Question

What is the electronic configuration of Nitrogen monoxide?

Answer 1

Hint : In molecular orbital theory, the bonding orbital is used to explain the favorable relations between two or more atoms' atomic orbitals in a molecule. Electrons are depicted as moving in waves in the MO principle.

Complete Step By Step Answer:
Steps involved in molecular orbital theory are: Considering electrons to be delocalized in the molecule, integrating atomic orbitals to form molecular orbitals $(\sigma ,{\sigma ^*},\pi ,{\pi ^*})$, producing bonding and antibonding relationships depending on which orbitals are filled, and predicting electron structure in molecules.
$\sigma 2s$Bonding MO is represented by $1{a_1}$.
$\sigma *2s$Antibonding MO is represented by $2{a_1}$.
$\pi 2{P_x}$Bonding MO is represented by $1{b_1}$.
$\pi 2{P_y}$Bonding MO is represented by $1{b_2}$.
$\sigma 2{P_x}$Bonding MO is represented by $3{a_1}$.
$\pi *2{P_x}$Antibonding MO is represented by $2{b_1}$.
$\pi *2{P_y}$Antibonding MO is represented by $2{b_2}$.
$\sigma 2{P_x}$Antibonding MO is represented by $4{a_1}$.
Additionally, the $2s - 2s$ overlap is the same concept as the $1s - 1s$ overlap. As a result, the molecular electron structure will be written in the same way as the atomic version, but with molecular orbitals instead of atomic orbitals.
Hence, we get,
${({\sigma _{1s}})^2}{(\sigma _{1s}^*)^2}{({\sigma _{2s}})^2}{(\sigma _{2s}^*)^2}{({\pi _{2px}})^2}{({\pi _2}_{py})^2}{({\sigma _{2px}})^2}{(\pi _{2px}^*)^1}$

Note :
The valence-bond principle fails to understand exactly how many compounds, such as resonance-stabilized molecules, contain two or more identical bonds whose bond orders lie between those of a single bond and those of a double bond. This is where the molecular orbital concept proved to be more strong than the valence-bond theory