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.

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Considering the important roles of biothiols in lysosomes of live organisms, and unique photophysical / photochemical properties of ruthenium(II) complexes, a novel ruthenium(II) complex, Ru-2, has been developed as a molecular probe for phosphorescence and time-gated luminescence assay of biothiols in human sera, live cells, and in vivo. Ru-2 is weakly luminescent due to the effective photoinduced electron transfer (PET) from Ru(II) luminophore to electron acceptor, 2,4-dinitrobenzene-sulfonyl (DNBS). In the presence of biothiols, such as glutathione (GSH), cysteine (Cys), and homocysteine (Hcy), the emission of Ru-2 solution was switched ON, as a result of the cleavage of quencher to form the product, Ru-1. Ru-2 showed high selectivity and sensitivity for the detection of biothiols under physiological conditions, with detection limits of 62 nM, 146 nM, and 115 nM for GSH, Cys, and Hcy, respectively. The emission lifetimes of Ru-1 and Ru-2 were measured to be 405 and 474 ns,…

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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Considering the important roles of biothiols in lysosomes of live organisms, and unique photophysical / photochemical properties of ruthenium(II) complexes, a novel ruthenium(II) complex, Ru-2, has been developed as a molecular probe for phosphorescence and time-gated luminescence assay of biothiols in human sera, live cells, and in vivo. Ru-2 is weakly luminescent due to the effective photoinduced electron transfer (PET) from Ru(II) luminophore to electron acceptor, 2,4-dinitrobenzene-sulfonyl (DNBS). In the presence of biothiols, such as glutathione (GSH), cysteine (Cys), and homocysteine (Hcy), the emission of Ru-2 solution was switched ON, as a result of the cleavage of quencher to form the product, Ru-1. Ru-2 showed high selectivity and sensitivity for the detection of biothiols under physiological conditions, with detection limits of 62 nM, 146 nM, and 115 nM for GSH, Cys, and Hcy, respectively. The emission lifetimes of Ru-1 and Ru-2 were measured to be 405 and 474 ns,…

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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).