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(C) Hund's rule of maximum multiplicity states that for a given electron configuration,the term with the maximum multiplicity has the lowest energy. I

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Hund's rule

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(C) Hund's rule of maximum multiplicity states that for a given electron configuration,the term with the maximum multiplicity has the lowest energy. In the case of nitrogen $(Z = 7)$,the electronic configuration is $1s^2 2s^2 2p^3$. According to Hund's rule,electrons fill degenerate orbitals (like $2p_x, 2p_y, 2p_z$) singly first before pairing occurs. Therefore,$1s^2 2s^2 2p_x^1 2p_y^1 2p_z^1$ is the correct ground state configuration,while $1s^2 2s^2 2p_x^2 2p_y^1 2p_z^0$ represents an excited state.

According to which principle is the electronic configuration of nitrogen $1s^2 2s^2 2p_x^1 2p_y^1 2p_z^1$ and not $1s^2 2s^2 2p_x^2 2p_y^1 2p_z^0$?

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