In which of the following ionization processes the bond energy has increased and also the magnetic behaviour has changed from paramagnetic to diamagnetic ?
Show Hint
- \(\mathrm{NO \rightarrow NO^{+}}\)
- \(\mathrm{N_2 \rightarrow N_2^{+}}\)
- \(\mathrm{C_2 \rightarrow C_2^{+}}\)
- \(\mathrm{O_2 \rightarrow O_2^{+}}\)
The Correct Option is A
Solution and Explanation
(1) NO has 15 electrons: B.O. = 2.5, one unpaired electron in \(\pi^*2p\) (paramagnetic). NO\(^+\) has 14 electrons: B.O. = 3, no unpaired electrons (diamagnetic). Bond order increases and paramagnetic \(\rightarrow\) diamagnetic. This fits.
(2) \(\mathrm{N_2}\) (B.O. = 3, diamagnetic) \(\rightarrow\) \(\mathrm{N_2^{+}}\) (B.O. = 2.5, paramagnetic): bond energy decreases and the change is diamagnetic \(\rightarrow\) paramagnetic. Not correct.
(3) \(\mathrm{C_2}\) (B.O. = 2, diamagnetic) \(\rightarrow\) \(\mathrm{C_2^{+}}\) (B.O. = 1.5, paramagnetic): not correct.
(4) \(\mathrm{O_2}\) (B.O. = 2, paramagnetic) \(\rightarrow\) \(\mathrm{O_2^{+}}\) (B.O. = 2.5, still paramagnetic): the bond energy increases but the magnetic behaviour does not change to diamagnetic. Not correct.
Only NO \(\rightarrow\) NO\(^+\) satisfies both conditions.
Answer: (1) \(\mathrm{NO \rightarrow NO^{+}}\)
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