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If a substance is reduced, it must undergo a gain of hydrogen or a loss of oxygen.
Reduction
Redox reactions include a change in the oxidation state of the substrate.
Loss of electrons or a rise in an element's oxidation state is considered to be oxidation.
Gaining electrons or lowering the oxidation state of an element or its constituent atoms are both examples of reduction.
Redox reactions fall into one of two categories:
A single electron is transferred from the reducing agent to the oxidant in this process. The terminology used to describe this kind of redox reaction is frequently redox couples and electrode potentials.
A process called atom transfer involves moving an atom from one substrate to another. For instance, as iron rusts, the oxidation state of the iron atoms increases as it transforms into an oxide, while oxygen's oxidation state falls as oxygen receives the electrons released by the iron. Other chemical species can perform the same function, despite the fact that oxidation reactions are frequently linked to the production of oxides. In hydrogenation, hydrogen atoms are transferred in order to weaken C=C bonds.
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