Final answer:
Molecular geometry with two bonding pairs and one lone pair is bent or V-shaped with angles less than 109.5°.
Step-by-step explanation:
The question asks about the molecular geometry when there are a total of three electron groups around the central atom with two of these being bonding pairs. According to VSEPR theory (Valence Shell Electron Pair Repulsion), the geometry is determined by the total number of bonding pairs (BP) and lone pairs (LP). Given that there are three total regions, these are arranged tetrahedrally if they are all bonding pairs. However, if there are bonding pairs and a lone pair, the molecular structure adjusts. With two bonding pairs and one lone pair, the molecular geometry is bent or V-shaped. This shape can be considered as a trigonal planar structure with one vertex missing, which would be the position of a lone pair. In this context, the bond angles are expected to be less than the omni-directional 120° of a perfect trigonal planar arrangement because of the extra space taken up by the lone pair, resulting in angles typically less than 120°, and very close to or slightly less than 109.5°.