Question:
What is the bond angle Cl-B-Cl and molecular geometry of \(\text{BCl}_{3}\) molecule?
What is the bond angle Cl-B-Cl and molecular geometry of \(\text{BCl}_{3}\) molecule?
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Boron has three bond pairs and no lone pair, so it is sp2 hybridised.
Updated On: Nov 12, 2026
- \(120^{\circ }\) and trigonal bipyramidal
- \(109^{\circ }28'\) and tetrahedral
- \(107^{\circ }18'\) and tetrahedral
- \(120^{\circ }\) and trigonal planar
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The Correct Option is D
Solution and Explanation
Step 1: Understanding the Concept
The shape of a molecule depends on the number of bond pairs and lone pairs on the central atom.
Step 2: Boron in BCl3
Boron has 3 valence electrons and forms three B-Cl bonds. There is no lone pair, so there are three electron pairs and the hybridisation is \(sp^2\).
Step 3: Result
Three pairs spread as far apart as possible in one plane, at \(120^{\circ}\) to each other. The shape is trigonal planar.
Final Answer:
The Cl-B-Cl angle is 120 degrees and the shape is trigonal planar, which is option (D). \[ \boxed{\text{(D) }120^{\circ}\text{ and trigonal planar}} \]
The shape of a molecule depends on the number of bond pairs and lone pairs on the central atom.
Step 2: Boron in BCl3
Boron has 3 valence electrons and forms three B-Cl bonds. There is no lone pair, so there are three electron pairs and the hybridisation is \(sp^2\).
Step 3: Result
Three pairs spread as far apart as possible in one plane, at \(120^{\circ}\) to each other. The shape is trigonal planar.
Final Answer:
The Cl-B-Cl angle is 120 degrees and the shape is trigonal planar, which is option (D). \[ \boxed{\text{(D) }120^{\circ}\text{ and trigonal planar}} \]
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