Natural abundance

Natural abundance

Deuterium occurs in trace amounts naturally as deuterium gas, written as ²H₂ or D₂. However, most deuterium atoms in the universe are bonded with typical ¹H atoms to form the gas called hydrogen deuteride (HD or ¹H²H).

The abundance of deuterium in the oceans  of Earth  is approximately one atom in 6500 hydrogen atoms (about 154 parts per million (ppm)). Deuterium thus accounts for approximately 0.015 percent (on a weight basis, 0.030 percent) of all naturally occurring hydrogen atoms in the oceans on Earth; the abundance changes slightly from one kind of natural water to another.The abundance of deuterium on Jupiter is about 6 atoms in 10,000 (0.06 percent atom basis). There is little deuterium in the interior of the sun , because thermonuclear reactions destroy it. However, it persists in the outer solar atmosphere at roughly the same concentration as in Jupiter.

The existence of deuterium on Earth, elsewhere in the Solar system  (as confirmed by planetary probes), and in  stars (as indicated by their spectra), is an important piece of information in cosmology. Stellar fusion destroys deuterium, and there are no known natural processes (such as cluster decay), other than the Big Bang nucleosynthesis process, which might have produced deuterium at anything close to its observed natural abundance. This abundance seems to be a very similar fraction of hydrogen, wherever hydrogen is found. Thus, the existence of deuterium at its present abundance is one of the arguments in favor of the    Big Bang theory over the steady state theory of the universe. It is estimated that the abundances of deuterium have not changed significantly since their production more than 14 billion years ago.

The world's leading "producer" of deuterium (technically, enricher or concentrator of deuterium) was Canada, until 1997, when the last plant was shut down. Canada uses heavy water as a neutron moderator for the operation of its CANDU reactors. Currently, India is probably the world's largest concentrator of heavy water, also used in nuclear power reactors.

Ref: http://www.newworldencyclopedia.org/entry/Deuterium

Uses of Deuterium

Uses of Deuterium

 Deuterium is known also as heavy hydrogen, because of the greater molecular mass. Combining deuterium with oxygen you get heavy water (D2O), which in in raised quantities has negative biological effects.

Heavy water was produced for the first time in 1932, a few months after the discovery of deuterium. Once nuclear was discovered in 1938, a neutron moderator was needed to capture neutrons. This is how heavy water became an important component of the early nuclear energy programs.

Deuterium is used in chemistry, biochemistry, environmental sciences, hydrology, due to its reactive properties and the differences between deuterium and hydrogen.

Ref.: http://qlariviawater.com/en/uses-of-deuterium

 

Negative effects of Deuterium

Negative effects of Deuterium

Studies on deuterium and heavy water showed that these have negative effects on the immune system: a raised quantity of deuterium in the organism reduces the number of leukocytes in the blood and weakens the organism's response capacity to disturbances.

Experiments conducted on rodents showed that a high level of deuterium of as much as 25% in the body water causes sterility, because neither the gametes nor the zygotes can develop. Higher concentrations of heavy water kills fish, amphibians and insects.

Small mammals such as rodents die after approximately a week of consuming heavy water. The cause of death is similar to that of cytotoxic poisoning (the case of chemotherapy) or acute radiation syndrome. 

 Ref.: http://qlariviawater.com/en/deuterium-properties

Deuterium in nature

 

Deuterium in nature

The deuterium content of waters in our climate area is 150 ppm (parts per million), with a minimal fluctuation; of waters at the Equator - 155 ppm and of waters in northern Canada - 135 ppm. The deuterium quantity in the water varies according to latitude, but also altitude (with a value of 150 ppm at sea level and 130 ppm at 2000 meters). The deuterium quantity measured in the water in a certain geographic area is proportional to the deuterium concentration in the organisms that live in that area.

 

The deuterium concentration in an adult organism is of about 12-14 mmol/l (milimoles per liter). Although it doesn't seem much, compared to the masses of other vital elements in the blood, deuterium is approximately six times less than calcium and ten times less than magnesium.

Ref.: http://qlariviawater.com/en/deuterium-properties

 

 

 

Deuterium properties

Deuterium properties

Deuterium can have kinetic isotopic effects different than hydrogen has, and the physical and chemical properties of the deuterium compounds differ from those of hydrogen compounds. For example, D2O (heavy water) is more viscous and heavier than H2O (normal water).

Heavy water is approximately 10% more dense than normal water, enough for the ice formed of heavy water to sink in normal water.

The differences in connection energies and lengths of hydrogen isotope compounds are greater than the isotopic differences for any other element. The bonds between deuterium and tritium are stronger than those with hydrogen, these differences being enough to produce important changes in biological reactions.

Heavy water is toxic to eukaryotic organisms. If 25% of the water in the organisms is replaced by heavy water, problems in cell division and reproduction appear. If 50% of the water is replaced, the eukaryotic organisms die.

Ref.: http://qlariviawater.com/en/deuterium-properties

 

Deuterium Structure

Deuterium

Deuterium is one of the two hydrogen isotopes. The nucleus of most hydrogen atoms in nature contains one proton (chemical symbol: 1H), but the nucleus of some hydrogen atoms can contain one proton and one neutron or one proton and two neurons. In the first case, it is called deuterium (chemical symbol: 2H or D), and the second - tritium (chemical symbol: 3H or T).

The abundance of deuterium in the water on Earth is approximately one deuterium atom to 6.400 hydrogen atoms (156,25 parts per million-ppm), or 0.0156%. This deuterium concentration changes very little from a natural water source to another.

The deuterium concentration in the adult body is of approximately 120 to 140 ppm. Although it doesn't seem much, if we compare this quantity to the mass of other vital elements in the blood, we can see that deuterium is present in an amount six times greater than calcium and ten times greater than magnesium.

Ref:http://qlariviawater.com/en/what-is-deuterium

 

 

 

 

deuterium labeling

 deuterium labeling

 

Deuterium

Deuterium (chemical symbol D or ²H) is a stable isotope of hydrogen, found in extremely small amounts in nature. The nucleus of deuterium, called a deuteron, contains one proton and one  neutron, whereas the far more common hydrogen nucleus contains just one proton and no neutrons. Consequently, each atom of deuterium has roughly twice the  mass of an ordinary hydrogen atom, and deuterium is also called heavy hydrogen. water in which ordinary hydrogen atoms are replaced by deuterium atoms is known as heavy water.

Ref: http://www.newworldencyclopedia.org/entry/Deuterium