Match List - I with List - II

List - I	List - II
(a) PCl5	(i) Square pyramidal
(b) SF6	(ii) Trigonal planar
(c) BrF5	(iii) Octahedral
(d) BF3	(iv) Trigonal bipyramidal

Choose the correct answer from the options given below.

To match each compound in List‑I with its correct molecular geometry in List‑II we use the VSEPR (Valence Shell Electron‑Pair Repulsion) theory, which predicts the shape based on the number of bonding pairs and lone pairs around the central atom.

1. $PCl$₅ – Phosphorus is surrounded by five chlorine atoms and has no lone pair. Five‑coordinate species with no lone pairs adopt a trigonal bipyramidal geometry. In List‑II this corresponds to option (iv).

2. $SF$₆ – Sulfur is surrounded by six fluorine atoms and has no lone pair. Six‑coordinate species without lone pairs form an octahedral geometry, which is option (iii) in List‑II.

3. $BrF$₅ – Bromine is bonded to five fluorine atoms and possesses one lone pair. A five‑coordinate central atom with one lone pair gives a square pyramidal shape, matching option (i).

4. $BF$₃ – Boron is bonded to three fluorine atoms and has no lone pair. A three‑coordinate molecule with only bonding pairs adopts a trigonal planar geometry, which is option (ii).

Putting the matches together we obtain the following correspondence:

(a) PCl₅ → (iv) Trigonal bipyramidal
(b) SF₆ → (iii) Octahedral
(c) BrF₅ → (i) Square pyramidal
(d) BF₃ → (ii) Trigonal planar

Thus the correct answer is (a)-(iv), (b)-(iii), (c)-(i), (d)-(ii).