The three most stable oxides of carbon are carbon monoxide (CO), carbon dioxide (CO2), and carbon suboxide (C3O2). The space- filling models for these three compounds are For each oxide, draw the Lewis structure, predict the molecular structure, and describe the bonding (in terms of the hybrid orbitals for the carbon atoms).

The three most stable oxides of carbon are carbon monoxide (CO), carbon dioxide (CO2), and carbon suboxide (C3O2). The space- filling models for these three compounds are For each oxide, draw the Lewis structure, predict the molecular structure, and describe the bonding (in terms of the hybrid orbitals for the carbon atoms).

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter7: Covalent Bonding

Section: Chapter Questions

Problem 58QAP: Acrylonitrile, C3H3N is the building mer Orlon. Its Lewis structure is What is the hybridization of...

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What are the relationships among bond order, bond energy, and bond length? Which of these quantities can be measured?
What hybrid orbitals would be expected for the central atom in each of the following molecules or ions?
The percent ionic character of the bonds in several interhalogen Molecules (as estimated from their measured dipole moments and bond lengths) are ClF (11%), BrF(15%), BrCl (5.6%), ICl(5.8%), and IBr (10%). Estimate the percent ionic characters for each of these molecules, using the equation in Problem 37, and compare them with the given values.
Acrylonitrile, C3H3N is the building mer Orlon. Its Lewis structure is What is the hybridization of nitrogen and of the three numbered carbon atoms?
The 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.
Why do we hybtidize atomic orbitals to explain the bonding in covalent compounds? What type of bonds form from hybrid orbitals: sigma or pi? Explain.
The diatomic molecule OH exists in the gas phase. OH playsan important part in combustion reactions and is a reactiveoxidizing agent in polluted air. The bond length and bondenergy have been measured to be 97.06 pm and 424.7 kJ/mol,respectively. Assume that the OH molecule is analogous to theHF molecule discussed in the chapter and that the MOs resultfrom the overlap of a pz orbital from oxygen and the 1s orbitalof hydrogen (the OOH bond lies along the z axis).
The diagram that follows shows the highest-energy occupiedMOs of a neutral molecule CX, where element X is in thesame row of the periodic table as C. (a) Based on the numberof electrons, can you determine the identity of X? (b) Wouldthe molecule be diamagnetic or paramagnetic? (c) Considerthe p2p MOs of the molecule. Would you expect them to havea greater atomic orbital contribution from C, have a greateratomic orbital contribution from X, or be an equal mixtureof atomic orbitals from the two atoms?
Consider the molecule PF4Cl. (a) Draw a Lewis structure forthe molecule, and predict its electron-domain geometry.(b) Which would you expect to take up more space, a P¬Fbond or a P¬Cl bond? Explain. (c) Predict the molecular geometryof PF4Cl. How did your answer for part (b) influenceyour answer here in part (c)? (d) Would you expect the moleculeto distort from its ideal electron-domain geometry? Ifso, how would it distort?
The molecule 2-butene, C4H8, can undergo a geometricchange called cis-trans isomerization:As discussed in the “Chemistry and Life” box on the chemistryof vision, such transformations can be induced bylight and are the key to human vision. (a) What is the hybridizationat the two central carbon atoms of 2-butene?(b) The isomerization occurs by rotation about the centralC¬C bond. With reference to Figure 9.29, explainwhy the p bond between the two central carbon atoms isdestroyed halfway through the rotation from cis- to trans-2-butene. (c) Based on average bond enthalpies (Table 8.3),how much energy per molecule must be supplied to breakthe C¬C p bond? (d) What is the longest wavelength oflight that will provide photons of sufficient energy to breakthe C¬C p bond and cause the isomerization? (e) Is thewavelength in your answer to part (d) in the visible portionof the electromagnetic spectrum? Comment on the importanceof this result for human vision.
Ethyl acetate, C4H8O2, is a fragrant substance used both as asolvent and as an aroma enhancer. Its Lewis structure is (a) What is the hybridization at each of the carbon atomsof the molecule? (b) What is the total number of valenceelectrons in ethyl acetate? (c) How many of the valence electronsare used to make s bonds in the molecule? (d) Howmany valence electrons are used to make p bonds? (e) Howmany valence electrons remain in nonbonding pairs in themolecule?
(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)?