Calculate the Bond order.On a sheet of paper draw the MO diagram for S,Is it diamagnetic or paramagnetic. Use the O2 energy level.must show all your workWith 2s - 2p mixingWithout 2s - 2p mixing2P2p2p2p2p2p'2S! 2s2s2s2sO2s2sAOAOAOAOB MO energy levels for B2, C2, and N2A MO energy levels for 02, F2, and Ne2Energy

Given: The species given is S22+.

On a sheet of paper draw the MO diagram for S,+ Is it diamagnetic or paramagnetic. Use the O2 energy level. Calculate the Bond order. must show all your work Without 2s - 2p mixing With 2s - 2p mixing 62P 2p 2p 2p 2p 2s 2s 2s 2s 62s AO AO AO MO AO A MO energy levels for 02, F2, and Ne2 B MO energy levels for B2, C2, and N2 Energy

On a sheet of paper draw the MO diagram for S,+ Is it diamagnetic or paramagnetic. Use the O2 energy level. Calculate the Bond order. must show all your work Without 2s - 2p mixing With 2s - 2p mixing 62P 2p 2p 2p 2p 2s 2s 2s 2s 62s AO AO AO MO AO A MO energy levels for 02, F2, and Ne2 B MO energy levels for B2, C2, and N2 Energy

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter6: Quantum Mechanics And Molecular Structure

Section: Chapter Questions

Problem 61P: Discuss the nature of the bonding in the nitrite ion (NO2) . Draw the possible Lewis resonance...

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Similar questions

Predict whether the MO diagram S2 would show s-p mixing or not.
The bond dissociation energies for the species NO, CF , and CF+ are ordered as CF+NOCF . Use MO theory to explain this ordering.
Formulate the MO structure of (NO2+) for localized bonds and de-localized bonds. Is it linear or nonlinear? Do you expect it to be paramagnetic? Repeat the analysis for NO2 and for NO2 .
Explain the difference between the and MOs for homonuclear diatomic molecules. How are bonding and antibonding orbitals different? Why are there two MOs and one MO? Why are the MOs degenerate?
Discuss the nature of the bonding in the nitrite ion (NO2) . Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central nitrogen atom, and the geometry of the ion. Show how the use of resonance structures can be avoided by introducing a de-localized MO. What bond order does the MO model predict for the NO bonds in the nitrite ion?
Use MO theory to predict the bond order and the number of unpaired electrons in the super-oxide ion, , and the peroxide ion, .
a.) Sketch for yourself the MO diagram for the following three heteronuclear diatomic species. Give the bond order of: CO, NO, CN^- b.) Sketch for yourself the molecular orbital energy level diagram for KrF and deduce its ground state electron configurations. Is KrF likely to have a shorter or longer or same bond length as KrF+?
The orbital potential energies for the 4s and 4p of Br are -18.65 ev and -12.49 ev, respectively. Recall that the H 1s is -13.61 ev. The MO diagrams for HBr is not exactly the same as HF. Draw the MO diagram for HBr, including energy levels, each orbitals shape, each orbitals character (meaning what atomic orbitals contribute to each M.O. and how much), symmetry labels indicate the HOMO and LUMO, the bond order (show your work), whether the molecule is paramagnetic or diamagnetic. Compare and contrast the MO diagrams of HF and HBr.
Use the MO model to determine which of the following has the smallestionization energy: N2, O2, N22-, N2-, O2+. Explain your answer. Please provide me a very details answer. Thank You ~
Using a group theoretical approach, generate the MO diagrams for silane, SiH4. Be sure that your diagram is fully-labeled with MO assignments, is properly scaled in energy space, and provide a sketch of the MO. Determine the bond order for the silane molecule, and for the Si-H bond.
Antibonding MOs always have at least one node. Can abonding MO have a node? If so, draw an example.
a.) Give the bond order of Li2 ,Be2 ,C2 b.) Give the ground state electron configurations ofCO,NO ,CN- .The gerade and ungerade designation is technically not appropriate for heteronuclear diatomics, but rather use the "*" after S or P to represent antibonding. Still, S would stand for σ. Let P represent a pair of π MO's. Enclose each MO in parenthesis followed by the number of electrons in that MO, e.g., the entry (1S*)2 would represent 1σ* 2.