Question:
Identify the hybridization in \(\text{BF}_{3}\) molecule.
Identify the hybridization in \(\text{BF}_{3}\) molecule.
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Count the bond pairs and lone pairs around boron to get the steric number.
Updated On: Nov 12, 2026
- \(sp\) hybridization
- \(sp^{2}\) hybridization
- \(sp^{3}\) hybridization
- \(sp^{3}d\) hybridization
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The Correct Option is B
Solution and Explanation
Step 1: Understanding the Concept
Hybridisation follows from the number of sigma bonds plus lone pairs on the central atom.
Step 2: Boron in BF3
Boron forms three sigma bonds with fluorine and has no lone pair, so the steric number is 3.
Step 3: Result
One 2s and two 2p orbitals mix to give three \(sp^{2}\) orbitals. The shape is trigonal planar with \(120^{\circ}\) bond angles.
Final Answer:
Boron in BF3 is sp2 hybridised. \[ \boxed{\text{(B) }sp^{2}\text{ hybridization}} \]
Hybridisation follows from the number of sigma bonds plus lone pairs on the central atom.
Step 2: Boron in BF3
Boron forms three sigma bonds with fluorine and has no lone pair, so the steric number is 3.
Step 3: Result
One 2s and two 2p orbitals mix to give three \(sp^{2}\) orbitals. The shape is trigonal planar with \(120^{\circ}\) bond angles.
Final Answer:
Boron in BF3 is sp2 hybridised. \[ \boxed{\text{(B) }sp^{2}\text{ hybridization}} \]
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