What is the molecular geometry of the ion ICl_2^-?

• A. T-shaped
• B. Bent
• C. Linear
• D. Trigonal planar

Answer: (C)

Verified step by step guidance

1. Determine the total number of valence electrons for the ion ICl_2^-. Iodine (I) has 7 valence electrons, each chlorine (Cl) has 7 valence electrons, and the negative charge adds 1 extra electron. So, total valence electrons = 7 (I) + 2 × 7 (Cl) + 1 (charge).
2. Draw the Lewis structure by placing iodine as the central atom bonded to two chlorine atoms. Use the total valence electrons to complete the octets around chlorine atoms and place any remaining electrons as lone pairs on iodine.
3. Count the number of bonding pairs and lone pairs around the central iodine atom. This will help determine the electron pair geometry using the VSEPR (Valence Shell Electron Pair Repulsion) theory.
4. Apply the VSEPR model: with 2 bonding pairs and 3 lone pairs on iodine, the electron pair geometry is trigonal bipyramidal. The lone pairs occupy equatorial positions to minimize repulsion.
5. Determine the molecular geometry by considering only the positions of atoms (not lone pairs). With 3 lone pairs in equatorial positions and 2 bonding pairs in axial positions, the shape formed by the atoms is linear.