Hydrogen; Nature, History, Isotopes, Uses, Physical and Chemical Properties

Do you know what the sun or stars are made of? it is HYDROGEN. An element called hydrogen occurs naturally as a molecule. Since a molecule comprises two hydrogen atoms, its chemical formula is H2, with one proton and one electron. Though abundant in the cosmos, it is difficult to get in its native form on Earth. Hydrogen is one of the most vital elements of life then hence before you start knowing anything in Science, it is important to know about Hydrogen.

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Table of Content 
Nature of Hydrogen Gas 
History of Hydrogen Gas 
Isotopes of Hydrogen 
Physical Properties of Hydrogen 
Chemical Properties of Hydrogen
Uses of Hydrogen
 

Nature of Hydrogen Gas

The following is the nature of Hydrogen Gas:

• Very Light 
• Odourless
• Non-toxic
• Highly flammable
• Colourless
• Tasteless
• Non-corrosive

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History of Hydrogen Gas 

Early in the 1500s, the alchemist Paracelsus discovered that adding sulfuric acid to iron fillings resulted in the formation of flammable bubbles. In 1671, Robert Boyle made the same observation. However, none of them ever put their discovery of hydrogen into practice.

 Fe + H2SO4 = Fe SO4  + H2

Henry Cavendish amassed these bubbles in 1766 and established their difference from other gases. He later demonstrated that the primary component of it is water. Following the presence of water, Antoine Lavoisier named his invention "HYDROGEN," which is derived from the Greek terms "hydro" and "genes," which together indicate "water-former."

Water makes up 65% of our body and 71% of the surface of the world. Water has now become a crucial element of life. Its chemical formula is H2O, where a single molecule of water is made up of two hydrogen atoms and one oxygen atom.

2H2 + O2 = 2H2O

Strong hydrogen bonds are seen in the water. A unique kind of dipole-dipole interaction between molecules is the hydrogen bond. It has a 4kJ to 50kJ hydrogen atom per mole strength range.

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Isotopes of Hydrogen 

Isotopes are defined as atoms with the same atomic number but a different mass number. The isotopes of hydrogen are protium, tritium, and deuterium.

The most prevalent isotope in nature is protium(1H). It is deteriorating and only possesses one proton.

Deuterium(2H) is non-radioactive and has one proton and one neutron in its nucleus. Heavy water is an illustration of it. Applications include NMR spectroscopy, nuclear weapons, etc.

Two neutrons and one proton make up tritium (3H). When it comes into touch with atmospheric gases, it emits cosmic rays. It has a radioactive nature. Among the domains of use are the neutron initiator, ocean transient tracer, hydrogen bomb, and nuclear weapons.

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Physical Properties of Hydrogen 

The smallest element, hydrogen, is also the least common to find in pure form because of its high combustibility and reactivity. Other physical characteristics include:

• State: It has a melting point of 14 K and a boiling point of 20 K (-423 0F, -253 0C) (-434 0F, -259 0C).
• Pure hydrogen has no taste, odor, or color and is essentially undetectable in broad daylight.
• It is not poisonous by nature.
• Density: It has a liquid density of 0.70 g/L and a gaseous density of 0.090 g/L.
• Skin freezes when it comes into touch with liquid hydrogen.
• High pressure causes hydrogen to change into crystals that resemble snow.
• It is 14.5 times lighter than air because it is less thick.
• Because of the weak bonds it has with the lattice nodes, its crystal structure is readily broken.
• Hydrogen has a covalent radius of 31.5 pm.
• It has the ability to function as an oxidizing and reducing agent.

Chemical Properties of Hydrogen 

• Atomic number 1 and atomic weight 1,00797 g/mol are assigned to the hydrogen atom.

• H stands for the element hydrogen.

• The chemical formula for hydrogen is H2, with a molecular weight of 2.0159 and a solubility in water of 0.0214 cm3g-1 (00C, 1 atm).

• The temperature for auto-ignition is 500–571 0°C.

• Halides of hydrogen are created when it combines with halogen (HX).

• Where X might be fluorine, chlorine, bromine, or iodine, H2 + X2 = 2HX.
   

Uses of Hydrogen 

• Its liquid hydrogen form is utilized to power spaceships using rocket fuel. Hydrogen or dihydrogen is frequently used in the metallurgical operations of heavy metals, the hydrogenation of vegetable oils, and the production of vanaspati fat.
• It is employed in the production of methanol, HCl, and ammonia, the latter of which is utilized as fertilizer in agriculture. The mechanisms used to produce hydrogen from biomass and fossil fuels are identical.
• It is used to extract organic sulfur from crude oil during the oil-refining process.
• Drinkable water is produced as a byproduct as well.
• It is used in the pharmaceutical industry to make sugar alcohol, or sorbitol, which is utilized in adhesives, surfactants, cosmetics, and other products. Gas grills with propane and lighters with butane are two examples of hydrogen carbon in daily life.
• Hydrocarbon or hydrogen carbon is used as a raw ingredient in the production of rubber, polymers, and plastics.

 

Chemistry is a surprising subject. The surprising finding is that all kinds of hydrogen are bad for life. Some are also harmful. A colourless, toxic, and extremely combustible gas called hydrogen sulphide can cause the central nervous system to malfunction. There is still no antidote for it. Another one of it is carbon monoxide.

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