5. Draw molecular orbital diagrams for superoxide (O2¯), and peroxide (O2²-). A good startingpoint would be MO diagram for O2 given in your textbook. Then: a) calculate bond orders insuperoxide and in peroxide; indicate which species would have a stronger oxygen-oxygen bond;b) indicate which species would be a radical.(4 points)

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Answered: 5. Draw molecular orbital diagrams for…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter4: Polar Bonds, Polar Reactions

Section: Chapter Questions

Problem 7CTQ

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1) Draw the Lewis structure and all 5 possible resonance structures of the cyclopentadiene anion, C5H5-. Label all non-zero formal charges. (Hint: as the name suggests, the five carbons are arranged in cyclic (pentagonal) structure. As shown below. (10 points)
Divalent carbon species called carbenes are capable of fleeting existence. For example, methylene, :CH2, is the simplest carbene. The two unshared electrons in methylene can be either paired in a single orbital or unpaired in different orbitals. a. Identify the type of hybridization you expect carbon to adopt in singlet (spin-paired) methylene and draw an illustration of its orbital showing the location of its electrons. (4 marks) b. Identify the type of hybridization you expect carbon to adopt in triplet (spin-unpaired) methylene and draw an illustration of its orbital showing the location of its electrons.
2- Arrange SO2, SO3, and SO3 in order of decreasing S–O bond distance. Rank from highest S-O bond distance to the lowest. To rank items as equivalent, overlap them. Reset Help SO3 SO2 SO,? highest bond distance lowest bond distance OThe correct ranking cannot be determined. Submit Request Answer
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Consider the following Lewis structure. Note, all valence electrons are shown. a. Assign formal charges to any atoms that that have a formal charge.b. Draw another Lewis structure that is a more important contributor to the actual structure than the one shown. c. Listed to the right are some typical C-N bond lengths. From the choices below, circle the best estimate for the carbon-nitrogen bond in the actual structure above. (a)1.46 A (b) 1.43 A (c) 1.26 A (d) 1.36 A (e) 1.12 A
3. A molecular form of "dicarbon", C2, can be generated in gas phase. Its bond dissociation energy has been determined at 599 kJ/mol. Use molecular orbital theory to explain why energy of dissociation for C₂+ is 513 kJ/mol, and that for C2² is 818 kJ/mol. (10 points)
8.9
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