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If pure P orbitals were used in forming the B-F bonds in BF₃ angles 90° would be expected. The actual observed bond angle is 120°. What concept might be useful in explaining the observed angles?

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If pure P orbitals were used in forming the B-F bonds in BF₃ angles 90° would be expected. The actual observed bond angle is 120°. What concept might be useful in explaining the observed angles? Answer: Hybridization

The trigonal planar structure of BF₃ with bond angles of 120° is explained by sp² hybridization. Here, one s and two p orbitals of boron mix to form three equivalent sp² hybrid orbitals, which form bonds with fluorine atoms, resulting in 120° angles instead of 90°.

Question context

This question is part of 🔬 General Science within the broader 🌐 Current Affairs & GK subject and appears in the SPSC – Sindh Public Service Commission preparation collection. Reviewing the answer together with nearby questions helps reinforce the underlying concept and identify how it may appear in competitive exams.