Complete the table below, which lists information about some diatomic molecules or molecular ions. In particular: . Decide whether each molecule is stable or not. • Decide whether each molecule would be diamagnetic or paramagnetic. . Calculate each molecule's bond order. molecule Li₂ 0, B 2 stable? yes O no yes no O yes no diamagnetic or paramagnetic? diamagnetic paramagnetic diamagnetic paramagnetic diamagnetic O paramagnetic OO bond order 0 0 П 00 X

Complete the table below, which lists information about some diatomic molecules or molecular ions. In particular: . Decide whether each molecule is stable or not. • Decide whether each molecule would be diamagnetic or paramagnetic. . Calculate each molecule's bond order. molecule Li₂ 0, B 2 stable? yes O no yes no O yes no diamagnetic or paramagnetic? diamagnetic paramagnetic diamagnetic paramagnetic diamagnetic O paramagnetic OO bond order 0 0 П 00 X

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 17P

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Similar questions

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.
In the molecular orbital mode l, compare and contrast bonds with bonds. What orbitals form the bonds and what orbitals form the bonds? Assume the z-axis is the internuclear axis.
For each of the electron configurations in Problem 21, determine whether the molecule or molecular ion is paramagnetic or diamagnetic.
For each of the electron configurations in Problem 22, determine whether the molecule or molecular ion is paramagnetic or diamagnetic.
Identify the hybrid orbitals used by antimony in SbCl5 and in SbCl6, the ion formed from the reaction of SbCl5 and Cl. Explain your choices.
What hybrid orbitals would be expected for the central atom in each of the following molecules or ions?
Use MO theory to predict the bond order and the number of unpaired electrons in the super-oxide ion, , and the peroxide ion, .
Which of the period 2 homonuclear diatomic molecules are predicted to be paramagnetic?
Strike-anywhere matches contain a layer of KClO3 and a layer of P4S3. The heat produced by the friction of striking the match causes these two compounds to react vigorously, which sets fire to the wooden stem of the match. KCIO3 contains the ClO3 ion. P4S3 is an unusual molecule with the skeletal structure. (a) Write Lewis structures for P4S3 and the ClO3 ion. (b) Describe the geometry about the P atoms, the S atom, and the Cl atom in these species. (c) Assign a hybridization to the P atoms, the S atom, and the Cl atom in these species. (d) Determine the oxidation states and formal charge of the atoms in P4S3 and the ClO3 ion.
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.
Based on the discussion so far, identify a characteristic that is common to all situations where electron-region geometry and molecular geometry are the same for a molecule or a polyatomic ion.
• describe chemical bonding using a model based on the overlap of atomic orbitals and recognize sonic of the limitations of this simple model.