Given the Lewis structure for ClF_2^+, what is the electron-pair geometry around the central chlorine atom?

• A. Linear
• B. Octahedral
• C. Tetrahedral
• D. Trigonal bipyramidal

Answer: (D)

Verified step by step guidance

1. Identify the central atom in the molecule, which is chlorine (Cl) in ClF_2^+.
2. Count the total number of valence electrons for the central atom and the attached atoms, then adjust for the charge of the ion. Chlorine has 7 valence electrons, each fluorine has 7, and since the ion has a +1 charge, subtract one electron from the total count.
3. Determine the number of electron domains (regions of electron density) around the central chlorine atom. These include bonding pairs (to fluorine atoms) and lone pairs on chlorine.
4. Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the electron-pair geometry based on the number of electron domains. For 5 electron domains, the electron-pair geometry is trigonal bipyramidal.
5. Confirm that the molecular geometry (shape) may differ from the electron-pair geometry if lone pairs are present, but the question specifically asks for electron-pair geometry, which is trigonal bipyramidal for 5 electron domains.