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Oxidation State of Oxygen in Hydrogen Peroxide

On the oxidation state of oxygen in hydrogen peroxide

The way of tasting chemistry is macroscopic. For hydrogen peroxide, its molecular formula is\ (H_ {2} O_ {2}\), among which the oxidation state of oxygen is quite special and often attracts investigation.

The oxidation state of the husband, so the migration of the surface elements to the electrons in the compound is also the case. In general compounds, oxygen is more\ (-2\) valent, because of its high electronegativity, the force of electrons is strong. However, for hydrogen peroxide, the oxidation state of oxygen is not\ (-2\), but\ (-1\).

The reason is that in the structure of hydrogen peroxide, two oxygen atoms are connected by a single bond, and each oxygen atom is bonded to a hydrogen atom. Compared with hydrogen, the electronegativity of oxygen is greater, and the electron pair between hydrogen and oxygen is biased towards oxygen, which increases the potential of oxygen to gain electrons. Between two oxygen atoms, because of the same electronegativity, the electron pair is not biased towards any oxygen atom. Overall, the average electron obtained per oxygen atom is one less than the conventional\ (-2\) valence, so its oxidation state is\ (-1\).

This special oxidation state gives hydrogen peroxide unique chemical properties. Because the oxidation state of oxygen can rise or fall, it has both oxidizing and reducing properties. When it comes to strong reducing agents, the oxidation state of oxygen decreases and becomes oxidizing; when it comes to strong oxidizing agents, the oxidation state of oxygen increases and becomes reducing.

The oxidation state of oxygen in hydrogen peroxide shows that the wonders of chemistry lie between the fine structure and electron transfer. Knowing this, it is of great benefit to the study of chemistry and the application of substances.