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Why must all six atoms in $\mathrm{C}_{2} \mathrm{H}_{4}$ lie in the same plane?

   Why must all six atoms in $\mathrm{C}_{2} \mathrm{H}_{4}$ lie in the same plane?

Chemistry

Steven S. Zumdahl,… 8th Edition

Chapter 9, Problem 31

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Solved by Expert David Collins

05/22/2020

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C2H4 is an ethene molecule, which consists of two carbon atoms and four hydrogen atoms. Show more…

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Why must all six atoms in $\mathrm{C}_{2} \mathrm{H}_{4}$ lie in the same plane?

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Key Concepts

Pi Bond Formation

The double bond in C2H4 is composed of one sigma bond and one pi bond. The pi bond is formed by the side-by-side overlap of the unhybridized p orbitals, which must be parallel to each other. This requirement for parallel orientation further enforces that all atoms in the molecule lie in the same plane.

sp2 Hybridization

In molecules like C2H4, each carbon atom involved in the double bond is sp2 hybridized. This means that one s orbital and two p orbitals combine to form three hybrid orbitals that lie in a plane, resulting in a trigonal planar geometry around each carbon atom.

Trigonal Planar Geometry

The sp2 hybridization imposes a trigonal planar arrangement of atoms, where the bond angles are approximately 120°. This planar arrangement is essential for minimizing electron repulsions and stabilizing the molecule’s overall structure.

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