None The molecular orbitals of the dinitrogen molecule (N2) are shown in order of increasing energy. The asterisked MOs arepresented by Macmillan Learningantibonding, while the others are bonding.a. Fill in the MOS with the available electrons. Note: Only the 2s and 2p σ and л orbitals are shown.2po2pл*2pm2pл2ρπEnergy2poAnswer Bank2so1.2so

Answered: The molecular orbitals of the…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.87QE

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The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) CN (b) CO (c) BeB (d) BC+ Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
Write the molecular orbital configuration of the diatomic molecule BN. What is the bond order of BN? Is the substance diamagnetic or paramagnetic? Use the order of energies that was given for homonuelcar diatomic molecules.
Compare and contrast the MO model with the local electron model. When is each useful?
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?
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) LiBe+ (b) CO+ (c) CN (d) OF Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
Predict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. (a) Na,2+ (b) Mg,2 (c) AI,2 (d) Si,2 (e) p2+ (f) s,2 (g) F,2 (h) Ar,2 40. Predict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. (a) Na22+ (b) Mg22+ (c) Al22+ (d) Si22+ (e) P22+ (f) S22+ (g) F22+ (h) Ar22+
The molecular orbital diagram of NO shown in Figure 10.47 also applies to OF. Draw the complete molecular orbital diagram for OF. What is the OF bond order? Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
Explain why an electron in the bonding molecular orbital in the H2 molecule has a lower energy than an electron in the 1s atomic orbital of either of the separated hydrogen atoms.
For each of the electron configurations in Problem 22, determine whether the molecule or molecular ion is paramagnetic or diamagnetic.
Determine the bond order of each member of the following groups, and determine which member of each group is predicted by the molecular orbital model to have the strongest bond. (a) H2,H2+,H2 (b) O2,O22+,O22 (c) Li2,Be2+,Be2 (d) F2,F2+,F2 (e) N2,N2+,N2
Which of the period 2 homonuclear diatomic molecules are predicted to be paramagnetic?
You hear a student from a nearby group say that “Electron domains repel one another.” Citeevidence from Figure 1.2 to support or refute this statement.

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