The molecular geometry of XeF2 is linear.
To understand why it’s linear, let’s look at the structure of xenon difluoride. Xenon (Xe) is a noble gas that can form bonds with fluorine (F), a highly electronegative element. In XeF2, xenon is the central atom surrounded by two fluorine atoms.
When we analyze the electron geometry, we find that xenon has five electron pairs in total: two bonding pairs (from the Xe-F bonds) and three lone pairs. According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, these lone pairs will occupy positions that minimize repulsion. In the case of XeF2, the three lone pairs will arrange themselves around the xenon atom in a way that they occupy equatorial positions in a trigonal bipyramidal arrangement, while the two fluorine atoms will occupy the axial positions.
This specific arrangement causes the molecule to adopt a linear shape since the two fluorine atoms are placed opposite to each other, 180 degrees apart. Therefore, the correct answer is that the molecular geometry of XeF2 is linear.