Exams › JEE Main › Chemistry
In which of the following ionization processes, the bond order has increased and the magnetic behaviour has changed?
- N → N2+
- C2 → C2+
- NO → NO+
- O2 → O2+
Correct answer: NO → NO+
Solution
In the ionization of NO to NO+, the removal of an electron from a bonding orbital increases the bond order, resulting in a stronger bond. Additionally, this process changes the magnetic behavior from paramagnetic to diamagnetic, as the unpaired electron is removed.
Related JEE Main Chemistry questions
- Although the electronegativity gap between N and F is larger than that between N and H, ammonia has a dipole moment of 1.5 D while nitrogen trifluoride has only 0.2 D. The reason is that
- When N₂ is converted into N₂⁺, the dissociation energy of the N–N bond ______, and when O₂ is converted into O₂⁺, the dissociation energy of the O–O bond ______.
- From the ions listed below, which pair has geometries that can be accounted for by the same type of orbital hybridization? NO₂⁻, NO₃⁻, NH₂⁻, NH₄⁺, SCN⁻
- Atoms A and B have electronegativities of 1.20 and 4.0, respectively. What is the percentage ionic character of the A–B bond?
- In the phosphate ion, PO₄³⁻, what is the formal charge on an oxygen atom that is singly bonded to phosphorus in a P–O bond?
- Among the following species, which one has no unpaired electrons?
⚔️ Practice JEE Main Chemistry free + battle 1v1 →