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Ch.9 - Molecular Geometry and Bonding Theories
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All textbooksBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblem 102c

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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Hey everyone, we're told that the Lewis structure below shows the carbonate ion with its carbon oxygen bond lengths. All of the carbon oxygen bonds in the carbonate ion are equal in length and a little longer than the usual 123 PICO meters for a carbon oxygen double bond were asked does this mean that the carbon oxygen double bonds in the carbonate ion are weaker than the usual carbon oxygen double bonds. Now we've learned that bond strength and bond length are inversely proportional to one another. So this means bond strength decreases with increasing bond length due to that inversely proportional relationship. Now, since the bonds are longer in the carbonate ion, they must be weaker and that is due to residence, which introduces a fraction of single bond character on each carbon oxygen bond in the carbonate ion. So our answer here is going to be yes. The bonds are weaker in the carbonate ion and this is going to be our final answer. So I hope that made sense. And let us know if you have any questions
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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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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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