ICl2 is a molecule that consists of one iodine atom and two chlorine atoms. In order to determine its molecular structure, we need to consider the electron pair geometry and the molecular geometry.

1. Electron Pair Geometry:
The electron pair geometry describes the arrangement of all electron pairs (bonding and non-bonding) around the central atom. In the case of ICl2, the iodine atom is the central atom. It has seven valence electrons and forms single bonds with both chlorine atoms.

Using the VSEPR (Valence Shell Electron Pair Repulsion) theory, we can determine the electron pair geometry by considering the number of electron pairs around the central atom. In this case, there are two electron pairs (one bonding pair and one lone pair) around the iodine atom.

The presence of one lone pair indicates that the electron pair geometry is trigonal bipyramidal.

2. Molecular Geometry:
The molecular geometry describes the arrangement of only the bonding electron pairs around the central atom. In the case of ICl2, we ignore the lone pair and consider only the bonding pairs.

To determine the molecular geometry, we need to consider the repulsion between the bonding pairs. Since there are only two bonding pairs, they will repel each other and try to maximize the distance between them.

In a trigonal bipyramidal electron pair geometry, there are three possible molecular geometries: trigonal planar, T-shaped, and linear. The actual molecular geometry will depend on the positioning of the bonding pairs.

In the case of ICl2, the bonding pairs will arrange themselves in a way that minimizes their repulsion. This results in a distorted trigonal bipyramidal molecular geometry, where the two chlorine atoms are positioned in a bent or V-shape around the central iodine atom.

Therefore, the correct answer is option 'D' - distorted trigonal bipyramidal.