The set of oxides of nitrogen that are paramagnetic in nature is:

1. NO, N₂O

2. N₂O₃, NO

3. NO, NO₂

4. N₂O, NO₂

Which of the compounds given below will exhibit a linear structure?

1. NO₂

2. HOCl

3. O₃

4. N₂O

Match the compounds of Xe in Column I with the molecular structure in Column II.

Match the coordination number and type of hybridization with the distribution of hybrid orbitals in space based on Valence bond theory.

The potential energy (y) curve for H₂ formation as a function of internuclear distance (x) of the H atoms is shown below.

The bond energy of H₂ is:

How many (i) sp² hybridised carbon atoms and (ii) $\mathrm{\pi }$ bonds are present in the following compound?

Which orbital does the additional electron occupy when O₂ is converted to the O₂⁻ ion?

1.  $\pi$ $\mathrm{orbital}$ $$

2.  $\sigma *$ $\mathrm{orbital}$ $$

3.  $\sigma$ $\mathrm{orbital}$

4.  $\pi *$ $\mathrm{orbital}$ $$

Four diatomic species are listed below. Identify the correct order in which the bond order is increasing in them.
1. O₂^– < NO < C₂^2– < He₂⁺  
2. C₂^2– < He₂⁺ < O₂^– < NO  
3. He₂⁺ < O₂^– < NO < C₂^2–
4. NO < O₂^– < C₂^2– < He₂⁺  

The pairs of species of oxygen and their magnetic behaviours are given below. Which of the following represents the correct description?

1. $\mathrm{O},$ ${\mathrm{O}}_2^{2-}$ - Both paramagnetic
2. ${\mathrm{O}}_2^{-},$ ${\mathrm{O}}_2^{2-}$ - Both diamagnetic
3. ${\mathrm{O}}^{+},$ ${\mathrm{O}}_2^{2-}$ - Both paramagnetic
4. ${\mathrm{O}}_2^{+},$ ${\mathrm{O}}_2$ - Both paramagnetic