The angle between unhybridized p-orbital and three sp2 hybrid orbitals of each carbon atom in ethene is:
Correct answer: B. 90°
- A. 120°
- B. 90°
- C. 109.5°
- D. 180°
Explanation
Option B is correct. In ethene (C2H4) ,each carbon atom is sp2 hybridized. The three sp2 hybrid orbitals are arranged in a trigonal planar geometry, with bond angles of 90 degrees between them. The unhybridized p-orbital is perpendicular to the plane formed by the sp2 hybrid orbitals. Here's a link to an image from LibreTexts that illustrates the arrangement of the sp2 hybrid orbitals and the unhybridized p-orbital in ethene.
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Chemical bonding explains molecular shape through VSEPR theory and distinguishes sigma bonds from pi bonds. Questions involve hybridization, bond angles, dipole moment and bond energy, including how electron-pair repulsion determines geometry and how bond polarity differs from the overall polarity of a molecule.
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