3. Sketch the molecular orbital diagrams for O2, O2 (superoxide, 1e reduction of O2) and02 (peroxide, 2e reduction of O2). Using these diagrams, provide the bond order foreach of the molecules and state if they are diamagnetic or paramagnetic

Bond order for O2, It has two unpaired electron so it is paramagnetic.

Answered: 3. Sketch the molecular orbital…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Covalent Bonding: Orbitals

Section: Chapter Questions

Problem 15Q: Why does the molecular orbital model do a better job in explaining the bonding in NO and NO than the...

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Similar questions

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?
(a) Construct a molecular orbital energy diagram of N₂. (b) Use this diagram to explain why the first ionization of N₂ is greater than that of N. (b) Use this diagram to predict which is more favorable: the first electron affinity of N₂ or that of N.
Boron trifluoride (BF3) has no dipole moment (u = 0 D). Explain how this observation confirms the geometry of BF3 predicted by VSEPR theory.
Write down the electronic structure of NO and give its bond order on the basis of molecular orbital theory. If NO undergoes a simple redox reaction and the NO bond strength is now stronger in its derivative, predict the identity of the derivative and give its electronic structure.
Classify O2 and N2 as either paramagnetic or diamagnetic. explain your answer by completing the orbitals in the MO energy level diagrams and referring to the electronic structure of these two molecules
Draw the molecular orbital diagrams for Ne(2), N(2) ^2- and Be(2). Are they stable or unstable?
2. Using molecular orbital theory, explain whether the following reaction proceeds thermally or photochemically. + ?
Draw and explain all the properties of CO and NO with the help of molecular orbital diagram
(a) Sketch the occupied MOs of the valence shell for the N2 molecule. Label the orbitals as o or ™ orbitals, and specify which are bonding and which are antibonding. (b) If one electron is removed from the highest occupied orbital of N2, will the equilibrium N-N distance become longer or shorter? Explain briefly.
Give the Lewis structure, molecular structure, and hybridization of the oxygen atom for OF2. Would you expect OF2 to be a strong oxidizing agent like O2F2 discussed in Exercise 61?
Why does the molecular orbital model do a better job in explaining the bonding in NO and NO than the hybrid orbital model?

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3. Sketch the molecular orbital diagrams for O2, O2 (superoxide, 1e reduction of O2) and 02 (peroxide, 2e reduction of O2). Using these diagrams, provide the bond order for each of the molecules and state if they are diamagnetic or paramagnetic