Question

how would the electron configuration of nitrogen change to make a stable configuration?
(1 point)

it would gain two electrons

it would lose five electrons.

it would gain three electrons.

it would lose four electrons

Explanation:

Nitrogen has an atomic number of 7, with an electron configuration of \(1s^2 2s^2 2p^3\). The outermost (valence) shell (2nd shell) has 5 electrons (\(2s^2 2p^3\)). A stable electron configuration (like a noble gas) has a full valence shell (8 electrons for the 2nd shell, following the octet rule). To reach 8 valence electrons, nitrogen needs to gain \(8 - 5 = 3\) electrons. Losing 5 electrons would be difficult (requires a lot of energy) and other options don't align with the octet rule for stability.

Answer:

It would gain three electrons.