p)€Eiv)vi)€ON 3Given the molecule F, with seven valence electrons: 140 = 8Construct a completely labelled molecular orbital energy level diagram forFion.Write the electron configurationof sp, 64Identify bond orderState the HOMO and the LUMO.Give the magnetic property of F₂2 ion and briefly justify your answer.Compare the bond order, bond strength and bond length between F₂ andF₂²* ion.

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iii) iv) v) ) N 3 Given the molecule F with seven valence electrons: 1 v 40 = 8 Construct a completely labelled molecular orbital energy level diagram for F₂ ion. Write the electron configuration اء 64 6 sp Identify bond order. State the HOMO and the LUMO. Give the magnetic property of F₂2+ ion and briefly justify your answer. Compare the bond order, bond strength and bond length between F₂ and F₂²* ion.

iii) iv) v) ) N 3 Given the molecule F with seven valence electrons: 1 v 40 = 8 Construct a completely labelled molecular orbital energy level diagram for F₂ ion. Write the electron configuration اء 64 6 sp Identify bond order. State the HOMO and the LUMO. Give the magnetic property of F₂2+ ion and briefly justify your answer. Compare the bond order, bond strength and bond length between F₂ and F₂²* ion.

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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Similar questions

The diatomic molecule OH exists in the gas phase. The bond length and bond energy have been measured to be 97.06 pm and 424.7 kJ/mol, respectively. Assume that the OH molecule is analogous to the HF molecule discussed in the chapter and that molecular orbitals result from the overlap of a lowerenergy pz, orbital from oxygen with the higher-energy ls orbital of hydrogen (the OH bond lies along the z-axis). a. Which of the two molecular orbitals will have the greater hydrogen 1s character? b. Can the 2px orbital of oxygen form molecular orbitals with the 1s orbital of hydrogen? Explain. c. Knowing that only the 2p orbitals of oxygen will interact significantly with the 1s orbital of hydrogen, complete the molecular orbital energy-level diagram for OH. Place the correct number of electrons in the energy levels. d. Estimate the bond order for OH. e. Predict whether the bond order of OH+ will be greater than, less than, or the same as that of OH. Explain.
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.
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.
What are the relationships among bond order, bond energy, and bond length? Which of these quantities can be measured?
Compare Figs. 4-47 and 4-49. Why are they different? Because B2 is known to be paramagnetic, the 2p and 2p molecular orbitals must be switched from the first prediction. What is the rationale for this? Why might one expect the 2p to be lower in energy than the 2p? Why cant we use diatomic oxygen to help us decide whether the 2p, or 2p, is lower in energy?
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.
The cations O2+ and N2+ are formed when molecules of O2 and N2 are subjected to intense, high-energy solar radiation in Earths upper atmosphere. Write the electron configuration for O2+. Predict its bond order and magnetic behavior.
Compare and contrast the MO model with the local electron model. When is each useful?
Why do we hybtidize atomic orbitals to explain the bonding in covalent compounds? What type of bonds form from hybrid orbitals: sigma or pi? Explain.
Which of the period 2 homonuclear diatomic molecules are predicted to be paramagnetic?
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?