Answer: Lateral p orbital overlap is less effective than head-on axial overlap.
- A Lateral p orbital overlap is less effective than head-on axial overlap
- B Pi bonds generally span a greater bond length than sigma bonds as frequently described
- C Pi bonds contain fewer electrons than the corresponding sigma bond
- D Sigma bonds usually occupy inherently lower energy orbitals in most textbook accounts
Correct answer: A. Lateral p orbital overlap is less effective than head-on axial overlap
Explanation: Pi bonds form by sideways (lateral) overlap of p orbitals, which is less efficient than the direct head-on overlap of sigma bonds.
VSEPR theory predicts molecular shape from the number of bonding and lone electron pairs around the central atom.
Concept context
Understand how atoms join to form molecules. Covers ionic and covalent bonding, VSEPR theory, hybridization (sp, sp², sp³), molecular orbital theory, bond polarity, and intermolecular forces like hydrogen bonding.
Read the full Chemical Bonding and Molecular Structure notes →