Question:
What is the formal charge present on oxygen atom (numbered 1) in Lewis structure of $\text{CO}_2$ ?
What is the formal charge present on oxygen atom (numbered 1) in Lewis structure of $\text{CO}_2$ ?
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Shortcut:
Single bonded O with 3 lone pairs → Formal charge = -1
Updated On: May 8, 2026
- 0
- -1
- +1
- -2
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The Correct Option is B
Solution and Explanation
Concept: Formal charge formula \[ \text{Formal charge} = \text{Valence electrons} - \text{Non-bonding electrons} - \frac{1}{2}(\text{Bonding electrons}) \]
Step 1: Identify structure
Given structure is: \[ \text{:O} \equiv \text{C} - \text{O:} \] The oxygen (numbered 1) is singly bonded to carbon and has three lone pairs (6 non-bonding electrons).
Step 2: Apply formula for oxygen
\[ \text{Valence electrons of O} = 6 \] \[ \text{Non-bonding electrons} = 6 \] \[ \text{Bonding electrons} = 2 \] \[ \text{Formal charge} = 6 - 6 - \frac{2}{2} = 6 - 6 - 1 = -1 \] Conclusion:
Formal charge on the given oxygen atom is \(-1\) Final Answer: Option (B)
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