Question

how would the electron configuration of nitrogen change to make a stable configuration? (1 point)
it would lose four electrons
it would gain three electrons.
it would gain two electrons.
it would lose five electrons

Explanation:

Nitrogen has an atomic number of 7, so its electron configuration is \(1s^{2}2s^{2}2p^{3}\). The stable electron configuration (octet rule for main - group elements in period 2, which nitrogen is in) requires 8 electrons in the valence shell. Nitrogen has 5 valence electrons (\(2s^{2}2p^{3}\)). To achieve a stable configuration (similar to the noble gas neon which has \(2s^{2}2p^{6}\)), it needs to gain 3 electrons. Gaining three electrons will fill its \(2p\) sub - shell (\(2s^{2}2p^{6}\)). Losing electrons is less favorable for nitrogen to reach a stable configuration as losing 4 or 5 electrons would require a large amount of energy (especially for a non - metal like nitrogen) and would not lead to a noble - gas - like configuration. Gaining two electrons would give \(2s^{2}2p^{5}\), which is still not a full octet.

Answer:

B. It would gain three electrons