The electronic configuration of a nitrogen at | vedclass

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(A) The atomic number of nitrogen $(N)$ is $7$. Its electronic configuration is $1s^2 2s^2 2p^3$.According to Hund's rule of maximum multiplicity,for

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(A) The atomic number of nitrogen $(N)$ is $7$. Its electronic configuration is $1s^2 2s^2 2p^3$.According to Hund's rule of maximum multiplicity,for a given electron configuration,the term with the maximum multiplicity has the lowest energy. This means that electrons in the same subshell should occupy separate orbitals with parallel spins as far as possible.In the $2p$ subshell,there are $3$ electrons. Therefore,they should occupy the three $2p$ orbitals singly with parallel spins.Option $A$ (image $203-$a248) correctly shows $1s^2$ (paired),$2s^2$ (paired),and $2p^3$ (three unpaired electrons with parallel spins).

The electronic configuration of a nitrogen atom in its ground state is represented as follows:

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