A plot of the boiling point in kelvins versus the number of hydrogen atoms present in N e , H F , H 2 O , N H 3 a n d C H 4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained. Concept Introduction: Hydrogen bonding: Hydrogen bonding is a special form of dipole-dipole interaction. When a hydrogen atom is bonded to a small electronegative atom (like N , O a n d F ), then the electronegative atom pulls electron density away from the hydrogen atom. This results a partial positive charge on the hydrogen atom and a partial negative charge on the electronegative atom. The hydrogen atom on one molecule will be attracted to the electronegative atom on another molecule. Like this hydrogen bonding takes place. It is quite stronger than other intermolecular forces like dipole-dipole interactions and London forces. London forces: London(dispersion) forces happen because sometimes, when adjacent molecules line up so that they form temporary dipoles, there is a weak force of attraction between the end of one molecule where more of the electrons are accumulating at the moment and the end of a second molecule where the electrons are not staying at the moment.

Question

Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. chemical symbol, substance chemical formula boiling point or Lewis structure A СаО |(Choose one) v H H | Н — С — О — С — Н .. В (Choose one) H H C CO |(Choose one) ♥ H H Н — С С — О — Н |(Choose one) ♥ | н н - aC

Answer 1

Question

Chapter 9, Problem 119QRT

(a)

Interpretation Introduction

Interpretation:

A plot of the boiling point in kelvins versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Hydrogen bonding:

Hydrogen bonding is a special form of dipole-dipole interaction. When a hydrogen atom is bonded to a small electronegative atom (like N, O and F), then the electronegative atom pulls electron density away from the hydrogen atom. This results a partial positive charge on the hydrogen atom and a partial negative charge on the electronegative atom. The hydrogen atom on one molecule will be attracted to the electronegative atom on another molecule. Like this hydrogen bonding takes place. It is quite stronger than other intermolecular forces like dipole-dipole interactions and London forces.

London forces:

London(dispersion) forces happen because sometimes, when adjacent molecules line up so that they form temporary dipoles, there is a weak force of attraction between the end of one molecule where more of the electrons are accumulating at the moment and the end of a second molecule where the electrons are not staying at the moment.

(b)

Interpretation Introduction

Interpretation:

A plot of the molar vaporization enthalpy versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Refer to part (a).

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Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. chemical symbol, substance chemical formula boiling point or Lewis structure A СаО |(Choose one) v H H | Н — С — О — С — Н .. В (Choose one) H H C CO |(Choose one) ♥ H H Н — С С — О — Н |(Choose one) ♥ | н н - aC

Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. substance B C D chemical symbol, chemical formula or Lewis structure HI H H ** HICIO-C-H со Cao I I H H H II HICICIOIH I | | H H boiling point (Choose one) (Choose one) (Choose one) • (Choose one)

calculate the standard N-H bond enthalpy the following from data. 2 NH3 N2 ca) + 3 H2 (g2

Answer 2

Question

Chapter 9, Problem 119QRT

(a)

Interpretation Introduction

Interpretation:

A plot of the boiling point in kelvins versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Hydrogen bonding:

Hydrogen bonding is a special form of dipole-dipole interaction. When a hydrogen atom is bonded to a small electronegative atom (like N, O and F), then the electronegative atom pulls electron density away from the hydrogen atom. This results a partial positive charge on the hydrogen atom and a partial negative charge on the electronegative atom. The hydrogen atom on one molecule will be attracted to the electronegative atom on another molecule. Like this hydrogen bonding takes place. It is quite stronger than other intermolecular forces like dipole-dipole interactions and London forces.

London forces:

London(dispersion) forces happen because sometimes, when adjacent molecules line up so that they form temporary dipoles, there is a weak force of attraction between the end of one molecule where more of the electrons are accumulating at the moment and the end of a second molecule where the electrons are not staying at the moment.

(b)

Interpretation Introduction

Interpretation:

A plot of the molar vaporization enthalpy versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Refer to part (a).

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Answer 3

Question

Chapter 9, Problem 119QRT

(a)

Interpretation Introduction

Interpretation:

A plot of the boiling point in kelvins versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Hydrogen bonding:

Hydrogen bonding is a special form of dipole-dipole interaction. When a hydrogen atom is bonded to a small electronegative atom (like N, O and F), then the electronegative atom pulls electron density away from the hydrogen atom. This results a partial positive charge on the hydrogen atom and a partial negative charge on the electronegative atom. The hydrogen atom on one molecule will be attracted to the electronegative atom on another molecule. Like this hydrogen bonding takes place. It is quite stronger than other intermolecular forces like dipole-dipole interactions and London forces.

London forces:

London(dispersion) forces happen because sometimes, when adjacent molecules line up so that they form temporary dipoles, there is a weak force of attraction between the end of one molecule where more of the electrons are accumulating at the moment and the end of a second molecule where the electrons are not staying at the moment.

(b)

Interpretation Introduction

Interpretation:

A plot of the molar vaporization enthalpy versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Refer to part (a).

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Answer 4

Question

Chapter 9, Problem 119QRT

(a)

Interpretation Introduction

Interpretation:

A plot of the boiling point in kelvins versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Hydrogen bonding:

Hydrogen bonding is a special form of dipole-dipole interaction. When a hydrogen atom is bonded to a small electronegative atom (like N, O and F), then the electronegative atom pulls electron density away from the hydrogen atom. This results a partial positive charge on the hydrogen atom and a partial negative charge on the electronegative atom. The hydrogen atom on one molecule will be attracted to the electronegative atom on another molecule. Like this hydrogen bonding takes place. It is quite stronger than other intermolecular forces like dipole-dipole interactions and London forces.

London forces:

London(dispersion) forces happen because sometimes, when adjacent molecules line up so that they form temporary dipoles, there is a weak force of attraction between the end of one molecule where more of the electrons are accumulating at the moment and the end of a second molecule where the electrons are not staying at the moment.

(b)

Interpretation Introduction

Interpretation:

A plot of the molar vaporization enthalpy versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Refer to part (a).

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Answer 5

Chapter 9, Problem 119QRT

(a)

Interpretation Introduction

Interpretation:

A plot of the boiling point in kelvins versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Hydrogen bonding:

Hydrogen bonding is a special form of dipole-dipole interaction. When a hydrogen atom is bonded to a small electronegative atom (like N, O and F), then the electronegative atom pulls electron density away from the hydrogen atom. This results a partial positive charge on the hydrogen atom and a partial negative charge on the electronegative atom. The hydrogen atom on one molecule will be attracted to the electronegative atom on another molecule. Like this hydrogen bonding takes place. It is quite stronger than other intermolecular forces like dipole-dipole interactions and London forces.

London forces:

London(dispersion) forces happen because sometimes, when adjacent molecules line up so that they form temporary dipoles, there is a weak force of attraction between the end of one molecule where more of the electrons are accumulating at the moment and the end of a second molecule where the electrons are not staying at the moment.

(b)

Interpretation Introduction

Interpretation:

A plot of the molar vaporization enthalpy versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Refer to part (a).

Answer 6

Chapter 9, Problem 119QRT

(a)

Interpretation Introduction

Interpretation:

A plot of the boiling point in kelvins versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Hydrogen bonding:

Hydrogen bonding is a special form of dipole-dipole interaction. When a hydrogen atom is bonded to a small electronegative atom (like N, O and F), then the electronegative atom pulls electron density away from the hydrogen atom. This results a partial positive charge on the hydrogen atom and a partial negative charge on the electronegative atom. The hydrogen atom on one molecule will be attracted to the electronegative atom on another molecule. Like this hydrogen bonding takes place. It is quite stronger than other intermolecular forces like dipole-dipole interactions and London forces.

London forces:

London(dispersion) forces happen because sometimes, when adjacent molecules line up so that they form temporary dipoles, there is a weak force of attraction between the end of one molecule where more of the electrons are accumulating at the moment and the end of a second molecule where the electrons are not staying at the moment.

Answer 7

Chapter 9, Problem 119QRT

(a)

Interpretation Introduction

Interpretation:

A plot of the boiling point in kelvins versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Hydrogen bonding:

Hydrogen bonding is a special form of dipole-dipole interaction. When a hydrogen atom is bonded to a small electronegative atom (like N, O and F), then the electronegative atom pulls electron density away from the hydrogen atom. This results a partial positive charge on the hydrogen atom and a partial negative charge on the electronegative atom. The hydrogen atom on one molecule will be attracted to the electronegative atom on another molecule. Like this hydrogen bonding takes place. It is quite stronger than other intermolecular forces like dipole-dipole interactions and London forces.

London forces:

London(dispersion) forces happen because sometimes, when adjacent molecules line up so that they form temporary dipoles, there is a weak force of attraction between the end of one molecule where more of the electrons are accumulating at the moment and the end of a second molecule where the electrons are not staying at the moment.

Answer 8

(b)

Interpretation Introduction

Interpretation:

A plot of the molar vaporization enthalpy versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

A plot of the molar vaporization enthalpy versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Refer to part (a).

Answer 10

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Answer 11

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Answer 21

Ch. 9.1 - Prob. 9.1CE Ch. 9.2 - Prob. 9.2CE Ch. 9.2 - Prob. 9.1PSP Ch. 9.2 - What mass (g) of ethanol, CH3CH2OH(), can be...Ch. 9.3 - Prob. 9.3CE Ch. 9.3 - Prob. 9.4CE Ch. 9.3 - Prob. 9.3PSP Ch. 9.4 - What types of solids are these substances? (a) The...Ch. 9.4 - Prob. 9.5PSP Ch. 9.4 - Prob. 9.5E

Solution Summary: The author explains that hydrogen bonding is a special form of dipole-dipole interaction.

Interpretation:

A plot of the molar vaporization enthalpy versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Refer to part (a).

Chapter 9 Solutions

Solution Summary: The author explains that hydrogen bonding is a special form of dipole-dipole interaction.

Interpretation: A plot of the molar vaporization enthalpy versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained. Concept Introduction: Refer to part (a).

Chapter 9 Solutions

Interpretation:

A plot of the molar vaporization enthalpy versus the number of hydrogen atoms present in Ne, HF, H2O, NH3 and CH4 has to be drawn. Any trend that can be observed in terms of intermolecular forces has to be explained.

Concept Introduction:

Refer to part (a).