Answer the question on the basis of passage given below:
Nitrogen differs from rest of the members of group 15 due to its small size, high electronegativity, high ionization enthalpy and non-availability of d orbitals. Nitrogen has unique ability to form pл - рл multiple bonds with itself and with other elements having small size and high electronegativity. Heavier elements of this group do not form \(р\pi -р\pi \) bonds as their atomic orbitals are so large and diffuse that they cannot have effective overlapping.

Planar structures with \(N-N\) single bond are shown by

A. \(N_2O_3\)

B. \(N_2O_4\)

C. \(N_2O_5\)

D. \(N_2O\)

E. \(NO\)

Choose the correct answer from the options given below:

A and B only

The correct answer is option 1. A and B only.

Let us go through each of the given nitrogen oxides in detail to understand their structures, the presence or absence of \(N-N\) single bonds, and whether they are planar.

A. \(N_2O_3\) (Dinitrogen Trioxide)

\(N_2O_3\) is an anhydride of nitrous acid and consists of two nitrogen atoms connected by a single bond (\(N-N\)) and three oxygen atoms. The structure is planar because of the sp² hybridization of the nitrogen atoms.

The two nitrogen atoms are connected by an \(N-N\) single bond. Each nitrogen atom is also bonded to oxygen atoms.

The molecule is planar due to its symmetrical structure and the arrangement of the atoms, which minimizes strain and allows for a flat geometry.

Conclusion: Yes, \(N_2O_3\) has an \(N-N\) single bond and is planar.

B. \(N_2O_4\) (Dinitrogen Tetroxide)

\(N_2O_4\) is the dimer of nitrogen dioxide (\(NO_2\)), and it consists of two nitrogen atoms connected by a single bond (\(N-N\)) with four oxygen atoms attached. The molecule is planar in the gas phase.

There is an \(N-N\) single bond between the two nitrogen atoms, and each nitrogen atom is bonded to two oxygen atoms.

\(N_2O_4\) is planar because the atoms adopt a flat configuration that minimizes repulsion between the atoms. The \(N-N\) bond allows for a planar structure, and the molecule remains planar in the gas phase.

Conclusion: Yes, \(N_2O_4\) has an \(N-N\) single bond and is planar.

C. \(N_2O_5\) (Dinitrogen Pentoxide)

\(N_2O_5\) is an anhydride of nitric acid (\(HNO_3\)) and consists of two nitrogen atoms, but they are not directly bonded to each other by an \(N-N\) single bond. Instead, each nitrogen atom is bonded to three oxygen atoms, and the structure is not planar.

There is no \(N-N\) single bond in \(N_2O_5\). Each nitrogen atom is connected to oxygen atoms in a non-planar arrangement.

The structure of \(N_2O_5\) is not planar. The two nitrogen atoms are part of separate structural units that are connected through oxygen bridges, resulting in a three-dimensional arrangement.

Conclusion: No, \(N_2O_5\) does not have an \(N-N\) single bond and is not planar.

D. \(N_2O\) (Nitrous Oxide or Laughing Gas)

\(N_2O\) consists of two nitrogen atoms and one oxygen atom. The bonding is such that the two nitrogen atoms are connected by a triple bond (\(N \equiv N\)) and the terminal nitrogen is bonded to an oxygen atom.

There is no \(N-N\) single bond in \(N_2O\). The bond between the nitrogen atoms is a triple bond, making the structure linear rather than planar.

Since \(N_2O\) has a linear structure due to the triple bond between nitrogen atoms, it is not planar.

Conclusion: No, \(N_2O\) does not have an \(N-N\) single bond and is not planar (it is linear).

E. \(NO\) (Nitric Oxide)

\(NO\) consists of one nitrogen atom and one oxygen atom. There is no \(N-N\) bond in this molecule. The nitrogen atom is directly bonded to an oxygen atom via a single bond. There is no second nitrogen atom, so an \(N-N\) bond does not exist. Since \(NO\) is a diatomic molecule, the concept of planarity doesn’t apply in the same way as with polyatomic molecules.

Conclusion: No, \(NO\) does not have an \(N-N\) bond and is not planar.

Thus, the correct answer is: 1. A and B only.