Discuss the nature of the bonding in the nitrate ion (NO5). Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central N atom, and the geometry of the ion. Show how the use of resonance structures can be avoided by introducing a de-localized 7 MO. What bond order is predicted by the MO model for the N-O bonds in the nitrate ion?

Discuss the nature of the bonding in the nitrate ion (NO5). Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central N atom, and the geometry of the ion. Show how the use of resonance structures can be avoided by introducing a de-localized 7 MO. What bond order is predicted by the MO model for the N-O bonds in the nitrate ion?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter4: Molecular Structure And Orbitals

Section: Chapter Questions

Problem 80E: Describe the bonding in NO+, NO, and NO, using both the localized electron and molecular orbital...

See similar textbooks

Similar questions

Thallium forms the compound TlI₃. What is the apparentoxidation state of Tl in this compound? Given that the anion is I₃⁻, what is the actual oxidation state of Tl? Draw the shape ofthe anion, giving its VSEPR class and bond angles. Propose areason why the compound does not exist as (Tl³⁺)(I⁻)₃.
Draw the MO diagram for Trihydridoboron. Which orbital on boron is completely nonbonding? Explain why. Using character tables and their corresponding orbital shapes, draw the H3 group orbitals and how they bond/nonbond to boron.
Explain why SO2 is used as a reducing agent but SO3 is not
Using Wade's rules, derive the structure of a hypothetical heteroborane with the molecular formula B3Si2GaH5MeEt2. What kind of borane is this? What is the 3D geometry.
. For each of the following, draw the Lewis structure, predict the ONO bond angle, and give the hybridization of the nitrogen. You may wish to review the chapters on chemical bonding and advanced theories of covalent bonding for relevant examples. (a) NO2 (b) NO-2
List the individual steps used in constructing a Born–Habercycle for the formation of BaI2 from the elements. Which ofthe steps would you expect to be exothermic?
1.What are the molybdenum oxidation states , ground d-electron configurations and ground electronic spectroscopic states of Mo(CO)6 and Mo(OCH3)6 ? 2.Describe how the Mo-C π bonding in Mo(CO)6 is enhanced by the synergism with the Mo-CO sigma bonding interaction .
Platinum hexafluoride is an extremely strong oxidizing agent. It can even oxidize oxygen, its reaction with O2 giving O2+PtFt6. Sketch the molecular orbital energy level diagram for the O2+ ion. How many net and bonds does the ion have? What is the oxygen-oxygen bond order? How has the bond order changed on taking away electrons from O2 to obtain O2+? Is the O2+ ion paramagnetic?
Compare the nature of the bonds in PbCl2 to that of the bonds in PbCl4.
draw the structure of of Fe2(SO4)3.
1.What are the dominant energy terms that are responsible for cesium fluoride occurring as an ionic solid and hydrogen fluoride occurring as a diatomic gas at standard conditions? 2.Explain why the energy separation between the t2g and eg d molecular orbitals in Mo(OCH3)6 is smaller than the value for Mo(CO)6 even though the average Mo-OCH3 bond dissociation enthalpy is more than twice the M-CO
What is the charge (oxidation state) of the cation in Hg2O?