(a) Interpretation: The formula of the oxide that in its highest oxidation state should be written. 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 22.26CP

Interpretation Introduction

(a)

Interpretation:

The formula of the oxide that in its highest oxidation state should be written.

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 classified as basic, acidic or amphoteric.

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. Amphoteric oxides can react with both acids and bases.

Interpretation Introduction

(c)

Interpretation:

Which oxide is the most ionic and which oxide is the most covalent should be discussed.

Concept introduction:

When electronegativity difference between atoms in a bond is larger than two units, that bond is said to be ionic and when the difference is less than two, it is said to be a covalent bond.

Interpretation Introduction

(d)

Interpretation:

Which oxides are molecular and which are solids with an infinitely extended three-dimensional crystal structure 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.

Interpretation Introduction

(e)

Interpretation:

Which oxide has the highest melting point and which has the lowest melting point 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.

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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?

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) Write the Lewis structure for the simplest covalent compound that can form between aluminum and chlorine.(d) Will the oxide of each element be acidic, basic, or amphoteric?

Explain the differences in chemical and physical properties of metals and nonmetals, including the basicity of metal oxides and the acidity of nonmetal oxide?

Answer 2

Question

Chapter 22, Problem 22.26CP

Interpretation Introduction

(a)

Interpretation:

The formula of the oxide that in its highest oxidation state should be written.

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 classified as basic, acidic or amphoteric.

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. Amphoteric oxides can react with both acids and bases.

Interpretation Introduction

(c)

Interpretation:

Which oxide is the most ionic and which oxide is the most covalent should be discussed.

Concept introduction:

When electronegativity difference between atoms in a bond is larger than two units, that bond is said to be ionic and when the difference is less than two, it is said to be a covalent bond.

Interpretation Introduction

(d)

Interpretation:

Which oxides are molecular and which are solids with an infinitely extended three-dimensional crystal structure 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.

Interpretation Introduction

(e)

Interpretation:

Which oxide has the highest melting point and which has the lowest melting point 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.

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Answer 3

Question

Chapter 22, Problem 22.26CP

Interpretation Introduction

(a)

Interpretation:

The formula of the oxide that in its highest oxidation state should be written.

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 classified as basic, acidic or amphoteric.

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. Amphoteric oxides can react with both acids and bases.

Interpretation Introduction

(c)

Interpretation:

Which oxide is the most ionic and which oxide is the most covalent should be discussed.

Concept introduction:

When electronegativity difference between atoms in a bond is larger than two units, that bond is said to be ionic and when the difference is less than two, it is said to be a covalent bond.

Interpretation Introduction

(d)

Interpretation:

Which oxides are molecular and which are solids with an infinitely extended three-dimensional crystal structure 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.

Interpretation Introduction

(e)

Interpretation:

Which oxide has the highest melting point and which has the lowest melting point 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.

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Answer 4

Question

Chapter 22, Problem 22.26CP

Interpretation Introduction

(a)

Interpretation:

The formula of the oxide that in its highest oxidation state should be written.

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 classified as basic, acidic or amphoteric.

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. Amphoteric oxides can react with both acids and bases.

Interpretation Introduction

(c)

Interpretation:

Which oxide is the most ionic and which oxide is the most covalent should be discussed.

Concept introduction:

When electronegativity difference between atoms in a bond is larger than two units, that bond is said to be ionic and when the difference is less than two, it is said to be a covalent bond.

Interpretation Introduction

(d)

Interpretation:

Which oxides are molecular and which are solids with an infinitely extended three-dimensional crystal structure 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.

Interpretation Introduction

(e)

Interpretation:

Which oxide has the highest melting point and which has the lowest melting point 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.

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Answer 5

Chapter 22, Problem 22.26CP

Interpretation Introduction

(a)

Interpretation:

The formula of the oxide that in its highest oxidation state should be written.

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 classified as basic, acidic or amphoteric.

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. Amphoteric oxides can react with both acids and bases.

Interpretation Introduction

(c)

Interpretation:

Which oxide is the most ionic and which oxide is the most covalent should be discussed.

Concept introduction:

When electronegativity difference between atoms in a bond is larger than two units, that bond is said to be ionic and when the difference is less than two, it is said to be a covalent bond.

Interpretation Introduction

(d)

Interpretation:

Which oxides are molecular and which are solids with an infinitely extended three-dimensional crystal structure 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.

Interpretation Introduction

(e)

Interpretation:

Which oxide has the highest melting point and which has the lowest melting point 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 6

Chapter 22, Problem 22.26CP

Interpretation Introduction

(a)

Interpretation:

The formula of the oxide that in its highest oxidation state should be written.

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 22.26CP

Interpretation Introduction

(a)

Interpretation:

The formula of the oxide that in its highest oxidation state should be written.

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 classified as basic, acidic or amphoteric.

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. Amphoteric oxides can react with both acids and bases.

Answer 9

Interpretation Introduction

(b)

Interpretation:

Each oxide should be classified as basic, acidic or amphoteric.

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. Amphoteric oxides can react with both acids and bases.

Answer 10

Interpretation Introduction

(c)

Interpretation:

Which oxide is the most ionic and which oxide is the most covalent should be discussed.

Concept introduction:

When electronegativity difference between atoms in a bond is larger than two units, that bond is said to be ionic and when the difference is less than two, it is said to be a covalent bond.

Answer 11

Interpretation Introduction

(c)

Interpretation:

Which oxide is the most ionic and which oxide is the most covalent should be discussed.

Concept introduction:

When electronegativity difference between atoms in a bond is larger than two units, that bond is said to be ionic and when the difference is less than two, it is said to be a covalent bond.

Answer 12

Interpretation Introduction

(d)

Interpretation:

Which oxides are molecular and which are solids with an infinitely extended three-dimensional crystal structure 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:

Which oxides are molecular and which are solids with an infinitely extended three-dimensional crystal structure 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

Interpretation Introduction

(e)

Interpretation:

Which oxide has the highest melting point and which has the lowest melting point 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 15

Interpretation Introduction

(e)

Interpretation:

Which oxide has the highest melting point and which has the lowest melting point 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 16

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Answer 17

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Answer 18

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Answer 19

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 each oxide should be classified as basic, acidic or amphoteric.

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Chapter 22 Solutions