Inorganic Chemistry
5th Edition
ISBN: 9780321811059
Author: Gary L. Miessler, Paul J. Fischer, Donald A. Tarr
Publisher: Prentice Hall
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Textbook Question
Chapter 5, Problem 5.10P
The hypofluorite ion,
a. Prepare a molecular orbital energy level diagram for this ion.
b. What is the bond order, and how many unpaired electrons are in this ion?
c. What is the most likely position for adding
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Students have asked these similar questions
a. Using the molecular orbital diagram, calculate the bond order of F2+. Show show your work or give a brief explanation of the process.
b. Do you expect this to have a shorter or longer bond length than F2? Explain your answer.
c. Do you expect F2+ to be paramagnetic or diamagnetic? Explain your answer.
Please label your answers a-c and place them on separate lines. Be as specific in your explanation as you can.
Draw the electron correlation diagram for O2.
a. Identify which combinations of atomic orbitals form each molecular orbital and state whether this is the result of constructive or destructive interference between the electronic wavefunctions.
b. Label the molecular orbitals based on their symmetry.
c. What is the bond order of O2? O2+? O2-?
d. List these three molecules in order of decreasing bond length.
e. List them in order of decreasing bond energy.
f. Which of these three molecules would be attracted to a magnetic field?
This question is related to valence bond theory.
a. Explain the assumptions made in bonding models under valence bond theory. What best describes
bonding under these models?
b. Draw the Lewis structure of SO2. Identify bonds in the moldule as either sigma or pi bonds.
Draw orbital diagrams for ground state S and O atoms. Use these orbital diagrams determine the
geometry of SO2 using valence bond theory (hint: SO2 must be descried using hybrid atomic orbitals. In
other words, which orbitals on which atoms overlap to give rise to which bonds?
C.
d. Explain why valence bond theory does not adequately describe the bonding in SO2, even though it
accurately predicts the geometry/bond angle.
Chapter 5 Solutions
Inorganic Chemistry
Ch. 5.1 - Repeat the process in the preceding example for...Ch. 5.2 - Prob. 5.2ECh. 5.3 - Use a similar approach to the discussion of HF to...Ch. 5.4 - Sketch the energy levels and the molecular...Ch. 5.4 - Using the D2h character table shown, verify that...Ch. 5.4 - Using orbital potential energies, show that group...Ch. 5.4 - Prob. 5.7ECh. 5.4 - Prob. 5.8ECh. 5.4 - Prob. 5.9ECh. 5.4 - Use the projection operator method to derive...
Ch. 5.4 - Determine the types of hybrid orbitals that are...Ch. 5.4 - Determine the reducible representation for all the...Ch. 5 - Expand the list of orbitais considered in Figures...Ch. 5 - On the basis of molecular orbitals, predict the...Ch. 5 - On the basis of molecular orbitals, predict the...Ch. 5 - Compare the bonding in O22,O2 and O2 Include Lewis...Ch. 5 - Although the peroxide ion, O22 and the acetylide...Ch. 5 - High-resolution photoelectron spectroscopy has...Ch. 5 - a. Prepare a molecular orbital energy-level...Ch. 5 - a. Prepare a molecular orbital energy-level...Ch. 5 - NF is a known molecule a. Construct a molecular...Ch. 5 - The hypofluorite ion, OF can be observed only with...Ch. 5 - Prob. 5.11PCh. 5 - Although KrF+ and XeF+ have been studied, KrBr+...Ch. 5 - Prepare a molecular orbital energy level diagram...Ch. 5 - Methylene, CH2 plays an important role in many...Ch. 5 - Beryllium hydride, BeH2 is linear in the gas...Ch. 5 - In the gas phase, BeF2 forms linear monomeric...Ch. 5 - For the compound XeF2 do the following: a. Sketch...Ch. 5 - TaH5 has been predicted to have C4v symmetry, with...Ch. 5 - Describe the bonding in ozone, o3 on the basis of...Ch. 5 - Describe the bonding in SO3 by using group theory...Ch. 5 - The ion H3+ has been observed, but its structure...Ch. 5 - Use molecular orbital arguments to explain the...Ch. 5 - Prob. 5.23PCh. 5 - Prob. 5.24PCh. 5 - The isomenc ions NSO (thiazate) and SNO...Ch. 5 - Apply the projection operator method to derive the...Ch. 5 - Apply the projection operator method to derive the...Ch. 5 - A set of four group orbitals derived from four 3s...Ch. 5 - The projection operator method has applications...Ch. 5 - Although the cl2+ ion has not been isolated, it...Ch. 5 - BF3 is often described as a molecule in which...Ch. 5 - SF4 has C2v symmetry. Predict the possible...Ch. 5 - Consider a square pyramidal AB5 molecule. Using...Ch. 5 - Prob. 5.34PCh. 5 - For the molecule PCl5 : a. Using the character...Ch. 5 - Molecular modeling software is typically capable...Ch. 5 - Prob. 5.39PCh. 5 - Calculate and display the orbitals for the linear...Ch. 5 - Prob. 5.41PCh. 5 - Prob. 5.42PCh. 5 - Prob. 5.43PCh. 5 - Diborane, B2H6 , has the structure shown. a. Using...
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