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

10. (5pts) Provide the complete arrow pushing mechanism for the chemical transformation → depicted below Use proper curved arrow notation that explicitly illustrates all bonds being broken, and all bonds formed in the transformation. Also, be sure to include all lone pairs and formal charges on all atoms involved in the flow of electrons. CH3O II HA H CH3O-H H ①

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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10. (5pts) Provide the complete arrow pushing mechanism for the chemical transformation → depicted below Use proper curved arrow notation that explicitly illustrates all bonds being broken, and all bonds formed in the transformation. Also, be sure to include all lone pairs and formal charges on all atoms involved in the flow of electrons. CH3O II HA H CH3O-H H ①

Do the Lone Pairs get added bc its valence e's are a total of 6 for oxygen and that completes it or due to other reasons. How do we know the particular indication of such.

NGLISH b) Identify the bonds present in the molecule drawn (s) above. (break) State the function of the following equipments found in laboratory. Omka) a) Gas mask b) Fire extinguisher c) Safety glasses 4. 60cm³ of oxygen gas diffused through a porous hole in 50 seconds. How long w 80cm³ of sulphur(IV) oxide to diffuse through the same hole under the same conditions (S-32.0.0-16.0) (3 m 5. In an experiment, a piece of magnesium ribbon was cleaned with steel w clean magnesium ribbon was placed in a crucible and completely burnt in oxy cooling the product weighed 4.0g a) Explain why it is necessary to clean magnesium ribbon. Masterclass Holiday assignmen PB 2

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 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).