Textbook Question
Draw the following orbitals:
a. 3s orbital
b. 4s orbital
c. 3p orbital
1. A Review of General Chemistry
Molecular Orbitals
6:29 minutesProblem 1
Textbook Question
Draw the molecular orbital picture of trans-but-2-ene. Be sure to label all σ and π bonds. Is there free rotation around the C₂― C₃ bond? Why or why not?
Verified step by step guidance1
Start by drawing the Lewis structure of trans-but-2-ene. This molecule has a double bond between the second and third carbon atoms (C₂ and C₃), with the two methyl groups (CH₃) on opposite sides of the double bond, ensuring the 'trans' configuration.
Identify the bonding framework: The single bonds (σ bonds) are formed by the overlap of sp² hybrid orbitals from the carbon atoms with either hydrogen atoms or other carbon atoms. The double bond consists of one σ bond and one π bond. The π bond arises from the side-by-side overlap of unhybridized p orbitals on C₂ and C₃.
Draw the molecular orbital diagram: Represent the σ bonds as overlapping orbitals along the internuclear axis. For the π bond, show the unhybridized p orbitals on C₂ and C₃ overlapping above and below the plane of the molecule. Label all σ and π bonds clearly in your diagram.
Explain the lack of free rotation: The π bond in the C₂―C₃ double bond restricts rotation because breaking the π bond would require significant energy. The side-by-side overlap of the p orbitals must be maintained for the π bond to exist, which is not possible during rotation.
Conclude by emphasizing that the rigidity of the double bond is a key feature of alkenes, and it is this rigidity that gives rise to the distinct 'cis' and 'trans' isomerism observed in compounds like but-2-ene.
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6mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Orbitals
Molecular orbitals are formed by the combination of atomic orbitals when atoms bond together. In the case of trans-but-2-ene, the molecular orbital diagram will illustrate the distribution of electrons in σ (sigma) and π (pi) bonds. Sigma bonds result from head-on overlap of orbitals, while pi bonds arise from the side-to-side overlap of p orbitals, which is crucial for understanding the bonding in alkenes.
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Cis-Trans Isomerism
Cis-trans isomerism, also known as geometric isomerism, occurs in alkenes due to restricted rotation around the double bond. In trans-but-2-ene, the two methyl groups are on opposite sides of the double bond, which affects the molecule's physical properties and reactivity. Understanding this concept is essential for analyzing the structure and behavior of alkenes.
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Restricted Rotation
Restricted rotation refers to the inability of certain bonds, particularly double bonds, to rotate freely due to the presence of π bonds. In trans-but-2-ene, the C₂―C₃ double bond restricts rotation, leading to distinct geometric isomers. This restriction is a key factor in determining the stability and reactivity of alkenes, as it influences their spatial arrangement and interactions with other molecules.
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