Asked by Matthew Torres on Apr 27, 2024
Verified
From a molecular orbital perspective why isn't there relatively free rotation about the carbon-carbon double bond in ethene (CH2=CH2)?
Molecular Orbital
A mathematical function describing the wave-like behavior of an electron in a molecule. This concept is central to understanding chemical bonding and the electronic structure of molecules.
Carbon-carbon Double Bond
A type of chemical bond where two carbon atoms share two pairs of electrons, forming a stronger bond than a single bond.
Ethene
A colorless flammable gas with a faint sweet and musky odor, the simplest alkene with the chemical formula C2H4, used as a petrochemical precursor.
- Utilizing molecular orbital theory to elucidate the bonding and structure of molecules.
Verified Answer
ZK
Zybrea KnightMay 03, 2024
Final Answer :
Two carbon p atomic orbitals overlap side-to-side and in phase to form the π bond that is present. Rotation about the carbon-carbon bond axis requires quite a bit of energy because the π bond is broken as the overlap between the two p orbitals is disrupted.
Learning Objectives
- Utilizing molecular orbital theory to elucidate the bonding and structure of molecules.