The molecular shape of ICl3 is bent.
To understand why, we consider the central iodine atom, which is bonded to three chlorine atoms. Iodine has seven valence electrons, and when it forms bonds with the three chlorine atoms, it uses three of these valence electrons to form three single covalent bonds.
After forming these bonds, iodine is left with two lone pairs of electrons. The arrangement of these electron pairs around the central iodine atom is governed by the VSEPR theory (Valence Shell Electron Pair Repulsion theory), which predicts that electron pairs will position themselves as far apart as possible to minimize repulsion.
In the case of ICl3, the presence of the two lone pairs pushes down on the bonding pairs (the I-Cl bonds), creating a bent shape. Therefore, the correct answer for the molecular shape of ICl3 is bent.