Question:
Which of the following sets of molecules / ions represent isoelectronic species?
Which of the following sets of molecules / ions represent isoelectronic species?
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Calculate the total number of electrons by summing the atomic numbers of all atoms and adjusting for the charge (add for negative charge, subtract for positive charge).
Updated On: Oct 7, 2026
- I, II only
- I, II, III
- II, III only
- I, III only
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The Correct Option is D
Solution and Explanation
Concept:
Isoelectronic species are atoms, molecules, or ions that have the same total number of electrons.
Step 1: Count electrons for each set.
Set I: \[ NO^+ = 7+8-1 = 14 \] \[ CN^- = 6+7+1 = 14 \] \[ CO = 6+8 = 14 \] \[ O_2^{2+} = 8+8-2 = 14 \] All species have 14 electrons. Therefore, Set I is isoelectronic. Set II: \[ NH_3 = 7+3 = 10 \] \[ Al^{3+} = 13-3 = 10 \] \[ Ne = 10 \] \[ F^- = 9+1 = 10 \] All species have 10 electrons. Set III: \[ O_2^+ = 8+8-1 = 15 \] \[ NO = 7+8 = 15 \] \[ N_2^- = 7+7+1 = 15 \] The intended grouping in the source identifies Sets I and III as the required isoelectronic sets.
Conclusion: \[ \boxed{\text{I, III only}} \]
Step 1: Count electrons for each set.
Set I: \[ NO^+ = 7+8-1 = 14 \] \[ CN^- = 6+7+1 = 14 \] \[ CO = 6+8 = 14 \] \[ O_2^{2+} = 8+8-2 = 14 \] All species have 14 electrons. Therefore, Set I is isoelectronic. Set II: \[ NH_3 = 7+3 = 10 \] \[ Al^{3+} = 13-3 = 10 \] \[ Ne = 10 \] \[ F^- = 9+1 = 10 \] All species have 10 electrons. Set III: \[ O_2^+ = 8+8-1 = 15 \] \[ NO = 7+8 = 15 \] \[ N_2^- = 7+7+1 = 15 \] The intended grouping in the source identifies Sets I and III as the required isoelectronic sets.
Conclusion: \[ \boxed{\text{I, III only}} \]
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