Atomic Number: 1
Atomic Symbol: H
Atomic Weight: 1.0079
Electron Configuration: 1
(Gr. hydro, water, and genes, forming)
Hydrogen was prepared many years before it was recognized as a distinct substance by Cavendish in 1776.
It was named by Lavoisier.
Hydrogen is the most abundant of all elements in the universe, and it is thought that the heavier elements were, and still are, being built from hydrogen and helium.
It has been estimated that hydrogen makes up more than 90% of all the atoms or three quarters of the mass of the universe.
It is found in the sun and most stars, and plays an important part in the proton-proton reaction and carbon-nitrogen cycle, which accounts for the energy of the sun and stars.
It is thought that hydrogen is a major component of the planet Jupiter and that at some depth in the planet's interior the pressure is so great that solid molecular hydrogen is converted in solic metalic hydrogen.
In 1973, it was reported that a group of Russian experimenters may have produced metallic hydrogen at a pressure of 2.8 Mbar.
At the transition the density changed from 1.08 to 1.3 g/cm^3.
Earlier, in 1972, a Livermore (California) group also reported on a similar experiment in which they observed a pressure-volume point centered at 2 Mbar.
It has been predicted taht metallic hydrogen may be metastable; others have predicted it would be a superconductor at room temperature.
On earth, hydrogen occurs chiefly in combination with oxygen in water, but it is also present in organic matter such as living plants, petroleum, coal, etc.
It is present as the free element in the atmosphere, but only to the extent of less than 1 ppm by volume.
It is the lightest of all gases, and combines with other elements, sometimes explosively, to form compounds.
Great quantities are required commercially for the fixation of nitrogen form the air in the Haber ammonia process and for the hydrogenation of fats and oils.
It is alos used in large quantities in methanol production, in hydrodealkylation, hydrocracking, and hydrodesulfurization.,
It is also used as a rocket fuel, for welding, for production of hydrochloric acid, for the reduction of metallic ores, and for filling baloons.
The lifting power of 1 ft^3 of hydrogen gas is about 0.07 lb at 0C, 760 mm pressure.
Production of hydrogen in the U.S. alone now amounts to about 3 billion cubic feet per year.
It is prepared by the action of steam on heated carbon, by decomposition of certain hydrocarbons with heat, by electolysis of water, or by the displacement from acids by certain metals.
It is also produced by the action of sodium or potassium hydroxide on aluminum.
Liquid hydrogen is important in cryrogenics and in the study of superconductivity, as its melting point is only 20 degrees above absolute zero.
The ordinary isotope of hydrogen, H, is known as protium.
In 1932 Urey announced the preparation of a stable isotope, deuterium (2H or D) with an atomic weight of 2.
Two years later an unstable isotope, tritium, with atomic weight of 3 was discovered.
Tritium has a half-life of about 12.5 years.
One atom of deuterium is found in about 6000 ordinary hydrogen atoms.
Tritium atoms are also present but in much smaller proportion.
Tritium is readily produced in nuclear reactors and is used in the production of the hydrogen bomb.
It is also used as a radioactive agent in making luminous paints, and as a tracer.
The current price of tritium, to authorized personnel, is about $2/Ci; deuterium gas is readily available, without permit, at about $1/l.
Heavy water, deuterium oxide (D2O), which is used as a moderator to slow down neutrons, is available without permit at a cost of 6c to $1/g, depending on quantity and purity.
Quite apart from isotopes, it has been shown that hydrogen gas under ordinary conditions is a mixture of two kinds of molecules, known as ortho- and para-hydrogen, which differ from one another by the spins of their electrons and nuclei.
Normal hydrogen at room temperature contains 25% of the para form and 75% of the ortho form.
The ortho form cannot be prepared in the pure state.
Since the two forms differ in energy, the physical properties also differ.
The melting and boiling points of parahydrogen are about 0.1C lower than those of normal hydrogen.
Consideration is being given to an entire economy based on solar- and nuclear-generated hydrogen.
Located in remote regions, power plants would electrolyze sea water; the hydrogen produced would travel to distant cities by pipelines.
Pollution-free hydrogen could replace natural gas, gasoline, etc., and could serve as a reducing agent in metallurgy, chemical processing, refining, etc.
It could also be used to convert trash into methane and ethylene. Public acceptance, high capital investment, and the high present cost of hydrogen with respect to present fuels are but a few of the problems facing establishment of such an econonomy.
Isotopes: The ordinary isotope of hydrogen, H, is known as Protium, the other two isotopes are Deuterium and Tritium. Hydrogen is the only element whose isotopes have been given different names. Deuterium and Tritium are both used as fuel
for nuclear fusion reactors. One atom of Deuterium is found in about 6000 ordinary hydrogen atoms. Deuterium is used as a moderator to slow down neutrons. Tritium atoms are also present but in much smaller proportions. Tritium is readily produced in n
uclear reactors and is used in the production of the hydrogen (fusion) bomb. It is also used as a radioactive agent in making luminous paints, and as a tracer.