Properties Of Silicon

Silicon is an important element in chemistry as well as in electronics. It is abundantly found in earth crust and possess unique properties. The properties of silicon can be studied in two categories

• Physical Properties of Silicon
• Chemical Properties of Silicon

Physical Properties of Silicon

The physical properties of silicon are mentioned below:

State at Room Temperature: At standard room temperature silicon has a solid structure. It is formed from a hexagonal structure resembling crystals, resulting in an appealing metallic sheen.

Density: A silicon density tucked in approximately 2.3296 grams per cubic centimeter. Low density leads to the mouldings significance because it is lightweight.

Melting Point: Silicon has very high melting point of 1,414℃(2,577 ℉ )

Boiling Point: The melting point of silica is likewise very high approximating 2180℃(3915℉ ).

Crystal Structure: Silicon has cubic diamond crystal lattices that offer a degree of hardness and a strength to silicon.

Electrical Conductivity: Silicon is a semiconductor. It has medium electrical conductivity. This makes it suitable for usage in electronics sector.

Malleability and Ductility: Silicon is neither malleable or ductile. Rather it is hard and brittle

Chemical Properties of Silicon

The chemical properties of silicon are mentioned below:

Reactivity: Silicon is chemically harmless under normal circumstances. It does not readily react with the majority of acids or bases.

Oxidation: When the silicon meets oxygen, it forms an SiO₂ (Silicon dioxide) layer on its surface. This oxide layer act in passivation role, hence protecting underlying layer from oxidation.

Combustibility: Silicon does not react easily in standard atmospheric conditions; this is perfect for its use in high-temperature applications.

Hydride Formation: Silicon reacts with hydrogen creating hydrides, such as silane (SiH₄).

Halogen Reactivity: Reaction of silicon with halogens (fluorine, chlorine, bromine, iodine) gives silicon tetrahalides, e.g. silicon tetrafluoride (SiF₄) and silicon tetrachloride (SiCl₄).

Alloy Formation: Silicon forms compounds with metals that are lighter than it, such as ferrosilicon(iron and silicon alloy).

Amphoteric Nature: Silicon has a characteristic of being amphoteric which implies that it can react as an acid and as a base. It may form salts with either acid or base.

Reaction with Alkali Metals: Si interacts with alkali metals (such as sodium and potassium) to produce silicides.

Silicon is second most abundant element found in earth’s crust. It constitutes about 27.7% of the total mass of earth’s crust. Silicon is represented by the symbol ‘Si’. Its atomic number is 14 and is found in group 14 and the third period of the periodic table. It is metalloid in nature and forms the backbone of the semiconductor industry. Due to its low reactivity, it is also used in body implants.

In this article, we will learn in detail about silicon, its symbol, properties, and applications.