Silicon Atomic Number

Silicon has an atomic number of 14. So for an atom to be known as a Silicon atom, it must have 14 protons. For example, if an atom has 15 protons, it will no longer be silicon, but will instead be Phosphorus. Any atom that doesn’t have 14 protons. 14 Si Silicon 28.0855. Atomic Number: 14. Atomic Weight: 28.0855. Melting Point: 1687 K (1414°C or 2577°F) Boiling Point: 3538 K (3265°C or 5909°F) Density: 2.3296 grams per cubic centimeter. Phase at Room Temperature: Solid. Element Classification: Semi-metal. Period Number: 3. Group Number: 14. Group Name: none. What's in a name? The average silicon atom has fourteen protons, fourteen electrons, and most have 14 neutrons. This is a digram of a silicon atom. This shows the 14 protons in the nucleus and where the 14 electrons are located. The four electron, highlighted in green, that are located in the outer ring are the valence electrons. The atomic mass of an element is the average mass of the atoms of an element measured in atomic mass unit (amu, also known as daltons, D).The atomic mass is a weighted average of all of the isotopes of that element, in which the mass of each isotope is multiplied by the abundance of that particular isotope. Atomic Number: 14. Atomic symbol: Si. Atomic Weight: 28.0855. Electron affinity: -134 kJ/mol. Electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 2.

Silicon 28 Atomic Number
Silicon Atomic Number 32
Silicon Atomic Number And Mass Number
Silicon Atomic Number

In the modern periodic table, the elements are listed in order of increasing atomic number. The atomic number is the number of protons in the nucleus of an atom. The number of protons define the identity of an element (i.e., an element with 6 protons is a carbon atom, no matter how many neutrons may be present). The number of protons determines how many electrons surround the nucleus, and it is the arrangement of these electrons that determines most of the chemical behavior of an element.

In a periodic table arranged in order of increasing atomic number, elements having similar chemical properties naturally line up in the same column (group). For instance, all of the elements in Group 1A are relatively soft metals, react violently with water, and form 1+ charges; all of the elements in Group 8A are unreactive, monatomic gases at room temperature, etc. In other words, there is a periodic repetition of the properties of the chemical elements with increasing mass.

In the original periodic table published by Dimitri Mendeleev in 1869, the elements were arranged according to increasing atomic mass— at that time, the nucleus had not yet been discovered, and there was no understanding at all of the interior structure of the atom, so atomic mass was the only guide to use. Once the structure of the nucleus was understood, it became clear that it was the atomic number that governed the properties of the elements.

(left) Pure Silicon. (right) Silicon is not found free in nature, but occurs chiefly as the oxide and as silicates. Sand is one of the forms in which the oxide appears.

Silicon

Atomic Number:	14	Atomic Radius:	210 pm (Van der Waals)
Atomic Symbol:	Si	Melting Point:	1414 °C
Atomic Weight:	28.09	Boiling Point:	3265 °C
Electron Configuration:	[Ne]3s²3p²	Oxidation States:	4, 3, 2, 1[2] −1, −2, −3, −4 (an amphoteric oxide)

History

From the Latin. word silex, silicis, flint. In 1800, Davy thought silica to be a compound and not an element; but in 1811, Gay Lussac and Thenard probably prepared impure amorphous silicon by heating potassium with silicon tetrafluoride.

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

Sources

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

Silicon makes up 25.7% of the earth's crust, by weight, and is the second most abundant element, being exceeded only by oxygen. Silicon is not 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 the oxide appears. Granite, hornblende, asbestos, feldspar, clay, mica, etc. are but a few of the 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 or vaporized. The Czochralski process is commonly used to produce single crystals of silicon used for solid-state or semiconductor devices. Hyperpure silicon can be prepared by the thermal decomposition of ultra-pure trichlorosilane in a hydrogen atmosphere, and by a vacuum float zone process.

Silicon 28 Atomic Number

Uses

Silicon is one of man's most useful elements. In the form of sand and clay it is used to make concrete and brick; it is a useful refractory material for high-temperature work, and in the form of silicates it is used in making enamels, pottery, etc. Silica, as sand, is a principal ingredient of glass, one of the most inexpensive of materials with excellent mechanical, optical, thermal, and electrical properties. Glass can be made in a very great variety of shapes, and is used as containers, window glass, insulators, and thousands of other uses. Silicon tetrachloride can be used as iridize glass.

Microsoft edge youtube problems. Hyperpure silicon can be doped with boron, gallium, phosphorus, or arsenic to produce silicon for use in transistors, solar cells, rectifiers, and other solid-state devices which are used extensively in the electronics and space-age industries.

Hydrogenated amorphous silicon has shown promise in producing economical cells for converting solar energy into electricity.

Silicon is important to plant and animal life. Diatoms in both fresh and salt water extract Silica from the water to build their cell walls. Silica is present in the ashes of plants and in the human skeleton. Silicon is an important ingredient in steel; silicon carbide is one of the most important abrasives and has been used in lasers to produce coherent light of 4560 A.

Silcones are important products of silicon. They may be prepared by hydrolyzing a silicon organic chloride, such as dimethyl silicon chloride. Driver for hp laserjet 1010 for mac. Hydrolysis and condensation of various substituted chlorosilanes can be used to produce a very great number of polymeric products, or silicones, ranging from liquids to hard, glasslike solids with many useful properties.