Question:
Which of the following pair of species have different Lewis structures?
(A) \( \mathrm{SO_3^{2-}, CO_3^{2-}} \)
(B) \( \mathrm{O_2^{2-}, F_2} \)
(C) \( \mathrm{CN^- , CO} \)
(D) \( \mathrm{NH_3, H_3O^+} \)
(E) \( \mathrm{MnO_4^- , CrO_4^{2-}} \)
Which of the following pair of species have different Lewis structures?
(A) \( \mathrm{SO_3^{2-}, CO_3^{2-}} \)
(B) \( \mathrm{O_2^{2-}, F_2} \)
(C) \( \mathrm{CN^- , CO} \)
(D) \( \mathrm{NH_3, H_3O^+} \)
(E) \( \mathrm{MnO_4^- , CrO_4^{2-}} \)
(B) \( \mathrm{O_2^{2-}, F_2} \)
(C) \( \mathrm{CN^- , CO} \)
(D) \( \mathrm{NH_3, H_3O^+} \)
(E) \( \mathrm{MnO_4^- , CrO_4^{2-}} \)
Updated On: Apr 8, 2026
- (A) only
- (A) & (B) only
- (A) & (E) only
- (C) & (D) only
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Verified By Collegedunia
The Correct Option is A
Solution and Explanation
Step 1: Analyzing (A) \( \mathrm{SO_3^{2-}, CO_3^{2-}} \).
- \( \mathrm{SO_3^{2-}} \) and \( \mathrm{CO_3^{2-}} \) both have resonance structures. However, their Lewis structures are different due to the different atoms involved. \( \mathrm{SO_3^{2-}} \) has sulfur as the central atom, while \( \mathrm{CO_3^{2-}} \) has carbon as the central atom, resulting in distinct electron distributions and bonding.
Step 2: Analyzing (B) \( \mathrm{O_2^{2-}, F_2} \).
- Both \( \mathrm{O_2^{2-}} \) and \( \mathrm{F_2} \) have similar bonding, where each atom is bonded to the other by a single bond, with the extra electron pair creating the negative charge on the oxygen species. The Lewis structures are quite similar for these species.
Step 3: Analyzing (C) \( \mathrm{CN^- , CO} \).
- \( \mathrm{CN^-} \) and \( \mathrm{CO} \) both involve triple bonds (with a lone pair on nitrogen and oxygen), and both species have a formal charge, but the bonding and the lone pair positions lead to slight differences in the Lewis structures.
Step 4: Analyzing (D) \( \mathrm{NH_3, H_3O^+} \).
- Both \( \mathrm{NH_3} \) and \( \mathrm{H_3O^+} \) involve a nitrogen or oxygen atom with three single bonds, and the difference in formal charge does not significantly alter their overall Lewis structures.
Step 5: Analyzing (E) \( \mathrm{MnO_4^- , CrO_4^{2-}} \).
- \( \mathrm{MnO_4^-} \) and \( \mathrm{CrO_4^{2-}} \) have similar structures with four oxygen atoms surrounding the metal center. Both have resonance structures, but the central metal atoms (Mn and Cr) result in similar electron distributions and bonding.
Step 6: Conclusion.
The correct answer is (A) because \( \mathrm{SO_3^{2-}} \) and \( \mathrm{CO_3^{2-}} \) have different Lewis structures due to the different central atoms involved.
Final Answer: (A) (A) only.
- \( \mathrm{SO_3^{2-}} \) and \( \mathrm{CO_3^{2-}} \) both have resonance structures. However, their Lewis structures are different due to the different atoms involved. \( \mathrm{SO_3^{2-}} \) has sulfur as the central atom, while \( \mathrm{CO_3^{2-}} \) has carbon as the central atom, resulting in distinct electron distributions and bonding.
Step 2: Analyzing (B) \( \mathrm{O_2^{2-}, F_2} \).
- Both \( \mathrm{O_2^{2-}} \) and \( \mathrm{F_2} \) have similar bonding, where each atom is bonded to the other by a single bond, with the extra electron pair creating the negative charge on the oxygen species. The Lewis structures are quite similar for these species.
Step 3: Analyzing (C) \( \mathrm{CN^- , CO} \).
- \( \mathrm{CN^-} \) and \( \mathrm{CO} \) both involve triple bonds (with a lone pair on nitrogen and oxygen), and both species have a formal charge, but the bonding and the lone pair positions lead to slight differences in the Lewis structures.
Step 4: Analyzing (D) \( \mathrm{NH_3, H_3O^+} \).
- Both \( \mathrm{NH_3} \) and \( \mathrm{H_3O^+} \) involve a nitrogen or oxygen atom with three single bonds, and the difference in formal charge does not significantly alter their overall Lewis structures.
Step 5: Analyzing (E) \( \mathrm{MnO_4^- , CrO_4^{2-}} \).
- \( \mathrm{MnO_4^-} \) and \( \mathrm{CrO_4^{2-}} \) have similar structures with four oxygen atoms surrounding the metal center. Both have resonance structures, but the central metal atoms (Mn and Cr) result in similar electron distributions and bonding.
Step 6: Conclusion.
The correct answer is (A) because \( \mathrm{SO_3^{2-}} \) and \( \mathrm{CO_3^{2-}} \) have different Lewis structures due to the different central atoms involved.
Final Answer: (A) (A) only.
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