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?
Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 102b
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?
Verified step by step guidance1
Identify the structure of butadiene, which is CH2=CH-CH=CH2.
Determine the hybridization of each carbon atom in the molecule.
For the first carbon (CH2), it is involved in a double bond (C=C) and two single bonds (C-H), so it is sp2 hybridized.
For the second carbon (CH), it is involved in a double bond (C=C) and a single bond (C-C), so it is sp2 hybridized.
Repeat the same analysis for the third and fourth carbons, which are also sp2 hybridized due to their involvement in double bonds and single bonds.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
4mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals are used to form covalent bonds in molecules. In butadiene, the hybridization of carbon atoms can be determined by the types of bonds they form, such as single, double, or triple bonds.
Recommended video:
Guided course
00:51
Hybridization
Bond Lengths
Bond lengths are the average distances between the nuclei of two bonded atoms. They provide insight into the type of bond present; for example, triple bonds are generally shorter than double bonds, which are shorter than single bonds. In butadiene, the bond lengths of 1.20 Å and 1.48 Å indicate the presence of a triple bond and a single bond, respectively.
Recommended video:
Guided course
00:36Average Bond Order
Planarity of Molecules
The planarity of a molecule refers to its geometric arrangement in a two-dimensional plane. In butadiene, the planar structure allows for effective overlap of p-orbitals, which is essential for the formation of π bonds in double bonds. This planarity is crucial for understanding the hybridization and bonding characteristics of the carbon atoms in the molecule.
Recommended video:
Guided course
02:07Square planar complexes show the most complex splitting pattern.
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.
Textbook Question
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?
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.
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. (c) What are the formal charges on the atoms in the Lewis structure from part (b)? Given the electronegativities of B and N, do the formal charges seem favorable or unfavorable? What are the formal charges on the atoms in the Lewis structure from part (b)?