Question

Match the appropriate geometry on the right with each of the species on the left:

Hint:

In \(sp^3d\) systems with 3 lone pairs (like \(XeF_2\)), the geometry is always linear. With 2 lone pairs (like \(ClF_3\) or \(XeOF_2\)), the geometry is always T-shaped.

Answer 1

Step 1: Understanding the Concept:
Xenon compound geometries are predicted using VSEPR theory, based on the steric number (bond pairs + lone pairs) of the central Xenon atom.
Step 2: Detailed Explanation:
1. (A) \(FXeO(OSO_2F)\): Xenon is in the +2 state, bonded to two electronegative groups. It has 2 bond pairs and 3 lone pairs (\(sp^3d\) hybridization). To minimize repulsion, lone pairs occupy equatorial positions, making the molecular geometry linear. $\rightarrow$ (i)
2. (B) \(FXeN(SO_2F)_2\): Similarly, Xenon is in the +2 state with 2 bond pairs and 3 lone pairs. The geometry around Xe is linear. $\rightarrow$ (i)
3. (C) \(XeO_3\): Xenon is in the +6 state. It has 3 double bonds to oxygen and 1 lone pair (\(sp^3\) hybridization). This results in a trigonal pyramidal geometry. $\rightarrow$ (ii)
4. (D) \(XeOF_2\): Xenon is in the +4 state. It has 3 bonding pairs (1 \(Xe=O\), 2 \(Xe-F\)) and 2 lone pairs (\(sp^3d\) hybridization). In a TBP arrangement, lone pairs go to equatorial sites, leaving a T-shaped geometry. $\rightarrow$ (iii)
Step 3: Final Answer:
The correct matching is (A)-(i), (B)-(i), (C)-(ii), (D)-(iii).