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Hydrogen is a chemical element with the symbol H and the atomic number 1. Hydrogen is the lightest element. Hydrogen is a gas made of diatomic molecules with the formula H2 under normal conditions. It has no odour, no colour, is non-toxic, and is very combustible. Hydrogen is the most prevalent chemical element in the universe, making up roughly 75% of all ordinary matter.
Hydrogen Peroxide
Hydrogen peroxide is the most basic member of the peroxide family, having been discovered as a chemical compound in 1818 by French chemist J.L Thenard. Its chemical formula is H2O2. In the environment, hydrogen peroxide is found in extremely small concentrations. Gaseous hydrogen peroxide is produced by photochemical processes in the earth’s atmosphere. It serves as both a disinfectant and a bleaching agent. At 298 degrees Fahrenheit, it’s acidic, with a pH of 6 to 7.
Structure of H2O2
Peroxide, a chemical molecule, contains the peroxide ion (O2–2). The peroxide ion (O–O)2– is formed by a single bond between two oxygen atoms. It’s a very strong oxidant.
Hydrogen peroxide is a non-planar molecule made up of two oxygen atoms bonded together by a single covalent bond called the peroxide bond.
It’s formatted like a book. Each oxygen atom has a single connection connecting it to a hydrogen atom. The two bonds do not lie in the same plane because single pairs of electrons repel each other over oxygen atoms. The dihedral (interplanar) angle between two planes is 111.5o when hydrogen peroxide is gaseous, but 90.2o when it is crystalline. This is caused by intramolecular hydrogen bonding.
Preparation of Hydrogen Peroxide
Laboratory Method:
We get hydrogen peroxide when barium peroxide is acidified and the extra water is eliminated by evaporation under lower pressure. This will be clarified by the following reaction:
BaO28H2O(s)+H2SO4(aq) —> BaSO4(s)+H2O2(aq)+8H2O(I)
Industrial Method
The electrolysis of 30 percent ice-cold H2SO4 produces hydrogen peroxide. Peroxodisulphate is produced by electrolyzing an acidified sulphate solution at a high current density. Hydrolysis of peroxodisulphate yields hydrogen peroxide.
2HSO- (aq)[Electrolysis] →HO3 SOOSO3H(aq)[Hydrolysis]→2HSO-4(aq)+2H++H2O2(aq)
Physical properties
Hydrogen peroxide is a pale blue tint in its anhydrous state. It’s an odourless, viscous, syrupy liquid due to H– bonding.
It has a harsh flavour that creates blisters on the skin.
It is soluble in water, alcohol, and ether.
Water is less viscous and denser (1.44g/cm3) than hydrogen peroxide. Because H2O2 molecules have stronger H– bonds than H2O molecules, this occurs.
Its boiling point is 150 degrees Celsius, whereas its freezing point is –0.89 degrees Celsius. Because hydrogen peroxide’s intermolecular hydrogen bonding is stronger than that of water, its boiling point increases even higher.
The dipole moment of hydrogen peroxide (2.1D) is somewhat higher than that of water (1.84D).
Hydrogen peroxide is diamagnetic and has both polar and nonpolar bonds.
Uses of Hydrogen Peroxide
Hydrogen peroxide is a liquid that has a wide range of applications. It operates in a variety of environments, namely water, air, wastewater, and soils. It is sometimes used with other agents to improve and accelerate processes. Some of its applications are as follows:
The bleaching of pulp and paper consumes over half of the world’s hydrogen peroxide production.
Human hair is bleached using a mixture of diluted hydrogen peroxide and aqueous ammonia.
Hydrogen peroxide is used to eliminate new bloodstains.
Torpedoes and submarines use H2O2 solution as a propellant, and rocket fuel uses it as an oxidant.
Hydrogen peroxide is used in aquaculture to reduce mortality caused by certain bacteria.
It can be used to sanitise toothbrushes and sterilise cosmetic brushes.
Hydrogen peroxide is a moderate antiseptic which can be used to prevent infection in tiny cuts, scratches, and burns.
It can also be used to remove mucus and relieve minor mouth irritation as a mouthwash.
Helps clear algae-infested ponds and treat fungal infections in plants.
It’s used as an antichlor in the textile industry to remove excess chlorine after bleaching.
It’s used to make inorganic chemicals like sodium perborate and percarbonate, both of which are significant components of high-quality detergents.
Conclusion
When hydrogen peroxide is used correctly, most people are safe. However, if a person consumes the chemical in large quantities or too regularly, it might be harmful. It’s vital to use a concentration of no more than 3% and to use it sparingly to minimise discomfort. Children should not handle hydrogen peroxide because it poses a risk of ingesting.
