The shape of BCl₃, PCl₃, and ICl₃ molecules are:

• (A) Triangular
• (B) Pyramidal
• (C) T-shaped
• (D) All above are incorrect

The shapes of the molecules BCl₃, PCl₃, and ICl₃ vary due to differences in their molecular geometry influenced by the number of bonding pairs and lone pairs of electrons.

BCl₃ - Trigonal Planar

Boron trichloride (BCl₃) has a trigonal planar shape. This is because it has three bonding pairs of electrons and no lone pairs, resulting in a flat, triangular arrangement.

PCl₃ - Trigonal Pyramidal

Phosphorus trichloride (PCl₃) adopts a trigonal pyramidal shape. It has three bonding pairs and one lone pair of electrons, which pushes the chlorine atoms down, creating a pyramid-like structure.

ICl₃ - T-shaped

Iodine trichloride (ICl₃) has a T-shaped geometry. It contains three bonding pairs and two lone pairs, leading to a structure where the chlorine atoms form a T shape around the iodine atom.

Summary of Shapes

• BCl₃: Trigonal Planar
• PCl₃: Trigonal Pyramidal
• ICl₃: T-shaped

Therefore, the correct answer to the question is that all options provided (A, B, C) are indeed correct for different molecules. The answer (D) is incorrect.