Question

the electron configuration for nitrogen is $1s^{2}2s^{2}2p^{3}$. according to hunds rule, how are the electrons distributed in the three $2p$-orbitals? view available hint(s) two spin - paired electrons are in the first orbital, and there is one electron in each of the remaining orbitals. each of the $2p$-orbitals contains one electron. all three electrons reside in the first orbital, and the other two are empty. two spin - paired electrons are in the first orbital, one electron is in the second orbital, and the third orbital is empty. submit provide feedback next

Explanation:

Hund's rule states that electrons will occupy degenerate orbitals (orbitals of the same energy) singly first, with parallel spins, before pairing up. For the \(2p\) orbitals (which have three degenerate orbitals \(2p_x\), \(2p_y\), \(2p_z\)) and three electrons in the \(2p\) sub - shell of nitrogen (\(1s^{2}2s^{2}2p^{3}\)), each of the three \(2p\) orbitals will have one electron.

Answer:

Each of the \(2p\) - orbitals contains one electron.