(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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(a 4 shows scanning electron microscope (SEM) images of extruded actions of packing bed for two capillary columns of different diameters, al 750 (bottom image) and b) 30-μm-i.d. Both columns are packed with the same stationary phase, spherical particles with 1-um diameter. A) When the columns were prepared, the figure shows that the column with the larger diameter has more packing irregularities. Explain this observation. B) Predict what affect this should have on band broadening and discuss your prediction using the van Deemter terms. C) Does this figure support your explanations in application question 33? Explain why or why not and make any changes in your answers in light of this figure. Figure 4 SEM images of sections of packed columns for a) 750 and b) 30-um-i.d. capillary columns.³

fcrip = ↓ bandwidth Il temp 32. What impact (increase, decrease, or no change) does each of the following conditions have on the individual components of the van Deemter equation and consequently, band broadening? Increase temperature Longer column Using a gas mobile phase instead of liquid Smaller particle stationary phase Multiple Paths Diffusion Mass Transfer

34. Figure 3 shows Van Deemter plots for a solute molecule using different column inner diameters (i.d.). A) Predict whether decreasing the column inner diameters increase or decrease bandwidth. B) Predict which van Deemter equation coefficient (A, B, or C) has the greatest effect on increasing or decreasing bandwidth as a function of i.d. and justify your answer. Figure 3 Van Deemter plots for hydroquinone using different column inner diameters (i.d. in μm). The data was obtained from liquid chromatography experiments using fused-silica capillary columns packed with 1.0-μm particles. 35 20 H(um) 큰 20 15 90 0+ 1500 100 75 550 01 02 594 05 μ(cm/sec) 30 15 10

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 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