Why does hydrogen usually have an oxidation state of +1 in compounds with nonmetals?

Hydrogen is assigned an oxidation state of +1 in compounds with nonmetals because it is less electronegative than elements such as fluorine, oxygen, nitrogen, chlorine, sulfur, and carbon.1

The assignment of oxidation states is a formal calculation based on the distribution of shared electrons in a chemical bond. When hydrogen forms a bond with a more electronegative nonmetal, the shared electrons are conceptually assigned to the more electronegative atom. Because hydrogen loses the influence over its single valence electron in this process, it is assigned a +1 oxidation state.1

It is important to note that oxidation states are not physical realities but rather a method of accounting for electrons to help understand oxidation-reduction reactions. While hydrogen is typically +1 when bonded to nonmetals, it can exhibit different states in other contexts, such as in metal hydrides where it may be assigned a -1 state due to its relative electronegativity compared to the metal.12