MHT CET Chemistry Question (2026) — Solution

Step-by-step solution

The shape of the molecules can be determined using VSEPR theory by calculating the number of bond pairs (bp) and lone pairs (lp) on the central Xenon (Xe) atom, which has 8 valence electrons. For XeF _4: Xe forms 4 single bonds with F atoms, using 4 electrons. Remaining electrons = 4 (2 lone pairs). With 4 bp and 2 lp, the hybridization is sp^3d^2 and the shape is square planar. For XeF _6: Xe forms 6 single bonds with F atoms, using 6 electrons. Remaining electrons = 2 (1 lone pair). With 6 bp and 1 lp, the hybridization is sp^3d^3 and the shape is distorted octahedral. For XeO _3: Xe forms 3 double bonds with O atoms, using 6 electrons. Remaining electrons = 2 (1 lone pair). With 3 bp ( -bonds) and 1 lp, the hybridization is sp^3 and the shape is trigonal pyramidal. For XeOF _4: Xe forms 1 double bond with O and 4 single bonds with F, using 2 + 4 = 6 electrons. Remaining electrons = 2 (1 lone pair). With 5 bp ( -bonds) and 1 lp, the hybridization is sp^3d^2 and the shape is square pyramidal. Answer: XeOF _4