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Element information, Properties, Uses, Facts

Silicon Element Information

Silicon (Si), an important nonmetallic chemical element in the carbon family or Group 14 (IVA) of the periodic table uses as principal building materials of our civilization in the form of stones, sand, and clays. It is the second most abundant element after oxygen in the earth’s crust.

Position of metalloid Silicon on the periodic table elements

Silicon forms face-centered diamond-type cubic crystal lattice. Due to the larger size and weaker bond energy, the meting point of silicon lower than that of carbon. The trends of properties of group 14 elements may be largely understood from the valence shell electronic configuration. Some important atomic and physical properties of silicon are summarized below the table.

Silicon element chemical symbol and periodic table properties

Properties of Silicon
Atomic number 14
Atomic weight 28.085
Electronic Configuration [He] 3s2 3p2
Melting point 1414 °C, ​2577 °F
Boiling point 3265 °C, ​5909 °F
Density 2.3290 g/cm3
Oxidation number or states +4 and +2
Ionization energy 1st – 786.5 kJ/mol
2nd – 1577.1 kJ/mol
3rd – 3231.6 kJ/mol

Occurrence and Production

Silicon is the second most abundant element after oxygen that contains 27.6 percent of the earth’s crust but it cannot found free in nature. It has a high affinity for oxygen forming the stable SiO4 unit which combines with another to form a variety of silicates. Silica and silicates occur widely in the sand, clays, and various silicate minerals.

Silicon is produced by reducing SiO2 (sand) by high pure coke (carbon) in an electric arc furnace (SiO2 + 2C → Si + 2CO). The formation of SiC was prevented by using excess SiO2. The product is nearly 96 to 97 percent pure. It was purified by converting SiCl4. The compound SiCl4 was purified by distillation and reduced by magnesium and zinc to produced pure silicon. Super pure silicon used in the electronics industry can be obtained by zone refining.

Properties and Compounds

Silicon crystallizes like diamond form with Si-Si distance in the crystalline solid equal to 235 pm. At very high pressure, a denser distorted form may be produced, but Si-Si distance remains practically unchanged. The sum of four ionization energies for silicon is very high. Therefore, attaining a noble gas configuration by losing four electrons is unfavorable. In most cases, it attains by the formation of four covalent bonding with sp3 hybridization.

Multiple chemical bonding also formed by using its vacant 3d-orbital and filled p-orbital with oxygen, nitrogen, or halogens atom. It makes silicon compounds stereochemistry different from their carbon analogs. For example, (SiH3)3N is planar against tetrahedral (CH3)3N. The chemical behavior and compounds of Group-14 elements dominated under +4 and +2 oxidation states.


All the elements of Group-14 formed covalent volatile hydrides but the tendency of formation decreases down the group. Due to the strong tendency of catenation carbon formed a vast number of ring and chain compounds or hydrocarbons like alkanes or paraffin (CnH2n+2), alkenes or olefins (CnH2n), acetylene (CnH2n-2), and aromatic compounds. Silicon formed few saturated hydrides or silanes with the common chemical formula SinH2n+2. Acid hydrolysis of magnesium silicide (Mg2Si) gives a mixture of SiH4, Si2H6, Si3H8, and Si4H10. The hydrides are separated and purified by fractional distillation.


Silica or SiO2 is the most common oxides of silicon. The yellow color oxide due to iron (II) oxides is the major constituent of several rocks like granite and sandstone. Many oxides minerals of silicon that are used in gemstones are basically hydrated SiO2. Rose quartz (pink), morion (dark brown), amethyst (violet), citrine (yellow) are the example of such types of gemstones. Silica also occurs in different types of vegetables and animal organisms like straw of cereals, bamboo cane, and sponges.

Silica has different types of macromolecular structures build-up by tetrahedral SiO4 units joined by sharing of oxygen atoms. The two principal forms of silica are quartz and cristobalite.


Silicon tetrahalides may be prepared by the direct reaction of the element with halogens molecule. SiF4 is conveniently prepared by heating a mixture of CaF2 and silica in presence of concentrated sulfuric acid. Unlike the halides of carbon, silicon tetrahalides are rapidly hydrolyzed by water and alkali metals. The halides like SiF4 are partially hydrolyzed by water due to a secondary reaction between HF and SiF4 to produce hexafluorosilicate (SiF6-2).

Uses of Silicon

Most of the silicon compounds are used industrially without being purified. More than 90 percent of the Earth’s crust contains silicate minerals, which are the compounds of silicon and oxygen. Many of these compounds like clays, silica sand, and most kinds of stone can be commercially used in building materials of our civilization. Calcium silicates are used in making Portland cement in building mortar and modern stucco.

Ferrosilicon (a form of silicon) is used extensively for making corrosion-resistant steel. Small quantities of ultra-pure silicon are used in the electronic industry for making semiconductors. It becomes a p-type semiconductor when doped with group-13 elements like aluminum and gallium and n-type semiconductors when doped with group 15 elements like phosphorus and arsenic.