Alkali metal halide: Difference between revisions
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{{short description|Family of compounds consisting of an alkali metal bonded to a halogen}} |
{{short description|Family of compounds consisting of an alkali metal bonded to a halogen}} |
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'''Alkali metal halides''', or '''alkali halides''', are the family of [[inorganic compound]]s with the [[chemical formula]] MX, where M is an [[alkali metal]] and X is a [[halogen]]. These compounds are the often commercially significant sources of these metals and halides. The best known of these compounds is [[sodium chloride]], [[table salt]].<ref>Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. {{ISBN|0-7506-3365-4}}.</ref> |
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[[File:Halit-Kristalle.jpg|180px|right|thumb|[[Halite]] is the mineral form of [[sodium chloride]].]] |
[[File:Halit-Kristalle.jpg|180px|right|thumb|[[Halite]] is the mineral form of [[sodium chloride]].]] |
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Latest revision as of 16:33, 25 October 2023
Alkali metal halides, or alkali halides, are the family of inorganic compounds with the chemical formula MX, where M is an alkali metal and X is a halogen. These compounds are the often commercially significant sources of these metals and halides. The best known of these compounds is sodium chloride, table salt.[1]
Structure
[edit]Most alkali metal halides crystallize with the face-centered cubic lattices. In this structure both the metals and halides feature octahedral coordination geometry, in which each ion has a coordination number of six. Caesium chloride, bromide, and iodide crystallize in a body-centered cubic lattice that accommodates coordination number of eight for the larger metal cation (and the anion also).[2]
Properties
[edit]The alkali metal halides exist as colourless crystalline solids, although as finely ground powders appear white. They melt at high temperature, usually several hundred degrees to colorless liquids. Their high melting point reflects their high lattice energies. At still higher temperatures, these liquids evaporate to give gases composed of diatomic molecules.
These compounds dissolve in polar solvents to give ionic solutions that contain highly solvated anions and cations. Alkali halides dissolve large amounts of the corresponding alkali metal: caesium is completely miscible at all temperatures above the melting point.[3]
The table below provides links to each of the individual articles for these compounds. The numbers beside the compounds show the electronegativity difference between the elements based on the Pauling scale. The higher the number is, the more ionic the solid is.
| Alkali metals | |||||||
|---|---|---|---|---|---|---|---|
| Lithium | Sodium | Potassium | Rubidium | Caesium | |||
Halogens
|
Fluorine | LiF (3.0) | NaF (3.1) | KF (3.2) | RbF (3.2) | CsF (3.3) | |
| Chlorine | LiCl (2.0) | NaCl (2.1) | KCl (2.2) | RbCl (2.2) | CsCl (2.3) | ||
| Bromine | LiBr (1.8) | NaBr (1.9) | KBr (2.0) | RbBr (2.0) | CsBr (2.1) | ||
| Iodine | LiI (1.5) | NaI (1.6) | KI (1.7) | RbI (1.7) | CsI (1.8) | ||
References
[edit]- ^ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
- ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
- ^ Huheey, James E.; Keiter, Ellen A.; Kieter, Richard L. (1993). Inorganic chemistry : principles of structure and reactivity (4. ed.). Cambridge, Massachusetts [u.a.]: Harper. pp. 377. ISBN 006042995X.