Concept explainers
Interpretation: The preferred resonance form among the given ions is to be stated on the basis of formal charges.
Concept introduction: Formal charges play an important role in choosing between the possible molecular structures. The preferred structure is the one in which formal charges are zero.
To determine: The preferred resonance form among the given ions on the basis of formal charges.

Answer to Problem 8.92QP
Solution
The preferred resonance form in the
The preferred resonance form in the
The preferred resonance form in the
Explanation of Solution
Explanation
The given ion is
Therefore the total valence electrons are
The lone pair of electrons on oxygen and bonding electrons is delocalized which results in the formation of lewis structures. The lewis structures for
Figure 1
The formal charge on each atom of resonating structure (a) of
Formal charge is calculated as,
Number of valence electrons in nitrogen is
Number of lone pair electrons in nitrogen is
Number of bond pair electrons in nitrogen is
To calculate the formal charge on nitrogen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in oxygen is
Number of lone pair electrons in oxygen is
Number of bond pair electrons in oxygen is
To calculate the formal charge on oxygen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in carbon is
Number of lone pair electrons in carbon is
Number of bond pair electrons in carbon is
To calculate the formal charge on carbon, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
The formal charge on each atom of resonating structure (b) of
Number of valence electrons in nitrogen is
Number of lone pair electrons in nitrogen is
Number of bond pair electrons in nitrogen is
To calculate the formal charge on nitrogen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in oxygen is
Number of lone pair electrons in oxygen is
Number of bond pair electrons in oxygen is
To calculate the formal charge on oxygen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in carbon is
Number of lone pair electrons in carbon is
Number of bond pair electrons in carbon is
To calculate the formal charge on carbon, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
According to formal charge calculations, there is a formal charge of
The given ion is
Therefore the total valence electrons are
Since carbon is least electronegative, it will act as central atom. The lone pair of electrons on oxygen and bonding electrons is delocalized which results in the formation of lewis structures. The lewis structures for
Figure 2
The formal charge on each atom of resonating structure (a) of
Number of valence electrons in nitrogen is
Number of lone pair electrons in nitrogen is
Number of bond pair electrons in nitrogen is
To calculate the formal charge on nitrogen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in oxygen is
Number of lone pair electrons in oxygen is
Number of bond pair electrons in oxygen is
To calculate the formal charge on oxygen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in carbon is
Number of lone pair electrons in carbon is
Number of bond pair electrons in carbon is
To calculate the formal charge on carbon, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
The formal charge on each atom of resonating structure (b) of
Number of valence electrons in nitrogen is
Number of lone pair electrons in nitrogen is
Number of bond pair electrons in nitrogen is
To calculate the formal charge on nitrogen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in oxygen is
Number of lone pair electrons in oxygen is
Number of bond pair electrons in oxygen is
To calculate the formal charge on oxygen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in carbon is
Number of lone pair electrons in carbon is
Number of bond pair electrons in carbon is
To calculate the formal charge on carbon, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
The formal charge on each atom of resonating structure (c) of
Number of valence electrons in nitrogen is
Number of lone pair electrons in nitrogen is
Number of bond pair electrons in nitrogen is
To calculate the formal charge on nitrogen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in oxygen is
Number of lone pair electrons in oxygen is
Number of bond pair electrons in oxygen is
To calculate the formal charge on oxygen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in carbon is
Number of lone pair electrons in carbon is
Number of bond pair electrons in carbon is
To calculate the formal charge on carbon, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
According to formal charge calculations, there is a formal charge of
The given ion is
Figure 3
The formal charge on each atom of resonating structure (a) of
Number of valence electrons in nitrogen is
Number of lone pair electrons in nitrogen is
Number of bond pair electrons in nitrogen is
To calculate the formal charge on nitrogen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in oxygen is
Number of lone pair electrons in oxygen is
Number of bond pair electrons in oxygen is
To calculate the formal charge on oxygen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in carbon is
Number of lone pair electrons in carbon is
Number of bond pair electrons in carbon is
To calculate the formal charge on carbon, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
The formal charge on each atom of resonating structure (b) of
Number of valence electrons in nitrogen is
Number of lone pair electrons in nitrogen is
Number of bond pair electrons in nitrogen is
To calculate the formal charge on nitrogen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in oxygen is
Number of lone pair electrons in oxygen is
Number of bond pair electrons in oxygen is
To calculate the formal charge on oxygen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in carbon is
Number of lone pair electrons in carbon is
Number of bond pair electrons in carbon is
To calculate the formal charge on carbon, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
The formal charge on each atom of resonating structure (c) of
Number of valence electrons in nitrogen is
Number of lone pair electrons in nitrogen is
Number of bond pair electrons in nitrogen is
To calculate the formal charge on nitrogen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in oxygen is
Number of lone pair electrons in oxygen is
Number of bond pair electrons in oxygen is
To calculate the formal charge on oxygen, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
Number of valence electrons in carbon is
Number of lone pair electrons in carbon is
Number of bond pair electrons in carbon is
To calculate the formal charge on carbon, substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).
According to formal charge calculations, resonating structure (a) and (c) least electronegative atom carbon possess
Conclusion
The preferred resonance form in the
The preferred resonance form in the
The preferred resonance form in the
Want to see more full solutions like this?
Chapter 8 Solutions
EBK CHEMISTRY: THE SCIENCE IN CONTEXT,
- What are the missing reagents for the spots labeled 1 and 3? Please give a detailed explanation and include the drawings and show how the synthesis proceeds with the reagents.arrow_forwardhelp with the rf values i am so confusedarrow_forwardPredict the organic reactant of X and Y that are involved in the reaction below, and draw the skeletal ("line") structures of the missing organic reactant. Please include all steps & drawings & explanations.arrow_forward
- What are the missing reagents for the spots labeled 1 and 3? Please give a detailed explanation and include the drawings and show how the synthesis proceeds with the reagents.arrow_forwardPlease provide the complete mechanism for the reaction below and include all appropriate arrows, formal charges, and intermediates. Please draw out the answerarrow_forwardPredict the major organic product for this reaction.arrow_forward
- help me with the rf value i am so confusedarrow_forwardPredict the major organic product for this reaction.arrow_forward3) The following molecule, chloral is a common precursor to chloral hydrate, an acetal type molecule that was a first-generation anesthetic. Draw a mechanism that accounts for tis formation and speculate why it does not require the use of an acid catalyst, like most hemiacetal and acetal reaction: (10 pts) H H₂Oarrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples 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 EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY





