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Thus, deuterium accounts for about 0.0156% by number (0.0312% by mass) of all hydrogen in the ocean: 4.85 × 10 13 tonnes of deuterium – mainly as HOD (or 1 HO 2 H or 1 H 2 HO) and only rarely as D 2 O (or 2 H 2 O) (Deuterium Oxide, also known as Heavy Water)– in 1.4 × 10 18 tonnes of water.
Hydrogen (1 H) has three naturally occurring isotopes: 1 H, 2 H, and 3 H. 1 H and 2 H are stable, while 3 H has a half-life of 12.32(2) years. [3] [nb 1] Heavier isotopes also exist; all are synthetic and have a half-life of less than 1 zeptosecond (10 −21 s). [4] [5] Of these, 5 H is the least stable, while 7 H is the most.
Semiheavy water, HDO, exists whenever there is water with light hydrogen (protium, 1 H) and deuterium (D or 2 H) in the mix. This is because hydrogen atoms (1 H and 2 H) are rapidly exchanged between water molecules. Water containing 50% 1 H and 50% 2 H in its hydrogen, is actually about 50% HDO and 25% each of H 2 O and D 2 O, in dynamic ...
Inputs and outputs of the electrolysis of water production of hydrogen. Electrolysis of water is a conceptually simple method of producing hydrogen. 2 H 2 O(l) → 2 H 2 (g) + O 2 (g) Commercial electrolyzers use nickel-based catalysts in strongly alkaline solution. Platinum is a better catalyst but is expensive. [113]
Natural water consists mainly of the isotopes hydrogen-1 and oxygen-16, but there is also a small quantity of heavier isotopes oxygen-18, oxygen-17, and hydrogen-2 . The percentage of the heavier isotopes is very small, but it still affects the properties of water.
A large molecular dipole, points from a region between the two hydrogen atoms to the oxygen atom. The charge differences cause water molecules to aggregate (the relatively positive areas being attracted to the relatively negative areas). This attraction, hydrogen bonding, explains many of the properties of water, such as its solvent properties ...
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