Ch.9 - Molecular Geometry and Bonding Theories

Brown - Chemistry: The Central Science 15th Edition

Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970당신이 사용하는 게 아니라요?교과서 변경

Brown 15th Edition

Ch.9 - Molecular Geometry and Bonding Theories

문제 101c

9장, 문제 101c

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?

검증된 단계별 안내

Understand that bond length is inversely related to bond strength: shorter bonds are generally stronger.

Recognize that the middle C-C bond in butadiene is shorter (1.48 Å) than the average C-C single bond (1.54 Å).

Consider the concept of resonance in butadiene, which can lead to partial double bond character in the middle C-C bond.

Acknowledge that partial double bond character typically results in a bond that is shorter and stronger than a single bond.

Conclude that the middle C-C bond in butadiene is likely stronger than the average C-C single bond due to its shorter length and resonance effects.

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주요 개념

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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.

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.

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.

관련 실천

교과서 질문

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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교과서 질문

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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교과서 질문

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 π_2p-π_2p*, σ_s-σ_2s*, 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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교과서 질문

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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교과서 질문

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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교과서 질문

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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