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 molecular or a solid with an infinity extended three-dimensional structure

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:

The oxides which are likely to be a gas or a liquid and which are likely to be a high-melting solid should be determined.

Concept introduction:

Most of ionic oxides form crystal lattice structures. Lattice energies are very high, so, the bonds between atoms are difficult to break. So, ionic oxides have higher melting points. Most first row and second row nonmetal oxides have lower melting points, so, most of them exists as gas or liquid at room temperature.

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (2) and (3) 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 22.25CP

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 molecular or a solid with an infinity extended three-dimensional structure

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:

The oxides which are likely to be a gas or a liquid and which are likely to be a high-melting solid should be determined.

Concept introduction:

Most of ionic oxides form crystal lattice structures. Lattice energies are very high, so, the bonds between atoms are difficult to break. So, ionic oxides have higher melting points. Most first row and second row nonmetal oxides have lower melting points, so, most of them exists as gas or liquid at room temperature.

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (2) and (3) 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 22.25CP

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 22.25CP

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 molecular or a solid with an infinity extended three-dimensional structure

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 molecular or a solid with an infinity extended three-dimensional structure

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:

The oxides which are likely to be a gas or a liquid and which are likely to be a high-melting solid should be determined.

Concept introduction:

Most of ionic oxides form crystal lattice structures. Lattice energies are very high, so, the bonds between atoms are difficult to break. So, ionic oxides have higher melting points. Most first row and second row nonmetal oxides have lower melting points, so, most of them exists as gas or liquid at room temperature.

Answer 11

Interpretation Introduction

(c)

Interpretation:

The oxides which are likely to be a gas or a liquid and which are likely to be a high-melting solid should be determined.

Concept introduction:

Most of ionic oxides form crystal lattice structures. Lattice energies are very high, so, the bonds between atoms are difficult to break. So, ionic oxides have higher melting points. Most first row and second row nonmetal oxides have lower melting points, so, most of them exists as gas or liquid at room temperature.

Answer 12

Interpretation Introduction

(d)

Interpretation:

The identity of the other element in (2) and (3) 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 (2) and (3) 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 15

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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 how 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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