To determine which molecule or ion has a bent shape, we need to examine the molecular geometry of each option provided.
A. [tex]\(OF_2\)[/tex]
- Oxygen difluoride ([tex]\(OF_2\)[/tex]) has two bonding pairs and two lone pairs on the oxygen atom. The presence of lone pairs causes repulsion, resulting in a bent molecular geometry.
B. [tex]\(PH_3\)[/tex]
- Phosphine ([tex]\(PH_3\)[/tex]) has three bonding pairs and one lone pair on the phosphorus atom. This arrangement results in a trigonal pyramidal shape, not bent.
C. [tex]\(ClO_4^{-}\)[/tex]
- Perchlorate ion ([tex]\(ClO_4^{-}\)[/tex]) has four equivalent bonding pairs around the central chlorine atom. These pairs arrange themselves into a tetrahedral shape.
D. [tex]\(PCl_5\)[/tex]
- Phosphorus pentachloride ([tex]\(PCl_5\)[/tex]) has five bonding pairs around the phosphorus atom, which gives it a trigonal bipyramidal shape.
After reviewing the molecular geometries, we find that the molecule with a bent shape is:
A. [tex]\(OF_2\)[/tex]
Thus, the answer is 1, corresponding to Option A.
