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Ch.9 - Molecular Geometry and Bonding Theories
Brown - Chemistry: The Central Science 15th Edition
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Tutti i libri di testoBrown 15th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblema 101a
Capitolo 9, Problema 101a

Butadiene, C4H6, is a planar molecule that has the following carbon–carbon bond lengths:
Structural formula of butadiene, C4H6, showing bond lengths of 1.34 Å and 1.48 Å.
(a) Predict the bond angles around each of the carbon atoms and sketch the molecule.

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Identify the hybridization of each carbon atom in the butadiene molecule. The carbons involved in double bonds (C1, C2, C3, and C4) are sp2 hybridized.
Determine the bond angles for sp2 hybridized carbons. The bond angles around an sp2 hybridized carbon are approximately 120 degrees.
Sketch the molecule, ensuring that the bond angles around each carbon are approximately 120 degrees. The structure should show the planar arrangement of the molecule.
Label the bond lengths on the sketch. The double bonds (C1=C2 and C3=C4) have bond lengths of 1.34 Å, and the single bond (C2-C3) has a bond length of 1.48 Å.
Review the sketch to ensure it accurately represents the planar structure of butadiene with the correct bond angles and bond lengths.

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Hybridization

Hybridization is the concept that describes the mixing of atomic orbitals to form new hybrid orbitals, which can explain the geometry of molecular bonding. In butadiene, the carbon atoms undergo sp2 hybridization, resulting in a trigonal planar arrangement around each carbon atom, which influences bond angles and lengths.
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00:51
Hybridization

Bond Angles

Bond angles are the angles formed between adjacent bonds at a central atom in a molecule. In butadiene, due to the sp2 hybridization of the carbon atoms, the expected bond angles around each carbon atom are approximately 120 degrees, reflecting the planar structure of the molecule.
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01:53
Bond Angles

Resonance Structures

Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In butadiene, the presence of alternating double bonds allows for resonance, which stabilizes the molecule and affects the bond lengths, as seen with the varying bond lengths of 1.34 Å and 1.48 Å.
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01:42
Resonance Structures
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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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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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