To write the empirical and molecular formulas of the oxides of nitrogen for which two formulas are not the same from the given molecular models in Figure P7.1

Question

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Answer 1

Question

Chapter 7, Problem 7.1VP

Interpretation Introduction

To find:

To write the empirical and molecular formulas of the oxides of nitrogen for which two formulas are not the same from the given molecular models in Figure P7.1

Expert Solution & Answer

Answer to Problem 7.1VP

Solution:

From the given molecular models of oxides of nitrogen, the image (b) has different empirical and molecular formulas as Empirical formula = NO2 and Molecular formula =N2O4.

Explanation of Solution

Empirical formula is the simplest whole number ratio of the atoms of the elements in a compound.

Molecular formula represents the exact number and type of atoms in one molecule of a compound.

Empirical and molecular formulas can be the same or different. For example, consider the two compounds of carbon, carbon dioxide CO2 and butane C4H10.

For carbon dioxide,CO2 is a simplest whole ratio. We cannot reduce the ratio further without getting fractional values. But, in case of butane, the simplest whole number is C2H5. So, in this case, the empirical and molecular formulas for carbon dioxide is the same, but for butane the empirical formula is C2H5 and molecular formula is C4H10.

Ball-and-stick or space-filling models like the ones in Figure P7.1 use specific colors for different elements. For example, red is oxygen, blue is nitrogen, black is carbon. Based on this, the molecules in the figure are (a) N₂O₅, (b) N₂O₄, (c) NO, (d) N₂O₃, and (e) NO₂.

Out of these, only one formula, N₂O₄, can be reduced to one smaller whole number, NO₂. SO this is the only oxide for which the empirical and molecular formulas are not the same.

Conclusion:

We compared the ratio of atoms in a molecular formula. For even number of atoms, empirical and molecular formulas are different, but for odd ones, they are the same.

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Answer 2

Question

Chapter 7, Problem 7.1VP

Interpretation Introduction

To find:

To write the empirical and molecular formulas of the oxides of nitrogen for which two formulas are not the same from the given molecular models in Figure P7.1

Expert Solution & Answer

Answer to Problem 7.1VP

Solution:

From the given molecular models of oxides of nitrogen, the image (b) has different empirical and molecular formulas as Empirical formula = NO2 and Molecular formula =N2O4.

Explanation of Solution

Empirical formula is the simplest whole number ratio of the atoms of the elements in a compound.

Molecular formula represents the exact number and type of atoms in one molecule of a compound.

Empirical and molecular formulas can be the same or different. For example, consider the two compounds of carbon, carbon dioxide CO2 and butane C4H10.

For carbon dioxide,CO2 is a simplest whole ratio. We cannot reduce the ratio further without getting fractional values. But, in case of butane, the simplest whole number is C2H5. So, in this case, the empirical and molecular formulas for carbon dioxide is the same, but for butane the empirical formula is C2H5 and molecular formula is C4H10.

Ball-and-stick or space-filling models like the ones in Figure P7.1 use specific colors for different elements. For example, red is oxygen, blue is nitrogen, black is carbon. Based on this, the molecules in the figure are (a) N₂O₅, (b) N₂O₄, (c) NO, (d) N₂O₃, and (e) NO₂.

Out of these, only one formula, N₂O₄, can be reduced to one smaller whole number, NO₂. SO this is the only oxide for which the empirical and molecular formulas are not the same.

Conclusion:

We compared the ratio of atoms in a molecular formula. For even number of atoms, empirical and molecular formulas are different, but for odd ones, they are the same.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Question

Chapter 7, Problem 7.1VP

Interpretation Introduction

To find:

To write the empirical and molecular formulas of the oxides of nitrogen for which two formulas are not the same from the given molecular models in Figure P7.1

Expert Solution & Answer

Answer to Problem 7.1VP

Solution:

From the given molecular models of oxides of nitrogen, the image (b) has different empirical and molecular formulas as Empirical formula = NO2 and Molecular formula =N2O4.

Explanation of Solution

Empirical formula is the simplest whole number ratio of the atoms of the elements in a compound.

Molecular formula represents the exact number and type of atoms in one molecule of a compound.

Empirical and molecular formulas can be the same or different. For example, consider the two compounds of carbon, carbon dioxide CO2 and butane C4H10.

For carbon dioxide,CO2 is a simplest whole ratio. We cannot reduce the ratio further without getting fractional values. But, in case of butane, the simplest whole number is C2H5. So, in this case, the empirical and molecular formulas for carbon dioxide is the same, but for butane the empirical formula is C2H5 and molecular formula is C4H10.

Ball-and-stick or space-filling models like the ones in Figure P7.1 use specific colors for different elements. For example, red is oxygen, blue is nitrogen, black is carbon. Based on this, the molecules in the figure are (a) N₂O₅, (b) N₂O₄, (c) NO, (d) N₂O₃, and (e) NO₂.

Out of these, only one formula, N₂O₄, can be reduced to one smaller whole number, NO₂. SO this is the only oxide for which the empirical and molecular formulas are not the same.

Conclusion:

We compared the ratio of atoms in a molecular formula. For even number of atoms, empirical and molecular formulas are different, but for odd ones, they are the same.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Question

Chapter 7, Problem 7.1VP

Interpretation Introduction

To find:

To write the empirical and molecular formulas of the oxides of nitrogen for which two formulas are not the same from the given molecular models in Figure P7.1

Expert Solution & Answer

Answer to Problem 7.1VP

Solution:

From the given molecular models of oxides of nitrogen, the image (b) has different empirical and molecular formulas as Empirical formula = NO2 and Molecular formula =N2O4.

Explanation of Solution

Empirical formula is the simplest whole number ratio of the atoms of the elements in a compound.

Molecular formula represents the exact number and type of atoms in one molecule of a compound.

Empirical and molecular formulas can be the same or different. For example, consider the two compounds of carbon, carbon dioxide CO2 and butane C4H10.

For carbon dioxide,CO2 is a simplest whole ratio. We cannot reduce the ratio further without getting fractional values. But, in case of butane, the simplest whole number is C2H5. So, in this case, the empirical and molecular formulas for carbon dioxide is the same, but for butane the empirical formula is C2H5 and molecular formula is C4H10.

Ball-and-stick or space-filling models like the ones in Figure P7.1 use specific colors for different elements. For example, red is oxygen, blue is nitrogen, black is carbon. Based on this, the molecules in the figure are (a) N₂O₅, (b) N₂O₄, (c) NO, (d) N₂O₃, and (e) NO₂.

Out of these, only one formula, N₂O₄, can be reduced to one smaller whole number, NO₂. SO this is the only oxide for which the empirical and molecular formulas are not the same.

Conclusion:

We compared the ratio of atoms in a molecular formula. For even number of atoms, empirical and molecular formulas are different, but for odd ones, they are the same.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 7, Problem 7.1VP

Interpretation Introduction

To find:

To write the empirical and molecular formulas of the oxides of nitrogen for which two formulas are not the same from the given molecular models in Figure P7.1

Expert Solution & Answer

Answer to Problem 7.1VP

Solution:

From the given molecular models of oxides of nitrogen, the image (b) has different empirical and molecular formulas as Empirical formula = NO2 and Molecular formula =N2O4.

Explanation of Solution

Empirical formula is the simplest whole number ratio of the atoms of the elements in a compound.

Molecular formula represents the exact number and type of atoms in one molecule of a compound.

Empirical and molecular formulas can be the same or different. For example, consider the two compounds of carbon, carbon dioxide CO2 and butane C4H10.

For carbon dioxide,CO2 is a simplest whole ratio. We cannot reduce the ratio further without getting fractional values. But, in case of butane, the simplest whole number is C2H5. So, in this case, the empirical and molecular formulas for carbon dioxide is the same, but for butane the empirical formula is C2H5 and molecular formula is C4H10.

Ball-and-stick or space-filling models like the ones in Figure P7.1 use specific colors for different elements. For example, red is oxygen, blue is nitrogen, black is carbon. Based on this, the molecules in the figure are (a) N₂O₅, (b) N₂O₄, (c) NO, (d) N₂O₃, and (e) NO₂.

Out of these, only one formula, N₂O₄, can be reduced to one smaller whole number, NO₂. SO this is the only oxide for which the empirical and molecular formulas are not the same.

Conclusion:

We compared the ratio of atoms in a molecular formula. For even number of atoms, empirical and molecular formulas are different, but for odd ones, they are the same.

Answer 6

Chapter 7, Problem 7.1VP

Interpretation Introduction

To find:

To write the empirical and molecular formulas of the oxides of nitrogen for which two formulas are not the same from the given molecular models in Figure P7.1

Expert Solution & Answer

Answer to Problem 7.1VP

Solution:

From the given molecular models of oxides of nitrogen, the image (b) has different empirical and molecular formulas as Empirical formula = NO2 and Molecular formula =N2O4.

Explanation of Solution

Empirical formula is the simplest whole number ratio of the atoms of the elements in a compound.

Molecular formula represents the exact number and type of atoms in one molecule of a compound.

Empirical and molecular formulas can be the same or different. For example, consider the two compounds of carbon, carbon dioxide CO2 and butane C4H10.

For carbon dioxide,CO2 is a simplest whole ratio. We cannot reduce the ratio further without getting fractional values. But, in case of butane, the simplest whole number is C2H5. So, in this case, the empirical and molecular formulas for carbon dioxide is the same, but for butane the empirical formula is C2H5 and molecular formula is C4H10.

Ball-and-stick or space-filling models like the ones in Figure P7.1 use specific colors for different elements. For example, red is oxygen, blue is nitrogen, black is carbon. Based on this, the molecules in the figure are (a) N₂O₅, (b) N₂O₄, (c) NO, (d) N₂O₃, and (e) NO₂.

Out of these, only one formula, N₂O₄, can be reduced to one smaller whole number, NO₂. SO this is the only oxide for which the empirical and molecular formulas are not the same.

Conclusion:

We compared the ratio of atoms in a molecular formula. For even number of atoms, empirical and molecular formulas are different, but for odd ones, they are the same.

Answer 7

Chapter 7, Problem 7.1VP

Interpretation Introduction

To find:

To write the empirical and molecular formulas of the oxides of nitrogen for which two formulas are not the same from the given molecular models in Figure P7.1

Answer 8

Expert Solution & Answer

Answer to Problem 7.1VP

Solution:

From the given molecular models of oxides of nitrogen, the image (b) has different empirical and molecular formulas as Empirical formula = NO2 and Molecular formula =N2O4.

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Explanation of Solution

Empirical formula is the simplest whole number ratio of the atoms of the elements in a compound.

Molecular formula represents the exact number and type of atoms in one molecule of a compound.

Empirical and molecular formulas can be the same or different. For example, consider the two compounds of carbon, carbon dioxide CO2 and butane C4H10.

For carbon dioxide,CO2 is a simplest whole ratio. We cannot reduce the ratio further without getting fractional values. But, in case of butane, the simplest whole number is C2H5. So, in this case, the empirical and molecular formulas for carbon dioxide is the same, but for butane the empirical formula is C2H5 and molecular formula is C4H10.

Ball-and-stick or space-filling models like the ones in Figure P7.1 use specific colors for different elements. For example, red is oxygen, blue is nitrogen, black is carbon. Based on this, the molecules in the figure are (a) N₂O₅, (b) N₂O₄, (c) NO, (d) N₂O₃, and (e) NO₂.

Out of these, only one formula, N₂O₄, can be reduced to one smaller whole number, NO₂. SO this is the only oxide for which the empirical and molecular formulas are not the same.

Conclusion:

We compared the ratio of atoms in a molecular formula. For even number of atoms, empirical and molecular formulas are different, but for odd ones, they are the same.

Answer 12

Ch. 7 - Prob. 7.1VP Ch. 7 - Prob. 7.2VP Ch. 7 - Prob. 7.3VP Ch. 7 - Prob. 7.4VP Ch. 7 - Prob. 7.5VP Ch. 7 - Prob. 7.6VP Ch. 7 - Prob. 7.7QA Ch. 7 - Prob. 7.8QA Ch. 7 - Prob. 7.9QA Ch. 7 - Prob. 7.10QA

To write the empirical and molecular formulas of the oxides of nitrogen for which two formulas are not the same from the given molecular models in Figure P7.1

To find: To write the empirical and molecular formulas of the oxides of nitrogen for which two formulas are not the same from the given molecular models in Figure P7.1

Answer to Problem 7.1VP

Explanation of Solution

Want to see more full solutions like this?

Chapter 7 Solutions

To find:

To write the empirical and molecular formulas of the oxides of nitrogen for which two formulas are not the same from the given molecular models in Figure P7.1