Concept explainers
Videos
a.
Interpretation: The molecules that contain polar bonds; the polar molecules and the non-polar molecules from the given molecules are to be identified.
Concept introduction: Polarity in bond arises due to the difference in electronegativity of the bonded atoms.
If the net dipole moment of the molecule is zero, the molecule is non-polar.
If the molecule has some net dipole moment than the molecule is polar.
The overall polarity of the molecule is determined by calculating the vector sum of the individual bond polarities.
To identify: The molecules that contain polar bonds.
a.
Answer to Problem 9.45QP
Solution
All the molecules contain polar bonds in there structure.
Explanation of Solution
Explanation
Polarity in bond arises due to the difference in electronegativity of the bonded atoms.
For molecule (a)
In 
, there is difference in electronegativity of carbon and chlorine atoms because chlorine is more electronegative than carbon.
Therefore, the bonds in is polar.
For molecule (b)
In 
, there is difference in electronegativity of carbon and hydrogen atom because carbon is more electronegative than hydrogen.
Therefore, the 
bond in is polar.
In , there is difference in electronegativity of carbon and chlorine atom because chlorine is more electronegative than carbon.
Therefore, the 
bond in is polar.
For molecule (c)
In 
, there is difference in electronegativity of carbon and oxygen atoms because oxygen is more electronegative than carbon.
Therefore, the 
bonds in is polar.
For molecule (d)
In 
, there is difference in electronegativity of sulphur and hydrogen atom because sulphur is more electronegative than hydrogen.
Therefore, the 
bond in is polar.
For molecule (e)
In 
, there is difference in electronegativity of sulphur and oxygen atoms because oxygen is more electronegative than sulphur.
Therefore, the 
bond in is polar.
b.
To identify: The molecules that are polar.
b.
Answer to Problem 9.45QP
Solution
The polar molecules are , and .
Explanation of Solution
Explanation
Polarity in bond arises due to the difference in electronegativity of the bonded atoms.
If the net dipole moment of the molecule is zero, the molecule is non polar in nature.
If the molecule has some net dipole moment than the molecule is polar in nature.
The overall polarity of the molecule is determined by calculating the vector sum of the individual bond polarities.
For molecule (a)
In , there is difference in electronegativity of carbon and chlorine atoms because chlorine is more electronegative than carbon.
Therefore, the bonds in are polar.
The dipole moment of 
bonds get cancelled out to give zero net dipole moment to the molecule.
Therefore, the is non polar.
For molecule (b)
In , there is difference in electronegativity of carbon and hydrogen atom because carbon is more electronegative than hydrogen.
Therefore, the bond in is polar.
In , there is difference in electronegativity of carbon and chlorine atom because chlorine is more electronegative than carbon.
Therefore, the bonds in is polar.
The sum of dipole moment of one bond and three give a net dipole moment to the molecule.
Therefore, the molecule is polar.
For molecule (c)
In , there is difference in electronegativity of carbon and oxygen atoms because oxygen is more electronegative than carbon.
Therefore, the bonds in is polar.
The dipole moment of bonds get cancelled out to give zero net dipole moment to the molecule.
Therefore, the is non polar.
For molecule (d)
In , there is difference in electronegativity of sulphur and hydrogen atom because sulphur is more electronegative than hydrogen.
Therefore, the bondS in is polar.
The sum of dipole moment of two bonds gives a net dipole moment to the molecule.
Therefore, the molecule is polar.
For molecule (e)
In , there is difference in electronegativity of sulphur and oxygen atoms because oxygen is more electronegative than sulphur.
Therefore, the bonds in is polar.
The structure of is bent. The sum of dipole moment of two bonds gives a net dipole moment to the molecule.
Therefore, the molecule is polar.
c.
To identify: The molecules that are non polar.
c.
Answer to Problem 9.45QP
Solution
The polar molecules are and .
Explanation of Solution
Explanation
Polarity in bond arises due to the difference in electronegativity of the bonded atoms.
If the net dipole moment of the molecule is zero, the molecule is non polar in nature.
If the molecule has some net dipole moment than the molecule is polar in nature.
The overall polarity of the molecule is determined by calculating the vector sum of the individual bond polarities.
For molecule (a)
In , there is difference in electronegativity of carbon and chlorine atoms because chlorine is more electronegative than carbon.
Therefore, the bonds in is polar.
The dipole moment of bonds get cancelled out to give zero net dipole moment to the molecule.
Therefore, the is non polar.
For molecule (b)
In , there is difference in electronegativity of carbon and hydrogen atom because carbon is more electronegative than hydrogen.
Therefore, the bond in is polar.
In , there is difference in electronegativity of carbon and chlorine atom because chlorine is more electronegative than carbon.
Therefore, the bonds in is polar.
The sum of dipole moment of one bond and three give a net dipole moment to the molecule.
Therefore, the molecule is polar.
For molecule (c)
In , there is difference in electronegativity of carbon and oxygen atoms because oxygen is more electronegative than carbon.
Therefore, the bonds in is polar.
The dipole moment of bonds get cancelled out to give zero net dipole moment to the molecule.
Therefore, the is non polar.
For molecule (d)
In , there is difference in electronegativity of sulphur and hydrogen atom because sulphur is more electronegative than hydrogen.
Therefore, the bond in is polar.
The sum of dipole moment of two bonds gives a net dipole moment to the molecule.
Therefore, the molecule is polar.
For molecule (e)
In , there is difference in electronegativity of sulphur and oxygen atoms because oxygen is more electronegative than sulphur.
Therefore, the bonds in is polar.
The structure of is bent. The sum of dipole moment of two bonds gives a net dipole moment to the molecule.
Therefore, the molecule is polar.
Conclusion
- a. All the molecules contains polar bonds in there structure.
- b. The polar molecules are
, 
and 
. - c. The polar molecules are
and 
.
Want to see more full solutions like this?
Chapter 9 Solutions
Chemistry
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY