
Concept explainers
(a)
Interpretation:
Given uncharged molecule is to be identified as polar or nonpolar, using its electrostatic potential map. If the molecule is polar, the direction of its net molecular dipole moment it to be determined.
Concept introduction:
A polar bond is one in which the bond pair is unequally shared by the two atoms.
A partial positive charge is developed on the less electronegative atom while and an equal but negative partial charge is developed on the more electronegative atom.
Molecules that contain more than one polar bond may or may not have a net dipole moment. The dipole moment is a vector quantity. The net molecular dipole moment is the result of the vector addition of all the individual dipole moments. Depending on the symmetry of the molecule, the individual bond dipoles can partly or completely cancel or reinforce each other.
A bond dipole or a molecular dipole is represented by an arrow pointing from the atom or region with a partial positive charge toward an atom or region with a partial negative charge.
Electrostatic potential maps of molecules show the distribution of electron density in different parts of the molecule. The electron density is represented by different colors, ranging from blue to red. Blue color indicates a low electron density, an atom or region with a partial positive charge. Red color indicates high electron density, an atom or region with a partial negative charge.

Answer to Problem 2.40P
The electrostatic potential map shows that the molecule is nonpolar.
Explanation of Solution
The electrostatic potential map shows the molecule with a negative charge concentrated at the center, with positive charge distributed symmetrically around the center. This shows that the individual bond dipoles are all of equal magnitude, and they all point toward the center. The vector addition of these dipoles will be zero because of their symmetric distribution. Therefore, the molecule is nonpolar.
The net dipole moment of a molecule is the vector sum of the individual bond dipoles.
(b)
Interpretation:
Given uncharged molecule is to be identified as polar or nonpolar, using its electrostatic potential map. If the molecule is polar, the direction of its net molecular dipole moment it to be determined.
Concept introduction:
A polar bond is one in which the bond pair is unequally shared by the two atoms.
A partial positive charge is developed on the less electronegative atom while and an equal but negative partial charge is developed on the more electronegative atom.
Molecules that contain more than one polar bond may or may not have a net dipole moment. The dipole moment is a vector quantity. The net molecular dipole moment is the result of the vector addition of all the individual dipole moments. Depending on the symmetry of the molecule, the individual bond dipoles can partly or completely cancel or reinforce each other.
A bond dipole or a molecular dipole is represented by an arrow pointing from the atom or region with a partial positive charge toward an atom or region with a partial negative charge.
Electrostatic potential maps of molecules show the distribution of electron density in different parts of the molecule. The electron density is represented by different colors, ranging from blue to red. Blue color indicates a low electron density, an atom or region with a partial positive charge. Red color indicates high electron density, an atom or region with a partial negative charge.

Answer to Problem 2.40P
The electrostatic potential map shows that the molecule is nonpolar.
Explanation of Solution
The electrostatic potential map shows a molecule with a negative charge concentrated at the center, with positive charge distributed symmetrically around the center. This shows that the individual bond dipoles are all of equal magnitude, and they all point toward the center. The vector addition of these dipoles will be zero because of their symmetric distribution. Therefore, the molecule is nonpolar.
The net dipole moment of a molecule is the vector sum of the individual bond dipoles.
(c)
Interpretation:
The given uncharged molecule is to be identified as polar or nonpolar, using its electrostatic potential map. If the molecule is polar, the direction of its net molecular dipole moment it to be determined.
Concept introduction:
A polar bond is one in which the bond pair is unequally shared by the two atoms.
A partial positive charge is developed on the less electronegative atom while and an equal but negative partial charge is developed on the more electronegative atom.
Molecules that contain more than one polar bond may or may not have a net dipole moment. The dipole moment is a vector quantity. The net molecular dipole moment is the result of the vector addition of all the individual dipole moments. Depending on the symmetry of the molecule, the individual bond dipoles can partly or completely cancel or reinforce each other.
A bond dipole or a molecular dipole is represented by an arrow pointing from the atom or region with a partial positive charge toward an atom or region with a partial negative charge.
Electrostatic potential maps of molecules show the distribution of electron density in different parts of the molecule. The electron density is represented by different colors, ranging from blue to red. Blue color indicates a low electron density, an atom or region with a partial positive charge. Red color indicates high electron density, an atom or region with a partial negative charge.

Answer to Problem 2.40P
The electrostatic potential map shows that the molecule is polar.
The direction of the net molecular dipole is downward as shown below.
Explanation of Solution
The electrostatic potential map shows a molecule with an asymmetric charge distribution. The positive charge is concentrated on the atom at the top, while the negative charge is distributed on three atoms at the bottom. The individual bond dipoles will therefore not cancel completely. Therefore, the molecule is polar.
The direction of the molecular dipole will be downward, as shown below by the black arrow.
The net dipole moment of a molecule is the vector sum of the individual bond dipoles.
(d)
Interpretation:
The given uncharged molecule is to be identified as polar or nonpolar, using its electrostatic potential map. If the molecule is polar, the direction of its net molecular dipole moment it to be determined.
Concept introduction:
A polar bond is one in which the bond pair is unequally shared by the two atoms.
A partial positive charge is developed on the less electronegative atom while and an equal but negative partial charge is developed on the more electronegative atom.
Molecules that contain more than one polar bond may or may not have a net dipole moment. The dipole moment is a vector quantity. The net molecular dipole moment is the result of the vector addition of all the individual dipole moments. Depending on the symmetry of the molecule, the individual bond dipoles can partly or completely cancel or reinforce each other.
A bond dipole or a molecular dipole is represented by an arrow pointing from the atom or region with a partial positive charge toward an atom or region with a partial negative charge.
Electrostatic potential maps of molecules show the distribution of electron density in different parts of the molecule. The electron density is represented by different colors, ranging from blue to red. Blue color indicates a low electron density, an atom or region with a partial positive charge. Red color indicates high electron density, an atom or region with a partial negative charge.

Answer to Problem 2.40P
The electrostatic potential map shows that the molecule is polar.
The direction of the net molecular dipole is upward, as shown below.
Explanation of Solution
The electrostatic potential map shows a molecule with a negative charge distributed on two atoms at the top and the positive charge distributed on two atoms at the bottom. This shows that the individual bond dipoles both point approximately upward and slightly away from the center line. The vector addition of these dipoles will be nonzero. Therefore, the molecule is polar.
The direction of the net dipole moment will be upward as shown below.
The net dipole moment of a molecule is the vector sum of the individual bond dipoles.
(e)
Interpretation:
The given uncharged molecule is to be identified as polar or nonpolar, using its electrostatic potential map. If the molecule is polar, the direction of its net molecular dipole moment it to be determined.
Concept introduction:
A polar bond is one in which the bond pair is unequally shared by the two atoms.
A partial positive charge is developed on the less electronegative atom while and an equal but negative partial charge is developed on the more electronegative atom.
Molecules that contain more than one polar bond may or may not have a net dipole moment. The dipole moment is a vector quantity. The net molecular dipole moment is the result of the vector addition of all the individual dipole moments. Depending on the symmetry of the molecule, the individual bond dipoles can partly or completely cancel or reinforce each other.
A bond dipole or a molecular dipole is represented by an arrow pointing from the atom or region with a partial positive charge toward an atom or region with a partial negative charge.
Electrostatic potential maps of molecules show the distribution of electron density in different parts of the molecule. The electron density is represented by different colors, ranging from blue to red. Blue color indicates a low electron density, an atom or region with a partial positive charge. Red color indicates high electron density, an atom or region with a partial negative charge.

Answer to Problem 2.40P
The electrostatic potential map shows that the molecule is polar.
The direction of the net molecular dipole is upward as shown below.
Explanation of Solution
The electrostatic potential map shows a molecule with a negative charge concentrated on the atom at the top center, with positive charge distributed over atoms on the side and at the bottom. This shows that the individual bond dipoles are not symmetrically distributed and will not cancel out completely. Therefore, the molecule is polar.
The direction of the net molecular dipole will be upward because of the concentration of negative charge at the top and a symmetrical distribution of the positive charge in the rest of the molecule.
The net dipole moment of a molecule is the vector sum of the individual bond dipoles.
(f)
Interpretation:
The given uncharged molecule is to be identified as polar or nonpolar, using its electrostatic potential map. If the molecule is polar, the direction of its net molecular dipole moment it to be determined.
Concept introduction:
A polar bond is one in which the bond pair is unequally shared by the two atoms.
A partial positive charge is developed on the less electronegative atom while and an equal but negative partial charge is developed on the more electronegative atom.
Molecules that contain more than one polar bond may or may not have a net dipole moment. The dipole moment is a vector quantity. The net molecular dipole moment is the result of the vector addition of all the individual dipole moments. Depending on the symmetry of the molecule, the individual bond dipoles can partly or completely cancel or reinforce each other.
A bond dipole or a molecular dipole is represented by an arrow pointing from the atom or region with a partial positive charge toward an atom or region with a partial negative charge.
Electrostatic potential maps of molecules show the distribution of electron density in different parts of the molecule. The electron density is represented by different colors, ranging from blue to red. Blue color indicates a low electron density, an atom or region with a partial positive charge. Red color indicates high electron density, an atom or region with a partial negative charge.

Answer to Problem 2.40P
The electrostatic potential map shows that the molecule is nonpolar.
Explanation of Solution
The electrostatic potential map shows a charge distribution that is symmetric about the center of the molecule with two negative regions opposite each other across the center as well as two positive regions across the center. The individual bond dipoles will therefore cancel out completely. Therefore, the net dipole moment will be zero, and the molecule will be nonpolar.
The net dipole moment of a molecule is the vector sum of the individual bond dipoles.
Want to see more full solutions like this?
Chapter 2 Solutions
Organic Chemistry: Principles and Mechanisms (Second Edition)
- For each reaction below, decide if the first stable organic product that forms in solution will create a new CC bond, and check the appropriate box. Next, for each reaction to which you answered "Yes" to in the table, draw this product in the drawing area below. Note for advanced students: for this problem, don't worry if you think this product will continue to react under the current conditions - just focus on the first stable product you expect to form in solution. དྲ。 ✗MgBr ? O CI Will the first product that forms in this reaction create a new C-C bond? Yes No • ? Will the first product that forms in this reaction create a new CC bond? Yes No × : ☐ Xarrow_forwardPredict the major products of this organic reaction: OH NaBH4 H ? CH3OH Note: be sure you use dash and wedge bonds when necessary, for example to distinguish between major products with different stereochemistry. Click and drag to start drawing a structure. ☐ : Sarrow_forwardPredict the major products of this organic reaction: 1. LIAIHA 2. H₂O ? Note: be sure you use dash and wedge bonds when necessary, for example to distinguish between major products with different stereochemistry. Click and drag to start drawing a structure. X : ☐arrow_forward
- For each reaction below, decide if the first stable organic product that forms in solution will create a new C - C bond, and check the appropriate box. Next, for each reaction to which you answered "Yes" to in the table, draw this product in the drawing area below. Note for advanced students: for this problem, don't worry if you think this product will continue to react under the current conditions - just focus on the first stable product you expect to form in solution. NH2 tu ? ? OH Will the first product that forms in this reaction create a new CC bond? Yes No Will the first product that forms in this reaction create a new CC bond? Yes No C $ ©arrow_forwardAs the lead product manager at OrganometALEKS Industries, you are trying to decide if the following reaction will make a molecule with a new C-C bond as its major product: 1. MgCl ? 2. H₂O* If this reaction will work, draw the major organic product or products you would expect in the drawing area below. If there's more than one major product, you can draw them in any arrangement you like. Be sure you use wedge and dash bonds if necessary, for example to distinguish between major products with different stereochemistry. If the major products of this reaction won't have a new CC bond, just check the box under the drawing area and leave it blank. Click and drag to start drawing a structure. This reaction will not make a product with a new CC bond. G marrow_forwardIncluding activity coefficients, find [Hg22+] in saturated Hg2Br2 in 0.00100 M NH4 Ksp Hg2Br2 = 5.6×10-23.arrow_forward
- give example for the following(by equation) a. Converting a water insoluble compound to a soluble one. b. Diazotization reaction form diazonium salt c. coupling reaction of a diazonium salt d. indacator properties of MO e. Diazotization ( diazonium salt of bromobenzene)arrow_forward2-Propanone and ethyllithium are mixed and subsequently acid hydrolyzed. Draw and name the structures of the products.arrow_forward(Methanesulfinyl)methane is reacted with NaH, and then with acetophenone. Draw and name the structures of the products.arrow_forward
- 3-Oxo-butanenitrile and (E)-2-butenal are mixed with sodium ethoxide in ethanol. Draw and name the structures of the products.arrow_forwardWhat is the reason of the following(use equations if possible) a.) In MO preperation through diazotization: Addition of sodium nitrite in acidfied solution in order to form diazonium salt b.) in MO experiment: addition of sodium hydroxide solution in the last step to isolate the product MO. What is the color of MO at low pH c.) In MO experiment: addition of sodium hydroxide solution in the last step to isolate the product MO. What is the color of MO at pH 4.5 d.) Avoiding not cooling down the reaction mixture when preparing the diazonium salt e.) Cbvcarrow_forwardA 0.552-g sample of an unknown acid was dissolved in water to a total volume of 20.0 mL. This sample was titrated with 0.1103 M KOH. The equivalence point occurred at 29.42 mL base added. The pH of the solution at 10.0 mL base added was 3.72. Determine the molar mass of the acid. Determine the Ka of the acid.arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning
