What is the approximate bond angle in XeCl_2?

• A. 120^ext{o}
• B. 180^ext{o}
• C. 90^ext{o}
• D. 109.5^ext{o}

Answer: (B)

Verified step by step guidance

1. Identify the central atom and the atoms bonded to it. In XeCl_2, xenon (Xe) is the central atom bonded to two chlorine (Cl) atoms.
2. Determine the total number of valence electrons around the central atom. Xenon has 8 valence electrons, and each chlorine contributes 7 valence electrons, but only the bonding electrons directly affect the shape around Xe.
3. Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular geometry. Count the number of bonding pairs and lone pairs on the central atom. XeCl_2 has 2 bonding pairs and 3 lone pairs on xenon.
4. Recognize that 5 regions of electron density (2 bonding + 3 lone pairs) correspond to a trigonal bipyramidal electron geometry. Lone pairs occupy equatorial positions to minimize repulsion.
5. Conclude that the molecular shape is linear because the two bonded atoms occupy the axial positions, resulting in a bond angle of approximately \$180^\circ$ between the two chlorine atoms.