What is the molecular geometry of ClBr_3?

• A. Trigonal pyramidal
• B. Trigonal planar
• C. See-saw
• D. T-shaped

Answer: (D)

Verified step by step guidance

1. Determine the total number of valence electrons for ClBr_3 by adding the valence electrons of chlorine (Cl) and three bromine (Br) atoms. Chlorine has 7 valence electrons, and each bromine also has 7 valence electrons, so calculate the total as \$7 + 3 \times 7$.
2. Draw the Lewis structure by placing the chlorine atom as the central atom bonded to three bromine atoms. Then, distribute the remaining electrons to satisfy the octet rule for each atom, placing lone pairs on the central atom as needed.
3. Count the number of bonding pairs and lone pairs around the central chlorine atom. This will help determine the electron pair geometry using the VSEPR (Valence Shell Electron Pair Repulsion) theory.
4. Use the VSEPR theory to predict the molecular geometry based on the number of bonding pairs and lone pairs. For example, if there are three bonding pairs and two lone pairs, the electron geometry is trigonal bipyramidal, but the molecular shape will be T-shaped due to lone pair repulsions.
5. Confirm that the molecular geometry is T-shaped by considering the positions of the atoms and lone pairs in the trigonal bipyramidal electron geometry, where lone pairs occupy equatorial positions to minimize repulsion, resulting in a T-shaped molecular geometry.