Which family of elements typically has an oxidation number of -3?

The nitrogen family, also known as Group 15 of the periodic table, typically has an oxidation number of -3 due to the nature of its elements, which include nitrogen, phosphorus, arsenic, antimony, and bismuth. These elements have five valence electrons, and in order to achieve a stable electron configuration, they can gain three additional electrons in chemical reactions. This gaining of three electrons results in an oxidation state of -3.

In terms of their behavior, nitrogen and phosphorus compounds often exhibit this -3 oxidation state, particularly in simple ionic or covalent compounds. For example, in ammonia (NH₃), nitrogen assumes the -3 oxidation state because it needs three more electrons to complete its valence shell.

The other families of elements mentioned do not typically exhibit a -3 oxidation state. Halogens, for instance, generally have an oxidation state of -1, as they are one electron short of a complete valence shell. The oxygen family (Group 16) usually has oxidation states of -2. Finally, alkaline earth metals (Group 2) typically exhibit a +2 oxidation state due to their two valence electrons, which they readily lose in chemical reactions. Therefore, the distinct property of the nitrogen family to