Nitrogen Oxides Containing Nitrogen to Nitrogen Bonds

To determine which nitrogen oxide(s) contain $\text{N}-\text{N}$ bond(s), let us analyze the Lewis structures and bonding of each given oxide:

1. $\text{N}_2\text{O}$ (Dinitrogen monoxide):

   • The molecule is linear with the skeletal connectivity $\text{N}-\text{N}-\text{O}$.
   • It is represented by the major resonance contributors:
     $:\text{N}\equiv\overset{+}{\text{N}}-\ddot{\text{O}}:^{-} \longleftrightarrow {^{-}}\ddot{\text{N}}=\overset{+}{\text{N}}=\ddot{\text{O}}:$
   • Thus, $\text{N}_2\text{O}$ contains a direct $\text{N}-\text{N}$ bond.

2. $\text{N}_2\text{O}_3$ (Dinitrogen trioxide):

   • The molecule has a planar, asymmetric structure where a nitrosyl group ($-\text{NO}$) is bonded to a nitro group ($-\text{NO}_2$).
   • Its skeletal arrangement is:
     $\text{O}=\text{N}-\text{NO}_2$
   • Thus, $\text{N}_2\text{O}_3$ contains an $\text{N}-\text{N}$ single bond.

3. $\text{N}_2\text{O}_4$ (Dinitrogen tetroxide):

   • It is a planar dimer of nitrogen dioxide ($\text{NO}_2$) formed by coupling between the unpaired electrons on the two nitrogen atoms:
     $\text{O}_2\text{N}-\text{NO}_2$
   • Thus, $\text{N}_2\text{O}_4$ contains an $\text{N}-\text{N}$ bond.

4. $\text{N}_2\text{O}_5$ (Dinitrogen pentoxide):

   • In the gaseous/covalent molecular form, it consists of two planar $-\text{NO}_2$ groups linked by a bridging oxygen atom:
     $\text{O}_2\text{N}-\text{O}-\text{NO}_2$
   • In the solid state, it exists as an ionic crystal composed of nitronium and nitrate ions, $[\text{NO}_2]^+[\text{NO}_3]^-$.
   • Neither form possesses an $\text{N}-\text{N}$ bond.

Therefore, the nitrogen oxides containing $\text{N}-\text{N}$ bond(s) are $\text{N}_2\text{O}$, $\text{N}_2\text{O}_3$, and $\text{N}_2\text{O}_4$.

Correct Options: (A), (B), (C)