Question:
An odd electron molecule among the following is (2015)
An odd electron molecule among the following is (2015)
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Common odd electron molecules to remember: NO, NO$_2$, ClO$_2$. They are typically paramagnetic.
Updated On: Apr 20, 2026
- CO
- SO$_2$
- CO$_2$
- NO
- O$_2$
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The Correct Option is D
Solution and Explanation
Step 1: Understanding the Concept:
An odd electron molecule is one that has an odd total number of valence electrons. Such molecules often do not follow the octet rule.
a Step 2: Key Formula or Approach:
Calculate total valence electrons = sum of valence electrons of all atoms in the molecule.
Step 3: Detailed Explanation:
(A) CO: $4(\text{C}) + 6(\text{O}) = 10$ (Even)
(B) SO$_2$: $6(\text{S}) + 2 \times 6(\text{O}) = 18$ (Even)
(C) CO$_2$: $4(\text{C}) + 2 \times 6(\text{O}) = 16$ (Even)
(D) NO: $5(\text{N}) + 6(\text{O}) = 11$ (Odd)
(E) O$_2$: $2 \times 6(\text{O}) = 12$ (Even)
Since NO has 11 valence electrons, it is an odd electron molecule.
Step 4: Final Answer:
The odd electron molecule is NO.
An odd electron molecule is one that has an odd total number of valence electrons. Such molecules often do not follow the octet rule.
a Step 2: Key Formula or Approach:
Calculate total valence electrons = sum of valence electrons of all atoms in the molecule.
Step 3: Detailed Explanation:
(A) CO: $4(\text{C}) + 6(\text{O}) = 10$ (Even)
(B) SO$_2$: $6(\text{S}) + 2 \times 6(\text{O}) = 18$ (Even)
(C) CO$_2$: $4(\text{C}) + 2 \times 6(\text{O}) = 16$ (Even)
(D) NO: $5(\text{N}) + 6(\text{O}) = 11$ (Odd)
(E) O$_2$: $2 \times 6(\text{O}) = 12$ (Even)
Since NO has 11 valence electrons, it is an odd electron molecule.
Step 4: Final Answer:
The odd electron molecule is NO.
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