Question

A homonuclear diatomic gas molecule shows 2 electron magnetic moment. The one-electron and two-electron reduced species obtained from above gas molecule can act as both oxidizing and reducing agents. When the gas molecule is one-electron oxidized the bond length decreases compared to the neutral molecule. The gas molecule is:

• A. $N_2$
• B. $C{l}_2$
• C. $O_2$
• D. $B_2$

Answer 1

The correct option is C $O_2$

Oxygen $\left(O_2\right)$
The electronic configuration of $O_2$ is
${\sigma }_{1s}^2{\sigma }_{1s}^{\ast 2}{\sigma }_{2s}^2{\sigma }_{2s}^{\ast 2}{\sigma }_{2p_z}^2{\pi }_{2p_x}^2{\pi }_{2p_y}^2{\pi }_{2p_x}^{\ast 1}{\pi }_{2p_y}^{\ast 1}$

Since is has 2 unpaired electron so it shows two-electron magnetic moment.
The one-electron and two-electron reduced species of $O_2$ can loose as well as gain electron, hence, acts as both reducing as well as oxidizing agent.
When the gas molecule is one-electron oxidized the bond length decreases compared to the neutral molecule since electron goes from the antibonding orbital.