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Deuterium-depleted water has less deuterium (2 H) than occurs in nature at sea level. [1] Deuterium is a naturally-occurring, stable (non-radioactive) isotope of hydrogen with a nucleus consisting of one proton and one neutron. A nucleus of normal hydrogen (protium, 1 H) consists of one proton only, and no neutron.
Other natural processes are thought to produce only an insignificant amount of deuterium. Nearly all deuterium found in nature was produced in the Big Bang 13.8 billion years ago, as the basic or primordial ratio of 2 H to 1 H (≈26 atoms of deuterium per 10 6 hydrogen atoms) has its origin from that time. This is the ratio found in the gas ...
The concept of replacing hydrogen with deuterium is an example of bioisosterism, whereby similar biological effects to a known drug are produced in an analog designed to confer superior properties. [5] The first patent in the US granted for deuterated molecules was in the 1970s. Since then patents on deuterated drugs have become more common. [6]
Since one in about every 6,400 hydrogen atoms is deuterium, a 50-kilogram (110 lb) human containing 32 kilograms (71 lb) of body water would normally contain enough deuterium (about 1.1 grams or 0.039 ounces) to make 5.5 grams (0.19 oz) of pure heavy water, so roughly this dose is required to double the amount of deuterium in the body.
The kinetic isotopic effect of substitution of deuterium for hydrogen within the caffeine molecule and its potential role in altering caffeine’s pharmacokinetics was first described by Horning et al., [7] which demonstrated d9-caffeine to have a prolonged half-life in rodents relative to regular caffeine. Subsequent in vitro experiments with ...
Deuterium (2 H) has one neutron, and tritium (3 H) has two. Neutrons add mass to the atom, leading to different chemical physical properties. This effect is especially strong for hydrogen isotopes, since the added neutron doubles the mass from 1 H to 2 H. For heavier elements like carbon, nitrogen, oxygen, or sulfur, the mass difference is diluted.
Heavy isotope diet is the consumption of nutrients in which some atoms are replaced with their heavier non-radioactive isotopes, such as deuterium (2 H) or heavy carbon (13 C). Biomolecules that incorporate heavier isotopes give rise to more stable molecular structures under certain circumstances, which is hypothesized to increase resistance to ...
However, deuterium (the second label in the doubly labeled water) is lost only when body water is lost. Thus, the loss of deuterium in body water over time can be used to mathematically compensate for the loss of 18 O by the water-loss route. This leaves only the remaining net loss of 18 O in carbon dioxide. This measurement of the amount of ...