An atom of nitrogen with five valence electrons can become more chemically stable by achieving a full valence electron shell, which, in the case of nitrogen, is eight valence electrons. There are a few ways nitrogen can achieve this increased stability:
Electron gain: Nitrogen can gain three electrons to fill its valence shell. By accepting three additional electrons, nitrogen will have a total of eight valence electrons, similar to the stable configuration of the noble gas neon (Ne). This results in the formation of a nitride ion, N³⁻, which has a full valence shell.
Covalent bonding: Nitrogen can form covalent bonds by sharing electrons with other atoms. By sharing three pairs of electrons with three other atoms, nitrogen can complete its valence shell and achieve stability. This is commonly observed in nitrogen molecules (N₂), where two nitrogen atoms share three pairs of electrons, resulting in a triple bond.
Combination: Nitrogen can also combine both electron gain and covalent bonding to achieve stability. For example, nitrogen can form a compound with an element that readily donates one or more electrons, such as hydrogen or metals. By accepting electrons from these elements and forming covalent bonds, nitrogen can complete its valence shell and increase its stability.
Overall, nitrogen atoms strive to achieve a total of eight valence electrons through electron gain, covalent bonding, or a combination of both, enabling them to attain a more chemically stable configuration.