What is the electron geometry of ClF_3?

• A. Octahedral
• B. Square planar
• C. Trigonal bipyramidal
• D. T-shaped

Answer: (C)

Verified step by step guidance

1. Determine the total number of valence electrons around the central atom, chlorine (Cl). Chlorine has 7 valence electrons, and each fluorine (F) atom contributes 1 electron, so for ClF_3, total valence electrons = 7 + 3 × 1 = 10 electrons (or 5 electron pairs).
2. Draw the Lewis structure of ClF_3, placing chlorine in the center with three fluorine atoms bonded to it. Then, distribute the remaining electrons to satisfy the octet rule, placing lone pairs on the central chlorine atom as needed.
3. Count the number of electron pairs around the central atom, including both bonding pairs (Cl-F bonds) and lone pairs. For ClF_3, there are 3 bonding pairs and 2 lone pairs, making a total of 5 electron pairs.
4. Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to determine the electron geometry based on the total number of electron pairs. Five electron pairs arrange themselves in a trigonal bipyramidal geometry to minimize repulsion.
5. Identify the molecular shape by considering the positions of the atoms only (ignoring lone pairs). With 3 bonded atoms and 2 lone pairs in a trigonal bipyramidal electron geometry, the molecular shape is T-shaped.