Silicon is a chemical element with atomic number 14 which means there are 14 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

1. This is a list of the 118 chemical elements which have been identified as of 2021. A chemical element, often simply called an element, is a species of atoms which all have the same number of protons in their atomic nuclei (i.e., the same atomic number, or Z).
2. Si ATOMIC NUMBER 14 ATOMIC MASS 28.0855 FAMILY Group 14 (IVA) Carbon PRONUNCIATION SIL-i-con By the early 1800s, silicon was recognized as an element.

(L. silex, silicis, flint) Davy in 1800 thought silica to be a compound and not anelement; later in 1811, Gay Lussac and Thenard probably prepared impure amorphous siliconby heating potassium with silicon tetrafluoride.

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

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

Silicon makes up 25.7% of the earth's crust, by weight, and is the second most abundantelement, being exceeded only by oxygen. Silicon isnot 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 theoxide appears. Granite, hornblende, asbestos, feldspar, clay, mica, etc. are but a few ofthe 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 orvaporized. The Czochralski process is commonly used to produce single crystals of siliconused for solid-state or semiconductor devices. Hyperpure silicon can be prepared by thethermal decomposition of ultra-pure trichlorosilane in a hydrogen atmosphere, and by avacuum float zone process.

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Silicon 28 Atomic Number

Properties Of Silicon

Silicon (Si), a nonmetallic chemical element in the carbon family (Group 14 [IVa] of the periodic table). Silicon makes up 27.7 percent of Earth’s crust; it is the second most abundant element in the crust, being surpassed only by oxygen.

The name silicon derives from the Latin silex or silicis, meaning “flint” or “hard stone.” Amorphous elemental silicon was first isolated and described as an element in 1824 by Jöns Jacob Berzelius, a Swedish chemist. Impure silicon had already been obtained in 1811. Crystalline elemental silicon was not prepared until 1854, when it was obtained as a product of electrolysis. In the form of rock crystal, however, silicon was familiar to the predynastic Egyptians, who used it for beads and small vases; to the early Chinese; and probably to many others of the ancients. The manufacture of glass containing silica was carried out both by the Egyptians—at least as early as 1500 bce—and by the Phoenicians. Certainly, many of the naturally occurring compounds called silicates were used in various kinds of mortar for construction of dwellings by the earliest people.

Occurrence and distribution

On a weight basis, the abundance of silicon in the crust of Earth is exceeded only by oxygen. Estimates of the cosmic abundance of other elements often are cited in terms of the number of their atoms per 10⁶ atoms of silicon. Only hydrogen, helium, oxygen, neon, nitrogen, and carbon exceed silicon in cosmic abundance. Silicon is believed to be a cosmic product of alpha-particle absorption, at a temperature of about 10⁹K, by the nuclei of carbon-12, oxygen-16, and neon-20. The energy binding the particles that form the nucleus of silicon is about 8.4 million electron volts (MeV) per nucleon (proton or neutron). Compared with the maximum of about 8.7 million electron volts for the nucleus of iron, almost twice as massive as that of silicon, this figure indicates the relative stability of the silicon nucleus.

Silicon Physical Properties

Pure silicon is too reactive to be found in nature, but it is found in practically all rocks as well as in sand, clays, and soils, combined either with oxygen as silica (SiO₂, silicon dioxide) or with oxygen and other elements (e.g., aluminum, magnesium, calcium, sodium, potassium, or iron) as silicates. The oxidized form, as silicon dioxide and particularly as silicates, is also common in Earth’s crust and is an important component of Earth’s mantle. Its compounds also occur in all natural waters, in the atmosphere (as siliceous dust), in many plants, and in the skeletons, tissues, and body fluids of some animals.

In compounds, silicon dioxide occurs both in crystalline minerals (e.g., quartz, cristobalite, tridymite) and amorphous or seemingly amorphous minerals (e.g., agate, opal, chalcedony) in all land areas. The natural silicates are characterized by their abundance, wide distribution, and structural and compositional complexities. Most of the elements of the following groups in the periodic table are found in silicate minerals: Groups 1–6, 13, and 17 (I–IIIa, IIIb–VIb, and VIIa). These elements are said to be lithophilic, or stone-loving. Important silicate minerals include the clays, feldspar, olivine, pyroxene, amphiboles, micas, and zeolites.

Properties of the element

Elemental silicon is produced commercially by the reduction of silica (SiO₂) with coke in an electric furnace, and the impure product is then refined. On a small scale, silicon can be obtained from the oxide by reduction with aluminum. Almost pure silicon is obtained by the reduction of silicon tetrachloride or trichlorosilane. For use in electronic devices, single crystals are grown by slowly withdrawing seed crystals from molten silicon.

Pure silicon is a hard, dark gray solid with a metallic lustre and with a octahedral crystalline structure the same as that of the diamond form of carbon, to which silicon shows many chemical and physical similarities. The reduced bond energy in crystalline silicon renders the element lower melting, softer, and chemically more reactive than diamond. A brown, powdery, amorphous form of silicon has been described that also has a microcrystalline structure.

Because silicon forms chains similar to those formed by carbon, silicon has been studied as a possible base element for silicon organisms. The limited number of silicon atoms that can catenate, however, greatly reduces the number and variety of silicon compounds compared with those of carbon. The oxidation–reduction reactions do not appear to be reversible at ordinary temperatures. Only the 0 and +4 oxidation states of silicon are stable in aqueous systems.

Silicon, like carbon, is relatively inactive at ordinary temperatures; but when heated it reacts vigorously with the halogens (fluorine, chlorine, bromine, and iodine) to form halides and with certain metals to form silicides. As is true with carbon, the bonds in elemental silicon are strong enough to require large energies to activate, or promote, reaction in an acidic medium, so it is unaffected by acids except hydrofluoric. At red heat, silicon is attacked by water vapour or by oxygen, forming a surface layer of silicon dioxide. When silicon and carbon are combined at electric furnace temperatures (2,000–2,600 °C [3,600–4,700 °F]), they form silicon carbide (carborundum, SiC), which is an important abrasive. With hydrogen, silicon forms a series of hydrides, the silanes. When combined with hydrocarbon groups, silicon forms a series of organic silicon compounds.

Three stable isotopes of silicon are known: silicon-28, which makes up 92.21 percent of the element in nature; silicon-29, 4.70 percent; and silicon-30, 3.09 percent. Five radioactive isotopes are known.

Elemental silicon and most silicon-containing compounds appear to be nontoxic. Indeed, human tissue often contains 6 to 90 milligrams of silica (SiO₂) per 100 grams dry weight, and many plants and lower forms of life assimilate silica and use it in their structures. Inhalation of dusts containing alpha SiO₂, however, produces a serious lung disease called silicosis, common among miners, stonecutters, and ceramic workers, unless protective devices are used.

Silicon Period Number