The number of antibonding electron pair(s) present in \(O_{2}^{2-}\)is:

Increasing order of bond length is:

1. $N{O}^{-}$ $<$ $NO$ $<$ $N{O}^{+}$ $<$ $O_2^{-}$

2. $O_2^{-}$ $<$ $NO$ $<$ $N{O}^{-}$ $<$ $N{O}^{+}$ $$

3. $O_2^{-}$ $<$ $N{O}^{-}$ $<$ $NO<$ $N{O}^{+}$ $$

4. $N{O}^{+}$ $<$ $NO$ $<$ $N{O}^{-}$ $<$ $O_2^{-}$

The correct order of dissociation energy of N₂ and N₂⁺ is:

A species that does not exhibit paramagnetism is:

1. N₂⁺

2. O₂^–

3. CO

4. NO

If the main axis of a diatomic molecule is z, then the molecular orbital p_x and p_y overlap to form which of the following orbital:

1.  $\mathrm{\pi }$ molecular orbtial
2.  σ molecular orbital
3.  δ molecular orbtial
4.  No bond will form

The correct order in which the O-O bond length increases in the following is:

1. ${\mathrm{O}}_3<{\mathrm{H}}_2{\mathrm{O}}_2<{\mathrm{O}}_2$

2. ${\mathrm{O}}_2<{\mathrm{O}}_3<{\mathrm{H}}_2{\mathrm{O}}_2$

3. ${\mathrm{O}}_2<{\mathrm{H}}_2{\mathrm{O}}_2<{\mathrm{O}}_3$

4. ${\mathrm{H}}_2{\mathrm{O}}_2<{\mathrm{O}}_2<{\mathrm{O}}_3$