Question

Match isostructural species in Column I with Column II.

• A. A$\rightarrow$P, B$\rightarrow$S, C$\rightarrow$R, D$\rightarrow$Q
• B. A$\rightarrow$P, B$\rightarrow$Q, C$\rightarrow$R, D$\rightarrow$S
• C. A$\rightarrow$S, B$\rightarrow$R, C$\rightarrow$Q, D$\rightarrow$P
• D. A$\rightarrow$S, B$\rightarrow$Q, C$\rightarrow$R, D$\rightarrow$P

Hint:

To identify isostructural species quickly, count {bond pairs + lone pairs} on the central atom and apply VSEPR geometry.

Answer 1

The Correct Option is A

To determine the isostructural species between Column I and Column II, we need to consider the molecular geometry and the arrangement of atoms in each molecule. Isostructural species have the same molecular geometry and similar hybridization of the central atom. 

Column I	Column II
(A) XeF2	(P) I3-
(B) XeOF4	(Q) NH3
(C) XeO2F2	(R) SF4
(D) XeO3	(S) BrF5

1. For XeF₂ and I₃^-:
   • XeF₂ has a linear structure due to sp³d hybridization with a central atom surrounded by two bonded atoms and three lone pairs.
   • I₃^- also has a linear structure with the same hybridization, making them isostructural.
2. For XeOF₄ and BrF₅:
   • XeOF₄ has a square pyramidal geometry due to sp³d² hybridization.
   • BrF₅ also has a square pyramidal geometry with similar hybridization, making them isostructural.
3. For XeO₂F₂ and SF₄:
   • XeO₂F₂ has a see-saw shape due to sp³d hybridization.
   • SF₄ has the same see-saw shape and sp³d hybridization, making them isostructural.
4. For XeO₃ and NH₃:
   • XeO₃ has a trigonal pyramidal shape due to sp³ hybridization.
   • NH₃ also has a trigonal pyramidal shape with the same hybridization, making them isostructural.

Therefore, the correct matching of isostructural species is:

• (A) XeF₂ → (P) I₃^-
• (B) XeOF₄ → (S) BrF₅
• (C) XeO₂F₂ → (R) SF₄
• (D) XeO₃ → (Q) NH₃

So, the correct answer is: A→P, B→S, C→R, D→Q.