AIIMS 2018 Chemistry Molecular Geometry MCQ Question

Boron trifluoride (BF₃) exhibits a trigonal planar geometry due to its three bonding pairs of electrons and no lone pairs on the boron atom, resulting in a bond angle of 120°. In contrast, iodine trichloride (ICl₃) has a T-shaped geometry because it has three bonding pairs and two lone pairs of electrons on the iodine atom, leading to a distorted arrangement that minimizes electron pair repulsion. Other options may refer to incorrect molecular geometries or configurations that do not accurately represent the shapes of BF₃ or ICl₃. Understanding the VSEPR (Valence Shell Electron Pair Repulsion) theory is crucial for predicting molecular shapes based on electron pair arrangements.