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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 9, Problem 39E
Textbook Problem
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Rationalize the difference in boiling points for each of the following pairs of substances:

a. n-pentane CH3CH2CH2CH2CH3 36.2°C

Chapter 9, Problem 39E, Rationalize the difference in boiling points for each of the following pairs of substances: a.

b. HF 20°C

HCl −85°C

c. HCl −85°C

LiCl 1360°C

d. n-pentane CH3CH2CH2CH2CH3 36.2°C

n-hexane CH3CH2CH2CH2CH2CH3 69°C

a)

Interpretation Introduction

Interpretation:

The difference in the boiling points of the given set of compounds has to be rationalized.

Concept Introduction:

  • Boiling point of any compound, depends upon its strength of Intramolecular force and Intermolecular force present in it.
  • Intramolecular force refers to type of bonding between the atoms.
  • Intermolecular forces are the forces that bind the molecules together to attribute to a stability of a compound.
  • If the strength of intermolecular forces is high, boiling point will be high and if it is low, boiling point will be low.
  • They are collectively known as “Interparticle forces”. The classification can be summarized as follows –

Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  1

                                                             Figure 1

    Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  2

                                                               Figure 2

Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  3

Figure 3

The type of bonding between atoms or ions is Intramolecular force. The intramolecular force in ionic compounds is electrostatic force of attraction between the ions of opposite charges.  Usually ionic compounds are solids with high melting points. Covalent bonds are of two types, that is polar covalent bond and non-polar covalent bond. Covalent compounds are found as solids and liquids with moderate melting and boiling point. Metallic bond is formed between the metal atoms of an element.

Intermolecular forces are Van der Waals forces. They are weak and are of three types - London dispersion forces, dipole-dipole forces and hydrogen bonding. Hydrogen bonding is formed in polar covalent compounds containing hydrogen and other high electronegativity like fluorine, oxygen or nitrogen. These atoms in a molecule partially bond to hydrogen of the other same molecule or within a molecule. It is relatively the strongest one. Hydrogen bonded compounds are usually liquids. They exhibit high boiling point.

London dispersion forces exist in all types of molecules. This is the force responsible for the condensation of non-polar compounds into liquids or solids under low temperature.

Dipole-dipole forces exist in polar covalent compounds. Hydrogen bonding exists in polar covalent compounds containing Fluorine, Oxygen or Nitrogen directly bonded to Hydrogen.

Explanation of Solution

Understand the type of intramolecular force and intermolecular in Neopentane and n-pentane and their impact on respective boiling points.

Both Neopentane and n-pentane have covalent bonding and London dispersion forces as their intramolecular force and intermolecular force respectively. Boiling point of n-pentane is higher than that of Neopentane.

Both Neopentane and n-pentane are hydrocarbons. They are made of strong C-H covalent bonds. C-H covalent bonds are non-polar covalent bonds. Thus hydrocarbons have London dispersion forces as their intermolecular force. Molecules of greater size have high strength of London dispersion forces

b)

Interpretation Introduction

Interpretation:

The difference in the boiling points of the given set of compounds has to be rationalized.

Concept Introduction:

  • Boiling point of any compound, depends upon its strength of Intramolecular force and Intermolecular force present in it.
  • Intramolecular force refers to type of bonding between the atoms.
  • Intermolecular forces are the forces that bind the molecules together to attribute to a stability of a compound.
  • If the strength of intermolecular forces is high, boiling point will be high and if it is low, boiling point will be low.
  • They are collectively known as “Interparticle forces”. The classification can be summarized as follows –

Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  4

                                                             Figure 1

    Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  5

                                                               Figure 2

Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  6

Figure 3

The type of bonding between atoms or ions is Intramolecular force. The intramolecular force in ionic compounds is electrostatic force of attraction between the ions of opposite charges.  Usually ionic compounds are solids with high melting points. Covalent bonds are of two types, that is polar covalent bond and non-polar covalent bond. Covalent compounds are found as solids and liquids with moderate melting and boiling point. Metallic bond is formed between the metal atoms of an element.

Intermolecular forces are Van der Waals forces. They are weak and are of three types - London dispersion forces, dipole-dipole forces and hydrogen bonding. Hydrogen bonding is formed in polar covalent compounds containing hydrogen and other high electronegativity like fluorine, oxygen or nitrogen. These atoms in a molecule partially bond to hydrogen of the other same molecule or within a molecule. It is relatively the strongest one. Hydrogen bonded compounds are usually liquids. They exhibit high boiling point.

London dispersion forces exist in all types of molecules. This is the force responsible for the condensation of non-polar compounds into liquids or solids under low temperature.

Dipole-dipole forces exist in polar covalent compounds. Hydrogen bonding exists in polar covalent compounds containing Fluorine, Oxygen or Nitrogen directly bonded to Hydrogen.

c)

Interpretation Introduction

Interpretation:

The difference in the boiling points of the given set of compounds has to be rationalized.

Concept Introduction:

  • Boiling point of any compound, depends upon its strength of Intramolecular force and Intermolecular force present in it.
  • Intramolecular force refers to type of bonding between the atoms.
  • Intermolecular forces are the forces that bind the molecules together to attribute to a stability of a compound.
  • If the strength of intermolecular forces is high, boiling point will be high and if it is low, boiling point will be low.
  • They are collectively known as “Interparticle forces”. The classification can be summarized as follows –

Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  7

                                                             Figure 1

    Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  8

                                                               Figure 2

Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  9

Figure 3

The type of bonding between atoms or ions is Intramolecular force. The intramolecular force in ionic compounds is electrostatic force of attraction between the ions of opposite charges.  Usually ionic compounds are solids with high melting points. Covalent bonds are of two types, that is polar covalent bond and non-polar covalent bond. Covalent compounds are found as solids and liquids with moderate melting and boiling point. Metallic bond is formed between the metal atoms of an element.

Intermolecular forces are Van der Waals forces. They are weak and are of three types - London dispersion forces, dipole-dipole forces and hydrogen bonding. Hydrogen bonding is formed in polar covalent compounds containing hydrogen and other high electronegativity like fluorine, oxygen or nitrogen. These atoms in a molecule partially bond to hydrogen of the other same molecule or within a molecule. It is relatively the strongest one. Hydrogen bonded compounds are usually liquids. They exhibit high boiling point.

London dispersion forces exist in all types of molecules. This is the force responsible for the condensation of non-polar compounds into liquids or solids under low temperature.

Dipole-dipole forces exist in polar covalent compounds. Hydrogen bonding exists in polar covalent compounds containing Fluorine, Oxygen or Nitrogen directly bonded to Hydrogen.

d)

Interpretation Introduction

Interpretation:

The difference in the boiling points of the given set of compounds has to be rationalized.

Concept Introduction:

  • Boiling point of any compound, depends upon its strength of Intramolecular force and Intermolecular force present in it.
  • Intramolecular force refers to type of bonding between the atoms.
  • Intermolecular forces are the forces that bind the molecules together to attribute to a stability of a compound.
  • If the strength of intermolecular forces is high, boiling point will be high and if it is low, boiling point will be low.
  • They are collectively known as “Interparticle forces”. The classification can be summarized as follows –

Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  10

                                                             Figure 1

    Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  11

                                                               Figure 2

Chemistry: An Atoms First Approach, Chapter 9, Problem 39E , additional homework tip  12

Figure 3

The type of bonding between atoms or ions is Intramolecular force. The intramolecular force in ionic compounds is electrostatic force of attraction between the ions of opposite charges.  Usually ionic compounds are solids with high melting points. Covalent bonds are of two types, that is polar covalent bond and non-polar covalent bond. Covalent compounds are found as solids and liquids with moderate melting and boiling point. Metallic bond is formed between the metal atoms of an element.

Intermolecular forces are Van der Waals forces. They are weak and are of three types - London dispersion forces, dipole-dipole forces and hydrogen bonding. Hydrogen bonding is formed in polar covalent compounds containing hydrogen and other high electronegativity like fluorine, oxygen or nitrogen. These atoms in a molecule partially bond to hydrogen of the other same molecule or within a molecule. It is relatively the strongest one. Hydrogen bonded compounds are usually liquids. They exhibit high boiling point.

London dispersion forces exist in all types of molecules. This is the force responsible for the condensation of non-polar compounds into liquids or solids under low temperature.

Dipole-dipole forces exist in polar covalent compounds. Hydrogen bonding exists in polar covalent compounds containing Fluorine, Oxygen or Nitrogen directly bonded to Hydrogen.

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Chemistry: An Atoms First Approach
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