
a)
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 –
Figure 1
Figure 2
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.
b)
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 –
Figure 1
Figure 2
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:
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 –
Figure 1
Figure 2
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:
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 –
Figure 1
Figure 2
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.

Trending nowThis is a popular solution!

Chapter 10 Solutions
Student Solutions Manual for Zumdahl/Zumdahl/DeCoste?s Chemistry, 10th Edition
- Predict the major organic product(s) of the following reactions. Include stereochemistry when necessary. Write NR if no reaction, try to explain.arrow_forwardQ2: Explain why epoxides that react in an SN1 manner will not show any stereochemical inversion in the product. Q3: Rationalize why Alcohol B will react under the indicated reaction conditions, but Alcohol A will not. A ☑ OH B OH PBr3 R-Brarrow_forwardQ1: Predict the major organic product(s) of the following reactions. Include stereochemistry when necessary. Write NR if no reaction, try to explain. 1.) LDA, THF 2.) СОН CI OH H2SO4, heat OH m...... OH 1.) PCC, CH2Cl2 2.) CH3CH2MgBr, THF 3.) H3O+ 4.) TsCl, pyr 5.) tBuOK, tBuOH 1.) SOCI 2, CHCI 3 2.) CH3CH2ONA, DMF OH 1.) HBr 2.) Mg, THF 3.) H₂CO, THE 4.) H3O+ OH NaH, THFarrow_forward
- Problem 6-29 Identify the functional groups in the following molecules, and show the polarity of each: (a) CH3CH2C=N CH, CH, COCH (c) CH3CCH2COCH3 NH2 (e) OCH3 (b) (d) O Problem 6-30 Identify the following reactions as additions, eliminations, substitutions, or rearrangements: (a) CH3CH2Br + NaCN CH3CH2CN ( + NaBr) Acid -OH (+ H2O) catalyst (b) + (c) Heat NO2 Light + 02N-NO2 (+ HNO2) (d)arrow_forwardPredict the organic product of Y that is formed in the reaction below, and draw the skeletal ("line") structures of the missing organic product. Please include all steps & drawings & explanations.arrow_forwardPlease choose the best reagents to complete the following reactionarrow_forward
- Problem 6-17 Look at the following energy diagram: Energy Reaction progress (a) Is AG for the reaction positive or negative? Label it on the diagram. (b) How many steps are involved in the reaction? (c) How many transition states are there? Label them on the diagram. Problem 6-19 What is the difference between a transition state and an intermediate? Problem 6-21 Draw an energy diagram for a two-step reaction with Keq > 1. Label the overall AG°, transition states, and intermediate. Is AG° positive or negative? Problem 6-23 Draw an energy diagram for a reaction with Keq = 1. What is the value of AG° in this reaction?arrow_forwardProblem 6-37 Draw the different monochlorinated constitutional isomers you would obtain by the radical chlorination of the following compounds. (b) (c) Problem 6-39 Show the structure of the carbocation that would result when each of the following alkenes reacts with an acid, H+. (a) (b) (c)arrow_forwardPlease draw the major product of this reaction. Ignore inorganic byproducts and the carboxylic side productarrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning





