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Silicon


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Atomic symbol: Si
Atomic number: 14
Atomic weight: 28.0855
Atomic volume: 12.1 cm3/mol
Density: 2.33 g/cm3
Period Number: 3
Group number: 14
Group name: Non-Metal, Carbon group
Element classification: Semi-metal


States


Phase at room temperature: Solid
Melting Point: 1683.2 K
Boiling point: 3553 K
Heat of fusion: 50.550 kJ/mol
Heat of vaporization: 384.220 kJ/mol


Energies


Ionization Energy: 8.152 eV
1st ionization energy: 786.4 kJ/mole
2nd ionization energy: 1577 kJ/mole
3rd ionization energy: 3231.5 kJ/mole
Electronegativity: 1.9
Electron affinity: 133.6 kJ/mole
Specific heat: 0.71 J/gK
Heat atomization: 452 kJ/mole atoms


Oxidation & Electrons


Shells: 2,8,4
Electron Shell Configuration: [Ne] 3s2 3p2
Minimum oxidation number: -4
Maximum oxidation number: 4
Minimum common oxidation number: -4
Maximum common oxidation no: 4


Appearance & Characteristics


Structure:: diamond
Color: gray-black
Hardness: 7 mohs
Toxicity: ?
Characteristics: semimetal
Uses: comp chip,lubricant,glass


Reactions


Reaction with air: mild, =>SiO2
Reaction with 6M HCl: none
Reaction with 15M HNO3: none
Reaction with 6M NaOH: mild, =>silicates


Other Forms


Number of isotopes: 3
Oxide(s): SiO2
Hydride(s): SiH4 Si2H6 + more
Chloride(s): SiCl4 Si2Cl6 + more


Radius


Atomic Radius: 117.6 pm
Ionic radius (1- ion): pm
Ionic radius (1+ ion): pm
Ionic radius (2- ion): pm
Ionic radius (2+ ion): pm
Ionic radius (3+ ion): pm


Conductivity


Thermal conductivity: 149 J/m-sec-deg
Electrical conductivity: 0.012 1/mohm-cm
Polarizability: 5.4 A^3


Abundance


Source: Quartz (oxide)
Relative abundance solar system: 6.000 log
Abundance earth's crust: 5.5 log
Estimated crustal abundance: 2.82×105 milligrams per kilogram
Estimated oceanic abundance: 2.2 milligrams per liter
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 


History


(L. silex: silicis, flint) In 1800, Davy thought silica to be a compound and not an element; but in 1811, Gay Lussac and Thenard probably prepared impure amorphous silicon by heating potassium with silicon tetrafluoride.

In 1824 Berzelius, generally credited with the discovery, prepared amorphous silicon by the same general method and purified the product by removing the fluosilicates by repeated washings. Deville in 1854 first prepared crystalline silicon, the second allotropic form of the element.


Sources


Silicon is present in the sun and stars and is a principal component of a class of meteorites known as aerolites. It is also a component of tektites, a natural glass of uncertain origin.

Silicon makes up 25.7% of the earth's crust, by weight, and is the second most abundant element, being exceeded only by oxygen. Silicon is not found free in nature, but occurs chiefly as the oxide and as silicates. Sand, quartz, rock crystal, amethyst, agate, flint, jasper, and opal are some of the forms in which the oxide appears. Granite, hornblende, asbestos, feldspar, clay, mica, etc. are but a few of the numerous silicate minerals.

Silicon is prepared commercially by heating silica and carbon in an electric furnace, using carbon electrodes. Several other methods can be used for preparing the element. Amorphous silicon can be prepared as a brown powder, which can be easily melted or vaporized. The Czochralski process is commonly used to produce single crystals of silicon used for solid-state or semiconductor devices. Hyperpure silicon can be prepared by the thermal decomposition of ultra-pure trichlorosilane in a hydrogen atmosphere, and by a vacuum float zone process.


Properties


Crystalline silicon has a metallic luster and grayish color. Silicon is a relatively inert element, but it is attacked by halogens and dilute alkali. Most acids, except hydrofluoric, do not affect it. Elemental silicon transmits more than 95% of all wavelengths of infrared, from 1.3 to 6.y micro-m.


Uses


Silicon is one of man's most useful elements. In the form of sand and clay it is used to make concrete and brick; it is a useful refractory material for high-temperature work, and in the form of silicates it is used in making enamels, pottery, etc. Silica, as sand, is a principal ingredient of glass, one of the most inexpensive of materials with excellent mechanical, optical, thermal, and electrical properties. Glass can be made in a very great variety of shapes, and is used as containers, window glass, insulators, and thousands of other uses. Silicon tetrachloride can be used as iridize glass.

Hyperpure silicon can be doped with boron, gallium, phosphorus, or arsenic to produce silicon for use in transistors, solar cells, rectifiers, and other solid-state devices which are used extensively in the electronics and space-age industries.

Hydrogenated amorphous silicon has shown promise in producing economical cells for converting solar energy into electricity.

Silicon is important to plant and animal life. Diatoms in both fresh and salt water extract Silica from the water to build their cell walls. Silica is present in the ashes of plants and in the human skeleton. Silicon is an important ingredient in steel; silicon carbide is one of the most important abrasives and has been used in lasers to produce coherent light of 4560 A.

Silcones are important products of silicon. They may be prepared by hydrolyzing a silicon organic chloride, such as dimethyl silicon chloride. Hydrolysis and condensation of various substituted chlorosilanes can be used to produce a very great number of polymeric products, or silicones, ranging from liquids to hard, glasslike solids with many useful properties.

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