To solve this question, we need to analyze each ionization process and check two conditions: whether the bond energy increases and whether the magnetic behavior changes from paramagnetic to diamagnetic. Paramagnetic species have unpaired electrons and are attracted to magnetic fields, while diamagnetic species have all electrons paired and are repelled by magnetic fields. Bond energy is related to bond order, which can be calculated using molecular orbital theory.
Starting with Option A: NO→NO+
Nitric oxide (NO) has nitrogen (atomic number 7) and oxygen (atomic number 8), so the total number of valence electrons is 5 (from N) + 6 (from O) = 11. The molecular orbital configuration for NO is:
(σ2s)2,(σ2s∗)2,(π2p)4,(σ2pz)2,(π2p∗)1
Here, the unpaired electron in the π2p∗ orbital makes NO paramagnetic. The bond order is calculated as:
Bond order = 2number of bonding electrons−number of antibonding electrons
Bonding electrons: σ2s (2 electrons), π2p (4 electrons), σ2pz (2 electrons) → total 8 bonding electrons.
Antibonding electrons: σ2s∗ (2 electrons), π2p∗ (1 electron) → total 3 antibonding electrons.
Bond order of NO = 28−3=25=2.5
For NO+, one electron is removed from the highest occupied molecular orbital (HOMO), which is the π2p∗ orbital. The configuration becomes:
(σ2s)2,(σ2s∗)2,(π2p)4,(σ2pz)2
All electrons are now paired, so NO+ is diamagnetic. Bonding electrons: σ2s (2), π2p (4), σ2pz (2) → total 8. Antibonding electrons: σ2s∗ (2) → total 2. Bond order of NO+ = 28−2=26=3.
Bond order increases from 2.5 to 3, so bond energy increases. Magnetic behavior changes from paramagnetic (NO) to diamagnetic (NO+). Option A satisfies both conditions.
Now, Option B: N2→N2+
Nitrogen molecule (N2) has two nitrogen atoms (atomic number 7 each), so total valence electrons = 5 + 5 = 10. The molecular orbital configuration is:
(σ2s)2,(σ2s∗)2,(π2p)4,(σ2pz)2
All electrons are paired, so N2 is diamagnetic. Bonding electrons: σ2s (2), π2p (4), σ2pz (2) → total 8. Antibonding electrons: σ2s∗ (2) → total 2. Bond order = 28−2=3.
For N2+, one electron is removed from the σ2pz orbital (HOMO). Configuration becomes:
(σ2s)2,(σ2s∗)2,(π2p)4,(σ2pz)1
This has one unpaired electron, so paramagnetic. Bonding electrons: σ2s (2), π2p (4), σ2pz (1) → total 7. Antibonding electrons: σ2s∗ (2) → total 2. Bond order = 27−2=25=2.5.
Bond order decreases from 3 to 2.5, so bond energy decreases. Magnetic behavior changes from diamagnetic to paramagnetic, not paramagnetic to diamagnetic. Option B does not satisfy.
Option C: C2→C2+
Carbon molecule (C2) has two carbon atoms (atomic number 6 each), so total valence electrons = 4 + 4 = 8. The molecular orbital configuration is:
(σ2s)2,(σ2s∗)2,(π2p)4
All electrons are paired, so diamagnetic. Bonding electrons: σ2s (2), π2p (4) → total 6. Antibonding electrons: σ2s∗ (2) → total 2. Bond order = 26−2=2.
For C2+, one electron is removed from the π2p orbital. Configuration becomes:
(σ2s)2,(σ2s∗)2,(π2p)3
With three electrons in two degenerate π2p orbitals, one orbital has two electrons (paired) and the other has one (unpaired), so paramagnetic. Bonding electrons: σ2s (2), π2p (3) → total 5. Antibonding electrons: σ2s∗ (2) → total 2. Bond order = 25−2=23=1.5.
Bond order decreases from 2 to 1.5, so bond energy decreases. Magnetic behavior changes from diamagnetic to paramagnetic. Option C does not satisfy.
Option D: O2→O2+
Oxygen molecule (O2) has two oxygen atoms (atomic number 8 each), so total valence electrons = 6 + 6 = 12. The molecular orbital configuration is:
(σ2s)2,(σ2s∗)2,(σ2pz)2,(π2p)4,(π2p∗)2
The two electrons in the degenerate π2p∗ orbitals are unpaired (Hund's rule), so paramagnetic. Bonding electrons: σ2s (2), σ2pz (2), π2p (4) → total 8. Antibonding electrons: σ2s∗ (2), π2p∗ (2) → total 4. Bond order = 28−4=2.
For O2+, one electron is removed from the π2p∗ orbital. Configuration becomes:
(σ2s)2,(σ2s∗)2,(σ2pz)2,(π2p)4,(π2p∗)1
This has one unpaired electron, so paramagnetic. Bonding electrons: σ2s (2), σ2pz (2), π2p (4) → total 8. Antibonding electrons: σ2s∗ (2), π2p∗ (1) → total 3. Bond order = 28−3=25=2.5.
Bond order increases from 2 to 2.5, so bond energy increases. However, magnetic behavior remains paramagnetic (both have unpaired electrons). Option D does not satisfy the magnetic behavior change.
Only Option A satisfies both conditions: bond energy increases and magnetic behavior changes from paramagnetic to diamagnetic.
Hence, the correct answer is Option A.