Inorganic Chemistry
5th Edition
ISBN: 9780321811059
Author: Gary L. Miessler, Paul J. Fischer, Donald A. Tarr
Publisher: Prentice Hall
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Chapter 5, Problem 5.16P
In the gas phase,
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the three stable oxides of carbon monoxide (CO), Carbon dioxide(CO2), and carbon suboxide (C3O2). for each oxide draw the Lewis structure, predict the molecular structure, and described the bonding in terms of the hybrid orbitals for carbon atoms.
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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- Give the Lewis structure, molecular structure, and hybridization of the oxygen atom for OF2. Would you expect OF2 to be a strong oxidizing agent like O2F2 discussed in Exercise 61?arrow_forwardSketch the resonance structures for the N2O molecule. Is the hybridization of the N atoms the same or different in each structure? Describe the orbitals involved in bond formation by the central N atom.arrow_forwardWhat is the state of hybridization of boron and oxygen atoms in boric acid?arrow_forward
- What is the hybridization of the central atom in the Lewis structure for XeF2?arrow_forwardDraw the Lewis structures and molecular orbital diagrams for CO and NO. What are their bond orders? Are they similar to their Lewis structures? Explain.arrow_forwardWhat is the difference of the concepts of the Valence Bond theory and the Molecular orbital theory in terms of the formation of covalent bond?arrow_forward
- Write down the electronic structure of NO and give its bond order on the basis of molecular orbital theory. If NO undergoes a simple redox reaction and the NO bond strength is now stronger in its derivative, predict the identity of the derivative and give its electronic structure.arrow_forwardIn the gas phase, BeF2 forms linear monomeric molecules. Prepare a molecular orbital energy level diagram for BeF2, showing clearly which atomic orbitals are involved in bonding and which are nonbonding.arrow_forward(a) What are the C— C— C bond angles in diamond?(b) What are they in graphite (in one sheet)? (c) Whatatomic orbitals are involved in the stacking of graphitesheets with each other? The solid wedges in the figure indicate bonds from carbonthat come out of the plane of the page; the dashed wedgesindicate bonds that lie behind the plane of the page.(a) What is the hybridization of orbitals at each carbonatom? What angles do you expect between the bonds?(b) Now imagine that the polymer is polypropylenerather than polyethylene. Draw structures for polypropylenein which (i) the CH3 groups all lie on thesame side of the plane of the paper (this form is calledisotactic polypropylene), (ii) the CH3 groups lie on alternatingsides of the plane (syndiotactic polypropylene),or (iii) the CH3 groups are randomly distributedon either side (atactic polypropylene). Which of theseforms would you expect to have the highest crystallinityand melting point, and which the lowest? Explainin terms of…arrow_forward
- (a) The nitric oxide molecule, NO, readily loses one electronto form the NO+ ion. Which of the following is the best explanationof why this happens: (i) Oxygen is more electronegativethan nitrogen, (ii) The highest energy electron inNO lies in a p2*p molecular orbital, or (iii) The p2*p MO in NOis completely filled. (b) Predict the order of the N¬O bondstrengths in NO, NO+, and NO-, and describe the magneticproperties of each. (c) With what neutral homonuclear diatomicmolecules are the NO+ and NO- ions isoelectronic(same number of electrons)?arrow_forwardWhat is the molecular geometry of the PF4^+ (15P & 9F). Explain your answer brieflyarrow_forwardWhen considering the Lewis structure for HF, we might mistakenly conclude that HF contains three lone pairs on the F atom which are degenerate. Explain the nature of these three electron pairs by referring to the molecular orbital energy level diagram.arrow_forward
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