What is the process called that involves the loss of electrons, resulting in an increase in oxidation state?

The process that involves the loss of electrons, leading to an increase in the oxidation state, is called oxidation. During oxidation, an atom, ion, or molecule loses one or more electrons, which results in a higher oxidation state. This is fundamental in redox (reduction-oxidation) reactions, where the oxidation state of a substance changes due to the transfer of electrons.

In many chemical reactions, when a substance is oxidized, it often becomes more positively charged or less negatively charged, reflecting the loss of electrons. For example, when iron (Fe) oxidizes to form iron oxide (Fe2O3), iron loses electrons and its oxidation state increases from 0 in elemental iron to +3 in the oxide. This concept is critical in understanding how reactions occur in chemistry and how they relate to energy transfer.

The other terms refer to different processes: reduction involves gaining electrons and decreasing oxidation state, ionization is the process of forming ions from neutral atoms or molecules, and hydrogenation specifically refers to the addition of hydrogen to a compound.