Interpretation:
Among I, II and III, arrangement that possesses strongest intermolecular attractions has to be determined. Also, reason for the same has to be explained.
Concept Introduction:
Intermolecular forces are forces that are responsible for interaction between molecules. Such forces include both attractive as well as repulsive forces.
Types of intermolecular forces:
1. Ion-dipole forces: These forces come into play when ions interact with polar molecules. Ion gets attracted to oppositely charged end of polar molecule.
2. Dipole-dipole forces: These forces arise when there is interaction between oppositely charged ends of different dipoles.
3. London forces: These forces exist when there is interaction between nonpolar molecules. There occurs distortion in symmetry of electron clouds when two nonpolar molecules come closer to each other. Such forces exist in all molecules and therefore London forces are called universal.
4. Hydrogen bonding: This intermolecular force exists when hydrogen atoms are connected to highly electronegative elements like
Want to see the full answer?
Check out a sample textbook solutionChapter 3 Solutions
Chemical Principles: The Quest for Insight
- Predict which liquid—glycerol, HOCH2CH(OH)CH2OH, or hexane, C6H14—has the greater surface tension. Explain your prediction.arrow_forwardWhich of the following compounds would be expected to form intermolecular hydrogen bonds in the liquid state? (a) H2Se (b) HCO2H (formic acid) (c) HI (d) acetone, (CH3)2COarrow_forwardSilane SiH4, phosphine (PH3), and hydrogen sulfide (H2S) melt at 185 C, 133 C, and 85 C, respectively. What does this suggest about the polar character and intermolecular attractions of the three compounds?arrow_forward
- The compounds ethanol (C2H5OH) and dimethyl ether (CH3OCH3) have the same molecular formula. Which is expected to have the higher surface tension? Why?arrow_forwardDefine the following terms and describe how each depends on the strength of the intermolecular forces. a. surface tension b. viscosity c. melting point d. boiling point e. vapor pressurearrow_forwardName the type(s) of intermolecular forces that exists between molecules (or basic units) in each of the following species and identify the following species that are capable of hydrogen-bonding among themselves. (a) BeH2, (b) CH3COOHarrow_forward
- Silane (SiH4), phosphine (PH3), and hydrogen sulfide (H2S) melt at −185 °C, −133 °C, and −85 °C, respectively. What does this suggest about the polar character and intermolecular attractions of the three compounds?arrow_forwardIn which of these substances is hydrogen bonding likely to play an important role in determining physical properties: methane(CH4), hydrazine (H2NNH2), methyl fluoride (CH3F), hydrogen sulfide (H2S)?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: 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:OpenStax
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning