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Hydrogen is one of the lightest elements. Normal hydrogen is a gas made of diatomic molecules having the formula H2. It has no odour or colour, is non-toxic, and is very flammable. Hydrogen is the most plentiful chemical element in the universe, accounting for around 75% of all ordinary matter. In its plasma form, the Sun, for example, is mainly hydrogen. The majority of hydrogen on the earth exists in the form of molecules such as water and organic compounds. The most common hydrogen isotope (symbol 1H) contains one proton, one electron, and no neutrons. Hydrogen peroxide, the most basic member of the peroxide family, was discovered as a chemical compound in 1818 by French chemist J.L Thenard. Its chemical formula is H2O2.
Formula of Hydrogen peroxide
H2O2 is the formula for the chemical compound hydrogen peroxide. It is a pale blue liquid that is slightly viscous than pure water.
In the environment, hydrogen peroxide can be found in trace concentrations. Photochemical reactions in the earth’s atmosphere produce gaseous hydrogen peroxide. It is used as both a disinfectant and a bleaching agent. At 298 degrees Fahrenheit, it has an acidic pH of 6 to 7.
Properties of Hydrogen peroxide
Hydrogen peroxide is a pale blue liquid when it is anhydrous. It has no odour and is a thick syrupy liquid due to H– bonding.
It has a harsh flavour and produces skin blisters.
It is soluble in water, ethanol, and ether.
The viscosity and density of hydrogen peroxide (1.44g/cm3) are greater than those of water. BecauseH2O2 molecules have stronger H– bonds than H2O molecules, this is the case.
Its boiling point is 150°C and its freezing point is –0.89°C. Because the intermolecular hydrogen bonding in hydrogen peroxide is greater than in water, the boiling point rises even more.
The dipole moment of hydrogen peroxide is somewhat greater (2.1D) than that of water (1.84D).
Hydrogen peroxide, which is diamagnetic, has both polar and nonpolar bonds.
Characteristics of Hydrogen peroxide
H2O2 is a one-of-a-kind material due to its unique molecular structure. It is composed of oxygen atoms in the oxidation state -1, as opposed to the oxidation states 0 or -2 found in many other compounds. This means that, depending on the pH of its solution, this molecule can function as both an oxidising and reducing agent.
Decomposition through light exposure: H2O2 decomposes in the presence of light. As a result, it is maintained in wax-lined glass or plastic vessels containing stabilisers such as urea.
Auto-oxidation and auto-reduction are two terms that are used interchangeably. In its purest form, hydrogen peroxide is an extremely unstable liquid. It decomposes into water and oxygen when left out for an extended period of time or heated.
Metals such as platinum, gold, metal oxides (MnO2), or particular metal ions such as Fe2+ ions accelerate the breakdown process. Even a rough surface aids in its disintegration.
Nature’s Acidity
Because it turns blue litmus red, H2O2 is a weak acid. The aqueous solution has no effect on litmus. Because its dissociation constant (1.5510–12 at 293K) is slightly higher than H2O’s (1.010–14), H2O2 is just marginally stronger than H2O.
The acidic nature of hydrogen peroxide is demonstrated by its neutralising interactions with hydroxides and carbonates. For instance, Ba(OH)2 + H2O2 → BaO2 + 2H2O
H2O2 produces two types of salts since it contains two ionizable H–atoms: hydroperoxides (acidic salts) and peroxides (peroxides) (normal salts).
When strong oxidising agents are present, hydrogen peroxide works as a reducing agent in both acidic and alkaline mediums. In all of these reactions, the combination of H2O2 with the nascent oxygen [O] created by the strong oxidising agent generates molecular oxygen.
H2O2 + [O] (from oxidising agent) → H2O + O2
CONCLUSION
Hydrogen peroxide is an extremely unstable chemical molecule. Hydrogen Peroxide is formed when two molecules of hydrogen react with two molecules of oxygen. As a result, the chemical formula is H2O2. In its pure form, hydrogen peroxide is a pale blue, colourless liquid that is slightly viscous than water. It is the most basic type of peroxide (since it is a compound with an oxygen-oxygen single bond). Hydrogen peroxide is primarily used as an oxidant, bleaching agent, and antiseptic. Concentrated Hydrogen Peroxide, commonly known as “high-test Peroxide,” is a reactive oxygen species that has been utilised as a propellant in rocket propulsion. Because this chemical is unstable, it progressively decomposes in the presence of light. Because hydrogen peroxide is unstable, it is usually stored with a stabiliser in a mildly acidic solution. Peroxidases are enzymes that consume or degrade hydrogen peroxide.
