a.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of functional group and atoms of the molecule. London forces, ionic attractions, dipole-dipole attractions and hydrogen bonding are the main attractive forces present in pure compounds. Out of these forces, dispersion forces are the weakest forces present in almost all compounds and hydrogen bonding is stronger than dipole-dipole attractions.
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
b.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of functional group and atoms of the molecule. London forces, ionic attractions, dipole-dipole attractions and hydrogen bonding are the main attractive forces present in pure compounds. Out of these forces, dispersion forces are the weakest forces present in almost all compounds and hydrogen bonding is stronger than dipole-dipole attractions.
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
c.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of functional group and atoms of the molecule. London forces, ionic attractions, dipole-dipole attractions and hydrogen bonding are the main attractive forces present in pure compounds. Out of these forces, dispersion forces are the weakest forces present in almost all compounds and hydrogen bonding is stronger than dipole-dipole attractions.
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
d.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of functional group and atoms of the molecule. London forces, ionic attractions, dipole-dipole attractions and hydrogen bonding are the main attractive forces present in pure compounds. Out of these forces, dispersion forces are the weakest forces present in almost all compounds and hydrogen bonding is stronger than dipole-dipole attractions.
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
e.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of functional group and atoms of the molecule. London forces, ionic attractions, dipole-dipole attractions and hydrogen bonding are the main attractive forces present in pure compounds. Out of these forces, dispersion forces are the weakest forces present in almost all compounds and hydrogen bonding is stronger than dipole-dipole attractions.
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
f.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of functional group and atoms of the molecule. London forces, ionic attractions, dipole-dipole attractions and hydrogen bonding are the main attractive forces present in pure compounds. Out of these forces, dispersion forces are the weakest forces present in almost all compounds and hydrogen bonding is stronger than dipole-dipole attractions.
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
Want to see the full answer?
Check out a sample textbook solutionChapter 7 Solutions
Student's Study Guide for General, Organic, and Biological Chemistry
- Correct or incorrect a)Methanol is a polar molecule. True or False? b)List all the intermolecular forces available between methanol molecules in a pure solution? c)Dry ice (solid carbon dioxide) molecules will have dipole-dipole intermolecular forces between them. True or False?arrow_forwardAnswer each of the following questions correctly (This is all about Intermolecular Forces of Liquids and Solids; Solids and their Properties) Crystal: Uric acid in gout a. How is the crystal formed? b. Is it beneficial or harmful to man or both? Discuss how it is beneficial or harmful to man. c. If it is something harmful, what can be done to avoid its formation? If it is something beneficial, how can its formation be promoted?arrow_forwardHow do attractive forces between like molecules compare with attractive forces between unlike molecules in the system acetic acid-water?arrow_forward
- Substance A is composed of molecules that have stronger intermolecular forces than the molecules that compose substance B. Which substance has a lower boiling point? a. substance A b. substance B c. cannot be determined without more information.arrow_forwardCooking oil floats on top of water. From this observation, what conclusions can you draw regarding the polarity or hydrogen-bonding ability of molecules found in cooking oil?arrow_forward8.36 Why are dispersion forces attractive?arrow_forward
- Which compound would you expect to have the highest boiling point? Why? a.H2Ob.H2Sc.HClarrow_forwardWhen a doughnut is placed on a napkin, the napkin will often absorb a liquid and appear moist. What is most likely the nature of the liquid?arrow_forwardDraw a molecular scale picture to show how a crystal differs from a liquid.arrow_forward
- Consider the following electrostatic potential diagrams: Rank the compounds from lowest to highest boiling point and explain your answer.arrow_forwardWhat are the strongest and weakest forces of attraction between molecules? (strongest; weakest)arrow_forwardExplain (in one sentence) why Mg2+ has larger hydrated diameter compared to Ba2+.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning