Silicon element periodic table

Silicon is a chemical element with the symbol Si and atomic number 14. It is a hard, brittle, gray-white metalloid that belongs to the group 14 elements in the periodic table. About 90% of the minerals that make up the rocks of the Earth contain silicon. It is therefore a very common element in the crust of our planet. Almost all silicon minerals are compounds of silicon and oxygen, known as silicates. The most common silicate is quartz, the mineral form of silicon dioxide or silica. It is also the most common substance in sand and feldspar. Amethyst is a type of quartz. Quartz deposits are widely found in rocks such as granite and sandstone. A valuable type of silica is opal, which is used as a gemstone. Clays used to make pottery and ceramics are also silicates.

It is a semiconductor, which means it can conduct electricity under certain conditions. Silicon has many important uses, including in the production of silicon carbide and silicon wafers, which are used in the manufacture of semiconductor devices such as computer chips. In 1954, the first silicon transistor started what has become a global semiconductor market. Silicon is a key component of electronic chips and circuits. Wafers are very thin sheets of silicon used to make electronic circuits. It is a very versatile element, so it is also used to convert sunlight into electricity in solar panels. Artificial silica is used to create aerogel, a lightweight but tough substance that is a poor conductor of heat. It is also used in the production of ceramics, glass, and other products, for example, in the fireproof suits worn by firefighters. Another silicon derivative is silicone, which can be molded into any shape. It is used in a wide range of products, from baking molds to watches and breast implants.

Silicon element periodic table

Electron configuration

The electron configuration of an element describes the arrangement of electrons in the atoms of that element, and be used to predict its chemical properties and reactivity.

In the electron configuration notation, the letters "s", "p", "d", and "f" represent the different types of atomic orbitals, and the superscripts indicate the number of electrons in each orbital. The orbitals are filled in a specific order, starting with the lowest energy orbital and working up.

electron configuration of element Si

Emission spectra

Each element in the periodic table presents its own unique emission spectra, which is determined by the energy levels of its electrons. When an electron in an atom is excited to a higher energy level, it can de-excite by emitting a photon of light with an energy equal to the difference between the two levels. This results in a characteristic emission line in the spectra (which corresponds to specific wavelengths of light). These spectra are usefull to identify the elements present in a sample.

emmision spectra of element Si

Symmary of properties (Si)

Atomic weight[28.084, 28.086]
Discoverer (year)Berzelius, Jöns Jacob (1824)
Natural formnon-metallic solid (face-centred cubic)
Electron configuration[Ne] 3s2 3p2
M.p. (ºC)1410
B.p. (ºC)2355
Earth's crust abundance (ppm)282000
Isotope (abundance %)28Si (92.223), 29Si (4.685), 30Si (3.092)
Density (g/cm3)2.33
vdW radius (pm)210
Covalent radius (pm)114
Electronegativity (Pauling)1.9
Vaporisation enthalpy (Kj/mol)383.00
Fusion enthalpy (kJ/mol)50.21
Specific heat capacity (J/g·K) at 25ºC and 1 at0.71
Thermal conductivity (W/cm·K) at 25 ºC and 1 at1.490
Oxidation number+4, +2, -4
Electronic affinity (eV)1.39
1st Ionization energy (eV)8.1517

Definition of terms in the previous table

  • Atomic weight: The average mass of an element's atoms, typically given in atomic mass units (amu).
  • Natural form: The most stable and abundant form of an element that occurs naturally in the environment.
  • Electron configuration: The arrangement of electrons in an atom or molecule.
  • Melting point: The temperature at which a solid substance turns into a liquid.
  • Boiling point: The temperature at which a liquid substance turns into a gas.
  • Earth's crust abundance (ppm): The concentration of an element in the Earth's crust, typically given in parts per million (ppm).
  • Isotope (abundance %): A variant of an element that has the same number of protons in the nucleus, but a different number of neutrons. The abundance of an isotope is the percentage of the isotope in a sample of the element.
  • Density (g/cm3): The mass of a substance per unit volume.
  • vdW radius (pm): The radius of an atom or molecule as predicted by the van der Waals model, typically given in picometers (pm).
  • Covalent radius (pm): The distance from the center of an atom to the center of another atom with which it is bonded covalently, typically given in picometers (pm).
  • Electronegativity (Pauling): A measure of an atom's ability to attract electrons in a chemical bond, based on the Pauling scale.
  • Vaporisation enthalpy (kJ/mol): The amount of energy required to convert a substance from a liquid to a gas at a constant temperature.
  • Fusion enthalpy (kJ/mol): The amount of energy required to convert a substance from a solid to a liquid at a constant temperature.
  • Specific heat capacity (J/g·K) at 25ºC and 1 at: The amount of heat required to raise the temperature of 1 gram of a substance by 1 degree Celsius at a constant pressure.
  • Thermal conductivity (W/cm·K) at 25 ºC and 1 at: The ability of a substance to conduct heat, typically given in watts per centimeter per kelvin.
  • Oxidation number: A positive or negative integer that represents the number of electrons that an atom has gained or lost in a chemical compound.
  • Electronic affinity: The energy change associated with adding an electron to a neutral atom to form a negative ion.
  • 1st Ionization energy: The energy required to remove the most loosely bound electron from a neutral atom.

Back to the Periodic Table of the Elements.