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Sodium atoms have 11 electrons, one more than the stable configuration of the noble gas neon. As a result, sodium usually forms ionic compounds involving the Na + cation. [1] Sodium is a reactive alkali metal and is much more stable in ionic compounds. It can also form intermetallic compounds and organosodium compounds.
Sodium is a chemical element; it has symbol Na (from Neo-Latin natrium) and atomic number 11. It is a soft, silvery-white, highly reactive metal. Sodium is an alkali metal, being in group 1 of the periodic table. Its only stable isotope is 23 Na. The free metal does not occur in nature and must be prepared from compounds.
Solvated electrons are involved in the reaction of alkali metals with water, even though the solvated electron has only a fleeting existence. [10] Below pH = 9.6 the hydrated electron reacts with the hydronium ion giving atomic hydrogen, which in turn can react with the hydrated electron giving hydroxide ion and usual molecular hydrogen H 2 .
Reaction with an excess of the chalcogen can similarly result in lower chalcogenides, with chalcogen ions containing chains of the chalcogen atoms in question. For example, sodium can react with sulfur to form the sulfide (Na 2 S) and various polysulfides with the formula Na 2 S x (x from 2 to 6), containing the S 2− x ions. [65]
The oppositely charged ions – typically a great many of them – are then attracted to each other to form solid sodium fluoride. Ionic bonding is a type of chemical bonding that involves the electrostatic attraction between oppositely charged ions , or between two atoms with sharply different electronegativities , [ 1 ] and is the primary ...
A schematic electron shell diagram of sodium and fluorine atoms undergoing a redox reaction to form sodium fluoride. Sodium loses its outer electron to give it a stable electron configuration, and this electron enters the fluorine atom exothermically. The oppositely charged ions – typically a great many of them – are then attracted to each ...
Overall reaction: 2 H 2 O + 2 Cl − (aq) → H 2 (g) + Cl 2 (g) + 2 OH − (aq) As the overall reaction indicates, the concentration of chloride ions is reduced in comparison to OH − ions (whose concentration increases). The reaction also shows the production of gaseous hydrogen, chlorine and aqueous sodium hydroxide.
Illustration of a redox reaction Sodium chloride is formed through the redox reaction of sodium metal and chlorine gas. Redox reactions can be understood in terms of the transfer of electrons from one involved species (reducing agent) to another (oxidizing agent). In this process, the former species is oxidized and the latter is reduced. Though ...