Textbook Question
In ozone, O3, the two oxygen atoms on the ends of the molecule are equivalent to one another. (d) How many electrons are delocalized in the p system of ozone?
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Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 102c
Butadiene, C4H6, is a planar molecule that has the following carbon–carbon bond lengths:
(c) The middle C¬C bond length in butadiene (1.48 Å) is a little shorter than the average C¬C single bond length (1.54 Å). Does this imply that the middle C¬C bond in butadiene is weaker or stronger than the average C¬C single bond?
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Bond Length and Bond Strength
In general, shorter bond lengths indicate stronger bonds due to the increased overlap of atomic orbitals. Conversely, longer bonds tend to be weaker. This relationship is crucial for understanding how bond length can provide insights into the strength of a bond.
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00:36
Average Bond Order
Resonance in Molecules
Butadiene exhibits resonance, where the actual structure is a hybrid of multiple contributing structures. This delocalization of electrons can lead to bond lengths that differ from typical single or double bonds, affecting their strength and stability.
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01:42Resonance Structures
Comparison of Bond Types
C–C single bonds and double bonds have distinct characteristics. A single bond is generally longer and weaker than a double bond. Understanding these differences helps in analyzing the bond lengths in butadiene and determining the relative strength of the middle C–C bond.
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02:15Bonding Types
Related Practice
Textbook Question
Butadiene, C4H6, is a planar molecule that has the following carbon–carbon bond lengths:
(a) Predict the bond angles around each of the carbon atoms and sketch the molecule.
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Textbook Question
Butadiene, C4H6, is a planar molecule that has the following carbon–carbon bond lengths:
(b) From left to right, what is the hybridization of each carbon atom in butadiene?
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Textbook Question
The structure of borazine, B3N3H6, is a six-membered ring of alternating B and N atoms. There is one H atom bonded to each B and to each N atom. The molecule is planar. (a) Write a Lewis structure for borazine in which the formal charge on every atom is zero.
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Textbook Question
The structure of borazine, B3N3H6, is a six-membered ring of alternating B and N atoms. There is one H atom bonded to each B and to each N atom. The molecule is planar. (e) What are the hybridizations at the B and N atoms in the Lewis structures from parts (a) and (b)? Would you expect the molecule to be planar for both Lewis structures? Would you expect the molecule to be planar for both Lewis structures?
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Textbook Question
The highest occupied molecular orbital of a molecule is abbreviated as the HOMO. The lowest unoccupied molecular orbital in a molecule is called the LUMO. Experimentally, one can measure the difference in energy between the HOMO and LUMO by taking the electronic absorption (UV-visible) spectrum of the molecule. Peaks in the electronic absorption spectrum can be labeled as p2p9p2p*, s2s9s2s*, and so on, corresponding to electrons being promoted from one orbital to another. The HOMO-LUMO transition corresponds to molecules going from their ground state to their first excited state. (c) The electronic absorption spectrum of the N2 molecule has the lowest energy peak at 170 nm. To what orbital transition does this correspond?
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