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 5.4, Problem 5.10E
Use the projection operator method to derive normalized SALCs that define the group orbitals for
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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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- The B2 molecule is paramagnetic; show how this indicates that the energy ordering of the orbitals in this molecule is given by Figure 6.18a rather than 6.18b.arrow_forwardConsidering only the molecular orbitals formed by combinations of the 2s atomic orbitals, how many molecular orbitals can be formed by 1000 Li atoms? In the lowest energy state, how many of these orbitals will be populated by pairs of electrons and how many will be empty?arrow_forwardThe photoelectron spectrum of HBr has two main groups of peaks. The first has ionization energy 11.88 eV. The next peak has ionization energy 15.2 eV, and it is followed by a long progression of peaks with higher ionization energies. Identify the molecular orbitals corresponding to these two groups of peaks.arrow_forward
- (A)Write the Hückel Hamiltonian matrix for benzene. (B) The pictures below represent a top view of the π molecular orbitals for benzene. They are labeled from A to F, in no order. Place the labels A, B, C, etc., in the boxes according to their energy. SHOW THE NODES. (B)arrow_forwardN2 and CN' are both isoelectronic. (i) Draw the molecular orbital diagram for N2 and CN molecules. (ii) Explain why CN is a toxic substance but N2 isn't. (iii) N2(g) is an inert gas that is suitable for a wide range of application. Would you expect N2" to be a stable diatomic species in the gaseous state? Explain your answer.arrow_forwardApply the projection operator method to derive the group orbital SALCs for BF3arrow_forward
- How do you write the Huckel determinant for the pi electrons of butadiene? How would you find the energies of the molecular orbitals?arrow_forward1. Derive the following expression for the bonding and antibonding orbitals of a heteronuclear diatomic molecule consisting of two electrons in a molecular orbital of the form y = CAA + CBB with atomic orbitals A and B. Let aa=HAA, aB=HBB, B=HAB=HBA, SAA-SBB=1, and, as a simplification, let SAB=SBA=S=0 (zero-overlap approximation). Note that the assumption of SAB=SBA=S=0 is used simply to get a more transparent expression. Show that the secular determinant is given by a,-E - E and energies are given by 1/2 2B E̟ = }(a, +a,)±(a,-a,) For B<0, E+ is the lower energy solution.arrow_forwardProvide a diagram which depicts the relative energies of the pi molecular orbitals of benzene. Show which molecular orbitals are filled in benzene's ground state.arrow_forward
- Consider a ring system made up of 8 atoms (each one contributing a p atomic orbital to make 8 pi molecular orbitals). If the system is filled with 6 orbitals containing single, electrons, there will 6 orbitals containing pairs of electrons and 1 unpaired electrons. Hint: Use a Frost Circle. Use numbers rather than text for your answers.arrow_forwardThe molecule PtCl 2 - is an important square planar starting material in synthetic inorganic chemistry. Using the p orbitals of Cl as the basis find the irreducible representations of the p orbitals and indicate which orbitals could possibly overlap with any of the orbitals on Pt . Assume that the pz orbitals on Cl are orientated in the same direction as the principle rotation axis, px orbitals are pointed at the Pt , and the py orbitals are orthogonal to the px orbitals. Show the characters of each orbital and identify which orbitals on Pt would match from a pure symmetry standpoint.arrow_forwardSet up and solve the Hückel secular equations for the π electrons of the triangular, planar CO32− ion. Express the energies in terms of the Coulomb integrals αO and αC and the resonance integral β. Estimate the delocalization energy of the ion.arrow_forward
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