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In chemistry and atomic physics, an electron shell may be thought of as an orbit that electrons follow around an atom's nucleus.The closest shell to the nucleus is called the "1 shell" (also called the "K shell"), followed by the "2 shell" (or "L shell"), then the "3 shell" (or "M shell"), and so on further and further from the nucleus.
In chemistry and physics, valence electrons are electrons in the outermost shell of an atom, and that can participate in the formation of a chemical bond if the outermost shell is not closed. In a single covalent bond , a shared pair forms with both atoms in the bond each contributing one valence electron.
The valence electrons (here 3s 2 3p 3) are written explicitly for all atoms. Electron configurations of elements beyond hassium (element 108) have never been measured; predictions are used below. As an approximate rule, electron configurations are given by the Aufbau principle and the Madelung rule .
According to this theory a covalent bond is formed between two atoms by the overlap of half filled valence atomic orbitals of each atom containing one unpaired electron. Valence Bond theory describes chemical bonding better than Lewis Theory, which states that atoms share or transfer electrons so that they achieve the octet rule.
8 O 2 4 9 F 2 5 10 Ne 2 6 [Ne] 3s: 3p: 11 Na 1 - 12 Mg 2 - 13 Al 2 1 14 Si 2 2 15 P 2 3 16 S 2 4 17 Cl 2 5 18 Ar 2 6 [Ar] 4s: 3d: 4p: 19 K 1-- 20 Ca 2-- 21 Sc 2 1 - 22 Ti 2 2 - 23 V 2 3 - 24 Cr 1 5 - 25 Mn 2 5 - 26 Fe 2 6 - 27 Co 2 7 - 28 Ni 2 8 - 29 Cu 1 10 - 30 Zn 2 10 - 31 Ga 2 10 1 32 Ge 2 10 2 33 As 2 10 3 34 Se 2 10 4 35 Br 2 10 5 36 Kr 2 ...
This is a list of chemical elements and their atomic properties, ordered by atomic number (Z).. Since valence electrons are not clearly defined for the d-block and f-block elements, there not being a clear point at which further ionisation becomes unprofitable, a purely formal definition as number of electrons in the outermost shell has been used.
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In the bond valence model, the valence of an atom, V, is defined as the number of electrons the atom uses for bonding. This is equal to the number of electrons in its valence shell if all the valence shell electrons are used for bonding. If they are not, the remainder will form non-bonding electron pairs, usually known as lone pairs.