Question:
Identify linear molecule from following.
Identify linear molecule from following.
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Look for a central atom with two bond pairs and no lone pair.
Updated On: Oct 1, 2026
- \(\text{SO}_2\)
- \(\text{BCl}_3\)
- \(\text{CO}_2\)
- \(\text{NH}_3\)
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The Correct Option is C
Solution and Explanation
Step 1: Understanding the Concept:
The shape of a molecule follows from VSEPR theory. A molecule is linear when the central atom has two electron regions and no lone pair, so the bond angle is \(180^{\circ}\).
Step 2: Detailed Explanation of the keyed option:
In \(\text{CO}_2\) carbon forms two double bonds, \(\text{O=C=O}\), and has no lone pair. Two regions of electron density stay as far apart as possible, so the O-C-O angle is \(180^{\circ}\) and the molecule is linear (sp hybridised carbon).
Step 3: Why the other options are wrong.
\(\text{SO}_2\) has one lone pair on sulphur, which pushes the two S=O bonds into a bent shape of about \(119^{\circ}\). \(\text{BCl}_3\) has three bond pairs on boron and no lone pair, giving a trigonal planar shape with \(120^{\circ}\) angles. \(\text{NH}_3\) has three bond pairs and one lone pair on nitrogen, giving a pyramidal shape.
Final Answer:
Only carbon dioxide is linear, option (C). \[ \boxed{\text{CO}_2 \text{ (C)}} \]
The shape of a molecule follows from VSEPR theory. A molecule is linear when the central atom has two electron regions and no lone pair, so the bond angle is \(180^{\circ}\).
Step 2: Detailed Explanation of the keyed option:
In \(\text{CO}_2\) carbon forms two double bonds, \(\text{O=C=O}\), and has no lone pair. Two regions of electron density stay as far apart as possible, so the O-C-O angle is \(180^{\circ}\) and the molecule is linear (sp hybridised carbon).
Step 3: Why the other options are wrong.
\(\text{SO}_2\) has one lone pair on sulphur, which pushes the two S=O bonds into a bent shape of about \(119^{\circ}\). \(\text{BCl}_3\) has three bond pairs on boron and no lone pair, giving a trigonal planar shape with \(120^{\circ}\) angles. \(\text{NH}_3\) has three bond pairs and one lone pair on nitrogen, giving a pyramidal shape.
Final Answer:
Only carbon dioxide is linear, option (C). \[ \boxed{\text{CO}_2 \text{ (C)}} \]
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