What is an electron configuration of a nitrogen molecule?

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Answer 1 · 2016-08-24T01:28:43

The electron configuration of $N_{2}$ $"N"_2$ is
$(σ1s)^2(σ^"∗"1s)^2(σ2s)^2(σ^"∗"2s)^2(π2p_x)^2(π2p_y)^2(σ2p_z)^2$

The molecular orbitals of $"N"_2$ are formed by overlapping the atomic orbitals of the $"N"$ atoms.

The new molecular orbitals are formed as follows:

The $1s$ orbitals form a bonding $σ1s$ and an antibonding $σ"*"1s$ MO.
The $2s$ orbitals form a bonding $σ2s$ and an antibonding $σ"*"2s$ MO.
The $2p$ orbitals directed along the internuclear axis form a bonding $σ2p_z$ and an antibonding $σ"*"2p_z$ MO.
The $2p_x$ and $2p_y$ orbitals from each atom form bonding $π2p_x$ and $π2p_y$ bonding MOs and antibonding $π"*"2p_x$ and $π"*"2p_y$ MO.

The relative energy levels of the orbitals are

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Each $"N"$ atom contributes seven electrons, so we use the Aufbau Principle to fill the MOs starting at the lowest level.

The result is

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Thus, the electron configuration of $"N"_2$ is

$(σ1s)^2(σ^"∗"1s)^2(σ2s)^2(σ^"∗"2s)^2(π2p_x)^2(π2p_y)^2(σ2p_x)^2$