Organic Chemistry: A Guided Inquiry
Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Chapter 3, Problem 7E

Explain what is wrong with each of the following statements.
a. “A π bond is a double bond.
b. “A π bond consists of four electrons, one in each of the four p orbitals involved in the π bond.
c. “A π bond is twice as strong as a σ bond because it consists of two orbital overlaps insteadof just one.”

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a. One of the two known binary compounds of xenon and oxygen is XeO3. A Lewis structure is shown here, which may or may not be complete. How many lone pairs should be present on the central Xe atom? b. What is the electron pair geometry around the Xe? c. What is the molecular geometry of XeO3? d. What hybrid orbitals does the Xe atom use?
For a homonuclear diatomic molecule, what type of molecular orbital does the illustration shown below represent? Note: the represents each nuclei. a bonding o orbital formed from two p atomic orbitals. a bonding o orbital formed from two s atomic orbitals. a bonding o orbital formed from one p and one s atomic orbital. a bonding n orbital formed from one s and one p atomic orbital. a bonding n orbital formed from two p atomic orbitals.
Which bonds allow for a large, bonded network to be more directional and why? 1. Sigma bonds 2. Pi bonds Because 1. The orbitals overlap side-to-side to hold the bond in place. 2. The orbitals overlap end-to-end in several different directions. 3. Multiple of these bonds result in delocalized electrons. ο ο ο ο ο ο O 2,1 O2,2 O 1,3 O 1,2 O2,3 O 1,1 lyr
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