What is the value of the bond angle in XeF_2?

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

Answer: (A)

Verified step by step guidance

1. Identify the central atom and the number of bonded atoms and lone pairs around it. In XeF_2, xenon (Xe) is the central atom bonded to two fluorine (F) atoms, and it has three lone pairs of electrons.
2. Determine the electron domain geometry using the total number of electron pairs (bonding + lone pairs). For XeF_2, there are 2 bonding pairs and 3 lone pairs, making a total of 5 electron pairs, which corresponds to a trigonal bipyramidal electron geometry.
3. Apply the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular shape. Lone pairs occupy equatorial positions to minimize repulsion, and the two bonded atoms occupy the axial positions.
4. Recognize that the molecular shape of XeF_2 is linear because the two fluorine atoms are positioned opposite each other along the axis, with the three lone pairs in the equatorial plane.
5. Conclude that the bond angle between the two fluorine atoms in XeF_2 is 180 degrees, consistent with a linear molecular geometry.