Concept explainers
(a)
Interpretation:
The possible resonance structures for nitrate ion
Concept Introduction:
The steps to draw the Lewis structure of the molecule are as follows:
Step 1: Find the central atom and place the other atoms around it. The atom in a compound that has the lowest group number or lowest electronegativity considered as the central atom.
Step 2: Estimate the total number of valence electrons.
Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.
Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.
The formula to calculate formal charge of the atom is as follows:
Some molecules and ions do not have one unique Lewis structure. The Lewis structures that differ only in the placement of multiple bonds are called resonance structures.
Resonance structures are defined as a set of two or more Lewis structures that collectively describe the electronic bonding. The actual bonding is an average of the bonding in the resonance structures. Also, not all resonance structures contribute equally in every case. Resonance structures that have high formal charges or that place charges of the same sign on adjacent atoms do not contribute to the bonding.
(a)
Answer to Problem 9.66QE
Possible resonance structures are as follows:
Explanation of Solution
The skeleton structure is,
The resonance structures are as follows:
For structure I:
Substitute 5 for valence electrons, 0 for number of lone pairs of electrons and 8 for the number of shared electrons in equation (1) to calculate the formal charge on nitrogen atom.
Substitute 6 for valence electrons, 4 for number of lone pairs of electrons and 4 for the number of shared electrons in equation (1) to calculate the formal charge on first oxygen atom.
Substitute 6 for valence electrons, 6 for number of lone pairs of electrons and 2 for the number of shared electrons in equation (1) to calculate the formal charge on second oxygen atom.
Substitute 6 for valence electrons, 6 for number of lone pairs of electrons and 2 for the number of shared electrons in equation (1) to calculate the formal charge on third oxygen atom.
For structure II:
Substitute 5 for valence electrons, 0 for number of lone pairs of electrons and 8 for the number of shared electrons in equation (1) to calculate the formal charge on nitrogen atom.
Substitute 6 for valence electrons, 6 for number of lone pairs of electrons and 2 for the number of shared electrons in equation (1) to calculate the formal charge on first oxygen atom.
Substitute 6 for valence electrons, 4 for number of lone pairs of electrons and 4 for the number of shared electrons in equation (1) to calculate the formal charge on second oxygen atom.
Substitute 6 for valence electrons, 6 for number of lone pairs of electrons and 2 for the number of shared electrons in equation (1) to calculate the formal charge on third oxygen atom.
For structure III:
Substitute 5 for valence electrons, 0 for number of lone pairs of electrons and 8 for the number of shared electrons in equation (1) to calculate the formal charge on nitrogen atom.
Substitute 6 for valence electrons, 6 for lone pair of electrons and 2 for the number of shared electrons in equation (1) to calculate the formal charge on first oxygen atom.
Substitute 6 for valence electrons, 6 for number of lone pairs of electrons and 2 for the number of shared electrons in equation (1) to calculate the formal charge on second oxygen atom.
Substitute 6 for valence electrons, 4 for number of lone pair of electrons and 4 for the number of shared electrons in equation (1) to calculate the formal charge on third oxygen atom.
The possible resonance structures are as follows:
(b)
Interpretation:
The possible resonance structures for nitrous oxide
Concept Introduction:
Refer to part (a).
(b)
Answer to Problem 9.66QE
The possible resonance structures are,
Explanation of Solution
The given skeleton structure is,
The resonance structures are as follows:
For structure I:
Substitute 5 for valence electrons, 4 for the number of lone pairs of electrons and 4 for the number of shared electrons in equation (1) to calculate the formal charge on first
Substitute 5 for valence electrons, 0 for number of lone pairs of electrons and 8 for the number of shared electrons in equation (1) to calculate the formal charge on second nitrogen atom.
Substitute 6 for valence electrons, 4 for number of lone pairs of electrons and 4 for the number of shared electrons in equation (1) to calculate the formal charge on oxygen atom.
For structure II:
Substitute 5 for valence electrons, 2 for the number of lone pairs of electrons and 6 for the number of shared electrons in equation (1) to calculate the formal charge on first
Substitute 5 for valence electrons, 0 for number of lone pairs of electrons and 8 for the number of shared electrons in equation (1) to calculate the formal charge on second nitrogen atom.
Substitute 6 for valence electrons, 6 for number of lone pairs and 2 for the number of shared electrons in equation (1) to calculate the formal charge on third nitrogen atom.
For structure III:
Substitute 5 for valence electrons, 6 for the number of lone pairs of electrons and 2 for the number of shared electrons in equation (1) to calculate the formal charge on first
Substitute 5 for valence electrons, 0 for number of lone pairs of electrons and 8 for the number of shared electrons in equation (1) to calculate the formal charge on second nitrogen atom.
Substitute 6 for valence electrons, 2 for number of lone pairs of electrons and 6 for the number of shared electrons in equation (1) to calculate the formal charge on oxygen atom.
Possible resonance structures are as follows:
Want to see more full solutions like this?
Chapter 9 Solutions
Chemistry: Principles and Practice
- Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy of combustion of gaseous methane, CH4, to give water vapor and carbon dioxide gas.arrow_forwardPhosgene, a substance used in poisonous gas warfare during World War I, is so named because it was first prepared by the action of sunlight on a mixture of carbon monoxide and chlorine gases. Its name comes from the Greek words phos (light) and genes (born of). Phosgene has the following elemental composition: 12.14% C, 16.17% O, and 71.69% Cl by mass. Its molar mass is 98.9 g/mol. (d) Using average bond enthalpies, estimate H for the formation of gaseous phosgene from CO(g) and Cl2(g).arrow_forwardWe can define average bond enthalpies and bond lengthsfor ionic bonds, just like we have for covalent bonds. Whichionic bond is predicted to have the smaller bond enthalpy,Li—F or Cs—F?arrow_forward
- If a C-O bond length is 1.66 pm and a C=O bond length is 1.52 pm, how long would the carbon oxygen bonds in the carbonate ion be?arrow_forwardAcetyl chloride, CH₃C(O)Cl, is used as a reagent for the acylation of salicylic acid in the synthesis of aspirin. Draw the Lewis structure of CH₃C(O)Cl (with minimized formal charges) and then determine if the molecule is polar or nonpolar. +arrow_forwardThree resonance forms can be drawn for the molecule N2O. Which resonance form is likely to more closely resemble the structure of this molecule? (a) (b) (c)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_forwardSeveral Lewis structures can be written for perbromate ion, , the central Br with all single Br—O bonds, or with one, two, or three Br=O double bonds. Draw the Lewis structures of these possible resonance structures, and use formal charges to predict which makes the greatest contribution to the resonance hybrid.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: 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 & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningGeneral 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 Learning