Orbit Number Value of ‘l’ Number of subshells Number of orbitals Subshell name Electrons holding capacity Electron configuration 1 0 1 1 1s 2 1s2 2 01 2 13 2s2p 26 2s2 2p6 3 012 3 135 3s3p3d 2610 3s2 4s4p4d4f 261014 4s2 4p6 4d10 4f14 In this system, the s-energy shell has one orbital the p-energy shell has three orbitals, and so on, up to the f-energy shell, which has seven orbitals. The orbit number n can be used to determine the Azimuthal number ‘ I.’ ‘I’ ranges from 0 to n-1. These are based on the Aufbau principle and are represented by s,p,d, and f. The electronic configuration of Silicon can also be expressed as a function of orbital sub-energy levels determined by the Azimuthal quantum number. The 14 electrons can be distributed amongst the first three atomic shells in a 2,8,4 configuration.
Then, the electronic configuration of an element describes how its electrons are distributed in its orbitals. The number of electrons in K orbit = 2(1) 2 = 2. The electron capacity of each orbit is given by 2 n 2. The first four orbits are labeled K, L, M, and N, where n = 1,2,3 & 4, respectively. Orbits can be expressed using the symbol n. Electrons in the atom revolve around the nucleus in paths known as orbits. Scientist Niels Bohr first described electron structures and orbits in 1913. Semiconductor electronics are a multi-billion dollar industry. Adding donor and acceptor atoms in the crystalline silicon lattice allows for positive and negative types of extrinsic conduction. Silicon’s electronic structure makes it an extremely valuable semiconductor. Let us dive deeper into its electron structure in the next section. Other silicon-based compounds and minerals, such as silica and quartz, are used in construction and glassware. High-grade pure Silicon is infused with boron, arsenic, and phosphorus to produce silicon wafers used in transistors, diodes, liquid crystal displays, and integrated circuitry. Most Silicon used commercially is unprocessed however, Silicon has played a key role in ushering in the digital age we know today. Silicon also reacts with Carbon and hydrogen to form silicon carbide (SiC) and hydrides. Silicon forms a continuous layer of SiO 2 over the metallic surface to protect it from Oxidation. Silicon is relatively inert but reacts vigorously with halides and metals at high temperatures. Silicon binds with oxygen to form silicates commonly found in the earth’s crust. Silicon appears as a dark blue-grey solid with a metallic luster. It can be found under Carbon (Z = 6) in the periodic table of elements and is commonly classified as a metalloid. Silicon is a chemical element with the atomic number Z = 14.
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