What Are the Different Isotopes of Hydrogen?
Isotopes of Hydrogen
Protium (1H), Deuterium (2H), and Tritium (3H) are the three naturally occurring isotopes of hydrogen (3H). Four additional isotopes, 4H through 7H, have been identified by scientists and researchers, but they are unstable and do not occur in natural forms. Synthetic isotopes with a lifespan shorter than a zeptosecond, i.e., 10-21 seconds, are used. Protium and Deuterium are categorised as stable hydrogen isotopes. Tritium is a stable radioactive isotope of hydrogen with a half-life of about 12.3 years. 5H is the most stable isotope of hydrogen among the other heavier isotopes, whereas 7H is the least stable.
To minimise difficulties while figuring out chemical formulae, the International Union of Pure and Applied Chemistry (IUPAC) recommends using standard isotopic symbols. Protium, often known as 1H, is the most common isotope of hydrogen, with a single proton in its nucleus. Its atomic number equals its mass number. It’s usually present in ‘s molecular formula. Because monoatomic hydrogen is rare, this diatomic gas is extremely reactive, flammable, and simple to mix with other atoms in various compounds.
With a natural abundance of 99.8%, the H-H bond is the most lasting connection on the earth. Until high temperatures are achieved, it dissociates to a relatively little level. The H-H bond has a dissociation energy of 435.8 kj/mol at 298K, which indicates the strength of the corresponding chemical bond. Protium has an average mass of 1.007825 amu. Several modern ideas on Particle physics suggest that a proton can decay, albeit the process is protracted. Deuterium, sometimes known as 2H, is another stable hydrogen isotope. The electrolytic method of concentration was used to produce pure deuterium. Deuterium’s nucleus, commonly known as the “Deuteron,” is made up of one proton and one neutron, giving it a mass number of two, whereas protium’s nucleus contains no neutrons. As a result, Deuterium has a mass of 2.014102 amu, which is nearly double that of protium. Deuterium is most commonly found in trace amounts as natural deuterium gas, or D2.
It is found in the cosmos coupled with protium 1H atoms to produce the gas Hydrogen deuteride, often known as 1H or simply HD. It is also non-radioactive due to its natural availability, which accounts for approximately 0.0156 percent of all hydrogen found on the globe. Heavy Hydrogen (O) or ‘Deuterium Oxide,’ which is roughly 10.6 percent denser than regular water, is made up of deuterium enriched molecules in water instead of conventional hydrogen. Despite the fact that it is not radioactive, it poses no substantial toxicity risk to humans. However, it can be mildly harmful to multicellular eukaryotic creatures, producing a 25% body water replacement. This can also create serious issues with cell division. It can potentially result in mortality due to bone marrow failure and gastrointestinal lining failure, which is referred to as ‘Cytotoxic syndrome.’ Water fractional distillation can also be used to get deuterium in its concentrated form. Deuterium and tritium chemical bonds are relatively stronger than protium chemical bonds. These variations are sufficient to cause biological responses to alter.
Applications of Deuterium
‘Heavy water’ is also utilised as a neutron moderator and a nuclear reactor coolant. It has the potential to be used as a potential fuel for nuclear fusion, as well as for amateur fusors and neutron generators. It’s also utilised in fusion reactor prototypes. Another application is NMR spectroscopy which is a type of nuclear magnetic resonance spectroscopy. In 1935, Tritium, or 3H, was created by bombarding Deuterium with high-energy deuterons, resulting in 2D+ 2D 1H+ 3T. It is one of the most stable hydrogen radioisotopes. In its nucleus, it has one proton and two neutrons. Tritium can decay into extremely light (low energy) negative beta particles and convert into helium-3, according to scientific expectations. It can be found in trace amounts in natural water. It is constantly produced in the high atmosphere as a result of cosmic ray nuclear reactions and interactions with atmospheric gases. Cosmic rays, which are primarily high-energy protons, interact with nitrogen atoms to produce neutrons. These neutrons then combine with additional nitrogen atoms to produce Tritium, which then falls to the earth’s surface as rain.
Applications of Tritium
The creation of luminous paints. In biological labelling investigations, self-powered lighting systems, or radio luminescent light sources, it is used as a radiolabel. It’s a type of radioactive tracer. In beta, voltaic devices are used to make the atomic batter, which is used to generate energy. Used as a transient tracer in the ocean. Used in the secondary stages of hydrogen bombs.
Heavier Synthetic Isotopes
The nucleus of 4H, or Hydrogen-4, has one proton and three neutrons. Tritium is bombarded with fast-moving deuterium nuclei or deuterons to produce it. It was discovered by detecting the photons it released. It decomposes into Hydrogen-3 through neutron emission. It is a highly unstable Hydrogen isotope. Another unstable hydrogen isotope is 5H, or Hydrogen-5. It has a single proton and four neutrons in its nucleus. By hitting Tritium with fast-moving tritium nuclei, it has been produced or obtained. It has the ability to decay into Hydrogen-3 via double neutron emission. It has a 910 yoctosecond half-life. 6H or Hydrogen-6 decays into Hydrogen-2 via triple or quadruple neutron emission. It has a 290 yoctosecond half-life. It’s insecure and nearly outdated. Hydrogen-7 is made up of one proton and six neutrons. By blasting hydrogen with helium-8 atoms, it was created. It has a 23-yoctosecond half-life.
Learn More: Hydrogen From Class11 Chemistry
