| Revision as of 09:52, 13 October 2002 view sourceMav (talk | contribs)Extended confirmed users77,874 edits nl:Waterstof← Previous edit | Revision as of 01:24, 14 October 2002 view source 212.229.115.84 (talk)m Mentioned point about reacting with F and ClNext edit → | ||
| Line 106: | Line 106: | ||
| Hydrogen has two stable isotopes: ] with one ] and no ]s (H-1) and ] with one proton and one neutron (H-2, D). Deuterium comprises 0.0184-0.0082% of all hydrogen (]); ratios of deuterium to protium are reported relative to the ] standard reference water. A radioactive isotope, ] (T or H-3) is another isotope and has one proton and two neutrons. | Hydrogen has two stable isotopes: ] with one ] and no ]s (H-1) and ] with one proton and one neutron (H-2, D). Deuterium comprises 0.0184-0.0082% of all hydrogen (]); ratios of deuterium to protium are reported relative to the ] standard reference water. A radioactive isotope, ] (T or H-3) is another isotope and has one proton and two neutrons. | ||
| == Precautions == | == Precautions == | ||
| <font color="red">Hydrogen is a highly ] gas.</font> | <font color="red">Hydrogen is a highly ] gas. It also reacts violently with ] and ]</font> | ||
| D<sub>2</sub>O, or ], is toxic to many species. The quantity required to kill a human, however, is substantial. | D<sub>2</sub>O, or ], is toxic to many species. The quantity required to kill a human, however, is substantial. | ||
Revision as of 01:24, 14 October 2002
]
Hydrogen is a chemical element in the periodic table that has the symbol H and atomic number 1.
Notable Characteristics
At standard temperature and pressure conditions, hydrogen forms a diatomic gas, H2, with a boiling point of only 20.27 K and a melting point of 14.02 K. Under exceedingly high pressures, like those found at the center of gas giants, the molecules lose their identity and the hydrogen becomes a liquid metal. Under the exceedingly low pressure conditions found in space, hydrogen tends to exist as individual atoms, simply because there is no way for them to combine; clouds of H2 form and are associated with star formation.
Applications
Large quantities of hydrogen are needed industrially, notably in the Haber process for the production of ammonia, the hydrogenation of fats and oils, and the production of methanol. Other industrial processes include hydrodealkylation, hydrodesulfurization, and hydrocracking. Other industrial uses include the manufacture of hydrochloric acid, welding, rocket fuels, and the reduction of metallic ores.
Hydrogen has been used as a lifting agent in balloons and zeppelins.
Hydrogen can be burned in internal combustion engines, and a fleet of hydrogen burning cars is maintained by Chrysler-BMW. Hydrogen fuel cells are being looked into as a way to provide potentially cheap, pollution- free power.
Deuterium is used in nuclear applications as a moderator to slow down neutrons, and deuterium compounds have applications in chemistry and biology in studies of reaction isotope effects. Tritium is used as an isotopic label in the biosciences, as a radiation source in luminous paints, and in making hydrogen bombs.
History
Hydrogen (French for water-maker, from Greek hudôr, "water and gennen "generate") was first recognized as a distinct substance in 1776 by Henry Cavendish. Antoine Lavoisier gave the element its name.
Occurrence
Hydrogen is the most abundant element in the universe, making up around 75% of normal matter (some sources claim 90%). Hydrogen is the lightest chemical element; its atoms consist of a single proton and electron. The most common isotope has no neutrons, although there are two others - deuterium with one, and radioactive tritium with two neutrons.
Compounds
Hydrogen has an electronegativity of 2.2, so it forms compounds where it is the more non-metallic and where it is the more metallic element. The former are called hydrides, where hydrogen either exists as H ions or just as a solute within the other element (as in Palladium hydride). The latter tend to be covalent, since the H ion would be a bare nucleus and so has a strong tendency to pull electrons to itself. Thus even in an acidic solution one sees ions like H3O as the protons latch on to something.
Hydrogen combines with oxygen to form water, H2O, and releases a lot of energy in doing so, burning explosively in air. Deuterium oxide, or D2O, is commonly referred to as heavy water.
Hydrogen forms a vast array of compounds with carbon. Because of their association with living things, these compounds are called organic compounds, and the study of the properties of these compounds is called organic chemistry.
Isotopes
Hydrogen has two stable isotopes: protium with one proton and no neutrons (H-1) and deuterium with one proton and one neutron (H-2, D). Deuterium comprises 0.0184-0.0082% of all hydrogen (IUPAC); ratios of deuterium to protium are reported relative to the VSMOW standard reference water. A radioactive isotope, tritium (T or H-3) is another isotope and has one proton and two neutrons.
Precautions
Hydrogen is a highly flammable gas. It also reacts violently with chlorine and fluorine
D2O, or heavy water, is toxic to many species. The quantity required to kill a human, however, is substantial.
See also: Periodic Table, hydrogen bond, hydrogen atom, Antihydrogen