Question:
Which of the following statement is correct?
Which of the following statement is correct?
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Remember the formula $VSEPR$: Carbon is $sp$ hybridized in $CO_2$, leading to a linear shape and double bonds to satisfy the valency of 4 for Carbon.
Updated On: Jun 26, 2026
- $CO_2$ molecule contains one C-O and one C=O bonds and one lone pair on each oxygen atom.
- $CO_2$ molecule contains two C-O bonds and one lone pair on each oxygen atom
- $CO_2$ molecule contains one C-O bond and one C=O bond with two lone pairs on each oxygen atom.
- $CO_2$ molecule contains one C-O bond and one C$\equiv$O and one lone pair on each oxygen atom.
- $CO_2$ contains two $C=O$ bonds and two lone pairs on each oxygen atom
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The Correct Option is
Solution and Explanation
Step 1: Understanding the Concept:
Carbon dioxide ($CO_2$) is a linear molecule where the central Carbon atom forms double bonds with two Oxygen atoms.
Step 2: Detailed Explanation:
1. Carbon has 4 valence electrons and Oxygen has 6.
2. To achieve octets, Carbon shares 2 electrons with each Oxygen, forming two $C=O$ double bonds.
3. The Lewis structure is: $\text{:\,Ö=C=Ö\,:}$
4. Each Oxygen atom uses 2 electrons for the double bond, leaving 4 electrons (2 lone pairs) on each oxygen atom.
5. Carbon has no lone pairs.
Step 3: Final Answer:
The correct statement is that $CO_2$ contains two $C=O$ bonds and two lone pairs on each oxygen atom.
Carbon dioxide ($CO_2$) is a linear molecule where the central Carbon atom forms double bonds with two Oxygen atoms.
Step 2: Detailed Explanation:
1. Carbon has 4 valence electrons and Oxygen has 6.
2. To achieve octets, Carbon shares 2 electrons with each Oxygen, forming two $C=O$ double bonds.
3. The Lewis structure is: $\text{:\,Ö=C=Ö\,:}$
4. Each Oxygen atom uses 2 electrons for the double bond, leaving 4 electrons (2 lone pairs) on each oxygen atom.
5. Carbon has no lone pairs.
Step 3: Final Answer:
The correct statement is that $CO_2$ contains two $C=O$ bonds and two lone pairs on each oxygen atom.
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