Sílíkọ́nù

Lát'ọwọ́ Wikipedia, ìwé ìmọ̀ ọ̀fẹ́
Lọ sí: atọ́ka, àwárí
Sílíkọ́nù
14Si
C

Si

Ge
aluminiumsílíkọ́nùphosphorus
Ìhànsójú
crystalline, reflective with bluish-tinged faces


Spectral lines of Silicon
Àwọn ìdámọ́ wíwọ́pọ̀
Orúkọ, àmì-ìdámọ́, nọ́mbà sílíkọ́nù, Si, 14
Ìpèlóhùn /ˈsɪlɪkən/ SIL-ə-kən or /ˈsɪlɪkɒn/ SIL-ə-kon
Ẹ̀ka ẹ́límẹ̀nti metalloid
Ẹgbẹ́, àsìkò, àdìpò 143, p
Ìwúwo átọ́mù 28.085(1)
Ìtòléra ẹ̀lẹ́ktrónì [Ne] 3s2 3p2
2, 8, 4
Electron shells of silicon (2, 8, 4)
Ìtàn
Ìsọtẹ́lẹ̀ Antoine Lavoisier (1787)
Ìwárí Jöns Jacob Berzelius[1][2] (1824)
Ìyàsọ́tọ̀ àkọ́kọ́ Jöns Jacob Berzelius (1824)
Named by Thomas Thomson (1831)
Physical properties
Phase solid
Density (near r.t.) 2.3290 g·cm−3
Liquid density at m.p. 2.57 g·cm−3
Melting point 1687 K, 1414 °C, 2577 °F
Boiling point 3538 K, 3265 °C, 5909 °F
Heat of fusion 50.21 kJ·mol−1
Heat of vaporization 359 kJ·mol−1
Molar heat capacity 19.789 J·mol−1·K−1
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 1908 2102 2339 2636 3021 3537
Atomic properties
Oxidation states 4, 3, 2, 1[3] -1, -2, -3, -4
(amphoteric oxide)
Electronegativity 1.90 (Pauling scale)
Ionization energies
(more)
1st: 786.5 kJ·mol−1
2nd: 1577.1 kJ·mol−1
3rd: 3231.6 kJ·mol−1
Atomic radius 111 pm
Covalent radius 111 pm
Van der Waals radius 210 pm
Miscellanea
Crystal structure diamond cubic
Sílíkọ́nù has a diamond cubic crystal structure
Magnetic ordering diamagnetic[4]
Electrical resistivity (20 °C) 103[5]Ω·m
Thermal conductivity 149 W·m−1·K−1
Thermal expansion (25 °C) 2.6 µm·m−1·K−1
Speed of sound (thin rod) (20 °C) 8433 m·s−1
Young's modulus 130-188[6] GPa
Shear modulus 51-80[6] GPa
Bulk modulus 97.6[6] GPa
Poisson ratio 0.064 - 0.28[6]
Mohs hardness 7
CAS registry number 7440-21-3
Band gap energy at 300 K 1.12 eV
Àwọn ísótòpù dídúró jùlọ
Main article: Àwọn ísótòpù sílíkọ́nù
iso NA half-life DM DE (MeV) DP
28Si 92.23% 28Si is stable with 14 neutrons
29Si 4.67% 29Si is stable with 15 neutrons
30Si 3.1% 30Si is stable with 16 neutrons
32Si trace 153 y β 13.020 32P
· r

Sílíkọ́nù, a tetravalent metalloid, is a chemical element with the symbol Si and atomic number 14. It is less reactive than its chemical analog carbon, the nonmetal directly above it in the periodic table, but more reactive than germanium, the metalloid directly below it in the table. Controversy about silicon's character dates to its discovery: silicon was first prepared and characterized in pure form in 1823. In 1808, it was given the name silicium (from Látìnì: silicis, flints), with an -ium word-ending to suggest a metal, a name which the element retains in several non-English languages. However, its final English name, first suggested in 1817, reflects the more physically similar elements carbon and boron.

Silicon is the eighth most common element in the universe by mass, but very rarely occurs as the pure free element in nature. It is most widely distributed in dusts, sands, planetoids, and planets as various forms of silicon dioxide (silica) or silicates. Over 90% of the Earth's crust is composed of silicate minerals, making silicon the second most abundant element in the Earth's crust (about 28% by mass) after oxygen.[7]

Most silicon is used commercially without being separated, and indeed often with little processing of compounds from nature. These include direct industrial building-use of clays, silica sand and stone. Silica is used in ceramic brick. Silicate goes into Portland cement for mortar and stucco, and when combined with silica sand and gravel, to make concrete. Silicates are also in whiteware ceramics such as porcelain, and in traditional quartz-based soda-lime glass. More modern silicon compounds such as silicon carbide form abrasives and high-strength ceramics. Silicon is the basis of the ubiquitous synthetic silicon-based polymers called silicones.

Elemental silicon also has a large impact on the modern world economy. Although most free silicon is used in the steel refining, aluminum-casting, and fine chemical industries (often to make fumed silica), the relatively small portion of very highly purified silicon that is used in semiconductor electronics (< 10%) is perhaps even more critical. Because of wide use of silicon in integrated circuits, the basis of most computers, a great deal of modern technology depends on it.

Silicon is an essential element in biology, although only tiny traces of it appear to be required by animals,[8] however various sea sponges as well as microorganisms like diatoms need silicon in order to have structure. It is much more important to the metabolism of plants, particularly many grasses.

Itokasi[àtúnṣe | àtúnṣe àmìọ̀rọ̀]

  1. Weeks, Mary Elvira (1932). "The discovery of the elements: XII. Other elements isolated with the aid of potassium and sodium: beryllium, boron, silicon, and aluminum". Journal of Chemical Education: 1386–1412. 
  2. Voronkov, M. G. (2007). "Silicon era". Russian Journal of Applied Chemistry 80 (12): 2190. doi:10.1134/S1070427207120397. 
  3. Ram, R. S. et al. (1998). "Fourier Transform Emission Spectroscopy of the A2D–X2P Transition of SiH and SiD". J. Mol. Spectr. 190: 341–352. PMID 9668026. http://bernath.uwaterloo.ca/media/184.pdf. 
  4. Magnetic susceptibility of the elements and inorganic compounds, in Àdàkọ:RubberBible86th
  5. Physical Properties of Silicon. New Semiconductor Materials. Characteristics and Properties. Ioffe Institute
  6. 6.0 6.1 6.2 6.3 [1] Hopcroft, et al., "What is the Young's Modulus of Silicon?" IEEE Journal of Microelectromechanical Systems, 2010
  7. Nave, R. Abundances of the Elements in the Earth's Crust, Georgia State University
  8. Nielsen, FH (1984). "Ultratrace Elements in Nutrition". Annual Review of Nutrition 4: 21–41. doi:10.1146/annurev.nu.04.070184.000321. PMID 6087860.