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Beryllium


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Atomic symbol: Be
Atomic number: 4
Atomic weight: 9.01218
Atomic volume: 5.0 cm3/mol
Density: 1.848 g/cm3
Period Number: 2
Group number: 2
Group name: Alkali Earth
Element classification: Metal


States


Phase at room temperature: Solid
Melting Point: 1551.2 K
Boiling point: 2773 K
Heat of fusion: 12.20 kJ/mol
Heat of vaporization: 292.40 kJ/mol


Energies


Ionization Energy: 9.323 eV
1st ionization energy: 899.4 kJ/mole
2nd ionization energy: 1757.1 kJ/mole
3rd ionization energy: 14848.3 kJ/mole
Electronegativity: 1.57
Electron affinity: kJ/mole
Specific heat: 1.82 J/gK
Heat atomization: 324 kJ/mole atoms


Oxidation & Electrons


Shells: 2,2
Electron Shell Configuration: [He] 2s2
Minimum oxidation number: 0
Maximum oxidation number: 2
Minimum common oxidation number: 0
Maximum common oxidation no: 2


Appearance & Characteristics


Structure:: hcp: hexagonal close pkd
Color: steel gray
Hardness: mohs
Toxicity: yes
Characteristics: toxic
Uses: Cu alloys, X-ray windows


Reactions


Reaction with air: vigorous, w/ht=>BeO,Be3N2
Reaction with 6M HCl: mild, =>H2
Reaction with 15M HNO3: none
Reaction with 6M NaOH: mild, =>H2, [Be(OH)4](2-)


Other Forms


Number of isotopes: 1
Oxide(s): BeO
Hydride(s): BeH2
Chloride(s): BeCl2


Radius


Atomic Radius: 112 pm
Ionic radius (1- ion): pm
Ionic radius (1+ ion): pm
Ionic radius (2- ion): pm
Ionic radius (2+ ion): 59 pm
Ionic radius (3+ ion): pm


Conductivity


Thermal conductivity: 201 J/m-sec-deg
Electrical conductivity: 250 1/mohm-cm
Polarizability: 5.6 A^3


Abundance


Source: Beryl (silicate)
Relative abundance solar system: -0.137 log
Abundance earth's crust: 0.4 log
Estimated crustal abundance: 2.8 milligrams per kilogram
Estimated oceanic abundance: 5.6×10-6 milligrams per liter
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 


History


(Gr. beryllos: beryl; also called Glucinium or Glucinum, Gr. glykys: sweet) Discovered in the oxide form by Vauquelin in both beryl and emeralds in 1798. The metal was isolated in 1828 by Wohler and by Bussy independently by the action of potassium on beryllium chloride.


Sources


Beryllium is found in some 30 mineral species, the most important of which are bertrandite, beryl, chrysoberyl, and phenacite. Aquamarine and emerald are precious forms of beryl. Beryl and bertrandite are the most important commercial sources of the element and its compounds. Most of the metal is now prepared by reducing beryllium fluoride with magnesium metal. Beryllium metal did not become readily available to industry until 1957.


Properties


The metal, steel gray in color, has many desirable properties. As one of the lightest of all metals, it has one of the highest melting points of the light metals. Its modulus of elasticity is about one third greater than that of steel. It resists attack by concentrated nitric acid, has excellent thermal conductivity, and is nonmagnetic. It has a high permeability to X-rays and when bombarded by alpha particles, as from radium or polonium, neutrons are produced in the amount of about 30 neutrons/million alpha particles.

At ordinary temperatures, beryllium resists oxidation in air, although its ability to scratch glass is probably due to the formation of a thin layer of the oxide.


Uses


Beryllium is used as an alloying agent in producing beryllium copper, which is extensively used for springs, electrical contacts, spot-welding electrodes, and non-sparking tools. It is applied as a structural material for high-speed aircraft, missiles, spacecraft, and communication satellites. Other uses include windshield frame, brake discs, support beams, and other structural components of the space shuttle.

Because beryllium is relatively transparent to X-rays, ultra-thin Be-foil is finding use in X-ray lithography for reproduction of micro-miniature integrated circuits.

Beryllium is used in nuclear reactors as a reflector or moderator for it has a low thermal neutron absorption cross section.

It is used in gyroscopes, computer parts, and instruments where lightness, stiffness, and dimensional stability are required. The oxide has a very high melting point and is also used in nuclear work and ceramic applications.

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