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 5.19P
Describe the bonding in ozone,
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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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- What are the relationships among bond order, bond energy, and bond length? Which of these quantities can be measured?arrow_forwardThe structure of amphetamine, a stimulant, is shown below. (Replacing one H atom on the NH2, or amino, group with CH3 gives methamphetamine a particularly dangerous drug commonly known as speed.) (a) What are the hybrid orbitals used by the C atoms of the C6 ring. by the C atoms of the side chain, and by the N atom? (b) Give approximate values for the bond angles A, B, and C. (c) How many bonds and bonds are in the molerule? (d) Is the molecule polar or nonpolar? (e) Amphetamine reacts readily with a proton (H+) in aqueous solution. Where does this proton attach to the molecule? Explain how the electrostatic potential map predicts this site of protonation.arrow_forwardThe 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.arrow_forward
- For each of the following molecules, write the Lewis structure(s), predict the molecular structure (including bond angles), give the expected hybrid orbitals of the central atom, and predict the overall polarity. a. CF4 b. NF3 c. OF2 d. BF3 e. BeH2 f. TeF4 g. AsF5 h. KrF2 i. KrF4 j. SeF6 k. IF5 l. IF3arrow_forwardIt is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?arrow_forwardIn 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.arrow_forward
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