Question:medium

Based upon VSEPR theory, match the shape (geometry) of the molecules in List-I with the molecules in
List-II and select the most appropriate option.
  List-I                            List-II
(Shape)                    (Molecules)
(A) T-shaped             (I) XeF4
(B) Trigonal planar     (II) SF4
(C) Square planar       (III) CIF3
(D) See-saw                (IV) BF3

Updated On: Mar 20, 2026
  • (A)-(I), (B)-(II), (C)-(III), (D)-(IV)
  • (A)-(III), (B)-(IV), (C)-(I), (D)-(II)
  • (A)-(III), (B)-(IV), (C)-(II), (D)-(I)
  • (A)-(IV), (B)-(III), (C)-(I), (D)-(II)
Show Solution

The Correct Option is B

Solution and Explanation

 To determine the correct matches between the shapes (geometries) of molecules in List-I and the molecules in List-II using VSEPR (Valence Shell Electron Pair Repulsion) theory, we will analyze each option step by step:

  1. (A) T-shaped:
    • VSEPR theory states that a T-shaped geometry typically occurs when there are three bonds and two lone pairs around the central atom.
    • Example: ClF3 (Chlorine trifluoride) - This molecule has three bonded pairs and two lone pairs, leading to a T-shaped geometry.
  2. (B) Trigonal planar:
    • According to VSEPR theory, a trigonal planar shape results from three bonds and no lone pairs around the central atom.
    • Example: BF3 (Boron trifluoride) - In this molecule, boron forms three bonds with no lone pairs, giving it a trigonal planar shape.
  3. (C) Square planar:
    • A square planar shape arises when there are four bonds and two lone pairs around the central atom.
    • Example: XeF4 (Xenon tetrafluoride) - Xenon forms four bonds with fluorine and has two lone pairs, resulting in a square planar shape.
  4. (D) See-saw:
    • In VSEPR theory, a see-saw shape is characteristic of a central atom with four bonds and one lone pair.
    • Example: SF4 (Sulfur tetrafluoride) - Sulfur has four bonded pairs and one lone pair, leading to a see-saw shape.

Based on the analysis above, the correct matches are:

List-I (Shape)List-II (Molecule)
(A) T-shaped(III) ClF3
(B) Trigonal planar(IV) BF3
(C) Square planar(I) XeF4
(D) See-saw(II) SF4

Thus, the most appropriate option is (A)-(III), (B)-(IV), (C)-(I), (D)-(II).

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