Chemistry - CHEMICAL BONDING Question with Solution | TestHub

To find the correct order of bond angles, we analyze the hybridization and geometry of each molecule:

BF₃ and BCl₃: Both have sp² hybridization and a trigonal planar geometry, resulting in a bond angle of exactly $120^{\circ }$. Thus, BCl₃ = BF₃.

BF₄⁻ and CCl₄: Both have sp³ hybridization and a tetrahedral geometry, resulting in a bond angle of approximately $109.5^{\circ }$. Thus, BF₄⁻ = CCl₄.

Comparing these, $120^{\circ }$ (trigonal planar) is greater than $109.5^{\circ }$ (tetrahedral).

Therefore, (B) BF₃ ($120^{\circ }$) > BF₄⁻ ($109.5^{\circ }$) and (D) CCl₄ ($109.5^{\circ }$) < BF₃ ($120^{\circ }$).