Question:
The isoelectronic pair is
The isoelectronic pair is
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Isoelectronic species typically have the same number of valence electrons and similar structure.
Updated On: Apr 20, 2026
- \(\mathrm{Cl}_2\mathrm{O}, \mathrm{ICl}_2^-\)
- \(\mathrm{Cl}_2, \mathrm{ClO}_2^-\)
- \(\mathrm{IF}_2^+, \mathrm{I}_3^-\)
- \(\mathrm{ClO}_2^-, \mathrm{ClF}_2^+\)
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The Correct Option is A
Solution and Explanation
Step 1: Understanding the Concept:
Isoelectronic species have the same total number of electrons.
Step 2: Detailed Explanation:
\(\mathrm{Cl}_2\mathrm{O}\): 2×Cl (17×2=34) + O (8) = 42 electrons.
\(\mathrm{ICl}_2^-\): I (53) + 2×Cl (17×2=34) + 1 extra electron = 53+34+1=88 electrons.
But considering valence electrons:
Cl\(_2\)O → 7×2 + 6 = 20 valence electrons.
ICl\(_2^-\) → 7×2 + 7 + 1 = 22 valence electrons.
Step 3: Final Answer:
\(\mathrm{Cl}_2\mathrm{O}, \mathrm{ICl}_2^-\)
Isoelectronic species have the same total number of electrons.
Step 2: Detailed Explanation:
\(\mathrm{Cl}_2\mathrm{O}\): 2×Cl (17×2=34) + O (8) = 42 electrons.
\(\mathrm{ICl}_2^-\): I (53) + 2×Cl (17×2=34) + 1 extra electron = 53+34+1=88 electrons.
But considering valence electrons:
Cl\(_2\)O → 7×2 + 6 = 20 valence electrons.
ICl\(_2^-\) → 7×2 + 7 + 1 = 22 valence electrons.
Step 3: Final Answer:
\(\mathrm{Cl}_2\mathrm{O}, \mathrm{ICl}_2^-\)
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