This is done by systematically analyzing the valence electrons of the constituent atoms. Still, it is helpful to visualize the overall skeletal structure of the molecule, its bonds, and its lone pairs. We shall discuss the chemical bonding nature of H2O2 in this article.įirst, we shall draw the Lewis structure of H2O2.Ī Lewis structure may not give us a complete description of the molecular geometry. It is toxic and corrosive and hence must be handled with caution. H2O2 is a toxic byproduct of several biological processes, and several enzymatic reactions are dedicated to the decomposition of H2O2.
It is also used as an oxidizer in spacecraft since oxygen is not available for combustion in outer space. It also plays a vital role in organic synthesis, used in the oxidation/reduction of various functional groups. It is a strong oxidizing agent, and hence, it finds wide applications as a bleaching agent and disinfectant. This is an example of a comproportionation reaction, i.e., the reverse of a disproportionation reaction. The reaction is as follows :ĢH2O + O2 → 2H2O2 (in the presence of Anthraquinone) Industrially, H2O2 is prepared using Anthraquinone as a catalyst. It also exhibits a relatively high boiling point of 150.2 Celsius (302.4 Fahrenheit), attributed to strong hydrogen bonding interactions with water and other H2O2 molecules.
A low melting point indicates the tendency of the compound to remain in the liquid state. H2O2 has a melting point of -0.43 Celsius (31.23 Fahrenheit). This is an example of a disproportionation reaction as O is a -1 state on the left-hand side while it exists in -2 and +0 oxidation states on the right-hand side. It is a pale blue liquid in its standard state and slowly reacts with sunlight and decomposes into water and oxygen.ĢH2O2 → 2H2O + O2 (in the presence of sunlight) It is the simplest peroxide compound, i.e., a molecule containing an Oxygen-Oxygen single bond. H2O2 is a chemical compound with the IUPAC name Hydrogen Peroxide.
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