Beryllium (Be)
Beryllium (Be) is a rare and lightweight structural metal, with an atomic number of 4, primarily found in the Earth's igneous rocks at a concentration of about 0.0006 percent. It exists only in mineral form and is not found in its free state in nature, with the main producers being the United States, China, and several African nations. Known for its unique physical properties, beryllium is primarily used in various industrial applications, including alloys for watch springs, welding electrodes, and X-ray tube windows due to its high transparency to X-rays.
The metal is characterized by its steel-gray color, hardness, and brittleness, although it becomes ductile at higher temperatures. With a melting point of 1,285° Celsius and a boiling point of 2,970° Celsius, beryllium is notable for its oxidation resistance and high electrical conductivity. The mining and processing of beryllium can pose health risks, as dust and fumes are toxic, leading to various health issues. Historically, it was discovered as an oxide in 1798 and has since been utilized in a range of applications, including aerospace technology and glass manufacturing, showcasing its versatility and significance in modern industries.
Beryllium (Be)
Where Found
The element beryllium is believed to occur in the Earth’s igneous rocks to the extent of 0.0006 percent. It does not occur in its free state in nature; it is found only in minerals. The leading producers are the United States, China, and some African countries.
Primary Uses
Beryllium has a number of important industrial and structural applications. Its widest use is in the preparation of alloys used in the manufacture of watch springs, welding electrodes, hypodermic needles, dentures, and molds for casting plastics. Metallic beryllium is used to make windows in X-ray tubes because of its high degree of transparency. Finally, beryllium compounds have various uses in glass manufacture, in aircraft spark plugs, and as ultra-high-frequency radar insulators.
Technical Definition
Beryllium (abbreviated Be), atomic number 4, belongs to Group II of the periodic table of the elements and is one of the rarest and lightest structural metals. It has four naturally occurring isotopes and an average atomic weight of 9.0122.
Description, Distribution, and Forms
Pure beryllium is a steel-gray, light, hard, and brittle metal that becomes ductile at higher temperatures and may be rolled into a sheet. Beryllium burns with a brilliant flame, but it becomes oxidized easily and forms a protective coating of the oxide. Beryllium has a density of 1.85 grams per cubic centimeter, a melting point of 1,285° Celsius, and a boiling point of 2,970° Celsius.
Among the elements, beryllium ranks thirty-second in order of abundance. Like lithium, it is usually isolated from silicate minerals. It is believed that its nucleus, like the nucleus of lithium and boron, is destroyed by high-energy protons in the Sun and other stars. As a result it cannot survive the hot, dense interiors of the stars, where elements are formed, which accounts for its low abundance. At least fifty beryllium-containing minerals are known, but only beryl and bertrandite—which contain up to 15 percent beryllium oxide and whose clear varieties are the gems aquamarine and emerald—are the major producers of the metal. The richest beryllium-containing ore deposits are pegmatite varieties of granite rocks. Many beryllium compounds have properties that resemble those of aluminum compounds. Beryllium oxide absorbs carbon dioxide readily and is moisture sensitive. Beryllium hydroxide is a gelatinous precipitate that is easily soluble in acid. All beryllium halides are easily hydrolyzed by water and emit hydrogen halides.
History
Beryllium was discovered as an oxide by Louis-Nicolas Vauquelin during an analysis of emerald in 1798 and was originally named glucinum because of the sweet taste of its salts. It was first isolated as a free metal by Friedrich Wöhler and Antoine Bussy, who reduced beryllium chloride with potassium metal.
Obtaining Beryllium
Beryllium ore is usually converted to a more reactive compound, such as beryllium fluoride, which is then electrolyzed with magnesium. The element is inert with respect to water.
Beryllium exists in the atmosphere of urban and coal-burning neighborhoods in much greater quantities than in rural areas. Dry dust, fumes, and aqueous solutions of the metal compounds are toxic, creating dermatitis, and inhaling them produces the effects of phosgene gas. Its toxicity is believed to result from the substitution of the smaller beryllium atoms for magnesium atoms in enzymes, which are the biochemical catalysts.
Uses of Beryllium
As a result of beryllium’s unusual physical properties, such as its high melting point, high electrical conductivity, high heat capacity, and oxidation resistance, beryllium serves as a component in alloys of elements such as copper, where it adds a high tensile strength to the metal. The added beryllium is no more than 3 percent of the alloy. Beryllium’s ability to transmit X rays seventeen times more effectively than aluminum makes it useful in cases where high-intensity X-ray beams are needed.
Bibliography
U.S. Department of Labor: Occupational Safety and Health Administration.
U.S. Geological Survey.