Concept explainers
Draw all of the resonance structures for the following species and show formal charges: (a) HCO, (b) CH2NO. The relative positions of the atoms are as follows:
(a)
Interpretation: The resonance structure of
Concept Introduction: Sometimes the chemical bonding of a molecule cannot be represented using a single Lewis structure. In these cases, the chemical bonding are described by delocalization of electrons and is known as resonance.
In some molecules, there is possibility of more than one Lewis structure where all the structures are equally acceptable. One of the acceptable Lewis structures of these molecules is called resonance structure.
All the possible resonance structures are imaginary whereas the resonance hybrid is real.
Any of the possible structure does not exist as such like a stable real molecule. So it is not possible to isolate one resonance structure.
These structures will differ only in the arrangement of the electrons not in the relative position of the atomic nuclei.
Structure with greater number of covalent bonds are more stable comparing to that with lower number of covalent bonds.
Structure which does not involve charge separation is more stable when comparing with structure having positive and negative charge separation.
While drawing resonance structure of a molecule some rules should be followed where the position, over whole charge and chemical framework remains intact. Also only π and nonbonding electron has been moved in all the three resonance structures
Formal charge:
A formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.
This method is used to identify the most probable Lewis structures if more than one possibility exists for a compound.
The Lewis structure with formal charge on each of the atoms close to zero is taken as the most plausible structure.
Formal charge of an atom can be determined by the given formula.
Answer to Problem 6.35QP
Resonance structure:
Formal charges:
Explanation of Solution
Determine the resonance structure for
In the case of chlorate ion, the chemical bonding of a molecule cannot be represented using a single Lewis structure. The chemical bonding are described by delocalization of electrons forming 2 possible resonance structures. Both the resonance structures are similar. In all the 2 resonance structures the position, over whole charge and chemical framework remains intact.
Structure of the chlorate ion chlorate ion is given below.
The formal charge of the given compound is calculated,
- Hydrogen atom
Substituting these values to the equation,
- Carbon atom
Substituting these values to the equation,
- First oxygen atom having double bond with carbon
Substituting these values to the equation,
- Oxygen atom which having single bond with carbon
Substituting these values to the equation,
(b)
Interpretation: The resonance structure of
Concept Introduction: Sometimes the chemical bonding of a molecule cannot be represented using a single Lewis structure. In these cases, the chemical bonding are described by delocalization of electrons and is known as resonance.
In some molecules, there is possibility of more than one Lewis structure where all the structures are equally acceptable. One of the acceptable Lewis structures of these molecules is called resonance structure.
All the possible resonance structures are imaginary whereas the resonance hybrid is real.
Any of the possible structure does not exist as such like a stable real molecule. So it is not possible to isolate one resonance structure.
These structures will differ only in the arrangement of the electrons not in the relative position of the atomic nuclei.
Structure with greater number of covalent bonds are more stable comparing to that with lower number of covalent bonds.
Structure which does not involve charge separation is more stable when comparing with structure having positive and negative charge separation.
While drawing resonance structure of a molecule some rules should be followed where the position, over whole charge and chemical framework remains intact. Also only π and nonbonding electron has been moved in all the three resonance structures
Formal charge:
A formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.
This method is used to identify the most probable Lewis structures if more than one possibility exists for a compound.
The Lewis structure with formal charge on each of the atoms close to zero is taken as the most plausible structure.
Formal charge of an atom can be determined by the given formula.
Answer to Problem 6.35QP
Resonance structure:
Formal charges:
Explanation of Solution
Resonance structure of
In the case of chlorate ion, the chemical bonding of a molecule cannot be represented using a single Lewis structure. The chemical bonding are described by delocalization of electrons forming 2 possible resonance structures. Both the resonance structures are similar. In all the 2 resonance structures the position, over whole charge and chemical framework remains intact.
Structure of the chlorate ion chlorate ion is given below.
The formal charge of the given compound is calculated,
- First hydrogen atom
Substituting these values to the equation,
- Second hydrogen atom
Substituting these values to the equation,
- Carbon atom
Substituting these values to the equation,
- Nitrogen atom
Substituting these values to the equation,
- First oxygen atom having double bond with nitrogen
Substituting these values to the equation,
- Oxygen atom which having single bond with nitrogen
Substituting these values to the equation,
Want to see more full solutions like this?
Chapter 6 Solutions
CHEMISTRY: ATOMS FIRST ALEKS CODE
- Write the correct Lewis structure and assign a formal charge to each atom in fulminate ion, CNO.arrow_forwardWrite the Lewis structures for the following species, and indicate whether each is an odd-electron species, an electron-deficient species, or an expanded valence shell species. (a) BI3 (b) IF5 (c) HN2arrow_forwardDraw resonance structures for each of these ions: NSO− and SNO−. (The atoms are bonded in the order given in each case, that is, S is the central atom in NSO−.) Use formal charges to determine which ion is likely to be more stable. Explain why the two ions cannot be considered resonance structures of each other.arrow_forward
- Draw resonance formulas of the phosphoric acid molecule, (HO)3PO. Obtain formal charges for the atoms in these resonance formulas. From this result, which resonance formula would you expect to most closely approximate the actual electron distribution?arrow_forwardTwo Lewis structures can be written for nitrosyl fluoride, which contains one nitrogen, one oxygen, and one fluorine atom per molecule. Write the two Lewis structures land assign a formal charge to each atom.arrow_forwardThree known isomers exist of N2CO, with the atoms in these sequences: NOCN; ONNC; and ONCN. Write resonance structures for each isomer and use formal charge to predict which isomer is the most stable.arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning