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Which of the following pairs of ions are isoelectronic and isostructural?
medium
Chemical bonding and Molecular structure
2015
chemistry
ClO 3 − _3^- 3 − and CO 3 2 − _3^{2-} 3 2 −
SO 3 2 − _3^{2-} 3 2 − and NO 3 − _3^- 3 −
ClO 3 − _3^- 3 − and SO 3 2 − _3^{2-} 3 2 −
CO 3 2 − _3^{2-} 3 2 − and SO 3 2 − _3^{2-} 3 2 −
Explanation To determine which pairs of ions are isoelectronic and isostructural, we need to analyze each option. \\
Isoelectronic species have the same number of electrons. \\
Isostructural species have the same shape or geometry. \\
Let's evaluate each option: \\
Option 1: ClO 3 − _3^- 3 −
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and CO
• ClO
Chlorine (Cl) has 17 electrons, and each oxygen (O) has 8 electrons.
Total electrons = 17 + 3(8) + 1 (for the negative charge) = 34 electrons.
• CO
Carbon (C) has 6 electrons, and each oxygen (O) has 8 electrons.
Total electrons = 6 + 3(8) + 2 (for the 2- charge) = 32 electrons.
These ions are not isoelectronic.
Option 2:
SO
and NO
• SO
Sulfur (S) has 16 electrons, and each oxygen (O) has 8 electrons.
Total electrons = 16 + 3(8) + 2 (for the 2- charge) = 42 electrons.
• NO
Nitrogen (N) has 7 electrons, and each oxygen (O) has 8 electrons.
Total electrons = 7 + 3(8) + 1 (for the negative charge) = 32 electrons.
These ions are not isoelectronic.
Option 3:
ClO
and SO
• ClO
Total electrons = 34 electrons (as calculated above).
• SO
Total electrons = 42 electrons (as calculated above).
These ions are not isoelectronic.
Option 4:
CO
and SO
• CO
Total electrons = 32 electrons (as calculated above).
• SO
Total electrons = 42 electrons (as calculated above).
These ions are not isoelectronic.
Upon reviewing the options, it seems there was an error in the provided correct option.
Let's re-evaluate:
The correct pair should be isoelectronic and isostructural.
Re-evaluating:
Option 3:
ClO
and SO
are not isoelectronic.
The correct answer should be:
None of the given pairs are both isoelectronic and isostructural.
Please verify the correct option as the provided answer seems incorrect.